General Chemistry
General Chemistry
4th Edition
ISBN: 9781891389603
Author: Donald A. McQuarrie, Peter A. Rock, Ethan B. Gallogly
Publisher: University Science Books
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Chapter 12, Problem 12.28P
Interpretation Introduction

Interpretation:

Mass of silver iodide formed along with the concentration of various ions after the completion of reaction has to be calculated.

Concept Introduction:

The formula to evaluate moles from molarity is given as follows:

  n=MV

Here,

M denotes molarity.

n denotes number of moles.

V denotes volume.

Expert Solution & Answer
Check Mark

Answer to Problem 12.28P

Mass of silver iodide formed is 34.922 g. Concentration of Ca2+, NO3 and I0.31875 mol/L, 0.49583 mol/L and 0.14166 mol/L respectively.

Explanation of Solution

The conversion factor to convert liters to milliliters is as follows:

  1 L=1000 mL

Hence convert 175 mL to L as follows:

  Volume=(175 mL)(1 L1000 mL)=0.175 L

Hence convert 125 mL to L as follows:

  Volume=(125 mL)(1 L1000 mL)=0.125 L

The formula to evaluate moles from molarity is given as follows:

  n=MV        (1)

Substitute 0.850 mol/L for M and 0.175 L for V in equation (1) to calculate moles of AgNO3.

  n=(0.850 mol/L)(0.175 L)=0.14875 mol

Substitute 0.765 mol/L for M and 0.125 L for V in equation (1)to calculate moles of CaI2.

  n=(0.765 mol/L)(0.125 L)=0.095625 mol

The balanced chemical reaction is given as follows:

  2AgNO3(aq)+CaI2(aq)2AgI(s)+Ca(NO3)2(aq)        (2)

According to the stoichiometry of the balanced equation (2), two moles of AgNO3 can give 2 mol AgI. Thus moles of AgI formed from 0.14875 mol AgNO3 is calculated as follows:

  Moles of AgI=(0.14875 mol AgNO3)(2 mol AgI2 mol AgNO3)=0.14875 mol AgI

Similarly, one mole CaI2 can give 2 mol AgI. Thus moles of AgI formed from 0.095625 mol CaI2 is calculated as follows:

  Moles of AgI=(0.095625 mol CaI2)(2 mol AgI1 mol CaI2)=0.19125 mol AgI

Since moles of AgNO3 available are less thus it is limiting reagent. Thus moles of AgI formed is 0.14875 mol.

The formula to convert mass in gram to moles is as follows:

  Mass=(Number of moles)(Molar mass)        (3)

Substitute 0.14875 mol for moles and 234.77 g/mol for molar mass of AgI in equation (3).

  Mass=(0.14875 mol)(234.77 g/mol)=34.922 g

Since all the Ag+ present in AgNO3 is consumed and is converted to precipitate AgI, Ionic species present in solution after reaction include Ca2+, NO3 and I ions.

The initial concentration of Ca2+ present in 0.765 M CaI2 is calculated as follows:

  Concentration of Ca2+=(0.125 L)(0.765 mol CaI21 L)(1 mol Ca2+1 mol CaI2)=0.095625 mol

Similarly, the initial concentration of NO3  is calculated as follows:

  Concentration of NO3=(0.175 L)(0.850 mol AgNO31 L)(1 mol NO31 mol AgNO3)=0.14875 mol

When solutions are mixed total volume of solution is calculated as follows:

  Total volume=0.175 L+0.125 L=0.3 L

Thus the concentration of Ca2+ after the reaction is calculated as follows:

  Concentration of Ca2+=(0.095625 mol0.3 L)=0.31875 mol/L

The concentration of NO3 the present after the reaction is calculated as follows:

  Concentration of NO3=(0.14875 mol )0.3 L=0.49583 mol/L

Thus I present in excess is calculated as follows:

  Concentration of Excess I=(0.095625 mol CaI2)(2 mol I1 mol CaI2)=0.19125 mol

Thus moles after the reaction is the difference of excess I and I precipitated as AgI calculated as follows:

  Moles of I=Excess IIprecipitated=(0.19125 mol0.14875 mol)=0.0425 mol

The concentration of I present after the reaction is calculated as follows:

  Concentration of I=(0.0425 mol )0.3 L=0.14166 mol/L

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Chapter 12 Solutions

General Chemistry

Ch. 12 - Prob. 12.11PCh. 12 - Prob. 12.12PCh. 12 - Prob. 12.13PCh. 12 - Prob. 12.14PCh. 12 - Prob. 12.15PCh. 12 - Prob. 12.16PCh. 12 - Prob. 12.17PCh. 12 - Prob. 12.18PCh. 12 - Prob. 12.19PCh. 12 - Prob. 12.20PCh. 12 - Prob. 12.21PCh. 12 - Prob. 12.22PCh. 12 - Prob. 12.23PCh. 12 - Prob. 12.24PCh. 12 - Prob. 12.25PCh. 12 - Prob. 12.26PCh. 12 - Prob. 12.27PCh. 12 - Prob. 12.28PCh. 12 - Prob. 12.29PCh. 12 - Prob. 12.30PCh. 12 - Prob. 12.31PCh. 12 - Prob. 12.32PCh. 12 - Prob. 12.35PCh. 12 - Prob. 12.36PCh. 12 - Prob. 12.37PCh. 12 - Prob. 12.38PCh. 12 - Prob. 12.39PCh. 12 - Prob. 12.40PCh. 12 - Prob. 12.41PCh. 12 - Prob. 12.42PCh. 12 - Prob. 12.43PCh. 12 - Prob. 12.44PCh. 12 - Prob. 12.45PCh. 12 - Prob. 12.46PCh. 12 - Prob. 12.47PCh. 12 - Prob. 12.48PCh. 12 - Prob. 12.49PCh. 12 - Prob. 12.50PCh. 12 - Prob. 12.51PCh. 12 - Prob. 12.52PCh. 12 - Prob. 12.53PCh. 12 - Prob. 12.54PCh. 12 - Prob. 12.55PCh. 12 - Prob. 12.56PCh. 12 - Prob. 12.58PCh. 12 - Prob. 12.59PCh. 12 - Prob. 12.60PCh. 12 - Prob. 12.61PCh. 12 - Prob. 12.62PCh. 12 - Prob. 12.63PCh. 12 - Prob. 12.64PCh. 12 - Prob. 12.65PCh. 12 - Prob. 12.66PCh. 12 - Prob. 12.67PCh. 12 - Prob. 12.68PCh. 12 - Prob. 12.69PCh. 12 - Prob. 12.70PCh. 12 - Prob. 12.71PCh. 12 - Prob. 12.72PCh. 12 - Prob. 12.73PCh. 12 - Prob. 12.74PCh. 12 - Prob. 12.75PCh. 12 - Prob. 12.76PCh. 12 - Prob. 12.77PCh. 12 - Prob. 12.78PCh. 12 - Prob. 12.79PCh. 12 - Prob. 12.80PCh. 12 - Prob. 12.81PCh. 12 - Prob. 12.82PCh. 12 - Prob. 12.83PCh. 12 - Prob. 12.84PCh. 12 - Prob. 12.85P
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