{"id":105948,"date":"2026-07-17T18:06:23","date_gmt":"2026-07-17T12:36:23","guid":{"rendered":"https:\/\/seminarsonly.com\/news\/?p=105948"},"modified":"2026-07-17T18:06:23","modified_gmt":"2026-07-17T12:36:23","slug":"class-10-chemistry-chapter-2-notes","status":"publish","type":"post","link":"https:\/\/seminarsonly.com\/news\/class-10-chemistry-chapter-2-notes\/","title":{"rendered":"Class 10 Chemistry Chapter 2 Notes: Acids, Bases and Salts (NCERT)"},"content":{"rendered":"<article style=\"font-family: -apple-system,BlinkMacSystemFont,'Segoe UI',Roboto,Oxygen,Ubuntu,sans-serif; line-height: 1.75; color: #1e293b; padding: 0 16px; box-sizing: border-box;\"><!-- FEATURED IMAGE --><br \/>\n<img decoding=\"async\" style=\"width: 100%; max-width: 1200px; height: auto; border-radius: 12px; margin: 0 auto 28px auto; display: block; box-shadow: 0 8px 24px rgba(0,0,0,0.12);\" src=\"https:\/\/seminarsonly.com\/news\/wp-content\/uploads\/2026\/07\/class-10-chemistry-chapter-2-featured.jpg\" alt=\"Class 10 Chemistry Chapter 2 Acids Bases and Salts notes banner with pH scale, chemistry flask, and salt crystals, NCERT board exam guide\" width=\"1200\" height=\"675\" \/><!-- QUICK ANSWER --><\/p>\n<div style=\"background: linear-gradient(135deg,#10b981 0%,#059669 100%); color: #fff; padding: 28px 32px; border-radius: 16px; margin: 0 0 28px 0; box-shadow: 0 8px 24px rgba(16,185,129,0.25); border-left: 6px solid #34d399;\" role=\"region\" aria-label=\"Quick Answer\">\n<h2 style=\"color: #fff; margin: 0 0 12px 0; font-size: 1.45em; font-weight: bold; border: none; padding: 0;\">\u26a1 Quick Answer<\/h2>\n<p style=\"margin: 0; font-size: 1.05em; line-height: 1.7;\"><strong style=\"color: #fef3c7;\">Class 10 Chemistry Chapter 2<\/strong> covers <strong>Acids, Bases and Salts<\/strong>. Key topics include: <span style=\"background: rgba(254,243,199,0.25); padding: 2px 8px; border-radius: 4px; font-weight: bold; color: #fff;\">definitions and examples of acids and bases<\/span>, <span style=\"background: rgba(254,243,199,0.25); padding: 2px 8px; border-radius: 4px; font-weight: bold; color: #fff;\">the pH scale (0-14)<\/span>, <span style=\"background: rgba(254,243,199,0.25); padding: 2px 8px; border-radius: 4px; font-weight: bold; color: #fff;\">chemical properties and reactions<\/span>, and <span style=\"background: rgba(254,243,199,0.25); padding: 2px 8px; border-radius: 4px; font-weight: bold; color: #fff;\">important salts like common salt, baking soda, and washing soda<\/span>. This chapter carries 5 marks in the CBSE Class 10 Board Exam.<\/p>\n<\/div>\n<p><!-- TLDR BOX --><\/p>\n<div style=\"background: linear-gradient(135deg,#f59e0b 0%,#d97706 100%); color: #fff; padding: 24px 28px; border-radius: 14px; margin: 0 0 28px 0; box-shadow: 0 6px 20px rgba(245,158,11,0.2); border-left: 6px solid #fcd34d;\" role=\"region\" aria-label=\"TLDR Summary\">\n<h3 style=\"color: #fff; margin: 0 0 12px 0; font-size: 1.25em; font-weight: bold; border: none; padding: 0;\">\ud83d\udccb TL;DR \u2014 Chapter 2 at a Glance<\/h3>\n<ul style=\"margin: 0; padding-left: 20px;\">\n<li style=\"margin-bottom: 8px; font-size: 0.98em;\"><strong>Acids<\/strong> are sour, turn blue litmus red, and release H\u207a ions in water. Examples: HCl, H\u2082SO\u2084, citric acid.<\/li>\n<li style=\"margin-bottom: 8px; font-size: 0.98em;\"><strong>Bases<\/strong> are bitter, turn red litmus blue, and release OH\u207b ions. Examples: NaOH, Ca(OH)\u2082, KOH.<\/li>\n<li style=\"margin-bottom: 8px; font-size: 0.98em;\"><strong>pH scale<\/strong> measures acidity (0-6), neutrality (7), and alkalinity (8-14). Universal indicator gives different colours.<\/li>\n<li style=\"margin-bottom: 8px; font-size: 0.98em;\"><strong>Salts<\/strong> are formed by neutralization. Important salts: NaCl (common salt), NaHCO\u2083 (baking soda), Na\u2082CO\u2083\u00b710H\u2082O (washing soda).<\/li>\n<\/ul>\n<\/div>\n<h2 style=\"color: #059669; font-size: 1.75em; margin: 40px 0 16px 0; padding: 0 0 10px 0; border-bottom: 3px solid #10b981; font-weight: bold; line-height: 1.3;\">Introduction to Acids, Bases and Salts<\/h2>\n<p style=\"margin: 0 0 1.2em 0;\">Chapter 2 of the NCERT Class 10 Science textbook introduces you to the fascinating world of <strong>Acids, Bases and Salts<\/strong> \u2014 three fundamental categories of chemical compounds that surround us every day. From the citric acid in your oranges to the baking soda in your kitchen, from the hydrochloric acid in your stomach to the soap you use to wash your hands, this chapter explains the chemistry behind substances we encounter constantly.