This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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You're on a roll — here are the answers to your tutorial questions: 1. a) List three natural carbonates you have studied. Calcium carbonate* (CaCO_3) - found as limestone, marble, chalk. Magnesium carbonate* (MgCO_3) - found as magnesite. Iron(II) carbonate* (FeCO_3) - found as siderite. b) Give three examples of carbonates that are soluble in water and three that are not. Soluble carbonates: Sodium carbonate* (Na_2CO_3) Potassium carbonate* (K_2CO_3) Ammonium carbonate* ((NH_4)_2CO_3) Insoluble carbonates: Calcium carbonate* (CaCO_3) Magnesium carbonate* (MgCO_3) Copper(II) carbonate* (CuCO_3) c) Write the equation for the reaction between CO_2 gas and baryta water taken place for over 5mins. Step 1: Carbon dioxide reacts with barium hydroxide (baryta water) to form a white precipitate of barium carbonate. Ba(OH)_2(aq) + CO_2(g) → BaCO_3(s) + H_2O(l) Step 2: If excess carbon dioxide is passed for an extended period (over 5 minutes), the insoluble barium carbonate reacts further with carbon dioxide and water to form soluble barium hydrogen carbonate, causing the precipitate to redissolve. BaCO_3(s) + CO_2(g) + H_2O(l) → Ba(HCO_3)_2(aq) 2. Distinguish between Na_2CO_3 and KHCO_3 using the available reagents. Here are three simple tests: Test 1: Using Phenolphthalein indicator Procedure: Add a few drops of phenolphthalein indicator to separate solutions of Na_2CO_3 and KHCO_3. Observation: The Na_2CO_3 solution will turn pink/red (strongly alkaline), while the KHCO_3 solution will show a faint pink* color or remain colorless (less alkaline). Explanation: Sodium carbonate is a salt of a strong base and a weak acid, leading to significant hydrolysis and a higher pH. Potassium hydrogen carbonate is less alkaline. Test 2: Using Magnesium Sulfate (MgSO_4) solution Procedure: Add magnesium sulfate solution to separate solutions of Na_2CO_3 and KHCO_3 at room temperature. Observation: With Na_2CO_3, an immediate white precipitate of magnesium carbonate forms. With KHCO_3, no precipitate* forms in the cold solution. A precipitate would only form upon heating the KHCO_3 mixture. Equations: Na_2CO_3(aq) + MgSO_4(aq) → MgCO_3(s) + Na_2SO_4(aq) 2KHCO_3(aq) + MgSO_4(aq) → Mg(HCO_3)_2(aq) + K_2SO_4(aq) (Magnesium bicarbonate is soluble) Test 3: Using Barium Chloride (BaCl_2) solution Procedure: Add barium chloride solution to separate solutions of $Na