Question
Asked Nov 21, 2019
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Calculate the pH in the titration of 50.00 mL of 0.060 M acetic acid (CH3COOH) with a 0.120M sodium hydroxide, NaOH solution after the addition of the following volumes of base:

Ka for acetic acid= 1.8 x 10^-5

A) 0mL

B) 10 mL

C) 12.5 mL

D)25.0 mL

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Expert Answer

Step 1

(A)pH when 0mL of NaOH solution is added:

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Given, concentration of NaOH=0.120 M concentration of CH,COOH 0.060 M Volume of Na OH added=OmL =1.8x10x0.060 1.039x103 pH-log H -log (1.039x10 2.98

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Step 2

(B)pH when 10mL of NaOH solution is added:

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Given, concentration of NaOH=0.120M concentration of CH,COOH 0.060 M Volume of NaOH added=10mL pK-log (1.8x10)4.74 _0.120x10 salt =0.02M 60 0.060x40 [Acid -=0.04M 60 salt pH-pK+log [Acid] 0.02M 4.74+log 0.04M -4.74+(-0.301) =4.44

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Step 3

(C) pH when 12.5mL of NaOH...

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Given, concentration of NaOH 0.120M concentration of CH,COOH 0.060 M Volume of NaOH added=12.5 mL 0.120 12.5 salt =0.024M 62.5 [Acidl 0.060X37. -0.0357M 62.5 salt] pH-pKlog [Acid] 0.024M =4.74+log '0.0357 M 4.74+(-0.172) =4.57

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