<\/p>\n<p style=\"margin: 0 0 1.2em 0;\">For the <strong>CBSE Class 10 Board Exam<\/strong>, this chapter is critical. It typically carries <strong>5 marks<\/strong> and includes questions on definitions, chemical equations, the pH scale, and practical applications of salts. Understanding the concepts clearly here will also help you in Class 11 Chemistry, where these topics are explored in much greater depth.<\/p>\n<div style=\"background: #ecfdf5; border-left: 5px solid #10b981; padding: 18px 22px; border-radius: 0 12px 12px 0; margin: 20px 0;\"><strong>\ud83d\udca1 Exam Tip:<\/strong> Focus on <strong>chemical equations<\/strong> and <strong>the pH scale<\/strong> \u2014 these are the most frequently asked topics in Board Exams. Write and practice every reaction at least 3 times before the exam.<\/div>\n<h2 style=\"color: #059669; font-size: 1.75em; margin: 40px 0 16px 0; padding: 0 0 10px 0; border-bottom: 3px solid #10b981; font-weight: bold; line-height: 1.3;\">What Are Acids? Definition, Types and Examples<\/h2>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">Definition of Acids<\/h3>\n<p style=\"margin: 0 0 1.2em 0;\">An <strong>acid<\/strong> is a substance that tastes sour, turns blue litmus paper red, and releases hydrogen ions (H\u207a) when dissolved in water. The word &#8220;acid&#8221; comes from the Latin <em>acidus<\/em>, meaning sour. All acids contain hydrogen as an essential constituent.<\/p>\n<p style=\"margin: 0 0 1.2em 0;\">According to the <strong>Arrhenius theory<\/strong>, acids are substances that dissociate in water to produce hydrogen ions (H\u207a). For example:<\/p>\n<p style=\"margin: 0 0 1.2em 0; font-family: 'Courier New',monospace; background: #f1f5f9; padding: 12px 16px; border-radius: 8px; font-size: 0.95em;\">HCl \u2192 H\u207a + Cl\u207b<br \/>\nH\u2082SO\u2084 \u2192 2H\u207a + SO\u2084\u00b2\u207b<\/p>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">Types of Acids<\/h3>\n<table style=\"width: 100%; border-collapse: collapse; margin: 20px 0; border-radius: 12px; overflow: hidden; box-shadow: 0 4px 16px rgba(0,0,0,0.08); font-size: 0.95em;\" role=\"table\" aria-label=\"Types of acids with examples\">\n<thead>\n<tr style=\"background: linear-gradient(135deg,#059669 0%,#10b981 100%); color: #fff; text-align: left;\">\n<th style=\"padding: 14px 16px; font-weight: bold;\">Type<\/th>\n<th style=\"padding: 14px 16px; font-weight: bold;\">Definition<\/th>\n<th style=\"padding: 14px 16px; font-weight: bold;\">Examples<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr style=\"border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>Mineral Acids (Inorganic)<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Derived from minerals; strong and corrosive<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">HCl, H\u2082SO\u2084, HNO\u2083<\/td>\n<\/tr>\n<tr style=\"background: #f8fafc; border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>Organic Acids<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Found in plants and animals; weak acids<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Citric acid, acetic acid, tartaric acid<\/td>\n<\/tr>\n<tr style=\"border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>Strong Acids<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Completely dissociate in water<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">HCl, H\u2082SO\u2084, HNO\u2083<\/td>\n<\/tr>\n<tr style=\"background: #f8fafc; border-bottom: 2px solid #059669;\">\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\"><strong>Weak Acids<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\">Partially dissociate in water<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\">CH\u2083COOH, carbonic acid (H\u2082CO\u2083)<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">Physical Properties of Acids<\/h3>\n<ul style=\"padding-left: 24px; margin: 0 0 1.2em 0;\">\n<li style=\"margin-bottom: 10px;\">Sour taste (e.g., lemon, vinegar)<\/li>\n<li style=\"margin-bottom: 10px;\">Turn <strong>blue litmus paper red<\/strong><\/li>\n<li style=\"margin-bottom: 10px;\">Conduct electricity in aqueous solution (electrolytes)<\/li>\n<li style=\"margin-bottom: 10px;\">React with metals to produce hydrogen gas<\/li>\n<li style=\"margin-bottom: 10px;\">Strong acids are corrosive and cause burns on skin<\/li>\n<\/ul>\n<h2 style=\"color: #059669; font-size: 1.75em; margin: 40px 0 16px 0; padding: 0 0 10px 0; border-bottom: 3px solid #10b981; font-weight: bold; line-height: 1.3;\">What Are Bases? Definition, Types and Examples<\/h2>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">Definition of Bases<\/h3>\n<p style=\"margin: 0 0 1.2em 0;\">A <strong>base<\/strong> is a substance that tastes bitter, feels soapy to touch, turns red litmus paper blue, and releases hydroxide ions (OH\u207b) when dissolved in water. According to the <strong>Arrhenius theory<\/strong>, bases are substances that dissociate in water to produce hydroxide ions.