Steven S. Zumdahl + 1 other

ISBN: 9781337399425

Steven S. Zumdahl + 1 other

ISBN: 9781337399425

Textbook Problem

Exercise 16.2 Calculate [H⁺] in a solution in which [ OH − ] = 2.0 × 10 − 2 M . Is this solution acidic, neutral, or basic?

Interpretation Introduction

Interpretation:

[H+] in a solution in which [OH−] = 2.0×10−2 M should be calculated and identify whether the solution is acidic, basic or neutral.

Concept Introduction:

Water is an amphoteric in nature implies it can act as an acid as well as base.

Ionization of water is given as:

H2O(l)+H2O(l)⇀↽H+(aq)+OH−(aq)

Here, one water molecule is act as an acid by accepting proton and another molecule of water act as a base by donating proton.

At 25°C, the actual concentrations of the products are:

[H+][OH−]=1×10−14

The mathematical product of both [H+] and [OH−] concentrations are always constant known as ion product constant ( Kw )

[H+][OH−]=1×10−14=Kw.

Given information:

[OH−] = 2.0×10−2 M

The relation between [H+] and [OH−] is given by:

[H+][OH−]=1×10−14

Put the value of [OH−], we get:

[H+]×2.0×10−2 =1×10−14

[H+]=1×10−142

Check out a sample textbook solution.

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Exercise 16.2 Calculate [H+] in a solution in which [ OH − ] = 2.0 × 10 − 2 M . Is this solution acidic, neutral, or basic?

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Exercise 16.2 Calculate [H⁺] in a solution in which [ OH − ] = 2.0 × 10 − 2 M . Is this solution acidic, neutral, or basic?

The axial skeleton consists of the __, while the appendicular skeleton consists of the _