Textbook Question
Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. a. AgI b. Cu3(PO4)2 c. CoCO3 d. K3PO4
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Ch.5 - Introduction to Solutions and Aqueous Solutions
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 5, Problem 46
A 55.0-mL sample of a 0.102 M potassium sulfate solution is mixed with 35.0 mL of a 0.114 M lead(II) acetate solution and this precipitation reaction occurs: K2SO4(aq) + Pb(C2H3O2)2(aq) → 2 KC2H3O2(aq) + PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 1.01 g. Determine the limiting reactant, theoretical yield, percent yield.
Verified step by step guidance1
Determine the moles of K_2SO_4: Use the formula \( \text{moles} = \text{molarity} \times \text{volume in liters} \). Convert 55.0 mL to liters and multiply by 0.102 M to find the moles of K_2SO_4.
Determine the moles of Pb(C_2H_3O_2)_2: Similarly, convert 35.0 mL to liters and multiply by 0.114 M to find the moles of Pb(C_2H_3O_2)_2.
Identify the limiting reactant: Use the stoichiometry of the balanced equation. Compare the mole ratio of K_2SO_4 to Pb(C_2H_3O_2)_2 (1:1) to determine which reactant is limiting.
Calculate the theoretical yield of PbSO_4: Use the moles of the limiting reactant to find the moles of PbSO_4 produced, using the 1:1 mole ratio from the balanced equation. Then, convert moles of PbSO_4 to grams using its molar mass.
Calculate the percent yield: Use the formula \( \text{percent yield} = \left( \frac{\text{actual yield}}{\text{theoretical yield}} \right) \times 100\% \). Substitute the actual yield (1.01 g) and the theoretical yield calculated in the previous step.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Limiting Reactant
The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. To identify it, one must compare the mole ratios of the reactants based on the balanced chemical equation and the initial amounts of each reactant. The reactant that produces the least amount of product is the limiting reactant.
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Limiting Reagent Concept
Theoretical Yield
The theoretical yield is the maximum amount of product that can be generated from a given amount of reactants, calculated using stoichiometry based on the balanced chemical equation. It assumes complete conversion of the limiting reactant into product without any losses. This value is essential for determining the efficiency of a reaction when compared to the actual yield obtained.
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Percent Yield
Percent yield is a measure of the efficiency of a chemical reaction, calculated by dividing the actual yield of the product by the theoretical yield and multiplying by 100. It provides insight into how much of the expected product was actually produced in the experiment. A percent yield less than 100% indicates that some reactants did not convert to products, which can be due to various factors such as incomplete reactions or losses during processing.
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Related Practice
Textbook Question
What is the molarity of ZnCl2 that forms when 25.0 g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 275 mL. Zn(s) + CuCl2(aq) → ZnCl2(aq) + Cu(s)
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Textbook Question
Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. a. AgNO3 b. Pb(C2H3O2)2 c. KNO3 d. (NH4)2S
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Textbook Question
Classify each compound as a strong electrolyte or nonelectrolyte. a. K2SO4 b. C6H12O6 c. K2CO3 d. CH3OH
Textbook Question
A 25.0-mL sample of a 1.20 M potassium chloride solution is mixed with 15.0 mL of a 0.900 M lead(II) nitrate solution and this precipitation reaction occurs: 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) The solid PbCl2 is collected, dried, and found to have a mass of 2.45 g. Determine the the percent yield.
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