Worksheet Chapter 6: Acid, Base and Salt

1. Solid Y is a white salt. When Y is dissolved in water and tested: - Portion 1: Adding NaOH solution forms a white precipitate that dissolves in excess NaOH. - Portion 2: Adding NH3 solution forms a white precipitate that DOES NOT dissolve in excess NH3. - Portion 3: Adding dilute HNO3 followed by AgNO3 produces a white precipitate. (a) Identify the cation and anion present in salt Y. (b) Write the chemical formula for salt Y. (c) Write an ionic equation for the reaction taking place in Portion 3.

2. Fill in the blank: The reaction between an acid and a base to produce salt and water only is known as ________.

3. Calculate the mass of Sodium Hydroxide (NaOH) required to prepare 250 cm3 of 0.2 mol dm-3 NaOH solution. [Relative atomic mass: Na = 23, O = 16, H = 1]

4. State two agricultural or household applications of neutralisation.

5. True or False: All nitrate salts (NO3-) are soluble in water.

6. Which of the following salt solutions forms a yellow precipitate when added to potassium iodide (KI) solution?

7. A student wants to prepare a sample of Copper(II) sulfate (CuSO4) salt in the laboratory. (a) Name suitable starting reactants to prepare this salt. (b) Outline the main steps involved in purifying and obtaining copper(II) sulfate crystals.

8. Describe the chemical tests to confirm the presence of sulfate ions (SO42-) and nitrate ions (NO3-) in two separate test tubes.

9. True or False: Lead(II) chloride (PbCl2) is insoluble in cold water but dissolves in hot water.

10. Explain why 0.1 mol dm-3 Hydrochloric acid (HCl) has a lower pH value than 0.1 mol dm-3 Ethanoic acid (CH3COOH).