What is the pH of 0.01 M glycine solution? For glycine, K a 1 = 4.5 × 1 0 − 3 and K a 2 = 1.7 × 1 0 − 10 at 298 K ?

K = K a 1 × K a 2 = 4.5 × 1 0 − 3 × 1.7 × 1 0 − 10 = 7.65 × 1 0 − 13 [ H + ] = K C = 7.65 × 1 0 − 13 × 0.01 = 7.65 × 1 0 − 15 = 0.87 × 1 0 − 7 pH = − lo g 0.87 × 1 0 − 7 = 7 − 0.93 = 6.07

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Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumpH of Strong and Weak Acids and BasesMedium2 minPYQ_2004

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What is the $pH$ of $0.01 M$ glycine solution? For glycine, $K_{a_{1}} = 4.5 \times 1 0^{- 3}$ and $K_{a_{2}} = 1.7 \times 1 0^{- 10}$ at $298 K$ ?

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Answer:

Solution:

$K = K a_{1} \times K a_{2} = 4.5 \times 1 0^{- 3} \times 1.7 \times 1 0^{- 10} = 7.65 \times 1 0^{- 13} [H^{+}] = K C = 7.65 \times 1 0^{- 13} \times 0.01 = 7.65 \times 1 0^{- 15} = 0.87 \times 1 0^{- 7} pH = - lo g 0.87 \times 1 0^{- 7} = 7 - 0.93 = 6.07$

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

⏱ 2mℹ️ Source: PYQ_2004

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