Determine the pH of a buffer that is 0.95 M HBRO and 0.68 M KBRO. The value of pka for HBRO is 8.68. 2. NEXT Based on the given values, set up ICE table in order to determine the unknown. HBRO(aq) H.O(1) H,O (aq) BrO(aq) %3D Initial (M) Change (M) Equilibrium (M) 5 RESET 0.95 0.68 8.68 +x x- +2x 0.95 + 2x 0.95 - 2x 0.68 + x 0.68 - x 0.68 + 2x -2x 0.95 + x 0.95 - x 0.68 - 2x
Determine the pH of a buffer that is 0.95 M HBRO and 0.68 M KBRO. The value of pka for HBRO is 8.68. 2. NEXT Based on the given values, set up ICE table in order to determine the unknown. HBRO(aq) H.O(1) H,O (aq) BrO(aq) %3D Initial (M) Change (M) Equilibrium (M) 5 RESET 0.95 0.68 8.68 +x x- +2x 0.95 + 2x 0.95 - 2x 0.68 + x 0.68 - x 0.68 + 2x -2x 0.95 + x 0.95 - x 0.68 - 2x
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...
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I need help with this practice problem regarding acid base and ice tables
![**Buffer pH Calculation**
**Problem Statement:**
Determine the pH of a buffer that is 0.95 M HBrO and 0.68 M KBrO. The value of pKa for HBrO is 8.68.
**Instructions:**
Based on the given values, set up an ICE table in order to determine the unknown.
**ICE Table Setup:**
The following table outlines the initial concentrations, changes in concentrations, and equilibrium concentrations for the reaction:
\[
\begin{array}{ccccc}
\text{HBrO(aq)} & + & \text{H}_2\text{O(l)} & \rightleftharpoons & \text{H}_3\text{O}^+(aq) + \text{BrO}^-(aq) \\
\hline
\text{Initial (M)} & & & & \\
& 0.95 & & & 0.68 \\
\text{Change (M)} & & & & \\
& -x & & & +x \\
\text{Equilibrium (M)} & & & & \\
& 0.95 - x & & & 0.68 + x \\
\end{array}
\]
**Interactive Options:**
Below the table, there is a selection of potential calculations and variables for automated computation including:
- Symbols: 0, 0.95, 0.68, 8.68, +x, -x, +2x
- Expressions: 0.95 + x, 0.95 - x, 0.95 - 2x, 0.68 + x, 0.68 - x, 0.68 - 2x, 0.68 + 2x
There is a RESET button to clear selections.
**Purpose:**
This educational tool assists in calculating buffer pH by setting up and solving ICE tables.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5c6d7610-fae0-4fdd-8afb-1e0bd9bb140b%2F249f38d0-43dd-4018-91c1-c87eee4af304%2F8cst1o9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Buffer pH Calculation**
**Problem Statement:**
Determine the pH of a buffer that is 0.95 M HBrO and 0.68 M KBrO. The value of pKa for HBrO is 8.68.
**Instructions:**
Based on the given values, set up an ICE table in order to determine the unknown.
**ICE Table Setup:**
The following table outlines the initial concentrations, changes in concentrations, and equilibrium concentrations for the reaction:
\[
\begin{array}{ccccc}
\text{HBrO(aq)} & + & \text{H}_2\text{O(l)} & \rightleftharpoons & \text{H}_3\text{O}^+(aq) + \text{BrO}^-(aq) \\
\hline
\text{Initial (M)} & & & & \\
& 0.95 & & & 0.68 \\
\text{Change (M)} & & & & \\
& -x & & & +x \\
\text{Equilibrium (M)} & & & & \\
& 0.95 - x & & & 0.68 + x \\
\end{array}
\]
**Interactive Options:**
Below the table, there is a selection of potential calculations and variables for automated computation including:
- Symbols: 0, 0.95, 0.68, 8.68, +x, -x, +2x
- Expressions: 0.95 + x, 0.95 - x, 0.95 - 2x, 0.68 + x, 0.68 - x, 0.68 - 2x, 0.68 + 2x
There is a RESET button to clear selections.
**Purpose:**
This educational tool assists in calculating buffer pH by setting up and solving ICE tables.
![**Determine the pH of a Buffer Solution**
**Problem Statement:**
Determine the pH of a buffer that is composed of 0.95 M HBrO and 0.68 M KBrO. The given value of pKa for HBrO is 8.68.
---
**Instructions:**
Based on your ICE (Initial, Change, Equilibrium) table and the definition of Ka (acid dissociation constant), set up the expression for Ka in order to determine the unknown. Do not combine or simplify terms.
---
**Expression for Ka:**
\[ K_a = \]
---
**Available Values and Expressions:**
- [0]
- [0.95]
- [0.68]
- [8.68]
- [x]
- [2x]
- [2]^2
- [0.95 + x]
- [0.95 - x]
- [0.95 + 2x]
- [0.95 - 2x]
- [0.68 + x]
- [0.68 - x]
- [0.68 + 2x]
- [0.68 - 2x]
- 0.939
- 4.79 x 10^-6
- 2.09 x 10^-2
---
**Button:**
- Reset
Use these values and expressions to correctly set up the equation for Ka.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5c6d7610-fae0-4fdd-8afb-1e0bd9bb140b%2F249f38d0-43dd-4018-91c1-c87eee4af304%2Fga1f4t_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Determine the pH of a Buffer Solution**
**Problem Statement:**
Determine the pH of a buffer that is composed of 0.95 M HBrO and 0.68 M KBrO. The given value of pKa for HBrO is 8.68.
---
**Instructions:**
Based on your ICE (Initial, Change, Equilibrium) table and the definition of Ka (acid dissociation constant), set up the expression for Ka in order to determine the unknown. Do not combine or simplify terms.
---
**Expression for Ka:**
\[ K_a = \]
---
**Available Values and Expressions:**
- [0]
- [0.95]
- [0.68]
- [8.68]
- [x]
- [2x]
- [2]^2
- [0.95 + x]
- [0.95 - x]
- [0.95 + 2x]
- [0.95 - 2x]
- [0.68 + x]
- [0.68 - x]
- [0.68 + 2x]
- [0.68 - 2x]
- 0.939
- 4.79 x 10^-6
- 2.09 x 10^-2
---
**Button:**
- Reset
Use these values and expressions to correctly set up the equation for Ka.
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