Question

the pH of a 0.001M aqueous solution of sodium hydroxide will be

1) 5.0
2) 7.5
3) 9.0
4) 11.0​

Answer 1

Answer:

d) 11.0

Explanation:

pOH = -log10 ( OH-)

pOH = -log 10 (0.001)

pOH = 3

pH +pOH = 14

pH + 3 = 14

pH = 11

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Answer 2

Answer:

The pH of a 0.001M aqueous solution of sodium hydroxide will be 11.

Explanation:

The pH of a solution is a measurement of how acidic or basic it is. The scale runs from 0 to 14, with 7 being the neutral value. Acidity is indicated by a pH less than 7, while a pH greater than 7 indicates a base.

pH is reported in "logarithmic units"

pH = -log[$H^{+}$]

Given concentration of sodium hydroxide = 0.001 M

Since sodium hydroxide is a base, it dissociates as:

$NaOH$ ⇄ $Na^{+} + OH^{-}$

∴pOH = -log[$OH^{-}$]

          = -log(0.001) = 3

We know that pH + pOH = 14

⇒pH = 14 - pOH

        = 14 - 3 = 11

Therefore the pH of a 0.001M aqueous solution of sodium hydroxide will be 11.