If the hydroxide ion concentration of an aqueous solution is 3.0 x 10-4, what is the [H+] in the solution? Is the solution acidic, basic, or neutral?

[H+] is  3.31 × 10^-11 M

Solution: Basic

Explanation:

In the question we are given;

Concentration of Hydroxide ion [OH-] as 3.0 × 10^-4 M

We are required to determine the [H+] and whether the solution is acidic, basic or neutral.

We know that;

pOH + pH = 14

and that;

pOH = - log [OH-]

Therefore;

pOH = - log ( 3.0 × 10^-4)

       = 3.52

But;

pH = 14 - pOH

Thus;

pH = 14 - 3.52

     = 10.48

But, we know that;

pH = - log[H+]

Therefore;

H+ = Antilog -pH

    = Antilog -10.48

    = 3.31 × 10^-11

Thus, the concentration of H+ ions [H+] is  3.31 × 10^-11 M

Also since the pH is 10.48, then the solution is basic

in chemistry, a solution’s concentration is how much of a dissolvable substance, known as a solute, is mixed with another substance, called the solvent. the standard formula is c = m/v, where c is the concentration, m is the mass of the solute dissolved, and v is the total volume

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