Consider the titration of 50.0 mL of 0.183-M of KX with 0.090-M HCl. The pKa of...

Question

Question

Consider the titration of 50.0 mL of 0.183-M of KX with 0.090-M HCl. The pKa of HX = 8.13. Give all pH values to 0.01 pH units.

a) What is the pH of the original solution before addition of any acid? pH = 10.70

b) How many mL of acid are required to reach the equivalence point? VA = 101.67 mL

c) What is the pH at the equivalence point? pH = 4.67

d) What is the pH of the solution after the addition of 45.8 mL of acid? pH = 8.22

e) What is the pH of the solution after the addition of 122.0 mL of acid? pH = ???

Answer 1

Answer #1

ku tHX Run kx +Hel n = 1 mote ng=lmol pka HX - 813 ; Ka 4 #x= 10813-7.413 8109 kx is salt of weak and HX and strong base KOH

Answer 2

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