A 0.10 M aqueous solution of a weak acid HA has a pH of 4.00. What is the values

Question

A 0.10 M aqueous solution of a weak acid HA has a pH of 4.00. What is the values of K_c for HA? A) 1.1 times 10^-4 B) 1.0 times 10^-4 C) 1.0 times 10^-4 D) 1.0 times 10^-4 E) 1.0 times 10^-5 For the reaction given below, 2.00 mol of A and 3.00 mol of B are placed in a 6.00-L container. A (g) + 2B(g) C(g) At equilibrium, the concentration of A is 0.208 mol/L. What is the concentration of B at equilibrium? A) 0.500 mol/L. B) 0.208 mol/L C) 0.416 mol/L D) 0.249 mol/L. E) none of these In which of the following reactions does an instantaneous increase in the volume of the reaction vessel favor formation of the products? A) PCI_5(g) PCI_3(g) + Cl_(g) B) N_2(g) + 3H_2(g) 2NH_3(g) C) N_2(g) + O_2(g) 2NO(g) D) MgO(s) + CO_2(g) MgCO_3(s) E) H_2(g) + I_2(g) 2HI(g)

Explanation / Answer

(6)

pH = 4.00

- Log[H+] = 4.00

[H+] = 10-4

For weak acid, According to Ostwald's theory,

[H+] = sqrt.(Ka*C)

Ka * C = [H+]2

Ka * 0.10 = (10-4)2

Ka = 10-7 M

(A)

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