Complete the following sentences by choosing the correct word(s) from the brackets:

(a) …………… solution forms a coloured precipitate with ammonium hydroxide which is soluble in excess of ammonium hydroxide. [Ferrous chloride / Copper nitrate]

(b) Zinc blende is converted to zinc oxide by ……………. [Calcination / Roasting]

(c) …………… conducts electricity by the movement of ions. [Molten iron / Molten sodium chloride]

(d) The reaction that takes place at the anode during the electrolysis of aqueous Sodium argentocyanide with silver electrodes is ……………. [Ag ⟶ Ag⁺ + e^–/ Ag⁺ + e^– ⟶ Ag]

(e) The salt formed when ZnO reacts with hot concentrated NaOH is …………… . [sodium zincate / zinc hydroxide]

State the terms for the following: (a) Undistilled alcohol containing a large amount of methanol. (b) A salt formed by the partial replacement of the hydroxyl group of a di-acidic or a tri-acidic base by an acid radical. (c) Organic compounds having the same molecular formula but different structural formula. (d) The tendency of an atom to attract the shared pair of electrons towards itself when combined in a compound. (e) The type of covalent bond in which electrons are shared unequally between the combining atoms.

Rohit took two different salt solutions in test tubes C and D as shown in the figure below. He added dilute HCl to each of the two test tubes. The products formed in the test tubes C and D are silver chloride and lead chloride respectively. State: (a) one common observation made by Rohit in both the reactions. (b) the observations made by him on addition of excess of ammonium hydroxide to the products formed in: 1. test tube C 2. test tube D

Match the Column A with Column B: Column A Column B (a) N2 + 3H2 ⇌ 2NH3 1. Vanadium Pentoxide (b) 4NH3 + 5O2 ⟶ 4NO + 6H2O 2. Nickel (c) 2SO2 + O2 ⇌ 2SO3 3. Iron (d) C2H4 + H2 ⟶ C2H6 4. Concentrated Sulphuric acid (e) CuSO4.5H2O ⟶ CuSO4 + 5H2O 5. Platinum

Which pair of reactants can be best used to produce lead (II) sulphate? (a) Sulphuric acid + Lead (b) Sulphuric acid + Lead hydroxide (c) Sodium sulphate + Lead nitrate (d) Potassium sulphate + Lead oxide

Differentiate between the following pairs of compounds using the reagent given in the bracket: (a) Ammonium chloride and Sodium chloride (using an alkali) (b) Zinc Nitrate solution and Calcium Nitrate solution (using excess sodium hydroxide solution)

Acidulated water is electrolysed using platinum electrodes. Answer the following questions: (a) Why is dilute sulphuric acid added to water? (b) Write the reaction taking place at the cathode. (c) What is the observation at the anode?

Answer the following questions with reference to the concentration of bauxite ore. (a) Name the process used to concentrate the ore. (b) Give a balanced chemical equation for the conversion of aluminium hydroxide to pure alumina.

Give one significant observation when: (a) Barium chloride solution is added to zinc sulphate solution. (b) Lead nitrate is heated strongly. (c) Chlorine gas is passed through moist starch iodide paper.

P, Q, R and S are the different methods of preparation of salts. P – Simple displacement Q – Neutralisation by titration R – Precipitation S – Direct combination Choose the most appropriate method to prepare the following salts: (a) PbCl2 (b) FeCl3 (c) Na2SO4

Given below is a diagram showing the placement of five different oxides. With respect to the given diagram answer the following questions: (a) Name the type of oxide represented in region X in the diagram. (b) Identify the oxide which has been incorrectly placed in the above diagram. (c) Name the oxide from the above diagram which will form an alkali when dissolved in water.

Justify the following statements: (a) Anode is known as the oxidizing electrode. (b) Graphite electrodes are preferred in the electrolysis of molten lead bromide.

Aqueous copper (II) sulphate is electrolysed using copper electrodes. Which statement about the electrolysis is not correct? (a) An oxidation reaction occurs at the positive electrode. (b) The current is carried through the electrolyte by ions. (c) The positive electrode loses mass. (d) The number of copper (II) ions in the electrolyte decreases.