Chemical And Ionic Equilibrium Test Online

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

2. 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:

3. The solubility of PbF₂ in water at 25°C is ~ 10⁻³ M. What is its solubility in 0.05 M NaF solution? Assume the later to be fully ionised.   

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

5. 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:

6. The value of K_p for the reaction: 2H₂S_(g) = 2H₂ _(g) + S₂ _(g) is 1.2 x 10⁻² at 1065°C. The value for K_C is:

7. 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.

8. What is the pH value of M H₂SO₄?

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

10. 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:

11. In which of the following cases, pH is greater than 7?

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

13. In which of the following reactions, the concentration of the product is higher than the concentration of reactant at equilibrium? (K = equilibrium constant)

14. The pH of a solution having the H⁺ ion concentration of 1 x 10⁻⁴ ions/liter is:

15. Which one of the following is NOT a buffer solution?