Question

Given the following pH values, determine the [OH-] for each solution. a. 7.00 c. 4.00 b. 11.00 d. 6.00

Answer 1

The hydroxide ion concentrations for pH values

a. 7.00 - 1×
`10^(-7)`M

b. 11.00 - 1×
`10^(-11)`M

c. 4.00 - 1×
`10^(-4)`M

d. 6.00 - 1×
`10^(-6)`M

To determine the hydroxide ion concentration ([
`OH^(-)`]) for each given pH value, we can use the formula:

`[OH^(-)] =10^(-pH)`

a. pH 7.00:

For a neutral solution with pH 7.00, the [OH^-] is calculated as
`10^(-7)`, resulting in a hydroxide ion concentration of 1×
`10^(-7)`M. In neutral water, the concentration of
`H^(+)` is also 1×
`10^(-7)`M.

b. pH 11.00:

For a basic solution with pH 11.00, the
`[OH^-]`is calculated as
`10^(-11)`. The resulting hydroxide ion concentration is 1×
`10^(-11)`M. Basic solutions have lower
`[H^(+) ]` concentrations and higher
`[OH^(-)]` concentrations.

c. pH 4.00:

For an acidic solution with pH 4.00, the
`[OH^-]` is calculated as
`10^(-4)`, resulting in a hydroxide ion concentration of 1×
`10^(-4)`M. Acidic solutions have higher
`[H^(+)]` concentrations and lower
`[OH^(-) ]` concentrations.

d. pH 6.00:

For a slightly acidic solution with pH 6.00, the
`[OH^-]` is calculated as
`10^(-6)`, resulting in a hydroxide ion concentration of 1×
`10^(-6)`M. The solution is more acidic than neutral but less acidic than a solution with pH 4.00.

The hydroxide ion concentrations for pH values 7.00, 11.00, 4.00, and 6.00 are 1×
`10^(-7)`M, 1×
`10^(-11)`M, 1×
`10^(-4)`M and 1×
`10^(-6)`M respectively.