Question

What is the [oh−] of a solution with ph 5.75

Answer 1

[ H₃O⁺] = 10 ^- pH

[ H₃O⁺] = 10 ^ (- 5.75 )

[H₃O⁺] = 1.778x10⁻⁶ M

Kw = [ H₃O⁺] x [ OH⁻]

1x10⁻¹⁴ = 1.778x10⁻⁶ x [OH⁻]

[OH⁻] = 1x10⁻¹⁴ / 1.778x10⁻⁶

[OH⁻] = 5.62x10⁻⁹ M

hope this helps!

Answer 2

Step-by-step explanation:

pH means potential of hydrogen and it is defined as the measure of concentration of hydrogen ions in a solution.

Mathematically, pH =
`-log[H^(+)]`

Also, it is known that relationship between pH and pOH is as follows.

pH + pOH = 14

or pOH = 14 - pH

Therefore, putting the value of pH in the above relationship as follows.

pOH = 14 - pH

= 14 - 5.75

= 8.25

Hence, pOH =
`-log [OH^(-)]`

or,
`[OH^(-)]` = antilog (-8.25)

=
`5.62 * 10^(-9)`

Thus, we can conclude that the [oh−] of a solution with ph 5.75 is
`5.62 * 10^(-9)`.