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[H + ]. [OH - ] = Kw / [H + ]. [OH - ]. [H + ] > [OH - ]. [H + ] < [OH - ]. [H + ] = [OH - ]. Acidic Solution. Basic Solution. Neutral Solution. What are the concentrations of H + and OH - in a 0.0012 M NaOH solution? Answer: NaOH s completely dissociated:

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H

[H+]

[OH-] = Kw / [H+]

[OH-]

[H+]>[OH-]

[H+]<[OH-]

[H+]=[OH-]

Acidic

Solution

Basic

Solution

Neutral

Solution

What are the concentrations of H+ and OH- in a 0.0012 M NaOH solution?

Answer:

NaOH s completely dissociated:

0.0012 M NaOH (ac)  0.0012 M Na+(ac) +

Substituting [OH]- in the Kw equation: Kw = 1x10-14 = [H+][OH-]

1x10-14 = [H+](0.0012)

[H+] = 1x10-14/0.0012 =

0.0012 M OH- (ac)

8.3x10-12 M


H

[H+] pH [OH-] pOH

14,00

13,00

12,00

11,00

10,50

10,00

9,00

8,00

7,00

6,00

5,00

4,50

4,00

3,00

2,00

1,00

0,00

0,00

1,00

2,00

3,50

3,00

4,00

5,00

6,00

7,00

8,00

9,00

10,00

10,50

11,00

12,00

13,00

14,00

BASIC

More Basic

NEUTRAL

More Acidic

ACIDIC


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