<\/p>\n<p style=\"margin: 0 0 1.2em 0; font-family: 'Courier New',monospace; background: #f1f5f9; padding: 12px 16px; border-radius: 8px; font-size: 0.95em;\">NaOH \u2192 Na\u207a + OH\u207b<br \/>\nCa(OH)\u2082 \u2192 Ca\u00b2\u207a + 2OH\u207b<\/p>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">Types of Bases<\/h3>\n<table style=\"width: 100%; border-collapse: collapse; margin: 20px 0; border-radius: 12px; overflow: hidden; box-shadow: 0 4px 16px rgba(0,0,0,0.08); font-size: 0.95em;\" role=\"table\" aria-label=\"Types of bases with examples\">\n<thead>\n<tr style=\"background: linear-gradient(135deg,#059669 0%,#10b981 100%); color: #fff; text-align: left;\">\n<th style=\"padding: 14px 16px; font-weight: bold;\">Type<\/th>\n<th style=\"padding: 14px 16px; font-weight: bold;\">Definition<\/th>\n<th style=\"padding: 14px 16px; font-weight: bold;\">Examples<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr style=\"border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>Strong Bases<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Completely dissociate in water<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">NaOH, KOH, Ca(OH)\u2082<\/td>\n<\/tr>\n<tr style=\"background: #f8fafc; border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>Weak Bases<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Partially dissociate in water<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">NH\u2084OH (ammonium hydroxide), Mg(OH)\u2082<\/td>\n<\/tr>\n<tr style=\"border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>Alkalis<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Bases that dissolve in water<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">NaOH, KOH, Ca(OH)\u2082<\/td>\n<\/tr>\n<tr style=\"background: #f8fafc; border-bottom: 2px solid #059669;\">\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\"><strong>Metal Oxides \/ Hydroxides<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\">Basic oxides that react with acids<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\">CuO, ZnO, Na\u2082O, CaO<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">Physical Properties of Bases<\/h3>\n<ul style=\"padding-left: 24px; margin: 0 0 1.2em 0;\">\n<li style=\"margin-bottom: 10px;\">Bitter taste (e.g., soap, baking soda)<\/li>\n<li style=\"margin-bottom: 10px;\">Turn <strong>red litmus paper blue<\/strong><\/li>\n<li style=\"margin-bottom: 10px;\">Feel soapy or slippery to touch<\/li>\n<li style=\"margin-bottom: 10px;\">Conduct electricity in aqueous solution<\/li>\n<li style=\"margin-bottom: 10px;\">Strong bases are caustic and cause skin burns<\/li>\n<\/ul>\n<div style=\"background: #fffbeb; border-left: 5px solid #f59e0b; padding: 18px 22px; border-radius: 0 12px 12px 0; margin: 20px 0;\"><strong>\u26a0\ufe0f Safety Note:<\/strong> Never taste or touch acids and bases directly in the lab. Strong acids and bases are both corrosive and can cause severe burns. Always use dilute solutions and wear safety equipment.<\/div>\n<h2 style=\"color: #059669; font-size: 1.75em; margin: 40px 0 16px 0; padding: 0 0 10px 0; border-bottom: 3px solid #10b981; font-weight: bold; line-height: 1.3;\">The pH Scale: Measuring Acidity and Alkalinity<\/h2>\n<p style=\"margin: 0 0 1.2em 0;\">The <strong>pH scale<\/strong> is a measure of the acidity or alkalinity of a solution. It ranges from <strong>0 to 14<\/strong>, where pH stands for &#8220;potential of hydrogen.&#8221; The concentration of hydrogen ions [H\u207a] determines the pH value.