   # 4.50 Aluminum hydroxide can be dissolved in hydrochloric acid to form aluminum chloride and water. Write a balanced chemical equation for this reaction. How many mL of 3.37 M HCI is needed to react with 10.0 g of Al(OH) 3 ? ### Chemistry for Engineering Students

3rd Edition
Lawrence S. Brown + 1 other
Publisher: Cengage Learning
ISBN: 9781285199023

#### Solutions ### Chemistry for Engineering Students

3rd Edition
Lawrence S. Brown + 1 other
Publisher: Cengage Learning
ISBN: 9781285199023
Chapter 4, Problem 4.52PAE
Textbook Problem
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## 4.50 Aluminum hydroxide can be dissolved in hydrochloric acid to form aluminum chloride and water. Write a balanced chemical equation for this reaction. How many mL of 3.37 M HCI is needed to react with 10.0 g of Al(OH)3?

Interpretation Introduction

Interpretation:

To write a chemical equation and calculate the volume of HCl required.

Concept introduction:

• The maximum yield is obtained by reacting all the limiting reactant.
• Percent yield relates actual versus theoretical yields.
• Molarity measures molar concentration.

Given:

Molarity =3.37MHClmass =10.0gAl(OH)3Molecular Weight Al(OH)3=78.0 g/mol

### Explanation of Solution

When performing calculations with molar concentration (molarity) it is much easier to change all units to moles.

Step 1: Balance Reaction

HCl(aq)+Al(OH)3(aq)H2O(l)+AlCl3(aq)3HCl(aq)+Al(OH)3(aq)3H2O(l)+AlCl3(aq)

Reaction is balanced

Step 2: Change all amounts to mol

molAl(OH)3=massMolecular Weight=10.078.0=0.1282 mole

Step 3: Relate stoichiometry

Ratio=1:3

molHCl=3×(molAl(OH)3=3×0

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