2nd WEEK Day 1: Pg: 18 Step – 1 Study the following topic from textbook: Acids and bases in the laboratory Reaction of acids and bases with metals Step – 2 Study the same topics in the following part of Extra mark app Ch- Acids, Bases and Salts→ Detailed learning →Understanding concepts Step – 3 Clear your doubts (if any) from subject teacher Step – 4 Revise using following Bullet points: Reaction of Acids and Bases with Metals → Reaction of Acids with Metals • Acids react with metal to form metal salt and releases Hydrogen Gas. Acid + Metal → Salt + Hydrogen Gas • Example: Zinc granules react with dilute Hydrochloric acid in a test tube. 2HCl + Zn → ZnCl2 + H2 → Reaction of Bases with Metals • Bases react with metal to evolve hydrogen Gas. Also, note that all metals do not react with bases. The metal must be more reactive than the metals present in the base for the reaction to take place. Base + Metal → Salt + Hydrogen gas • Example: Zinc granules react with NaOH solution to form sodium zincate and evolve hydrogen gas. 2NaOH + Zn → Na2ZnO2 + H2 • Hydrogen gas released can be tested by bringing burning candle near gas bubbles, it burst with pop sound. End of Day – 1 Day 2: Pg:20 Step – 1 Study the following topic from textbook: Reaction of acids with metal carbonates and bicarbonates Reaction of acid with base Step – 2 Study the same topics in the following part of Extra mark app Ch- Acids, Bases and Salts→ Detailed learning →Understanding concepts Step – 3 Clear your doubts (if any) from subject teacher Step – 4 Revise using following Bullet points: Reaction of Acids with Metal Carbonates and Metal Hydrogencarbonates • Acids reacts with Metal Carbonates and Metal Hydrogencarbonates to form Salt, Carbon dioxide and water. Metal carbonate/Metal hydrogen carbonate + Acid → Salt + Carbon dioxide + Water • Examples: (i) 2HCl + Na2CO3 → 2NaCl + CO2 + H2O (ii) HCl + NaHCO3 → NaCl + CO2 + H2O • CO2 can be tested by passing it through lime water. It turns lime water milky. Ca(OH)2 + CO2 → CaCO3 + H2O • When excess CO2 is passed, milkiness disappears. CaCO3 + CO2 + H2O → Ca(HCO)3 • Bases do not react with Metal Carbonates and Metal Hydrogencarbonates. Base + Metal Carbonate/Metal Hydrogen Carbonate → No Reaction Reaction of Acids and Bases with each other • Acids and Bases react to form salt and water. Acid + Base → Salt + H2O • Neutralisation Reaction: Reaction of acid with a base is called as neutralization reaction. Example: HCl + NaOH → NaCl + H2O • Strong Acid + Weak Base → Acidic salt + H2O • Weak Acid + Strong Base → Basic salt + H2O • Strong Acid + Strong Base → Neutral salt + H2O • Weak Acid + Weak Base → Neutral salt + H2O End of Day – 2 Day 3: Pg:21 Step – 1 Study the following topic from textbook: Reaction of acids with metallic oxides Reaction of bases with basic oxide Step – 2 Study the same topics in the following part of Extra mark app Ch- Acids, Bases and Salts→ Detailed learning →Understanding concepts Step – 3 Clear your doubts (if any) from subject teacher Step – 4 Revise using following Bullet points: Reaction of Metallic Oxides with Acids → Metallic oxides are basic in nature. Example: CaO, MgO are basic oxides. Metallic Oxide + Acid → Salt + H2O CaO + 2HCl → CaCl2 + H2O Reaction of Non-metallic Oxides with Bases → Non-metallic oxides are acidic in nature. → Non-metallic Oxide + Base → Salt + H2O CO2 + Ca(OH)2 → CaCO3 + H2O End of Day – 3 Day 4: Assessment Solve the following questions given in the text book 1. Which gas is usually liberated when an acid reacts with a metal? How will you test for the gas? 2. What is a neutralization reaction? 3. Name two indicators which are widely used in laboratories. 4. A solution turns red litmus blue. Is the solution acid or a base? 5. What are olfactory indicators? Give an example. 6. What would happen if a small amount of copper oxide is taken in a beaker and dilute HCI is added to it? 7. How metal oxides react with acids? 8. How non- metal oxides react with base? 9. Which gas is usually liberated when an acid reacts with a metal carbonate? How will you test for the gas? End of Day – 4 .