1. Molarity of Acetic acid(M1) of each trial is given below
Molarity Of NaOH (M2)= 0.252M
Volume of NaOH in each Trial is= V2
Volume of Acetic Acid in each Trial is= V1
Now use M1V1 =M2V2 , So M1=M2V2/V1
For trial I
Molarity of Acetic acid(M1) = 0.252M*27.67mL/42.35mL = 0.165M
For trial II
Molarity of Acetic acid(M1) = 0.252M*32.51mL/30.00mL = 0.273M
For trial III
Molarity of Acetic acid(M1) = 0.252M*40.45mL/30.00mL = 0.340M
AverageMolarity of Acetic acid = (0.165M+0.273M+0.340M)/3 = 0.256M
AverageMolarity of Acetic acid = 0.256M
2.Percentage of Acetic acid
Density = 1.01g/mL
Average Molarity of Acetic acid = 0.256M
We know that for saturated Acetic acid 99.5% molarity is 17.4M , which having 1.01g/mL density
Note: You also take this data from any standard reference book.
So % acetic acid is = 0.256M*100/17.4M = 1.47%
3. Actual molarity of acetic acid is not given
When you obtain ,
Then use this formula to calculated % error of acetic acid molarity
% error of acetic acid molarity =(Actual molarity - Experimental molarity)*100/Actual molarity
4. If calculation is not in 5 % error of acetic acid molarity
Then your NaOH solution Molarity may not correct due to preparation of this is long time that may react with CO2 in the atmosphere
which act as acid and react lit bit to NaOH to give carbonic acid. So change the concentration of NaOH , So prepare fresh solution of NaOH
POST LAB QUESTIONS
1.
Molarity of HBr (M1) =?
Molarity Of NaOH (M2)= 0.150M
Volume of NaOH(V2) is = 18.8mL
Volume of HBr(V1) = 25.00mL
Now use M1V1 =M2V2 , So M1=M2V2/V1
Molarity of HBr (M1) = 0.150M*18.8mL/25.00mL = 0.1128M
So, Molarity of HBr (M1) = 0.1128M
2.
Molarity of H2SO4 (M1) =?
Molarity Of NaOH (M2)= 0.100M
Volume of NaOH(V2) is = 45.65mL
Volume of H2SO4(V1) = 20.00mL
Now use M1V1 =M2V2 , So M1=M2V2/V1
Molarity of HBr (M1) = 0.100M*45.65mL/20.00mL = 0.22825M
So, Molarity of H2SO4 (M1) = 0.22825M
U Experiment 17B: Acid-Base Titration Report Data Table Trial 1 Trial 2 T Trial 3 Volume...
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