Question

Answer the procedure below.

You will start with a 50mM solution of your amino acid in 100mL of water. How many grams (and moles) of asparagine will you need?

Assuming a start at about pH of 6-7, how many equivalents of HClwill you need to add to ensure that the fully protonated form predominates (predict the pH youwill attain)? What volume of 1M HCl solution could you add to do this?

How many equivalents of NaOH will you add per titration point, what volume of 1M NaOH solution does this correspond to?

Answer 1

The molecular formula of asparagine is C₄H₈N₂O₃

SO the total wight is 12*4+8+14*2+16*3= 87g

to make 1M solution we nedd 87g

to male 50mM solution we need 87/1000g in 100ml of water

to make 50mM solution we need 87*10/1000g in 100ml of water

so weight of asparagine in 50mM 100ml slotion is 0.87g

The isoelectric point of aspargine of 5.41, so any acid with pH less than 5.41 will protonate the aspargine

The pH of 1M HCL would be zero. so addicng the 1M HCL would make the asparagine protonated.

No question is how much HCL is needed

Use this formula

M1*V1 ( molarity and volume of aspargine) = M2*V2 ( molarity and volume of HCL)

50*10^_-3 * 100 = 1*V2

V2 = 5ml

We nee 5ml of NAOH to neutralize the HCL