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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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. For each of the following, calculate the indicated quantity.
a. [ OH - ] = 2.11 × 10 4 M , [ H + ] = ?

b. [ OH - ] = 7.34 × 10 6 M , pH = ?

c. [ OH - ] = 9.81 × 10 8 M , pOH = ?

d. pH = 9.32 , pOH = ?

e. [ H + ] = 5.87 × 10 11 M , pH = ?

f. pH = 5.83 , [ H + ] = ?

Interpretation Introduction

(a)

Interpretation:

The concentration of H+ ion in the given solution that contains 2.11×104MOH ion is to be calculated.

Concept Introduction:

The ionic product of water is the product of concentration of OH and H+ ion in water at a given temperature. The ionic product of water is represented as,

Kw=[H+][OH]

Where,

  • [OH] represents the concentration of OH ions in the solution.
  • [H+] represents the concentration of H+ ions in the solution.
  • Kw represents the ionic product of water.
Explanation

The concentration of OH in the solution is 2.11×104M.

The value of ionic product of water at 25°C is 1.00×1014M2.

The ionic product of water is represented as,

Kw=[H+][OH]

Where,

  • [OH] represents the concentration of OH ions in the solution.
  • [H+] represents the concentration of H+ ions in the solution.
  • Kw represents the ionic product of water.

Rearrange the above equation for the value of [H+]

Interpretation Introduction

(b)

Interpretation:

The pH of the given solution that contains 7.34×106MOH ion is to be calculated.

Concept Introduction:

The term pH referred to the power of hydrogen. The pH of a solution is mathematically equal to the negative logarithm of concentration of H+ ion in solution. The pH of a solution is represented as,

pH=log[H+]

Where,

  • [H+] represents the concentration of H+ ions in the solution.
Interpretation Introduction

(c)

Interpretation:

The pOH of the given solution that contains 9.81×108MOH ion is to be calculated.

Concept Introduction:

The pOH of a solution is used to measure the alkalinity of the solution. The pOH of a solution is mathematically equal to the negative logarithm of concentration of OH ion in solution. The pOH of a solution is represented as,

pOH=log[OH]

Where,

  • [OH] represents the concentration of OH ions in the solution.
Interpretation Introduction

(d)

Interpretation:

The pOH of the given solution that have 9.81pH is to be calculated.

Concept Introduction:

The pOH of a solution is used to measure the alkalinity of the solution. The pOH of a solution is mathematically equal to the negative logarithm of concentration of OH ion in solution. The pOH of a solution is represented as,

pOH=log[OH]

Where,

  • [OH] represents the concentration of OH ions in the solution.
Interpretation Introduction

(e)

Interpretation:

The pH of the given solution that contains 5.87×1011MH+ ion is to be calculated.

Concept Introduction:

The term pH referred to the power of hydrogen. The pH of a solution is mathematically equal to the negative logarithm of concentration of H+ ion in solution. The pH of a solution is represented as,

pH=log[H+]

Where,

  • [H+] represents the concentration of H+ ions in the solution.
Interpretation Introduction

(f)

Interpretation:

The concentration of H+ ions in the given solution that has 5.83pH is to be calculated.

Concept Introduction:

The term pH referred to the power of hydrogen. The pH of a solution is mathematically equal to the negative logarithm of concentration of H+ ion in solution. The pH of a solution is represented as,

pH=log[H+]

Where,

  • [H+] represents the concentration of H+ ions in the solution.

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