Question

Calculate the [ OH − ] and the pH of a solution with an [ H + ] = 0.090 M at 25 °C . [ OH − ] = M pH = Calculate the [ H + ] and the pH of a solution with an [ OH − ] = 0.00098 M at 25 °C . [ H + ] = M pH = Calculate the [ H + ] and the [ OH − ] of a solution with a pH = 10.15 at 25 °C . [ H + ] = M [ OH − ] =

Answer 1

Answer: a)
`[OH^-]=1.09* 10^(-13)` and pH = 1.04

b)
`[H^+]=1.02* 10^(-11)` and
`pH=10.99`

c)
`[H^+]=7.08* 10^(-11)` and
`[OH^-]=1.41* 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.

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

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

`pH+pOH=14`

a)
`[H^+]=0.090M`

`pH=-\log [0.090]=1.04`

`pOH=14-1.04=12.96`

`12.96=-log[OH^-]`

`[OH^-]=1.09* 10^(-13)`

b)
`[OH^-]=0.00098M`

`pOH=-\log [0.00098]=3.01`

`pH=14-3.01=10.99`

`10.99=-log[H^+]`

`[H^+]=1.02* 10^(-11)`

c)
`pH=10.15`

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

`[H^+]=7.08* 10^(-11)`

`pOH=14-10.15=3.85`

`3.85=-log[OH^-]`

`[OH^-]=1.41* 10^(-4)`