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Calculate the volume of 0.169 M MgCl, that is needed to react completely with 80.5 mL of 0.450 M NaOH.

Calculate the volume of 0.169 M MgCl, that is needed to react completely with 80.5 mL of 0.450 M NaOH.

Chemistry
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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### Chemical Reaction Calculation Example **Problem Statement:** Consider the following reaction: \[ \text{MgCl}_2(\text{aq}) + 2 \text{NaOH}(\text{aq}) \rightarrow \text{Mg(OH)}_2(\text{s}) + 2 \text{NaCl}(\text{aq}) \] **Question:** Calculate the volume of 0.169 M \(\text{MgCl}_2\) that is needed to react completely with 80.5 mL of 0.450 M \(\text{NaOH}\). **Choices:** 1. 214 mL 2. 429 mL 3. 15.1 mL 4. 107 mL **Detailed Diagram Explanation:** There are no diagrams or graphs in this problem; it is purely a stoichiometric calculation based on the given chemical equation and concentrations. **Solution Approach:** To solve this, use the stoichiometry of the balanced chemical equation and the concept of molarity (moles per liter): 1. **Identify the molar ratio from the balanced equation:** - According to the balanced chemical equation, 1 mole of \(\text{MgCl}_2\) reacts with 2 moles of \(\text{NaOH}\). 2. **Calculate the moles of \(\text{NaOH}\):** - Molarity (M) = Moles of solute / Volume of solution in liters. - Convert 80.5 mL of \(\text{NaOH}\) to liters: \( 80.5 \, \text{mL} = 0.0805 \, \text{L} \) - Moles of \(\text{NaOH}\) = Molarity × Volume in liters - Moles of \(\text{NaOH}\) = \( 0.450 \, \text{M} \times 0.0805 \, \text{L} \) - Moles of \(\text{NaOH}\) = 0.036225 moles 3. **Use the stoichiometry to find moles of \(\text{MgCl}_2\):** - Moles of \(\text{MgCl}_2\) = \( \frac{1}{2} \times \text{
Transcribed Image Text:### Chemical Reaction Calculation Example **Problem Statement:** Consider the following reaction: \[ \text{MgCl}_2(\text{aq}) + 2 \text{NaOH}(\text{aq}) \rightarrow \text{Mg(OH)}_2(\text{s}) + 2 \text{NaCl}(\text{aq}) \] **Question:** Calculate the volume of 0.169 M \(\text{MgCl}_2\) that is needed to react completely with 80.5 mL of 0.450 M \(\text{NaOH}\). **Choices:** 1. 214 mL 2. 429 mL 3. 15.1 mL 4. 107 mL **Detailed Diagram Explanation:** There are no diagrams or graphs in this problem; it is purely a stoichiometric calculation based on the given chemical equation and concentrations. **Solution Approach:** To solve this, use the stoichiometry of the balanced chemical equation and the concept of molarity (moles per liter): 1. **Identify the molar ratio from the balanced equation:** - According to the balanced chemical equation, 1 mole of \(\text{MgCl}_2\) reacts with 2 moles of \(\text{NaOH}\). 2. **Calculate the moles of \(\text{NaOH}\):** - Molarity (M) = Moles of solute / Volume of solution in liters. - Convert 80.5 mL of \(\text{NaOH}\) to liters: \( 80.5 \, \text{mL} = 0.0805 \, \text{L} \) - Moles of \(\text{NaOH}\) = Molarity × Volume in liters - Moles of \(\text{NaOH}\) = \( 0.450 \, \text{M} \times 0.0805 \, \text{L} \) - Moles of \(\text{NaOH}\) = 0.036225 moles 3. **Use the stoichiometry to find moles of \(\text{MgCl}_2\):** - Moles of \(\text{MgCl}_2\) = \( \frac{1}{2} \times \text{
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