<\/p>\n<table style=\"width: 100%; border-collapse: collapse; margin: 20px 0; border-radius: 12px; overflow: hidden; box-shadow: 0 4px 16px rgba(0,0,0,0.08); font-size: 0.95em;\" role=\"table\" aria-label=\"pH scale values and their meanings\">\n<thead>\n<tr style=\"background: linear-gradient(135deg,#059669 0%,#10b981 100%); color: #fff; text-align: left;\">\n<th style=\"padding: 14px 16px; font-weight: bold;\">pH Range<\/th>\n<th style=\"padding: 14px 16px; font-weight: bold;\">Nature<\/th>\n<th style=\"padding: 14px 16px; font-weight: bold;\">Examples<\/th>\n<th style=\"padding: 14px 16px; font-weight: bold;\">Universal Indicator Colour<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr style=\"border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>0 \u2013 2<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Strongly acidic<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Gastric juice, battery acid<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Red<\/td>\n<\/tr>\n<tr style=\"background: #f8fafc; border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>3 \u2013 4<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Weakly acidic<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Lemon juice, vinegar, soft drinks<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Orange<\/td>\n<\/tr>\n<tr style=\"border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>5 \u2013 6<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Very weakly acidic<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Coffee, milk, rainwater<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Yellow<\/td>\n<\/tr>\n<tr style=\"background: #f8fafc; border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>7<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>Neutral<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Pure water, blood plasma<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Green<\/td>\n<\/tr>\n<tr style=\"border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>8 \u2013 10<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Weakly alkaline<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Baking soda, egg white, sea water<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Blue<\/td>\n<\/tr>\n<tr style=\"background: #f8fafc; border-bottom: 2px solid #059669;\">\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\"><strong>11 \u2013 14<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\">Strongly alkaline<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\">Bleach, drain cleaner, oven cleaner<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\">Purple \/ Violet<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">Importance of pH in Daily Life<\/h3>\n<ul style=\"padding-left: 24px; margin: 0 0 1.2em 0;\">\n<li style=\"margin-bottom: 10px;\"><strong>Human body:<\/strong> Our blood has a pH of 7.4. Even a small change can be fatal. Antacids neutralize excess stomach acid (pH 1.5-3.5) to prevent acidity.<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Agriculture:<\/strong> Plants need soil pH between 6.5-7.5 for optimal growth. Acidic soil is treated with lime (CaO).<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Water treatment:<\/strong> Drinking water should have pH 6.5-8.5. Acidic water corrodes pipes; alkaline water tastes bitter.<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Tooth decay:<\/strong> Bacteria produce acids (pH &lt; 5.5) that damage tooth enamel. Toothpaste is basic to neutralize this.<\/li>\n<\/ul>\n<h2 style=\"color: #059669; font-size: 1.75em; margin: 40px 0 16px 0; padding: 0 0 10px 0; border-bottom: 3px solid #10b981; font-weight: bold; line-height: 1.3;\">Chemical Properties and Reactions<\/h2>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">1. Reaction of Acids with Metals<\/h3>\n<p style=\"margin: 0 0 1.2em 0;\">Acids react with active metals (above hydrogen in the reactivity series) to produce salt and hydrogen gas:<\/p>\n<p style=\"margin: 0 0 1.2em 0; font-family: 'Courier New',monospace; background: #f1f5f9; padding: 12px 16px; border-radius: 8px; font-size: 0.95em;\">Zn + 2HCl \u2192 ZnCl\u2082 + H\u2082\u2191<br \/>\nMg + H\u2082SO\u2084 \u2192 MgSO\u2084 + H\u2082\u2191<\/p>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">2. Reaction of Acids with Metal Carbonates and Hydrogen Carbonates<\/h3>\n<p style=\"margin: 0 0 1.2em 0;\">Acids react with metal carbonates and hydrogen carbonates to produce salt, water, and carbon dioxide gas. This is the basis of the <strong>lime water test<\/strong> for CO\u2082:<\/p>\n<p style=\"margin: 0 0 1.2em 0; font-family: 'Courier New',monospace; background: #f1f5f9; padding: 12px 16px; border-radius: 8px; font-size: 0.95em;\">Na\u2082CO\u2083 + 2HCl \u2192 2NaCl + H\u2082O + CO\u2082\u2191<br \/>\nNaHCO\u2083 + HCl \u2192 NaCl + H\u2082O + CO\u2082\u2191<\/p>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">3. Reaction of Acids with Bases (Neutralization)<\/h3>\n<p