Ch.18 - Aqueous Ionic Equilibrium

Tro - Chemistry: A Molecular Approach 6th Edition

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Tro 6th Edition

Ch.18 - Aqueous Ionic Equilibrium

Problem 73b

Chapter 18, Problem 73b

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. b. the volume of added base required to reach the equivalence point

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Identify the balanced chemical equation for the reaction: \( \text{HBr} + \text{KOH} \rightarrow \text{KBr} + \text{H}_2\text{O} \).

Determine the moles of \( \text{HBr} \) in the initial solution using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \). Convert the volume from mL to L.

Since the reaction is a 1:1 molar ratio, the moles of \( \text{KOH} \) required to reach the equivalence point will be equal to the moles of \( \text{HBr} \).

Calculate the volume of \( \text{KOH} \) solution needed using the formula: \( \text{volume} = \frac{\text{moles of KOH}}{\text{concentration of KOH}} \).

Convert the volume of \( \text{KOH} \) from liters to milliliters for the final answer.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Titration

Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant (a solution of known concentration) to a sample until the reaction reaches its equivalence point, where the amount of titrant added is stoichiometrically equivalent to the amount of substance in the sample.

Equivalence Point

The equivalence point in a titration is the stage at which the amount of titrant added is exactly enough to completely neutralize the analyte in the solution. At this point, the moles of acid equal the moles of base, and it is often indicated by a color change in an appropriate indicator or by measuring pH.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows for the determination of the relationships between the quantities of substances involved, which is essential for calculating the volume of titrant needed to reach the equivalence point in a titration.

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Textbook Question

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. c. the pH at 10.0 mL of added base

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. e. the pH after adding 5.0 mL of base beyond the equivalence point

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. a. the initial pH

Consider the curve shown here for the titration of a weak base with a strong acid and answer each question.

c. At what volume of added acid does pH = 14 - pK_b?

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Textbook Question

Consider the curve shown here for the titration of a weak base with a strong acid and answer each question.

d. At what volume of added acid is the pH calculated by working an equilibrium problem based on the concentration and K_a of the conjugate acid?

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