Q7 A 40.00ml sample of .10M weak acid with ka of 1.8x10-5 is titrated with a 0.10 M strong base. What is the pH after 20.00mL of base has been added?
9.26
7.00
1.8x10-5
4.74
let week acid is CH3COOH
let strong base is NaOH
no of moles of acid CH3COOH = molarity * volume in L
= 0.1*0.04 = 0.004 moles
no of moles of strong base NaOH = molarity * volume in L
= 0.1*0.02 = 0.002moles
CH3COOH + NaOH --------------> CH3COONa + H2O
I 0.004 0.002 0
C -0.002 -0.002 0.002
E 0.002 0 0.002
Pka = -logKa
= -log1.8^10^-5
= 4.74
PH = Pka + log[CH3COONa]/[CH3COOH]
= 4.754 + log0.002/0.002
= 4.74 + log1
= 4.74 + 0
= 4.74 >>>>answer
Q7 A 40.00ml sample of .10M weak acid with ka of 1.8x10-5 is titrated with a...
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