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Please explain! I know the answers already but I do not understand how to find them.H3 ОН (10) O(2) Question 2 (24 pts) This small protein has just the 6 ionizable side chains together with N and C termini (pK

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Answer #1

a) The approximte pH of the solution would be near 3 .

This can be predicted as pH=pK when half of the ion is ionised since a -COOH group is ionised completely it shows that pH is certainly above 2 and below 4 because other -COOH group having a pK of 4 is unionised showing that pH is in between 2 and 4 i.e. 3.

it can also be shown by Henderson-Hasselbach equation

pH = pK + log ([salt]/[acid])

(i) when acid is dissociated , conc.of salt is higher than acid and pH> pK

(ii) when acid is undissociated , conc. of salt is lower then acid and pH<pK

b) To calculate Isoelectric point just follow two steps

Step 1- Estimate the pH at which protein is neutral

Step 2- Find the average of the two pK values which are just above and below the pH at which protein is neutral

For this question if pH= 6 , then the protein will be neutral because all the three -COOH group will be ionised and will have negative charge and all three amino group will have positive charge thereby protein is neutral.

pK just below 6 = 5 of -COOH group

pK just above 6= 7 of -SH group

The average of 5 and 7 is 6, so 6 is the isoelectric point of the protein.

c) (i) For pH=4

Since pH of original solution is 3 to increase pH upto 4 , 1 mole of KOH is added

(ii) For pH = 6

3 moles of KOH is added to make the pH of the solution 6

(iii) For pH= 10

7 moles of KOH is added to make pH of the solution 10

d) The side chain having a lower pK value of 2 can be Aspartate it has a much lower pK value than other because it does not have more electron donating groups . The presence of electron donating group decreases the acidity and increases the pK . As electron donating group is not present it is more acidic and has a lower pK value

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