I just need Help with part B please. Our Professor said we need to solve it usin

Question

I just need Help with part B please. Our Professor said we need to solve it using the Henderson-Hasselbalch equation. I solved it without the HH equation and got it wrong. He said it will be on our final so I have to figure it out Thank you a head of time.

pH = pKa + log ( [A-] / [HA] )

Histidine pKa = 1.6

Consider the neutral form of the amino acid histidine, abbreviated HA. When the neutral form of histidine (HA) is titrated with HCIO4, write the sequence of reactions that occur. Draw structures of reactants and products. Given a pH of 3.00, how many mL of 0.050 0 M HCIO4 should be added to 25.0 mL of 0.0400 M HA? (hint: H3A2+ doubleheadarrow H2A+ doubleheadarrow HA doubleheadarrow A-)

Explanation / Answer

when we add HClO4, HA gives out salt as the product.

so [A-]=[HClO4]

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