Chemical And Ionic Equilibrium Test Online

1. The pH value of ordinary water is:

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

3. 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.

4. 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.   

5. 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]

6. 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:

7. 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:

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

9. The equilibrium constant for the following reaction will be: 3A + 2B → C.

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

11. One mole of CH₃COOH and one mole of C₂H₅OH reacts to produce 2/3 mol of CH₃COOC₂H₅. The equilibrium constant is:

12. The solubility of CuBr is 2 x 10⁻⁴ mol/L at 25°C. The K_sp value of CuBr is

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

14. In the manufacture of NH₃ in Haber’s continuous flow process involving the reaction N₂_(g) + 3H₂_(g)        2NH₃_(g),∆H = -22.08 kcal. The favourable conditions are:

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