Question

What is the [OH-] in a solution that has a [H3O+] = 1.0 x 10-6 M?

1.0 x 10-6 M

1.0 x 10-2 M

1.0 x 10-8 M

1.0 x 10-10 M

Answer 1

To find the [OH-] in a solution with [H3O+] of 1.0 x 10^-6 M, use the ionic product of water (Kw) and divide Kw by [H3O+]. The correct answer is 1.0 x 10^-8 M.

Step-by-step explanation:

The student asked what the hydroxide ion concentration ([OH-]) is in a solution that has a hydronium ion concentration ([H3O+]) of 1.0 x 10-6 M. In aqueous solutions at 25 °C, the product of the concentrations of these two ions is always constant, given by the ionic product of water (Kw), which is 1.0 x 10-14 at this temperature. Therefore, to find the [OH-], we use the formula:

Kw = [H3O+][OH-]

Substituting the known [H3O+] into the equation and solving for [OH-] gives:

1.0 x 10-14 = (1.0 x 10-6 M) × [OH-] →

[OH-] = × (1.0 x 10-14) / (1.0 x 10-6)

[OH-] = 1.0 x 10-8 M

The correct answer to the student's question is 1.0 x 10-8 M.

Answer 2

explanation

`kw = 1 * {10}^( - 14)`

`oh = {?}`

`h3o = 1.0 * 10 {}^( - 6)`

`formula`

`kw = h3o * oh`

`insert \: values`

`1.0 * 10 {}^( - 14) = 1.0 * {10}^( - 6) * oh`

`\frac{1.0 * 10 {}^( - 14) }{ 1.0 * 10 {}^( - 6) } = oh`

`1 * {10}^( - 8)`