style=\"margin: 0 0 1.2em 0;\">When an acid reacts with a base, they neutralize each other to form <strong>salt and water<\/strong>. This reaction is called <strong>neutralization<\/strong> and is exothermic:<\/p>\n<p style=\"margin: 0 0 1.2em 0; font-family: 'Courier New',monospace; background: #f1f5f9; padding: 12px 16px; border-radius: 8px; font-size: 0.95em;\">NaOH + HCl \u2192 NaCl + H\u2082O + Heat<br \/>\nCa(OH)\u2082 + H\u2082SO\u2084 \u2192 CaSO\u2084 + 2H\u2082O + Heat<\/p>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">4. Reaction of Bases with Metals<\/h3>\n<p style=\"margin: 0 0 1.2em 0;\">Not all metals react with bases. Only <strong>amphoteric metals<\/strong> like aluminium and zinc react with strong bases to produce salt and hydrogen:<\/p>\n<p style=\"margin: 0 0 1.2em 0; font-family: 'Courier New',monospace; background: #f1f5f9; padding: 12px 16px; border-radius: 8px; font-size: 0.95em;\">2Al + 2NaOH + 2H\u2082O \u2192 2NaAlO\u2082 + 3H\u2082\u2191<br \/>\nZn + 2NaOH \u2192 Na\u2082ZnO\u2082 + H\u2082\u2191<\/p>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">5. Reaction of Bases with Non-Metal Oxides<\/h3>\n<p style=\"margin: 0 0 1.2em 0;\">Non-metal oxides are acidic in nature. They react with bases to form salt and water:<\/p>\n<p style=\"margin: 0 0 1.2em 0; font-family: 'Courier New',monospace; background: #f1f5f9; padding: 12px 16px; border-radius: 8px; font-size: 0.95em;\">CO\u2082 + 2NaOH \u2192 Na\u2082CO\u2083 + H\u2082O<br \/>\nSO\u2082 + 2NaOH \u2192 Na\u2082SO\u2083 + H\u2082O<\/p>\n<div style=\"background: #ecfdf5; border-left: 5px solid #10b981; padding: 18px 22px; border-radius: 0 12px 12px 0; margin: 20px 0;\"><strong>\ud83d\udca1 Board Exam Tip:<\/strong> Always write the <strong>state symbols<\/strong> (s, l, g, aq) in chemical equations. For example: <code>Zn(s) + 2HCl(aq) \u2192 ZnCl\u2082(aq) + H\u2082(g)<\/code>. This earns you full marks in the exam.<\/div>\n<h2 style=\"color: #059669; font-size: 1.75em; margin: 40px 0 16px 0; padding: 0 0 10px 0; border-bottom: 3px solid #10b981; font-weight: bold; line-height: 1.3;\">Important Salts: Preparation, Properties and Uses<\/h2>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">1. Common Salt (Sodium Chloride \u2014 NaCl)<\/h3>\n<ul style=\"padding-left: 24px; margin: 0 0 1.2em 0;\">\n<li style=\"margin-bottom: 10px;\"><strong>Source:<\/strong> Obtained from seawater and rock salt mines.<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Preparation:<\/strong> Evaporation of seawater in salt pans.<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Uses:<\/strong> Food preservative, seasoning, manufacture of chlorine, caustic soda, and baking soda.<\/li>\n<\/ul>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">2. Baking Soda (Sodium Hydrogen Carbonate \u2014 NaHCO\u2083)<\/h3>\n<ul style=\"padding-left: 24px; margin: 0 0 1.2em 0;\">\n<li style=\"margin-bottom: 10px;\"><strong>Preparation:<\/strong> Solvay process: NaCl + NH\u2083 + CO\u2082 + H\u2082O \u2192 NaHCO\u2083 + NH\u2084Cl<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Properties:<\/strong> Mild, non-corrosive base. Releases CO\u2082 when heated or mixed with acid.<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Uses:<\/strong> Baking (makes cakes fluffy), antacid (relieves acidity), fire extinguisher (produces CO\u2082).<\/li>\n<\/ul>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">3. Washing Soda (Sodium Carbonate Decahydrate \u2014 Na\u2082CO\u2083\u00b710H\u2082O)<\/h3>\n<ul style=\"padding-left: 24px; margin: 0 0 1.2em 0;\">\n<li style=\"margin-bottom: 10px;\"><strong>Preparation:<\/strong> Heating baking soda: 2NaHCO\u2083 \u2192 Na\u2082CO\u2083 + H\u2082O + CO\u2082. Then recrystallizing in water.<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Properties:<\/strong> Strong base, removes hardness of water, efflorescent (loses water of crystallization).<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Uses:<\/strong> Laundry (removes dirt), glass manufacture, paper industry, water softening.<\/li>\n<\/ul>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">4. Bleaching Powder (Calcium Oxychloride \u2014 CaOCl\u2082)<\/h3>\n<ul style=\"padding-left: 24px; margin: 0 0 1.2em 0;\">\n<li style=\"margin-bottom: 10px;\"><strong>Preparation:<\/strong> Ca(OH)\u2082 + Cl\u2082 \u2192 CaOCl\u2082 + H\u2082O (Chlorine gas passed through dry slaked lime)<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Properties:<\/strong> Strong oxidizing agent. Releases chlorine on reaction with dilute acid.