If you could help me that would be great thank you!! For the titration of 30.0 m

Question

If you could help me that would be great thank you!!

For the titration of 30.0 mL of 0.200 M NH3 with .500 M HCI at 25degreeC, determine the relative pH at each of these points. before the addition of any HCI after 12.0 mL of HCI has been added after 27.0 mL of HCI has been added Classify each titration curve as representing a strong acid titrated with a strong base, a strong base titrated with a strong acid, a weak acid titrated with a strong base, a weak base titrated with a strong acid, or a polyprotic acid titrated with a strong base.

Explanation / Answer

a ) Before addition of HCl ,only NH3 is present .As NH3 is a base pH>7

pH> 7

b) NH3 + Hcl ---> NH4Cl

moles of NH3 = 30 x 0.2 /1000 = 6 x 10-3 M

moles of HCl = 12 x 0.5 /100 = 6 x 10-3 M

So they are completely reacted .

Only NH4Cl is present . it is a acidic salt

So pH < 7

c) moles of Hcl = 27 x 0.5 /1000 = 13.5 x 10-3

so HCl will be remained . Hcl is a acid

So pH < 7

2) strong acid / strong base ---> 1

stron base /strong acid ---> 5

  

weak acid /Strong base ----> 2

weak base /stron acid ---- > 3

polyprtoic acid /stromg base ---- 4

  

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