pH of a 0.01 M solution ( K a = 6.6 × 1 0 − 4 )

α = C K a = 0.01 6.6 × 1 0 − 4 = 6.6 × 1 0 − 2 = 0.257 [ H + ] = C α = 0.01 × 0.257 = 2.57 × 1 0 − 3 pH = 3 − lo g 2.5 = 2.60

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Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumpH of Strong and Weak Acids and BasesEasy2 minPYQ_2009

ChemistryEasysingle choice

$pH$ of a $0.01 M$ solution $(K_{a} = 6.6 \times 1 0^{- 4})$

Options:

Answer:

Solution:

$α = \frac{K _{a}}{C} = \frac{6.6 \times 1 0 ^{- 4}}{0.01} = 6.6 \times 1 0^{- 2} = 0.257 [H^{+}] = C α = 0.01 \times 0.257 = 2.57 \times 1 0^{- 3} pH = 3 - lo g 2.5 = 2.60$

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

⏱ 2mℹ️ Source: PYQ_2009

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