Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Educational Website Content**
---
### Titration Problem: Determining the pH of a Solution
**Problem Statement:**
What is the pH of the solution when 50.0 mL of 0.20 M HI is titrated with 40.0 mL of 0.139 M Sr(OH)₂?
**Chemical Equation:**
\[ 2 \text{HI} + \text{Sr(OH)}_2 \rightarrow \text{SrI}_2 + 2 \text{H}_2\text{O} \]
**Solution Calculation:**
\[ \text{pH} = \boxed{\ ?\ } \]
**Hint:**
Be careful of the mole ratios!
**Interactive Component:**
Below is an input field for you to provide the pH after considering the reaction and calculations:
\[ \text{pH at 40.0 mL base:} \underline{\hspace{150px}} \ \text{Enter} \]
**Detailed Explanation of Diagram:**
The diagram features a balanced chemical equation, showing that two moles of Hydrogen Iodide (HI) react with one mole of Strontium Hydroxide \(\text{Sr(OH)}_2\) to produce one mole of Strontium Iodide (\(\text{SrI}_2\)) and two moles of water (\(\text{H}_2\text{O}\)).
---
**Steps to Calculate the pH:**
1. **Calculate moles of HI and Sr(OH)₂:**
- Moles of HI: \( M \times V = 0.20 \, \text{M} \times 0.050 \, \text{L} = 0.010 \, \text{moles} \)
- Moles of Sr(OH)₂: \( M \times V = 0.139 \, \text{M} \times 0.040 \, \text{L} = 0.00556 \, \text{moles} \)
2. **Determine the limiting reagent:**
- 2 moles of HI react with 1 mole of Sr(OH)₂
- We need twice the moles of HI compared to Sr(OH)₂, i.e., 0.01112 moles of HI are required to react with 0](https://content.bartleby.com/qna-images/question/4f25db15-46c0-4416-96ae-dcfe4c7f9271/3bfea114-5c34-4c3f-bb32-b77dc256089d/1y1qrc_processed.jpeg)
Transcribed Image Text:**Educational Website Content**
---
### Titration Problem: Determining the pH of a Solution
**Problem Statement:**
What is the pH of the solution when 50.0 mL of 0.20 M HI is titrated with 40.0 mL of 0.139 M Sr(OH)₂?
**Chemical Equation:**
\[ 2 \text{HI} + \text{Sr(OH)}_2 \rightarrow \text{SrI}_2 + 2 \text{H}_2\text{O} \]
**Solution Calculation:**
\[ \text{pH} = \boxed{\ ?\ } \]
**Hint:**
Be careful of the mole ratios!
**Interactive Component:**
Below is an input field for you to provide the pH after considering the reaction and calculations:
\[ \text{pH at 40.0 mL base:} \underline{\hspace{150px}} \ \text{Enter} \]
**Detailed Explanation of Diagram:**
The diagram features a balanced chemical equation, showing that two moles of Hydrogen Iodide (HI) react with one mole of Strontium Hydroxide \(\text{Sr(OH)}_2\) to produce one mole of Strontium Iodide (\(\text{SrI}_2\)) and two moles of water (\(\text{H}_2\text{O}\)).
---
**Steps to Calculate the pH:**
1. **Calculate moles of HI and Sr(OH)₂:**
- Moles of HI: \( M \times V = 0.20 \, \text{M} \times 0.050 \, \text{L} = 0.010 \, \text{moles} \)
- Moles of Sr(OH)₂: \( M \times V = 0.139 \, \text{M} \times 0.040 \, \text{L} = 0.00556 \, \text{moles} \)
2. **Determine the limiting reagent:**
- 2 moles of HI react with 1 mole of Sr(OH)₂
- We need twice the moles of HI compared to Sr(OH)₂, i.e., 0.01112 moles of HI are required to react with 0
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