<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Uses:<\/strong> Bleaching cotton and linen, disinfecting water, making wool unshrinkable.<\/li>\n<\/ul>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">5. Plaster of Paris (Calcium Sulphate Hemihydrate \u2014 CaSO\u2084\u00b7\u00bdH\u2082O)<\/h3>\n<ul style=\"padding-left: 24px; margin: 0 0 1.2em 0;\">\n<li style=\"margin-bottom: 10px;\"><strong>Preparation:<\/strong> Gypsum (CaSO\u2084\u00b72H\u2082O) heated to 373K: CaSO\u2084\u00b72H\u2082O \u2192 CaSO\u2084\u00b7\u00bdH\u2082O + 1\u00bdH\u2082O<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Properties:<\/strong> Sets into hard mass on mixing with water (exothermic setting).<\/li>\n<li style=\"margin-bottom: 10px;\"><strong>Uses:<\/strong> Plastering walls, making toys, statues, casts for fractures, dental moulds.<\/li>\n<\/ul>\n<h2 style=\"color: #059669; font-size: 1.75em; margin: 40px 0 16px 0; padding: 0 0 10px 0; border-bottom: 3px solid #10b981; font-weight: bold; line-height: 1.3;\">Water of Crystallization and Hydrated Salts<\/h2>\n<p style=\"margin: 0 0 1.2em 0;\"><strong>Water of crystallization<\/strong> is the fixed number of water molecules present in one formula unit of a salt. These water molecules are loosely bonded and can be removed by heating.<\/p>\n<table style=\"width: 100%; border-collapse: collapse; margin: 20px 0; border-radius: 12px; overflow: hidden; box-shadow: 0 4px 16px rgba(0,0,0,0.08); font-size: 0.95em;\" role=\"table\" aria-label=\"Hydrated salts and their water of crystallization\">\n<thead>\n<tr style=\"background: linear-gradient(135deg,#059669 0%,#10b981 100%); color: #fff; text-align: left;\">\n<th style=\"padding: 14px 16px; font-weight: bold;\">Salt<\/th>\n<th style=\"padding: 14px 16px; font-weight: bold;\">Chemical Formula<\/th>\n<th style=\"padding: 14px 16px; font-weight: bold;\">Water of Crystallization<\/th>\n<th style=\"padding: 14px 16px; font-weight: bold;\">Colour<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr style=\"border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>Blue Vitriol<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">CuSO\u2084\u00b75H\u2082O<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">5 molecules<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Blue<\/td>\n<\/tr>\n<tr style=\"background: #f8fafc; border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>Green Vitriol<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">FeSO\u2084\u00b77H\u2082O<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">7 molecules<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Light green<\/td>\n<\/tr>\n<tr style=\"border-bottom: 1px solid #e2e8f0;\">\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\"><strong>Washing Soda<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">Na\u2082CO\u2083\u00b710H\u2082O<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">10 molecules<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 1px solid #e2e8f0;\">White<\/td>\n<\/tr>\n<tr style=\"background: #f8fafc; border-bottom: 2px solid #059669;\">\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\"><strong>Gypsum<\/strong><\/td>\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\">CaSO\u2084\u00b72H\u2082O<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\">2 molecules<\/td>\n<td style=\"padding: 12px 16px; border-bottom: 2px solid #059669;\">White<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<div style=\"background: #ecfdf5; border-left: 5px solid #10b981; padding: 18px 22px; border-radius: 0 12px 12px 0; margin: 20px 0;\"><strong>\ud83d\udca1 Memory Trick:<\/strong> Remember <strong>&#8220;Cu-Five, Fe-Seven, Na-Ten, Ca-Two&#8221;<\/strong> \u2014 CuSO\u2084 has 5H\u2082O, FeSO\u2084 has 7H\u2082O, Na\u2082CO\u2083 has 10H\u2082O, and CaSO\u2084 has 2H\u2082O. This rhyme saves you in MCQs!<\/div>\n<h2 style=\"color: #059669; font-size: 1.75em; margin: 40px 0 16px 0; padding: 0 0 10px 0; border-bottom: 3px solid #10b981; font-weight: bold; line-height: 1.3;\">Frequently Asked Questions (NCERT Based)<\/h2>\n<div>\n<div>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">What is the difference between an acid and a base?<\/h3>\n<div>\n<div>\n<p style=\"margin: 0 0 1.2em 0;\">An <strong>acid<\/strong> is a substance that tastes sour, turns blue litmus red, and releases H\u207a ions in water. A <strong>base<\/strong> tastes bitter, feels soapy, turns red litmus blue, and releases OH\u207b ions in water. Acids have pH less than 7, while bases have pH greater than 7. Acids react with metals to produce hydrogen gas, while bases react with non-metal oxides to form salt and water.