   # Consider a solution of an unknown salt having the general formula BHCl, where B is one of the weak bases in Table 13-3. A 0.10- M solution of the unknown salt has a pH of 5.82. What is the actual formula of the salt? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 124E
Textbook Problem
5 views

## Consider a solution of an unknown salt having the general formula BHCl, where B is one of the weak bases in Table 13-3. A 0.10-M solution of the unknown salt has a pH of 5.82. What is the actual formula of the salt?

Interpretation Introduction

Interpretation: The general formula of an unknown salt is given to be BHCl where B a weak base is. The pH value of a 0.10M solution of the unknown salt is 5.82 . The actual formula of the salt is to be stated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution.

The pH of a solution is calculated by the formula, pH=log[H+]

The sum, pH+pOH=14

The equilibrium constant for water is denoted by Kw and is expressed as,

Kw=[H+][OH]

The value of Kw is calculated by the formula,

Kw=KaKb

### Explanation of Solution

Explanation

To determine: The actual formula of the given unknown salt.

The [H+] is 1.51×10-6M_ .

Given

pH=5.82

The pH of a solution is calculated by the formula,

pH=log[H+]

Rearrange the above expression to calculate the value of [H+] .

[H+]=10pH

Substitute the given value of pH in the above expression.

[H+]=105.82=1.51×10-6M_

The equilibrium constant expression for the given reaction is, Ka=[B][H+][BH+]

The dominant equilibrium reaction is,

BH+(aq)B(aq)+H+(aq)

At equilibrium, the equilibrium constant expression is expressed by the formula,

Ka=ConcentrationofproductsConcentrationofreactants

Where,

• Ka is the acid dissociation constant.

The equilibrium constant expression for the given reaction is,

Ka=[B][H+][BH+] (1)

The Ka is 2.28×10-11_ .

The change in concentration of BH+ is assumed to be x .

The liquid components do not affect the value of the rate constant.

The ICE table for the stated reaction is,

BH+(aq)B(aq)+H+(aq)Inititialconcentration0.1000Changex+x+xEquilibriumconcentration0

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Find more solutions based on key concepts
Nutrition authorities often recommend. drinking water, plain or lightly flavored, to quench thirst staying hydr...

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

What is the plasma membrane, and what are its main functions?

Biology: The Dynamic Science (MindTap Course List)

What energy sources on Earth cannot be thought of as stored sunlight?

Horizons: Exploring the Universe (MindTap Course List)

What impact has recombinant DNA technology had on genetics and society?

Human Heredity: Principles and Issues (MindTap Course List)

How many equivalents of solute are in 73.1mL of 0.834NNaOH?

Introductory Chemistry: An Active Learning Approach

Why would the U.S. Navy have been interested in seeing such deep-water charts produced?

Oceanography: An Invitation To Marine Science, Loose-leaf Versin

Find the direction of the magnetic field acting on a positively charged particle moving in the various situatio...

Physics for Scientists and Engineers, Technology Update (No access codes included) 