In: Chemistry
DATA SHEET
Titration 1 | Titration 2 | Titration 3 | |
Mass of KHP, grams | .10 g | .10 g | .10 g |
Initial volume of NaOH, ml | 0.0 | 6.2 | 12.1 |
Final volume of NaOH, ml | 6.2 | 12.1 | 17.5 |
CALCULATIONS AND RESULTS
1. number of moles of KHP: n = mass KHP x (1 / 204 g/mol)
n 1 = ______________ n2 =_____________ n3 =___________________
2. number of moles of NaOH = number of moles of KHP
n 1 = __________________ n2 =___________________ n3 =______________________
3. Volume of NaOH used in each titration = final volume of NaOH - initial volume of NaOH
V 1 = _________________ V2 =___________________ V3 =_______________________
4. Molarity of NaOH solution = n/V
M 1 = _________________ M2 =___________________ M3 =______________________
2. Average molarity of NaOH:
M = (M1 + M2 + M3) / 3 = ________________________________________
1.
Number of moles of KHP
n1 = (0.1 g) / (204 g/mol) = 0.0005 mol
n2 = (0.1 g) / (204 g/mol) = 0.0005 mol
n3 = (0.1 g) / (204 g/mol) = 0.0005 mol
2.
Since, Number of moles of NaOH = number of moles of KHP
So,
n1 (NaOH)= n1 (KHP) = 0.0005 mol
n2 (NaOH)= n2 (KHP) = 0.0005 mol
n3 (NaOH)= n3 (KHP) = 0.0005 mol
3.
Volume of NaOH used in each titration = final volume of NaOH - initial volume of NaOH
V1 = 6.2 mL – 0.0 = 6.2 mL = 0.0062 L
V2 = 12.1 mL – 6.2 mL = 5.9 mL = 0.0059 L
V3 = 17.5 mL – 12.1 mL = 5.4 mL = 0.0054 L
4.
Molarity of NaOH solution = n/V
M1 = (0.0005 mol) / (0.0062 L) = 0.081 M
M2 = (0.0005 mol) / (0.0059 L) = 0.085 M
M3 = (0.0005 mol) / (0.0054 L) = 0.093 M
5.
Average molarity of NaOH:
M = (M1 + M2 + M3) / 3
=[ (0.081 M) + (0.085 M) + (0.093 M) ] / 3
= 0.259 M / 3
= 0.086 M