Chemical And Ionic Equilibrium Test Online

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

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

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. 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:

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

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

7. 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

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

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

10. 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:

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

12. The pH value of ordinary water is:

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

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

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