<\/p>\n<\/div>\n<\/div>\n<\/div>\n<div>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">Why does an aqueous solution of acid conduct electricity?<\/h3>\n<div>\n<div>\n<p style=\"margin: 0 0 1.2em 0;\">An aqueous solution of acid conducts electricity because acids <strong>dissociate in water<\/strong> to produce hydrogen ions (H\u207a) and anions. These ions are free to move in the solution and carry electric current. For example, HCl dissociates into H\u207a and Cl\u207b ions, making the solution an electrolyte. Dry HCl gas does not conduct electricity because it lacks free ions.<\/p>\n<\/div>\n<\/div>\n<\/div>\n<div>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">What is a neutralization reaction? Give two examples.<\/h3>\n<div>\n<div>\n<p style=\"margin: 0 0 1.2em 0;\">A <strong>neutralization reaction<\/strong> is a reaction between an acid and a base that produces salt and water, with the evolution of heat. The acid and base neutralize each other&#8217;s properties. Examples: (1) NaOH + HCl \u2192 NaCl + H\u2082O, and (2) Ca(OH)\u2082 + H\u2082SO\u2084 \u2192 CaSO\u2084 + 2H\u2082O. These reactions are exothermic and are used in antacids to treat acidity.<\/p>\n<\/div>\n<\/div>\n<\/div>\n<div>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">Why does dry HCl gas not change the colour of dry litmus paper?<\/h3>\n<div>\n<div>\n<p style=\"margin: 0 0 1.2em 0;\">Dry HCl gas does not change the colour of dry litmus paper because <strong>acids produce H\u207a ions only in the presence of water<\/strong>. Dry HCl gas exists as covalent molecules (HCl) and does not dissociate into H\u207a ions. Without H\u207a ions, the acidic property is not exhibited. When water is present, HCl dissociates: HCl + H\u2082O \u2192 H\u2083O\u207a + Cl\u207b, and the litmus changes colour.<\/p>\n<\/div>\n<\/div>\n<\/div>\n<div>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">What is the common name of CaOCl\u2082 and what are its uses?<\/h3>\n<div>\n<div>\n<p style=\"margin: 0 0 1.2em 0;\">The common name of CaOCl\u2082 is <strong>Bleaching Powder<\/strong> (chemical name: Calcium Oxychloride). It is prepared by passing chlorine gas through dry slaked lime. Its uses include: (1) bleaching cotton and linen in textile industry, (2) disinfecting drinking water and swimming pools, (3) making wool unshrinkable, and (4) as an oxidizing agent in chemical industries.<\/p>\n<\/div>\n<\/div>\n<\/div>\n<div>\n<h3 style=\"color: #d97706; font-size: 1.35em; margin: 28px 0 12px 0; font-weight: bold; line-height: 1.3;\">What is water of crystallization? Give two examples.<\/h3>\n<div>\n<div>\n<p style=\"margin: 0 0 1.2em 0;\"><strong>Water of crystallization<\/strong> is the fixed number of water molecules chemically combined in a definite ratio with one formula unit of a salt. These water molecules are part of the crystal structure and can be removed by heating. Examples: (1) Blue vitriol (CuSO\u2084\u00b75H\u2082O) contains 5 water molecules, and (2) Washing soda (Na\u2082CO\u2083\u00b710H\u2082O) contains 10 water molecules. When heated, these salts lose water and become anhydrous (white powder).<\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<h2 style=\"color: #059669; font-size: 1.75em; margin: 40px 0 16px 0; padding: 0 0 10px 0; border-bottom: 3px solid #10b981; font-weight: bold; line-height: 1.3;\">Related Class 10 Chemistry Notes<\/h2>\n<p style=\"margin: 0 0 1.2em 0;\">Explore more NCERT-aligned study material for your Board Exam preparation:<\/p>\n<ul style=\"padding-left: 24px; margin: 0 0 1.2em 0;\">\n<li style=\"margin-bottom: 10px;\">\ud83d\udc49 <a style=\"color: #059669; font-weight: 600; text-decoration: underline; text-decoration-color: #10b981; text-underline-offset: 3px;\" href=\"https:\/\/seminarsonly.com\/news\/adulteration-in-food-chemistry-investigatory-project\/\">Adulteration in Food <\/a> \u2014 Chemistry Investigatory Project<\/li>\n<li style=\"margin-bottom: 10px;\">\ud83d\udc49 <a style=\"color: #059669; font-weight: 600; text-decoration: underline; text-decoration-color: #10b981; text-underline-offset: 3px;\" href=\"https:\/\/seminarsonly.com\/news\/growing-crystals-science-project-science-fair-experiment\/\">Growing Crystals Science Project<\/a> \u2014 Learn Science Fair Experiment.