## Question 1 of 10### What volume in milliliters of 0.0130 M Ca(OH)₂ is required to neutralize 70.0 mL of 0.0300 M HBr?**Explanation:**To solve this problem, we need to use the concept of neutralization reactions, where an acid and a base react to form water and a salt. The balanced chemical equation for the reaction between calcium hydroxide (Ca(OH)₂) and hydrobromic acid (HBr) is:\[ \text{Ca(OH)}_2 + 2 \text{HBr} \rightarrow \text{CaBr}_2 + 2 \text{H}_2\text{O} \]This equation indicates that one mole of Ca(OH)₂ neutralizes two moles of HBr.We use the formula:\[ M_1V_1 = M_2V_2 \]where:- \( M_1 \) and \( V_1 \) are the molarity and volume of the acid (HBr) - \( M_2 \) and \( V_2 \) are the molarity and volume of the base (Ca(OH)₂)However, because the mole ratio is 1:2, we need to account for this by modifying the formula:\[ M_1V_1 = 2(M_2V_2) \]Given:- \( M_1 = 0.0300 \) M (HBr)- \( V_1 = 70.0 \) mL (HBr)- \( M_2 = 0.0130 \) M (Ca(OH)₂)We need to find \( V_2 \):\[ 0.0300 \, \text{M} \times 70.0 \, \text{mL} = 2 \times 0.0130 \, \text{M} \times V_2 \]\[ 2.1 \, \text{M}\cdot\text{mL} = 0.0260 \, \text{M} \times V_2 \]\[ V_2 = \frac{2.1 \, \text{M}\cdot\text{mL}}{0.0260 \, \text{M}} \]

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What volume in milliliters of 0.0130 M Ca(OH)2 is required to neutralize 70.0 mL of 0.0300 M HBr?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 66AP: Relative solubilities of salts in liquid ammonia can differsignificantly from those in water. Thus,...

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