(a) mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M NH3? NH3(aq) + HCN(aq) ⇒ NH4+ (aq) + CN ¯(aq) Kc = 0.71 M 4.0 (b) mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M K₂S? S² (aq) + HCN(aq) = HS¯(aq) + CN −(aq) Kc = 3.1 x 10³ 5.0e2 XM 4.0
(a) mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M NH3? NH3(aq) + HCN(aq) ⇒ NH4+ (aq) + CN ¯(aq) Kc = 0.71 M 4.0 (b) mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M K₂S? S² (aq) + HCN(aq) = HS¯(aq) + CN −(aq) Kc = 3.1 x 10³ 5.0e2 XM 4.0
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Chapter1: Chemical Foundations
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![**Equilibrium Concentration of CN⁻ Ion in Mixed Solutions**
What is the equilibrium concentration of CN⁻ ion after mixing the following solutions? *(Hint: Mixing the solutions dilutes the reactants.)*
**(a)** Mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M NH₃?
The chemical equation is:
\[ \text{NH}_3(aq) + \text{HCN}(aq) \rightleftharpoons \text{NH}_4^+(aq) + \text{CN}^-(aq) \]
The equilibrium constant, \( K_c \), is 0.71.
- Correct Answer:
\[ \boxed{4.0 \times 10^{-3} \text{ M}} \]
---
**(b)** Mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M K₂S?
The chemical equation is:
\[ \text{S}^{2-}(aq) + \text{HCN}(aq) \rightleftharpoons \text{HS}^-(aq) + \text{CN}^-(aq) \]
The equilibrium constant, \( K_c \), is \( 3.1 \times 10^3 \).
- Incorrect Answer Provided:
\[ 5.0 \times 10^{2} \text{ M} \]
---
**(c)** Mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M KF?
The chemical equation is:
\[ \text{F}^-(aq) + \text{HCN}(aq) \rightleftharpoons \text{HF}(aq) + \text{CN}^-(aq) \]
The equilibrium constant, \( K_c \), is \( 5.6 \times 10^{-7} \).
- Correct Answer:
\[ \boxed{3.7 \times 10^{-5} \text{ M}} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8b8a4ad9-b66e-4dbe-8b3f-39bf0adb3cae%2Ffa18c124-93b3-4314-a97f-4afdf1770db8%2F9kwxa4o_processed.png&w=3840&q=75)
Transcribed Image Text:**Equilibrium Concentration of CN⁻ Ion in Mixed Solutions**
What is the equilibrium concentration of CN⁻ ion after mixing the following solutions? *(Hint: Mixing the solutions dilutes the reactants.)*
**(a)** Mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M NH₃?
The chemical equation is:
\[ \text{NH}_3(aq) + \text{HCN}(aq) \rightleftharpoons \text{NH}_4^+(aq) + \text{CN}^-(aq) \]
The equilibrium constant, \( K_c \), is 0.71.
- Correct Answer:
\[ \boxed{4.0 \times 10^{-3} \text{ M}} \]
---
**(b)** Mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M K₂S?
The chemical equation is:
\[ \text{S}^{2-}(aq) + \text{HCN}(aq) \rightleftharpoons \text{HS}^-(aq) + \text{CN}^-(aq) \]
The equilibrium constant, \( K_c \), is \( 3.1 \times 10^3 \).
- Incorrect Answer Provided:
\[ 5.0 \times 10^{2} \text{ M} \]
---
**(c)** Mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M KF?
The chemical equation is:
\[ \text{F}^-(aq) + \text{HCN}(aq) \rightleftharpoons \text{HF}(aq) + \text{CN}^-(aq) \]
The equilibrium constant, \( K_c \), is \( 5.6 \times 10^{-7} \).
- Correct Answer:
\[ \boxed{3.7 \times 10^{-5} \text{ M}} \]
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