What is the molarity of an HCl solution if 11.0 mL HCI solution is titrated with 27.6 mL of 0.160 M NaOH solution? HCl(aq) + NaOH(aq)→¬N2CI(aq) + H;0(1)
What is the molarity of an HCl solution if 11.0 mL HCI solution is titrated with 27.6 mL of 0.160 M NaOH solution? HCl(aq) + NaOH(aq)→¬N2CI(aq) + H;0(1)
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
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![### Determining the Molarity of an HCl Solution through Titration
**Problem Statement:**
What is the molarity of an HCl solution if 11.0 mL of HCl solution is titrated with 27.6 mL of 0.160 M NaOH solution?
**Chemical Reaction:**
\[ \text{HCl(aq)} + \text{NaOH(aq)} \rightarrow \text{NaCl(aq)} + \text{H}_2\text{O(l)} \]
**Solution Method:**
1. **Identify the known quantities:**
- Volume of HCl solution (V_HCl) = 11.0 mL
- Volume of NaOH solution (V_NaOH) = 27.6 mL
- Molarity of NaOH solution (M_NaOH) = 0.160 M
2. **Write the expression for the titration reaction:**
- HCl and NaOH react in a 1:1 molar ratio.
3. **Calculate the moles of NaOH used:**
\[ \text{moles of NaOH} = M_{\text{NaOH}} \times V_{\text{NaOH}} \]
\[ \text{moles of NaOH} = 0.160 \, \text{M} \times \frac{27.6 \, \text{mL}}{1000} \]
\[ \text{moles of NaOH} = 0.004416 \, \text{mol} \]
4. **Since the reaction ratio is 1:1:**
- Moles of HCl = Moles of NaOH = 0.004416 mol
5. **Calculate the molarity of HCl:**
\[ M_{\text{HCl}} = \frac{\text{moles of HCl}}{V_{\text{HCl}}} \]
\[ M_{\text{HCl}} = \frac{0.004416 \, \text{mol}}{\frac{11.0 \, \text{mL}}{1000}} \]
\[ M_{\text{HCl}} = 0.401 \, \text{M} \]
**Express Your Answer Numerically in Molarity:**
- Molar](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd8345495-5282-4b9a-a515-8a335bc64c34%2Fb17de1f8-ac4d-4943-80aa-cf133c546312%2Ff5w8ywl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Determining the Molarity of an HCl Solution through Titration
**Problem Statement:**
What is the molarity of an HCl solution if 11.0 mL of HCl solution is titrated with 27.6 mL of 0.160 M NaOH solution?
**Chemical Reaction:**
\[ \text{HCl(aq)} + \text{NaOH(aq)} \rightarrow \text{NaCl(aq)} + \text{H}_2\text{O(l)} \]
**Solution Method:**
1. **Identify the known quantities:**
- Volume of HCl solution (V_HCl) = 11.0 mL
- Volume of NaOH solution (V_NaOH) = 27.6 mL
- Molarity of NaOH solution (M_NaOH) = 0.160 M
2. **Write the expression for the titration reaction:**
- HCl and NaOH react in a 1:1 molar ratio.
3. **Calculate the moles of NaOH used:**
\[ \text{moles of NaOH} = M_{\text{NaOH}} \times V_{\text{NaOH}} \]
\[ \text{moles of NaOH} = 0.160 \, \text{M} \times \frac{27.6 \, \text{mL}}{1000} \]
\[ \text{moles of NaOH} = 0.004416 \, \text{mol} \]
4. **Since the reaction ratio is 1:1:**
- Moles of HCl = Moles of NaOH = 0.004416 mol
5. **Calculate the molarity of HCl:**
\[ M_{\text{HCl}} = \frac{\text{moles of HCl}}{V_{\text{HCl}}} \]
\[ M_{\text{HCl}} = \frac{0.004416 \, \text{mol}}{\frac{11.0 \, \text{mL}}{1000}} \]
\[ M_{\text{HCl}} = 0.401 \, \text{M} \]
**Express Your Answer Numerically in Molarity:**
- Molar
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