In: Chemistry
10.00mL 5% acidity vinegar was used titrate with NaOH whose molarity is 0.1030M.
Exp. # |
Concentration of NaOH |
Initial volume of NaOH |
Final volume of NaOH |
Volume of NaOH used for titration |
1 |
0.1030M |
5.50mL |
21.65mL |
16.15mL |
2 |
0.1030M |
3.60mL |
19.00mL |
15.40mL |
3 |
0.1030M |
19.00mL |
35.91mL |
16.91mL |
The vinegar was diluted to make 100.00mL final volume before trtration. If the molar mass of acetic acid is 60.05g/mole and density is 1.00 g/mL. Calculate the mass percent of acetic acid in the original vinegar solution.
Solution
Given data
10.00 ml 5% vinegar solution titrated with 0.1030 M NaOH
We have three trials in which volume of the NaOH needed for the titration was calculated. So lets first calculate the average of the NaOH solution needed for the titration.
Balanced reaction equation
NaOH + CH3COOH ---- > CH3COONa + H2O
Avg. NaOH used = (16.15 ml + 15.40 ml +16.91 ml )/3 = 16.16 ml NaOH
Now lets calculate the moles of NaOH reacted using its molarity and volume in liter
Moles = molarity * volume in liter
16.16 ml * 1 L / 1000 ml = 0.01616 L
Lets use this value in the above formula
Moles of NaOH = 0.1030 mol per L * 0.01616 L
= 0.001664 mol NaOH
Mole ratio of the acetic acid and NaOH is 1 : 1
Therefore moles of acetic acid reacted are same as moles of NaOH used
So moles of acetic acid reacted = 0.001664 mol
Now lets convert moles of the acetic acid to its mass
Formula to calculate the mass using the moles is as follows
Mass = moles * molar mass
Mass of acetic acid = 0.001664 mol * 60.05 g per mol
= 0.0999 g acetic acid
Now lets calculate the mass percent of the acetic acid in vinegar
Volume of vinegar used = 10.00 ml
And density of vinegar = 1.00 g/ml
So the mass of solution = 10.00 g
Now lets calculate the percent by mass of the acetic acid in vinegar
% mass = (mass of acetic acid / mass of vinegar )*100%
= (0.0999 g / 10.00 g)*100%
= 0.999 % of acetic acid in vinegar.
So the mass percent of the acetic acid in vinegar = 0.999 %