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nadya68 [22]
3 years ago
15

The pKa of the α‑carboxyl group of serine is 2.21 , and the pKa of its α‑amino group is 9.15 . Calculate the average net charge

on serine if it is in a solution that has a pH of 8.30 .

Chemistry
1 answer:
sleet_krkn [62]3 years ago
8 0

Answer:

Net charge in serine at pH equal to 8.30 is "0"

Explanation:

  • At pH > pK_{a}, carboxyl group exists as -CO_{2}^{-} (charged)
  • At pH < pK_{a}, carboxyl group exists as -COOH (neutral)
  • At pH > pK_{a}, amino group exists as -NH_{2} (neutral)
  • At pH < pK_{a}, amino group exists as -NH_{3}^{+} (charged)
  • So, at pH = 8.30, both carboxyl and amino group exists in charged state.
  • Net charge in serine at pH equal to 8.30 is "0".
  • Structure of serine at pH equal to 8.30 has been shown below.

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Answer:

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Explanation:

Like the problem said, the first thing we can do is calculate the mass of each of the 3 elements in a 100-gram sample:

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Now we need to find the empirical formula from these. To do so, convert all of those masses into moles by using the molar mass for each element:

- the molar mass of H is 1.01 g/mol

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Our ratio of H : S : O is now:

1.98 mol : 1.02 mol : 4.08 mol

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1.98/1.02  :  1.02/1.02  :  4.08/1.02

1.94 : 1 : 4

1.94 ≈ 2

So:

2 : 1 : 4

Thus, the empirical formula is: H_2SO_4.

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