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Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 109c

A sample of 8.69 g of Zn(OH)2 is added to 155.0 mL of 0.750 M H2SO4. (c) How many moles of Zn(OH)2, H2SO4, ZnSO4 are present after the reaction is complete?

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Identify the chemical reaction: \( \text{Zn(OH)}_2 + \text{H}_2\text{SO}_4 \rightarrow \text{ZnSO}_4 + 2\text{H}_2\text{O} \).
Calculate the moles of \( \text{Zn(OH)}_2 \) using its molar mass: \( \text{moles of Zn(OH)}_2 = \frac{8.69 \text{ g}}{\text{molar mass of Zn(OH)}_2} \).
Calculate the moles of \( \text{H}_2\text{SO}_4 \) using its concentration and volume: \( \text{moles of H}_2\text{SO}_4 = 0.750 \text{ M} \times 0.155 \text{ L} \).
Determine the limiting reactant by comparing the mole ratio from the balanced equation.
Use the stoichiometry of the balanced equation to find the moles of \( \text{ZnSO}_4 \) produced from the limiting reactant.

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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 question, stoichiometry will help us find the moles of ZnSO4 formed from the reaction between Zn(OH)2 and H2SO4.
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Molarity

Molarity 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 substance is present in a given volume of solution. In this problem, the molarity of H2SO4 is given, which will be used to calculate the moles of H2SO4 available for the reaction.
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Limiting Reactant

The limiting reactant is the substance that is completely consumed in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is essential for calculating the final amounts of products, such as ZnSO4 in this case, as it dictates how much of the other reactant can react.
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Related Practice
Textbook Question
The discovery of hafnium, element number 72, provideda controversial episode in chemistry. G. Urbain, a Frenchchemist, claimed in 1911 to have isolated an elementnumber 72 from a sample of rare earth (elements 58–71)compounds. However, Niels Bohr believed that hafniumwas more likely to be found along with zirconium thanwith the rare earths. D. Coster and G. von Hevesy, workingin Bohr's laboratory in Copenhagen, showed in 1922 thatelement 72 was present in a sample of Norwegian zircon,an ore of zirconium. (The name hafnium comes from theLatin name for Copenhagen, Hafnia). (c) Solid zirconiumdioxide, ZrO2, reacts with chlorine gas in the presenceof carbon. The products of the reaction are ZrCl4 and twogases, CO2 and CO in the ratio 1:2. Write a balanced chemicalequation for the reaction.
Textbook Question

A sample of 8.69 g of Zn(OH)2 is added to 155.0 mL of 0.750 M H2SO4. (b) Which is the limiting reactant in the reaction?

Textbook Question

In 2014, a major chemical leak at a facility in West Virginia released 28,390 L of MCHM (4-methylcyclohexylmethanol, C8H16O) into the Elk River. The density of MCHM is 0.9074 g/mL. (a) Calculate the initial molarity of MCHM in the river, assuming that the first part of the river is 2.00 m deep, 90.0 m wide, and 90.0 m long.

Textbook Question
Ritalin is the trade name of a drug, methylphenidate, used to treat attention-deficit/hyperactivity disorder in young adults. The chemical structure of methylphenidate is (c) Ritalin has a half-life of 3 hours in the blood, which means that after 3 hours the concentration in the blood has decreased by half of its initial value. For the man in part (b), what is the concentration of Ritalin in his blood after 6 hours?