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General Chemistry 1: Week 11 – Titration
Preparation of KHP
Trial 1
Trial 2
Empty Container Mass
Mass of Container with KHP
Mass KHP
Moles KHP
Standardization of NaOH
Initial Buret Reading
Final Buret Reading
Total Volume NaOH
Moles NaOH
Molarity of NaOH
Mean NaOH Molarity
Percent Error
Standardization of Unknown Acid
Initial buret reading of NaOH (mL)
Final buret reading of NaOH(mL)
Total Volume of NaOH (mL)
Molarity of NaOH
Volume of Unknown Acid (mL)
Molarity of Unknown Acid
Avg Molarity
Percent Error
10.00
Trial 3
Titration
Lab time:
Click cell and select your lab time
North or
South
Click cell and select your side
Acid Name:
Do NOT enter units into
the cells
Data Collected (or given)
Calcuated values
Lab Times
T8
T11
T2
W11
W2
R8
N or S
North
South
Unknown Acid Con
Standardization of NaOH
KHP: Potassium hydrogen Phthalein (Clear acid/ Pink Basic)
Phenolphthalein
Sodium Hydroxide Solution Concentration Unknown
Acid Solution
KHP mass 0.6 to 0.7 grams
Add water & drops of Indicator
NaOH Solution (Basic)
Record Initial Buret Reading
Record Final Buret Reading (Pale Pink)
Equipment:
50 mL Buret
10 mL Pipet
Acid Solution (Concentration Unknown)
10.00 mL of HCl
Add water & drops of Indicator
NaOH Solution (Basic) 0.0937 M
Record Initial Buret Reading
Record Final Buret Reading (Pale Pink)
Determination of the Concentration of the NaOH Solution:
Part A
1. Balanced Equation for the reaction of KHP and NaOH:
NaOH (aq) + KHC8H4O4 (aq) →
Acid
Base
HOH (l) + KNaC8H4O4 (aq)
Water
Salt
2. The Grams of KHP
On the data table provided, we have provided the mass of the
An empty container and same container w/ KHP.
Use mass by difference to calculate the grams of KHP
3. Convert Grams to Moles
Use the following molar mass for KHP in this exercise
Molar mass of KHP 204.2g = 1 mole KHP
=
1
204.2
3 significant figures are required: 0.00356 (Yes)
0.003(No)
4. Moles of NaOH
You have completed the Titration and you stopped at the pale pink endpoint.
o What does this mean? The reaction is over. All the acid has been reacted.
Question: How many moles of NaOH where used in the reaction?
Moles of KHP = Moles of NaOH
Why?
#
1
= #
1
Therefore, if you calculated that you had 0.00325 moles of KHP then
you would have the same numbers of Moles of NaOH: 0.00325 .
5. Calculate the Volume of NaOH Delivered
a. We have provided you with the initial and final buret reading for each
trial. Use the Volume by difference calculation to determine the
volume delivered:
Final Buret Reading – Initial Burt Reading = Volume Delivered (mL)
6. To Calculate Concentration of NaOH (Molarity)
#
1000
=
( )
1
7. Calculate the Mean Value for your best three trials
8. Calculate the percent error for your best three trials
Proceed to Part B
100
Determination of Unknown Acid Concentration:
Part B
1. Balanced Equation for the reaction of HCL and NaOH:
HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq)
Acid
Base
Water
Salt
2. The moles of NaOH is calculated as follows
=
i.
The comes from the mean Molarity value
determined in the standardization of NaOH Part A.
ii.
To calculate the volume of NaOH Deliver use the technique:
Volume by difference:
Final Buret Reading – Initial Burt Reading Volume Delivered
iii.
At the pale pink end point the reaction is complete
1
=
1
Moles of HCl = Moles of NaOH
iv.
Calculate Concentration of HCL (Molarity = Moles/Liter)
?
1000
=
1
The volume of the acid was 10.00 mL
? 1000
=
10.00
1
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