If the [OH1-] of a solution at 25oC is 5.8x10^(-5) mol/L, calculate the [H1+] in mol/L, the pH, and the pOH.

1. [H⁺] = 1.58×10¯¹⁰ mol/L

2. pH = 9.8

3. pOH = 4.2

Explanation:

We'll begin by calculating the pOH of the solution. This can be obtained as follow:

Concentration of Hydroxide ion [OH¯] = 5.8×10¯⁵ mol/L

pOH =?

pOH = –Log [OH¯]

pOH = –Log 5.8×10¯⁵

pOH = 4.2

Next, we shall determine the pH of the solution. This can be obtained as follow:

pOH = 4.2

pH =?

pH + pOH = 14

pH + 4.2 = 14

Collect like terms

pH = 14 – 4.2

pH = 9.8

Finally, we shall determine the concentration of Hydrogen ion [H⁺] in the solution. This can be obtained as follow:

pH = 9.8

Concentration of Hydrogen ion [H⁺] =?

pH = –Log [H⁺]

9.8 = –Log [H⁺]

Multiply through by –1

–9.8 = Log [H⁺]

Take the anti log of –9.8

[H⁺] = antilog (–9.8)

[H⁺] = 1.58×10¯¹⁰ mol/L

SUMMARY:

1. [H⁺] = 1.58×10¯¹⁰ mol/L

2. pH = 9.8

3. pOH = 4.2

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