Skip to main content
Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 118

Find the volume of 0.110 M hydrochloric acid necessary to react completely with 1.52 g Al(OH)3.

Verified Solution

Video duration:
2m
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this case, stoichiometry will help us find the moles of hydrochloric acid needed to react with aluminum hydroxide.
Recommended video:
Guided course
01:16
Stoichiometry Concept

Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is crucial for determining how much of a solution is needed to achieve a desired reaction. In this question, the molarity of hydrochloric acid will be used to calculate the volume required for the reaction with aluminum hydroxide.
Recommended video:

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. It provides the mole ratios needed for stoichiometric calculations. For this problem, the balanced equation between hydrochloric acid and aluminum hydroxide will indicate how many moles of HCl are required to completely react with the given mass of Al(OH)3.
Recommended video:
Guided course
01:32
Balancing Chemical Equations
Related Practice
Textbook Question

Find the mass of barium metal (in grams) that must react with O2 to produce enough barium oxide to prepare 1.0 L of a 0.10 M solution of OH-.

1366
views
Textbook Question

A solution contains Cr3+ ions and Mg2+ ions. The addition of 1.00 L of 1.51 M NaF solution causes the complete precipitation of these ions as CrF3(s) and MgF2(s). The total mass of the precipitate is 49.6 g. Find the mass of Cr3+ in the original solution.

2317
views
Textbook Question

The nitrogen in sodium nitrate and in ammonium sulfate is available to plants as fertilizer. Which is the more economical source of nitrogen, a fertilizer containing 30.0% sodium nitrate by weight and costing $9.00 per 100 lb or one containing 20.0% ammonium sulfate by weight and costing $8.10 per 100 lb?

1338
views
Textbook Question

Treatment of gold metal with BrF3 and KF produces Br2 and KAuF4, a salt of gold. Identify the oxidizing agent and the reducing agent in this reaction.

906
views
Textbook Question

Treatment of gold metal with BrF3 and KF produces Br2 and KAuF4, a salt of gold. Find the mass of the gold salt that forms when a 73.5-g mixture of equal masses of all three reactants is prepared.

2630
views
Textbook Question

A solution contains one or more of the following ions: Ag+ , Ca2+ , and Cu2+ . When you add sodium chloride to the solution, no precipitate forms. When you add sodium sulfate to the solution, a white precipitate forms. You filter off the precipitate and add sodium carbonate to the remaining solution, producing another precipitate. Write net ionic equations for the formation of each of the precipitates observed.

3087
views