**Problem Statement:**If the pH of a 0.0850 M solution of HBrO₂ is 2.29, then what is the value for the acidity constant, \(K_a\), of HBrO₂?**Chemical Reaction:**\[\text{HBrO}_2(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{H}_3\text{O}^+(aq) + \text{BrO}_2^-(aq) \quad K_a = ?\]**Required Calculation:**Find \(K_a\) for HBrO₂: ____________

pH = -log[H+] Relation between [H+], Ka and C of a weak acid solution: [H+] = (Ka x C)1/2pH = -log[H+] 2.29 = -log[H+] -2.29 = log[H+] log 0.00513 = log[H+] [H+] = 0.00513 M C = 0.0850 mole/L [H+] = (Ka x C)1/2 0.00513 = (Ka x 0.0850)1/2 (0.00513)2 = Ka x 0.0850 Ka = (0.00513)2/0.0850 = 3.10 x 10-4

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If the pH of a 0.0850 M solution of HBrO2 is 2.29, then what is the value for the acidity constant, Ką, of HB1O2? HBRO2(aq) + H,0(1) H3O*(aq) + Br02 (aq) K¸ = ?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 60QAP: Consider a 0.33 M solution of the diprotic acid H2X. H2X H+(aq)+ HX(aq)Ka1=3.3 10 4 HX H+(aq)+...

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Question

**Problem Statement:**

If the pH of a 0.0850 M solution of HBrO₂ is 2.29, then what is the value for the acidity constant, \(K_a\), of HBrO₂?

**Chemical Reaction:**

\[
\text{HBrO}_2(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{H}_3\text{O}^+(aq) + \text{BrO}_2^-(aq) \quad K_a = ?
\]

**Required Calculation:**

Find \(K_a\) for HBrO₂: ____________

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