<\/li>\n<\/ul>\n<h2 style=\"color: #059669; font-size: 1.75em; margin: 40px 0 16px 0; padding: 0 0 10px 0; border-bottom: 3px solid #10b981; font-weight: bold; line-height: 1.3;\">Final Thoughts<\/h2>\n<p style=\"margin: 0 0 1.2em 0;\">Chapter 2 \u2014 <strong>Acids, Bases and Salts<\/strong> \u2014 is one of the most scoring chapters in the Class 10 Science Board Exam. The concepts are straightforward, the reactions follow clear patterns, and the questions are highly predictable. Focus on: (1) <strong>definitions with examples<\/strong>, (2) <strong>chemical equations with state symbols<\/strong>, (3) <strong>the pH scale and its applications<\/strong>, and (4) <strong>preparation and uses of important salts<\/strong>.<\/p>\n<p style=\"margin: 0 0 1.2em 0;\">Practice writing every reaction at least three times. Use the memory tricks and tables in this guide for quick revision the night before the exam. And remember \u2014 understanding <em>why<\/em> a reaction happens is just as important as memorizing <em>what<\/em> happens.<\/p>\n<p style=\"margin: 0 0 1.2em 0;\">If you found these notes helpful, bookmark this page and share it with your classmates. Good luck with your Board Exams!<\/p>\n<div style=\"display: flex; gap: 12px; flex-wrap: wrap; margin: 20px 0;\"><a style=\"background: linear-gradient(135deg,#059669 0%,#10b981 100%); color: #fff; border: none; padding: 12px 28px; border-radius: 50px; font-weight: bold; text-decoration: none; display: inline-block; box-shadow: 0 4px 14px rgba(5,150,105,0.3);\" role=\"button\" href=\"#\" aria-label=\"Print these chemistry notes\">\ud83d\udda8\ufe0f Print Notes<\/a><br \/>\n<a style=\"background: linear-gradient(135deg,#d97706 0%,#f59e0b 100%); color: #fff; border: none; padding: 12px 28px; border-radius: 50px; font-weight: bold; text-decoration: none; display: inline-block; box-shadow: 0 4px 14px rgba(217,119,6,0.3);\" role=\"button\" href=\"https:\/\/ncert.nic.in\/textbook.php?kesc1=2-13\" target=\"_blank\" rel=\"noopener noreferrer nofollow\" aria-label=\"Open official NCERT textbook\">\ud83d\udcda Official NCERT Textbook<\/a><\/div>\n<p><!-- AUTHOR BOX (EEAT) --><\/p>\n<div style=\"background: #f8fafc; border: 2px solid #e2e8f0; border-radius: 16px; padding: 24px; margin: 40px 0 20px 0; display: flex; gap: 20px; align-items: flex-start; flex-wrap: wrap;\">\n<div style=\"width: 64px; height: 64px; border-radius: 50%; background: linear-gradient(135deg,#059669,#10b981); display: flex; align-items: center; justify-content: center; color: #fff; font-size: 1.5em; font-weight: bold; flex-shrink: 0;\" aria-hidden=\"true\">E<\/div>\n<div style=\"flex: 1; min-width: 200px;\">\n<h4 style=\"margin: 0 0 6px 0; color: #1e293b; font-size: 1.1em;\">EduNotes Editorial Team<\/h4>\n<p style=\"margin: 0; font-size: 0.9em; color: #64748b; line-height: 1.5;\">Experienced CBSE educators and subject matter experts with 12+ years of teaching Chemistry at the secondary school level. Our notes are aligned with the latest NCERT syllabus and CBSE Board Exam pattern. Every concept is verified against official NCERT textbooks before publication.<\/p>\n<p style=\"margin-top: 8px; font-size: 0.9em; color: #64748b;\"><strong>Last Updated:<\/strong> <time datetime=\"2026-07-17\">July 17, 2026<\/time> | <strong>Aligned with:<\/strong> NCERT Class 10 Science (2026-27 Edition) &amp; CBSE Board Exam Pattern<\/p>\n<\/div>\n<\/div>\n<\/article>\n","protected":false},"excerpt":{"rendered":"<p>\u26a1 Quick Answer Class 10 Chemistry Chapter 2 covers Acids, Bases and Salts. Key topics include: definitions and examples of acids and bases, the pH scale (0-14), chemical properties and&hellip;<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"ai_generated_summary":"","footnotes":""},"categories":[6804],"tags":[6807,6812,340,6808,6810,6805,6813,6806,6809,6811],"class_list":["post-105948","post","type-post","status-publish","format-standard","hentry","category-cbse-notes","tag-acids-bases-salts","tag-board-exam-2026","tag-cbse-board-exam","tag-chapter-2-notes","tag-chemical-reactions","tag-class-10-chemistry","tag-class-10-science","tag-ncert-notes","tag-ph-scale","tag-science-notes"],"yoast_head":"<!-- This site is optimized with the Yoast SEO Premium plugin v27.7 (Yoast SEO v27.7) - https:\/\/yoast.com\/product\/yoast-seo-premium-wordpress\/ -->\n<title>Class 10 Chemistry Chapter 2 Notes: Acids, Bases and Salts (NCERT) - Seminarsonly.com<\/title>\n<meta name=\"description\" content=\"Free Class 10 Chemistry Chapter 2 notes on Acids, Bases and Salts. 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