Use the References to access important values if needed for this question. Consider the insoluble compound iron(II) hydroxide , Fe(OH)2 . The iron(II) ion also forms a complex with cyanide ions Write a balanced net ionic equation to show why the solubility of Fe(OH), (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Fe(CN),+, Kf=7.7x1036. Be sure to specify states such as (aq) or (s). 4- K= Submit Answer Retry Entire Group 9 more group attempts remaining
Use the References to access important values if needed for this question. Consider the insoluble compound iron(II) hydroxide , Fe(OH)2 . The iron(II) ion also forms a complex with cyanide ions Write a balanced net ionic equation to show why the solubility of Fe(OH), (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Fe(CN),+, Kf=7.7x1036. Be sure to specify states such as (aq) or (s). 4- K= Submit Answer Retry Entire Group 9 more group attempts remaining
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...
Related questions
Concept explainers
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question
![**Exercise: Solubility of Iron(II) Hydroxide in the Presence of Cyanide Ions**
**Objective:**
Understand and demonstrate why the solubility of iron(II) hydroxide, Fe(OH)₂, increases in the presence of cyanide ions.
---
**Instructions:**
Consider the insoluble compound iron(II) hydroxide, Fe(OH)₂. The iron(II) ion also forms a complex with cyanide ions.
**Task:**
Write a balanced net ionic equation to show why the solubility of Fe(OH)₂(s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction.
**Given Data:**
For the complex ion \([Fe(CN)_6]^{4-}\), the formation constant \( K_f \) is \( 7.7 \times 10^{36} \).
Be sure to specify states such as (aq) or (s).
\[
\begin{array}{c}
\text{Fe(OH)}_2(s) \longrightarrow \text{Fe}^{2+}(aq) + 2\text{OH}^-(aq) \\
\\
\text{Fe}^{2+}(aq) + 6\text{CN}^-(aq) \longrightarrow \text{[Fe(CN)}_6]^{4-}(aq)\\
\\
K = \frac{[\text{Product}]^x}{[\text{Reactant}]^y} \\
\end{array}
\]
Here is how the calculation steps and factors are visually represented:
1. Dissolution of Fe(OH)₂(s):
\[
\text{Fe(OH)}_2(s) \longrightarrow \text{Fe}^{2+}(aq) + 2\text{OH}^-(aq)
\]
2. Formation of the complex ion in solution:
\[
\text{Fe}^{2+}(aq) + 6\text{CN}^-(aq) \longrightarrow \text{[Fe(CN)}_6]^{4-}(aq)
\]
To find the equilibrium constant (K) for the overall reaction, multiply the solubility product constant \( K_{sp} \) of Fe(OH)₂ by the formation constant \( K_f \) of the complex ion:
\[
K = K_{sp}](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F16efa3d9-60e0-4c46-bd5d-02d294330639%2F7b849d61-5c7c-4a46-a41c-7ee7ef68db2b%2F14014kd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Exercise: Solubility of Iron(II) Hydroxide in the Presence of Cyanide Ions**
**Objective:**
Understand and demonstrate why the solubility of iron(II) hydroxide, Fe(OH)₂, increases in the presence of cyanide ions.
---
**Instructions:**
Consider the insoluble compound iron(II) hydroxide, Fe(OH)₂. The iron(II) ion also forms a complex with cyanide ions.
**Task:**
Write a balanced net ionic equation to show why the solubility of Fe(OH)₂(s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction.
**Given Data:**
For the complex ion \([Fe(CN)_6]^{4-}\), the formation constant \( K_f \) is \( 7.7 \times 10^{36} \).
Be sure to specify states such as (aq) or (s).
\[
\begin{array}{c}
\text{Fe(OH)}_2(s) \longrightarrow \text{Fe}^{2+}(aq) + 2\text{OH}^-(aq) \\
\\
\text{Fe}^{2+}(aq) + 6\text{CN}^-(aq) \longrightarrow \text{[Fe(CN)}_6]^{4-}(aq)\\
\\
K = \frac{[\text{Product}]^x}{[\text{Reactant}]^y} \\
\end{array}
\]
Here is how the calculation steps and factors are visually represented:
1. Dissolution of Fe(OH)₂(s):
\[
\text{Fe(OH)}_2(s) \longrightarrow \text{Fe}^{2+}(aq) + 2\text{OH}^-(aq)
\]
2. Formation of the complex ion in solution:
\[
\text{Fe}^{2+}(aq) + 6\text{CN}^-(aq) \longrightarrow \text{[Fe(CN)}_6]^{4-}(aq)
\]
To find the equilibrium constant (K) for the overall reaction, multiply the solubility product constant \( K_{sp} \) of Fe(OH)₂ by the formation constant \( K_f \) of the complex ion:
\[
K = K_{sp}
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 3 images
Knowledge Booster
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.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY