Give the conditions for a neutral aqueous solution at 258C, in terms of [H1], pH, and the relationship between [H1] and [OH2]. Do the same for an acidic solution and for a basic solution. As a solution becomes more acidic, what happens to pH, pOH, [H1], and [OH2]? As a solution becomes more basic, what happens to pH, pOH, [H1], and [OH2]?

Question

Dale Richard

Chemistry

27 January, 05:54

Give the conditions for a neutral aqueous solution at 258C, in terms of [H1], pH, and the relationship between [H1] and [OH2]. Do the same for an acidic solution and for a basic solution. As a solution becomes more acidic, what happens to pH, pOH, [H1], and [OH2]? As a solution becomes more basic, what happens to pH, pOH, [H1], and [OH2]?

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Answers (1)

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Mary Anthony · Answer 1

As solution becomes acidic:

pH decreases in value

pOH increases also in value

[H1] concentration increases in value

[OH2] concentration decreases in value

As solution becomes basic:

pH increases in value

pOH decreases also in value

[H1] concentration decreases in value

[OH2] concentration increases in value

Explanation:

pH is the negative logarithm of the hydrogen ion concentration. Increase in acidity corresponds with decrease in pH value.

pOH is the negative logarithm of the hydroxyl ion concentration. Increase in basicity corresponds with increase in pOH value.

pH + pOH = 14

[H1] and [OH2] corresponds to the hydrogen and hydroxyl ion concentrations which increases with acidicity and basicity respectively.