1. When sodium carbonate solution is titrated against HCl solution, the indicator used is

2. Which of the following mixtures in an aqueous solution of equimolar concentration acts as a buffer solution?

3. Find the pH of a solution when 0.01 M HCl and 0.1 M NaOH are mixed in equal volumes

4. A base according to Bronsted concept is a substance which can

5. On increasing the concentration of reactants in a reversible reaction, then equilibrium constant will

6. A  weak acid HX has the dissociation constant 1 × 10^-5 M. It forms a salt NaX on reaction with alkali. The degree of hydrolysis of 0.1 M solution of NaX is

7. Aluminium chloride is

8. Find the conjugate acid of NH₂^–

9. A physician wishes to prepare a buffer solution at pH = 3.85 that efficiently resists changes in pH yet contains only small concentration of the buffering agents. Which of the following weak acids together with its sodium salt would be best to use?

10. Among the following the weakest Bronsted base is

11. A certain buffer solution contains equal concentration of X^– and HX. The k_a for HX is 10^-8. The pH of the buffer is

12. In 0.10 M aqueous solution of pyridine (C₅H₅N), find the percentage of pyridine that forms pyridinium ion (C₅H₅N⁺H) (K_b for C₅H₅N = 1.7 x 10^-9 )

13. When equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed, the hydroxide ion concentration is

14. What is the pH of a 0.10 M solution of barium hydroxide, Ba (OH)₂?

15. Which of the following aqueous solution will be the best conductor of electricity?

16. In a reversible chemical reaction at equilibrium, if the concentration of any one of the reactants is doubled, then the equilibrium constant will

17. When a neutral atom undergoes oxidation, the atoms oxidation state

18. Highest pH will be recorded for which of the following solutions if they are equimolar

19. Which of the following aqueous solutions will have highest pH?

20. Solubility of M₂S salt is 3.5 × 10^-6 then find out solubility product.