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3 years ago

Consider a solution consisting of the following two buffer systems:

Chemistry

1 answer:

vazorg [7]3 years ago

7 0

Answer:

Option (e) is correct

Explanation:

According to Henderson - hasel balch equation

For H₂CO₃ / HCO₃⁻

$pH = pka + log\frac{[HCO^-_3]}{[H_2CO_3]} \\\\= 6.4 + log\frac{[HCO^-_3]}{[H_2CO_3]} -------(1)$

For H₂PO₄⁻ / HPO₄²⁻

$pH = pka + log\frac{[HPO_4^2^-]}{[H_2PO_4^-]} \\\\= 7.2 + log\frac{[HPO_4^2^-]}{[H_2PO_4^-]}-----(2)$

Now ph for buffer mixture is 6.4

pH = 6.4 in eqn(1) [HCO₃⁻]- [H₂CO₃]

pH = 6.4 in eqn(2) [H₂PO₄⁻] > [HPO₄²⁻]

Option (e) is correct

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KIM [24]

<u>Answer:</u> The sample of Carbon-14 isotope will take 2377.9 years to decay it to 25 %

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vaieri [72.5K]

Answer:

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Explanation:

Given data:

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