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Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 69c

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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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 allows us to determine the amount of product formed from given quantities of reactants. In this case, stoichiometry is essential to find the theoretical yield of lead(II) chloride (PbCl2) from the initial concentrations and volumes of potassium chloride (KCl) and lead(II) nitrate (Pb(NO3)2).
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Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of a product to the theoretical yield. It is expressed as a percentage and is calculated using the formula: (actual yield / theoretical yield) × 100%. In this problem, the actual yield is the mass of PbCl2 collected, while the theoretical yield is determined from stoichiometric calculations.
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Molarity and Dilution

Molarity (M) is a concentration unit defined as the number of moles of solute per liter of solution. It is crucial for determining the amount of reactants in a solution. In this question, the molarity of KCl and Pb(NO3)2 solutions is used to calculate the moles of each reactant before the reaction occurs, which is necessary for stoichiometric calculations and determining the theoretical yield.
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Related Practice
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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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Open 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 limiting reactant and the theoretical yield.
Textbook Question

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.

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Textbook Question

For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? a. CsCl b. CH3OH c. Ca(NO2)2 d. C6H12O6

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Textbook Question

Classify each compound as a strong electrolyte or nonelectrolyte. a. MgBr2 b. C12H22O11 c. Na2CO3 d. KOH

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