The hydronium ion concentration and the p H value for given neutral water at temperature 37 °C has to be calculated. Concept Introduction: Ionic-product constant for water: It is the hydronium ion concentration times the O H − concentration present in the solution. H 2 O ( l ) + H 2 O ( l ) H 3 O + ( a q ) + O H − ( a q ) K = [ H 3 O + ] [ O H − ] [ H 2 O ] [ H 2 O ] [ H 3 O + ] = [ O H − ] = 1.00 × 10 − 7 M ∴ K W = K [ H 2 O ] [ H 2 O ] = [ H 3 O + ] [ O H − ] K W = 1.00 × 10 − 14 M The K w will apply to all aqueous solution. For acidic solution [ H 3 O + ] is large that is [ H 3 O + ] > 10 − 7 M a n d [ O H − ] < 10 − 7 M For basic solution [ O H − ] is large that is [ H 3 O + ] < 10 − 7 M a n d [ O H − ] > 10 − 7 M pH : The concentration of hydrogen ion is measured using pH scale. The pH of a solution is a figure that expresses the acidity or the alkalinity of a given solution. It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration. pH = -log[H 3 O + ]

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Chapter 5, Problem 5.22P

(a)

Interpretation Introduction

Interpretation:

The hydronium ion concentration and the pH value for given neutral water at temperature 37 °C has to be calculated.

Concept Introduction:

Ionic-product constant for water: It is the hydronium ion concentration times the OH− concentration present in the solution.

H2O(l)+H2O(l)H3O+(aq)+OH−(aq)K=[ H3O+ ][ OH− ][ H2O ][ H2O ][ H3O+ ]=[ OH− ]=1.00×10−7M∴KW=K[ H2O ][ H2O ]=[ H3O+ ][ OH− ] KW= 1.00×10−14M

The Kw will apply to all aqueous solution.

For acidic solution [H3O+] is large that is [H3O+]>10−7M and [OH−]<10−7M

For basic solution [OH−] is large that is [H3O+]<10−7M and [OH−]>10−7M

pH: The concentration of hydrogen ion is measured using pH scale. The pH of a solution is a figure that expresses the acidity or the alkalinity of a given solution.

It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH = -log[H3O+]

(b)

Interpretation Introduction

Interpretation:

The hydroxide ion concentration and the pOH value for given neutral water at temperature 37 °C has to be calculated.

Concept Introduction:

Ionic-product constant for water: It is the hydronium ion concentration times the OH− concentration present in the solution.

H2O(l)+H2O(l)H3O+(aq)+OH−(aq)K=[ H3O+ ][ OH− ][ H2O ][ H2O ][ H3O+ ]=[ OH− ]=1.00×10−7M∴KW=K[ H2O ][ H2O ]=[ H3O+ ][ OH− ] KW= 1.00×10−14M

The Kw will apply to all aqueous solution.

For acidic solution [H3O+] is large that is [H3O+]>10−7M and [OH−]<10−7M .

For basic solution [OH−] is large that is [H3O+]<10−7M and [OH−]>10−7M .

pH: The concentration of hydrogen ion is measured using pH scale. The pH of a solution is a figure that expresses the acidity or the alkalinity of a given solution.

pH = -log[H3O+]

The pOH value is negative log of [OH-]-Hydroxide ion concentration.

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