Name: 4. What is the percent ionization (to two decimal places) of a 0.50 M HNO2 aqueous solution? HNO₂(aq) + H₂O(l) = H3O+ (aq) + NO₂ (aq) K₂(HNO₂) = 4.60 × 10-4 NetID: A: 3.03

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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## Exercise: Percent Ionization of HNO₂ Solution

### Question:
What is the percent ionization (to two decimal places) of a 0.50 M HNO₂ aqueous solution?

### Chemical Reaction:
\[ \text{HNO}_2 (aq) + \text{H}_2\text{O} (l) \rightleftharpoons \text{H}_3\text{O}^+ (aq) + \text{NO}_2^- (aq) \]

### Given:
- \( K_a (\text{HNO}_2) = 4.60 \times 10^{-4} \)

### Answer:
- 3.03%
Transcribed Image Text:## Exercise: Percent Ionization of HNO₂ Solution ### Question: What is the percent ionization (to two decimal places) of a 0.50 M HNO₂ aqueous solution? ### Chemical Reaction: \[ \text{HNO}_2 (aq) + \text{H}_2\text{O} (l) \rightleftharpoons \text{H}_3\text{O}^+ (aq) + \text{NO}_2^- (aq) \] ### Given: - \( K_a (\text{HNO}_2) = 4.60 \times 10^{-4} \) ### Answer: - 3.03%
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