Ch.4 - Chemical Quantities & Aqueous Reactions

Problem 35

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Chapter 4, Problem 35

For each of the acid–base reactions, calculate the mass (in grams) of each acid necessary to completely react with and neutralize 4.85 g of the base. b. 2 HNO₃(aq) + Ca(OH)₂(aq) → 2 H₂O(l) + Ca(NO₃)₂(aq)

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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 based on the balanced chemical equation. It involves using mole ratios derived from the coefficients of the balanced equation to determine the amount of substances needed or produced. In this case, stoichiometry will help calculate the mass of nitric acid required to neutralize a given mass of calcium hydroxide.

Acid-Base Neutralization

Acid-base neutralization is a chemical reaction where an acid reacts with a base to produce water and a salt. This process typically involves the transfer of protons (H+) from the acid to the base. Understanding the nature of the reactants, such as HNO3 being a strong acid and Ca(OH)2 being a strong base, is essential for predicting the products and calculating the amounts needed for complete reaction.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It is crucial for converting between grams and moles in stoichiometric calculations. To find the mass of nitric acid needed, one must first determine its molar mass and then use it in conjunction with the stoichiometric ratios from the balanced equation to find the required mass to neutralize the specified amount of base.

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Related Practice

Sulfuric acid dissolves aluminum metal according to the reaction:

2 Al(s) + 3 H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 3 H₂( g)

Suppose you want to dissolve an aluminum block with a mass of 15.2 g. What minimum mass of H₂SO₄ (in g) do you need? What mass of H₂ gas (in g) does the complete reaction of the aluminum block produce?

For each of the reactions, calculate the mass (in grams) of the product that forms when 3.67 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. a. Ba(s) + Cl2(g) → BaCl2(s) b. CaO(s) + CO2(g) → CaCO3(s) c. 2 Mg(s) + O2(g) → 2 MgO(s) d. 4 Al(s) + 3 O2(g) → 2 Al2O3(s)

Textbook Question

For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

a. 2 K(s) + Cl₂(g) → 2 KCl(s)

b. 2 K(s) + Br₂(l) → 2 KBr(s)

c. 4 Cr(s) + 3 O₂(g) → 2 Cr₂O₃(s)

d. 2 Sr(s) + O₂(g) → 2 SrO(s)

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Open Question

For each precipitation reaction, calculate how many grams of the first reactant are necessary to completely react with 55.8 g of the second reactant. a. 2 KI(aq) + Pb(NO3)2(aq) → PbI2(s) + 2 KNO3(aq) b. Na2CO3(aq) + CuCl2(aq) → CuCO3(s) + 2 NaCl(aq) c. K2SO4(aq) + Sr(NO3)2(aq) → SrSO4(s) + 2 KNO3(aq)

Textbook Question

Find the limiting reactant for each initial amount of reactants.

2 Na(s) + Br₂(g) → 2 NaBr(s)

a. 2 mol Na, 2 mol Br₂