Chemical And Ionic Equilibrium Test Online

1. In which of the following acid-base titration, pH is greater than 8 at equivalence point.

2. During titration of acetic acid with aq. NaOH solution, the neutralisation graph has a vertical line. This line indicates

3. When 10 mL of 0.1 M acetic acid (pK_a = 5.0), is titrated against 10 mL of 0.1 M ammonia solution (pK_b = 5.0), the equivalence point occurs at pH:

4. A + 2B⇌2C+D, initial concentration of B was 1.5 times that of A, but the equilibrium concentration of A and B are found to be equal. The equilibrium constant for the reaction is:

5. pK_a value of four acids are given below. The strongest acid is:

6. A weaqk acid, HA is found to be 10% ionized in 0.01 M aqueous solution. Calculate the pH of a solution which is 0.1 M in HA and 0.05 M in NaA.

7. What is the pH value of M H₂SO₄?

8. For reaction, 2NOC1_(g) ⇌ 2 NO_(g) + C1₂_(g) ; K_c at 427°C is 3 x 10⁻⁶ L mol⁻¹. The value of Kp is nearly:

9. The pH value of ordinary water is:

10. The pH value of N/10 Na OH is:

11. Solubility product of a salt AB is 1 x 10⁻⁸ in a solution in which the concentration of A⁺ ions is 10⁻³ M. The salt will precipitate when the concentration of B⁻ ions is kept

12. Air containing 79% of nitrogen and 21% of oxygen by volume is heated at 2200 K and 1 atm until equilibrium is established according to the reaction  N₂(g) + O₂(g) ⇌ 2NO(g) If the K_p of the reaction is 1.1 x 10⁻³, calculate the amount of nitric oxide produced in terms of volume percent.

13. Of the following which change will shift the reaction towards the product? I₂(g) ⇌ 2I(g), ∆H⁰_r (298 K) = + 150 kJ

14. The pH of the solution obtained on neutralization of 40 mL 0.1 M NaOH with 40 m1 0.1 M CH₃COOH is

15. The pH of solution containing 0.01 M sodium acetate and 0.03 M acetic acid is (pK_a for CH₃COOH = 4.57)