Determine the molarity of a solution of the weak acid HCIO2 (K. = 1.10 times 10^

Question

Determine the molarity of a solution of the weak acid HCIO2 (K. = 1.10 times 10^-2) if it has a pH of 1.084. 0.617 M 0.0824 M 7.49 M 12.9 M 1.235 M The following question refers to a solution that contains 1.68 M hydrofluoric acid, HF (K_a = 7.2 times 10^-4), and 3.00 M hydrocyanic acid. HCN (K_a = 6.2 times 10^-10). What is the pH of this mixture of weak acids? 0.00 1.46 2.92 4.37 12.54 The following question refers to a solution that contains 1.71 M hydrofluoric acid, HF (K_a = 7.2 times 10^-4), and 3.00 M hydrocyanic acid. HCN (K_a = 6.2 times 10^-10). Determine the [CN) at equilibrium. 1.9e-9 M 3.5e-2 M 5.3e-8 M 6.2e-10 M none of these Calculate the pH of a 0.19 M solution of Ca (OH)_2. 13.58 13.28 0.42 0.72 none of these

Explanation / Answer

6) HClO2 = H+ + ClO2-

[H+] = [ ClO2-]

pH = 1.084 i.e.- [H+] = 10 ^ - 1.084= 0.0824 M = [ ClO2-]

Ka = 1.10 x 10-2

Ka = [H+] * [ ClO2-] / [HClO2 ]

or, 1.10 x 10-2 = ( 0.0824) (0.0824) / [HClO2 ]

or, [HClO2 ] = 0.617 M

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