NaOH is a strong base. What will be pH of 5.0 × 1 0 − 2 M NaOH solution ? ( lo g 2 = 0.3 )

Given [ OH − ] = 5 × 1 0 − 2 ∴ pOH = − lo g 5 × 1 0 − 2 = − lo g 5 + 2 lo g 10 = 1.30 ∵ pH + pOH = 14 ∵ pH = 14 − pOH = 14 − 1.30 = 12.70

Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumpH of Strong and Weak Acids and BasesMedium2 minPYQ_2013

ChemistryMediumstatement

$NaOH$ is a strong base. What will be $pH$ of $5.0 \times 1 0^{- 2} M NaOH$ solution ? $(lo g 2 = 0.3)$

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Answer:

Solution:

Given $[OH^{-}] = 5 \times 1 0^{- 2}$ $∴ pOH = - lo g 5 \times 1 0^{- 2} = - lo g 5 + 2 lo g 10 = 1.30 ∵ pH + pOH = 14 ∵ pH = 14 - pOH = 14 - 1.30 = 12.70$

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:pH of Strong and Weak Acids and Bases

⏱ 2mℹ️ Source: PYQ_2013

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