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Brums [2.3K]
2 years ago
6

A histidine is involved in an interaction with a glutamic acid that stabilizes the charged form of the histidine, such that the

value of ∆Go for deprotonation is 15 kJ•mol –1 at pH 7.0 and 293 K (calculated using the biochemical standard state). What is the pKa of this histidine
Chemistry
1 answer:
Greeley [361]2 years ago
8 0

Answer:

pKa of the histidine = 9.67

Explanation:

The relation between standard Gibbs energy and equilibrium constant is shown below as:

\Delta{G^0} =-RT \ln \frac{[His]}{[His+]}

R is Gas constant having value = 0.008314 kJ / K mol  

Given temperature, T = 293 K

Given, \Delta{G^0}=15\ kJ/mol

So,  Applying in the equation as:-

15\ kJ/mol=-0.008314\ kJ/Kmol\times 293\ K\times \ln \frac{[His]}{[His+]}

Thus,

15\ kJ/mol=-0.008314\ kJ/Kmol\times 293\ K\times \ln \frac{[His]}{[His+]}

\frac{[His]}{[His+]}=e^{\frac{15}{-0.008314\times 293}

\frac{[His]}{[His+]}=0.00211

Also, considering:-

pH=pKa+log\frac{[His]}{[His+]}

Given that:- pH = 7.0

So, 7.0=pKa+log0.00211

<u>pKa of the histidine = 9.67</u>

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