Explanation Molarity can be determined as, number of moles of solute per liter solution, it can be expressed as: Molarity ( M ) = ( moles solute Liter solution ) When 100.0 mL of solution containing aqueous HCl and HBr is titrated with 0.1235 M NaOH of volume 47.14 mL, the moles of NaOH as solute in aqueous solution can be calculated as follows: Molarity ( M ) = ( moles solute Liter solution ) Moles solute = molarity × Liters solutions = 0 .1235 × ( 47 .14 × 1L 1000 mL ) = 0 .1235 M × 0 .04714 L = 0 .00582 mol The moles of NaOH will be equal to combined moles of HBr and HCl. Hence, the total moles of HCl and HBr, Moles of HBr and HCl = moles of NaOH = 0 .00582 mol Assuming the moles of AgCl be x, then the moles of AgBr will be, Moles of AgBr = ( total moles of AgBr and AgCl ) – ( moles of AgCl ) = ( 0 .00582 mol ) – ( x mol ) = ( 0 .00582 – x ) mol Further, calculating the mass of AgCl and AgBr such that, the total mass of silver halides is 0.9974 g. Calculating the mass of AgCl is 143.32 g/mol Moles of AgCl = ( mass of AgCl molar mass of AgCl ) Mass of AgCl = ( moles of AgCl × molar mass of AgCl ) = x × 143 .32 g/mol = 143 .32 x mol Calculating the mass of AgBr: The molar mass of AgBr is 187 .77 g/mol Moles of AgBr = ( mass of AgBr molar mass of AgBr ) Mass of AgBr = ( moles of AgBr x molar mass of AgBr ) = ( 0 .00582 – x ) × ( 187 .77 g/mol ) = ( 1 .092 – 187 .77 g/mol ) Therefore, Mass of silver halides = ( mass of AgBr ) + ( mass of AgCl ) 0

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ISBN: 9780134856230

Author: Robinson

Publisher: PEARSON

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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Chapter 4, Problem 4.141MP

Interpretation Introduction

Interpretation:

The molarities of HCl and HBr needs to be determined in the original solution.

Concept introduction:

The titration is the technique where a solution of measured concentration is utilized to calculate the concentration of an unknown solution. Classically, the titrant (the know solution) is added from a burette to a known quantity of the analyte (the unknown solution) till the reaction is finished.

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Chapter 4, Problem 4.140MP

Chapter 4, Problem 4.142MP

Chapter 4 Solutions

CHEMISTRY-TEXT

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Ch. 4 - Will a precipitation reaction occur when aqueous...Ch. 4 - APPLY 4.13 How might you use a precipitation...Ch. 4 - Conceptual PRACTICE 4.14 An aqueous solution...Ch. 4 - Conceptual APPLY 4.15 A solution containing the...Ch. 4 - Name the acids HI and HBrO2 .Ch. 4 - APPLY 4.17 Give likely chemical formulas...Ch. 4 - PRACTICE 4.18 Write a balanced ionic equation and...Ch. 4 - Milk of magnesia (active ingredient: magnesium...Ch. 4 - Prob. 4.19P Ch. 4 - Prob. 4.20A Ch. 4 - Prob. 4.21P Ch. 4 - Assume that the buret contains H+ ions, the flask...Ch. 4 - PRACTICE 4.24 Assign an oxidation number to each...Ch. 4 - APPLY 4.25 Chlorine can have several different...Ch. 4 - Identify the oxidizing agent and reducing agent in...Ch. 4 - APPLY 4.27 Police often use a Breathalyzer test to...Ch. 4 - PRACTICE 4.28 Predict whether the following...Ch. 4 - Use the following reactions to arrange the...Ch. 4 - Prob. 4.29P Ch. 4 - Prob. 4.30A Ch. 4 - A viramin-fortified brand of a sports...Ch. 4 - The nutritional label on Power ade specifies that...Ch. 4 - 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Solution Summary: The author explains the titration technique, where a solution of measured concentration is utilized to calculate the concentration of an unknown solution.

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Chapter 4 Solutions