Chemical And Ionic Equilibrium Test Online

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

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

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

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

5. 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.

6. A solution having hydrogen ion concentration is 0.0005 g eqvt. /liter, its pOH is:

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

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

9. 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:

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

11. 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:

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

13. 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.

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

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