Chemical And Ionic Equilibrium Test Online

1. On adding 0.1 M solution each of [Ag⁺], [Ba²⁺], [Ca²⁺] in a Na₂SO₄ solution, species first precipitated is [K_sp BaSO₄ = 10⁻¹¹, K_sp CaSO₄ = 10⁻⁶, K_sp Ag₂SO₄ = 10⁻⁵]

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

3. 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.

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

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

6. 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:

7. 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:

8. 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.   

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

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

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

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

13. The pH value of ordinary water is:

14. pK_a value of four acids are given below. The strongest acid 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)