(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

Chemistry
10th Edition
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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
icon
Related questions
Question
100%
**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: 
  \[ \boxed{3.7 \times 10^{-5} \text{ M}} \]
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: \[ \boxed{3.7 \times 10^{-5} \text{ M}} \]
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 images

Blurred answer
Knowledge Booster
Activities
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY