Question

What are the concentrations of hydroxide and hydronium ions in a solution with a pH of 10.2?

Answer 1

Answer:
`[H^+]=6.3* 10^(-11)` and
`[OH^-]=1.58* 10^(-4)`

Step-by-step explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration and pOH is calculated by taking negative logarithm of hydroxide ion concentration.

`pH=-\log [H^+]`

`pOH=-log[OH^-]`

`pH+pOH=14`

Given pH = 10.2

`10.2=-\log [H^+]`

`[H^+]=6.3* 10^(-11)`

`pOH=14-10.2=3.8`

`3.8=-log[OH^-]`

`[OH^-]=1.58* 10^(-4)`

Answer 2

Answer : The concentrations of hydroxide and hydronium ions in a solution with a pH of 10.2 are,
`1.58* 10^(-4)` and
`6.3* 10^(-11)` respectively.

Explanation : Given,

pH = 10.2

pH : It is defined as the negative logarithm of the hydrogen ion concentration.

First we have to calculate the hydrogen ion concentration
`(H^+)`

`pH=-\log [H^+]`

Now put the value of pH in this formula, we get the hydrogen ion concentration.

`10.2=-\log [H^+]`

`[H^+]=6.3* 10^(-11)`

Now we have to calculate the pOH of the solution.

`pH+pOH=14`

Now put the value of pH, we get the value of pOH.

`10.2+pOH=14`

`pOH=14-10.2`

`pOH=3.8`

Now we have to calculate the hydroxide ion concentration
`(OH^-)`

`pOH=-\log [OH^-]`

Now put the value of pOH in this formula, we get the hydroxide ion concentration.

`3.8=-\log [OH^-]`

`[OH^-]=1.58* 10^(-4)`

Therefore, the concentrations of hydroxide and hydronium ions in a solution with a pH of 10.2 are,
`1.58* 10^(-4)` and
`6.3* 10^(-11)` respectively.