Three Part Question: Part B= A 50.0 mL volume of .15 M HBr is titrated with .25

ID: 784068 • Letter: T

Question

Three Part Question:

Part B=

A 50.0 mL volume of .15 M HBr is titrated with .25 M KOH. Calculate the pH after the addition of 17.0 mL of KOH.

Express your answer numerically

Part C=

A 75.0 mL volume of .200 M NH3 (Kb=1.8x10^-5) is titrated with .500 M HNO3. Calculate the pH after the addition of 19.0 mL of HNO3.

Express your answer numerically

Part D=

A 52.0 mL volume of .35 M CH3COOH (Ka=1.8x10^-5) is titrated with .40 M NaOH. Calculate the pH after the addition of 29.0 mL NaOH.

Express your answer numerically

on addition of 17 ml of KOH

we have x*0.15=17*.25

x=28.33 ml

so HBr remained= 50-28.33= 65/3 ml

so mole of H+= 65.3*0.15*10^-3 mol

= 13/4 milli mol

so concentration = 13/4*67

=0.04850

so pH= -log[H+]

= -log0.04850

=1.314

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