# Chapter 16, Problem 16.36QP

FindFindarrow_forward

### CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933

#### Solutions

Chapter
Section
FindFindarrow_forward

### CHEMISTRY: ATOMS FIRST VOL 1 W/CON...

14th Edition
Burdge
ISBN: 9781259327933

(a)

Interpretation Introduction

Interpretation:

The concentration of HBr in the given solutions at 25C has to be calculated

Concept Information:

In strong acids, the ionization of acid is complete.  This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

At equilibrium (after the completion of ionization), the concentration of strong acid will be zero since no molecules remains after ionization.

The concentration after ionization will be as follows,

pH Definition:

The concentration of hydrogen ion is measured using pH scale. The acidity of aqueous solution is expressed by pH scale.

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH=-log[H3O+]

Rearranging the above equation to solve for  [H+] ion concentration, we get

[H3O+]=10-pH

(b)

Interpretation Introduction

Interpretation:

The concentration of HBr in the given solutions at 25C has to be calculated

Concept Information:

In strong acids, the ionization of acid is complete.  This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

At equilibrium (after the completion of ionization), the concentration of strong acid will be zero since no molecules remains after ionization.

The concentration after ionization will be as follows,

pH Definition:

The concentration of hydrogen ion is measured using pH scale. The acidity of aqueous solution is expressed by pH scale.

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH=-log[H3O+]

Rearranging the above equation to solve for  [H+] ion concentration, we get

[H3O+]=10-pH

(c)

Interpretation Introduction

Interpretation:

The concentration of HBr in the given solutions at 25C has to be calculated

Concept Information:

In strong acids, the ionization of acid is complete.  This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

At equilibrium (after the completion of ionization), the concentration of strong acid will be zero since no molecules remains after ionization.

The concentration after ionization will be as follows,

pH Definition:

The concentration of hydrogen ion is measured using pH scale. The acidity of aqueous solution is expressed by pH scale.

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH=-log[H3O+]

Rearranging the above equation to solve for  [H+] ion concentration, we get

[H3O+]=10-pH

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution