Question

Calculate either [ H 3 O + ] or [ OH − ] for each of the solutions.

Solution A: [ OH − ] = 3.33 × 10 − 7 M
Solution A: [ H 3 O + ] = M
Solution B: [ H 3 O + ] = 9.33 × 10 − 9 M
Solution B: [ OH − ] = M
Solution C: [ H 3 O + ] = 5.65 × 10 − 4 M
Solution C: [ OH − ] = M

Answer 1

Answer: Solution A :
`[H_3O^+]=0.300* 10^(-7)M`

Solution B :
`[OH^-]=0.107* 10^(-5)M`

Solution C :
`[OH^-]=0.177* 10^(-10)M`

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_3O^+]`

`pOH=-log[OH^-}`

`pH+pOH=14`

`[H_3O^+][OH^-]=10^(-14)`

a. Solution A:
`[OH^-]=3.33* 10^(-7)M`

`[H_3O^+]=(10^(-14))/(3.33* 10^(-7))=0.300* 10^(-7)M`

b. Solution B :
`[H_3O^+]=9.33* 10^(-9)M`

`[OH^-]=(10^(-14))/(9.33* 10^(-9))=0.107* 10^(-5)M`

c. Solution C :
`[H_3O^+]=5.65* 10^(-4)M`

`[OH^-]=(10^(-14))/(5.65* 10^(-4))=0.177* 10^(-10)M`