### Equilibrium Calculation for [Ag(CN)₂]⁻ Complex**Problem Statement:**- For the aqueous \( [\text{Ag}(\text{CN})_2]^{-} \) complex, the formation constant \( K_f = 1.26 \times 10^{21} \) at 25 °C.- Suppose equal volumes of 0.0022 M AgNO₃ solution and 0.48 M KCN solution are mixed. Calculate the equilibrium molarity of aqueous \( \text{Ag}^+ \) ion.- Round your answer to 2 significant digits.**Answer Format:**- The answer should be provided in molarity (M).**Diagram Explanation:**The image contains a rectangular box where the equilibrium molarity of \( \text{Ag}^+ \) ion should be entered. Next to it, there is a small control panel with options to input the response, such as multiplication by 10, a check mark, and a help button.This setup appears to be from an online educational platform, where students can input their calculated answer and possibly access hints or verify their response.### Detailed Steps for Solving the Problem:1. **Mixing Solutions:** - Initial concentration of AgNO₃ = 0.0022 M - Initial concentration of KCN = 0.48 M - When mixed, the concentration of each will halve due to equal volumes mixed: - \([ \text{Ag}^+ ]_{\text{initial}} = \frac{0.0022 \text{ M}}{2} = 0.0011 \text{ M}\) - \([ \text{CN}^- ]_{\text{initial}} = \frac{0.48 \text{ M}}{2} = 0.24 \text{ M}\)2. **Formation of Complex Ion:** - The reaction for the formation of the complex: \[ \text{Ag}^+ + 2 \text{CN}^- \leftrightharpoons [ \text{Ag}(\text{CN})_2 ]^- \] - The formation constant expression: \[ K_f = \frac{[ \text{Ag}(\text{CN})_2^- ]}{[\text{Ag}^+ ][ \text{CN}^- ]^

Formation constant of any complex ion gives the idea about the formation of that complex ion from…

For the aqueous [Ag (CN)₂] complex K₁=1.26 × 10²¹ at 25 °C. Suppose equal volumes of 0.0022M AgNO3 solution and 0.48M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Agion. Round your answer to 2 significant digits. M x10

For the aqueous [Ag (CN)₂] complex K₁=1.26 × 10²¹ at 25 °C. Suppose equal volumes of 0.0022M AgNO3 solution and 0.48M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Agion. Round your answer to 2 significant digits. M x10

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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Question

### Equilibrium Calculation for [Ag(CN)₂]⁻ Complex

**Problem Statement:**
- For the aqueous \( [\text{Ag}(\text{CN})_2]^{-} \) complex, the formation constant \( K_f = 1.26 \times 10^{21} \) at 25 °C.
- Suppose equal volumes of 0.0022 M AgNO₃ solution and 0.48 M KCN solution are mixed. Calculate the equilibrium molarity of aqueous \( \text{Ag}^+ \) ion.
- Round your answer to 2 significant digits.

**Answer Format:**
- The answer should be provided in molarity (M).

**Diagram Explanation:**
The image contains a rectangular box where the equilibrium molarity of \( \text{Ag}^+ \) ion should be entered. Next to it, there is a small control panel with options to input the response, such as multiplication by 10, a check mark, and a help button.

This setup appears to be from an online educational platform, where students can input their calculated answer and possibly access hints or verify their response.

### Detailed Steps for Solving the Problem:
1. **Mixing Solutions:**
- Initial concentration of AgNO₃ = 0.0022 M
- Initial concentration of KCN = 0.48 M
- When mixed, the concentration of each will halve due to equal volumes mixed:
- \([ \text{Ag}^+ ]_{\text{initial}} = \frac{0.0022 \text{ M}}{2} = 0.0011 \text{ M}\)
- \([ \text{CN}^- ]_{\text{initial}} = \frac{0.48 \text{ M}}{2} = 0.24 \text{ M}\)

2. **Formation of Complex Ion:**
- The reaction for the formation of the complex:
\[ \text{Ag}^+ + 2 \text{CN}^- \leftrightharpoons [ \text{Ag}(\text{CN})_2 ]^- \]
- The formation constant expression:
\[ K_f = \frac{[ \text{Ag}(\text{CN})_2^- ]}{[\text{Ag}^+ ][ \text{CN}^- ]^

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