This image displays a chemistry problem involving a reaction between hydrochloric acid (HCl) and lead(II) nitrate (Pb(NO₃)₂). The goal is to determine the volume of 0.500 M HCl needed to react completely with 0.100 moles of Pb(NO₃)₂.### Problem Statement10. What volume of 0.500 M HCl is needed to react completely with 0.100 mols of Pb(NO₃)₂?### SolutionThe balanced chemical equation for the reaction is:\[ 2 \text{HCl} + \text{Pb(NO}_3\text{)}_2 \rightarrow \text{PbCl}_2 + 2 \text{HNO}_3 \]**Step-by-step Calculation:**1. **Mole Calculation:** \[ \text{Moles of HCl required} = \frac{0.1}{2} = 0.05 \text{ mol} \]2. **Volume Calculation:** \[ V_{\text{HCl}} = \frac{\text{moles}}{\text{molarity}} = \frac{0.05}{0.5} = 0.1 \text{ L} \]Thus, the volume of HCl needed is 0.1 liters, or 100 milliliters.The solution uses stoichiometry to determine the amount of reactant required for the reaction. The volume calculation illustrates the use of molarity (concentration) in determining the needed quantity of a solution to react fully with a given amount of another reactant.

Answered: 10. What volume of 0.500 M HCI is…

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10. What volume of 0.500 M HCI is needed to react completely with 0.100 mols of Pb(NO3)2? 2HCI + foCl, to2 HNQ 2

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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Question

This image displays a chemistry problem involving a reaction between hydrochloric acid (HCl) and lead(II) nitrate (Pb(NO₃)₂). The goal is to determine the volume of 0.500 M HCl needed to react completely with 0.100 moles of Pb(NO₃)₂.

### Problem Statement
10. What volume of 0.500 M HCl is needed to react completely with 0.100 mols of Pb(NO₃)₂?

### Solution
The balanced chemical equation for the reaction is:
\[ 2 \text{HCl} + \text{Pb(NO}_3\text{)}_2 \rightarrow \text{PbCl}_2 + 2 \text{HNO}_3 \]

**Step-by-step Calculation:**

1. **Mole Calculation:**
\[
\text{Moles of HCl required} = \frac{0.1}{2} = 0.05 \text{ mol}
\]

2. **Volume Calculation:**
\[
V_{\text{HCl}} = \frac{\text{moles}}{\text{molarity}} = \frac{0.05}{0.5} = 0.1 \text{ L}
\]

Thus, the volume of HCl needed is 0.1 liters, or 100 milliliters.

The solution uses stoichiometry to determine the amount of reactant required for the reaction. The volume calculation illustrates the use of molarity (concentration) in determining the needed quantity of a solution to react fully with a given amount of another reactant.

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