Calculate [H+] and [OH-] as required for each of the following
solutions at 25 °C, and state whether the solution is neutral, acidic,
or basic.
a. 1.0x 10-5 MOH-
Q
b. 1.0x 10-7 MOH-
c. 10.0 MH+

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lawalj99 lawalj99 · Answer 1 · 2021-02-27T02:06:56+01:00

Explanation:

The relationship between H+ and OH- at 25 °C is given as;

[H+} x [OH-] = 1.0 x 10-14 M

a. 1.0 x 10-5 M OH-

[OH-] = 1.0 x 10-5 M

[H+] = 1.0 x 10-14 M / [OH-] = 1.0 x 10-14 M / 1.0 x 10-5 M

[H+] = 1.0 x 10^(-14+5)

[H+] = 1.0 x 10^(-9)

pH = - log [H+]

pH = - log [10^(-9)]

pH = 9

This is a basic solution

b. 1.0 x 10-7 M OH-

[OH-] = 1.0 x 10-7 M

[H+] = 1.0 x 10-14 M / [OH-] = 1.0 x 10-14 M / 1.0 x 10-7 M

[H+] = 1.0 x 10^(-14+7)

[H+] = 1.0 x 10^(-7)

This is a neutral solution since [H+] and [OH-] are equal

c. 10.0 M H+

[H+] = 1.0 x 10 M

[OH-] = 1.0 x 10-14 M / [H+] = 1.0 x 10-14 M / 1.0 x 10 M

[OH-] = 1.0 x 10^(-14-1)

[OH-] = 1.0 x 10^(-15)

pH = - log [H+]

pH = - log [10^(1)]

pH = -1

This is an acidic solution since it has a pH of -1