Question: standardisation of hydrochloric acid with a standard solution of sodium...
Question details
Standardisation of hydrochloric acid with a standard solution of sodium carbonate
Titration Data Set C
Calculating the concentration of Na2CO3
Weight weighing bottle + Na2CO3 = 2.8510 g
Weight weighing bottle  Na2CO3 = 1.5250 g
Volume of volumetric flask for Na2CO3 solution = 250 mL
Calculating the concentration of HCl
Titration data:
Burette readings (mL) 
Rough Titration (do not use) 
Accurate Titrations Place an asterisk (*) next to your concordant results 

Final 
21.40 
40.70 
22.55 
41.85 
25.80 
45.15 
Initial 
2.00 
21.40 
3.20 
22.55 
6.50 
25.70 
Titre 
19.40 
19.30 
19.35 
19.30 
19.30 
19.45 
Calculating the uncertainties
Absolute uncertainties:
Balance = ± 0.0002 g
Volumetric flask = ± 0.50 mL
Pipette = ± 0.05 mL
Burette = ± 0.05 mL
Procedural questions
1. Outline the steps involved for weighing by difference. Why is this important?
2. Why should all solid be dissolved before transfer of the solution from the 250 mL beaker to the volumetric flask?
3. Why is it necessary to thoroughly mix the solution after it has been made up to the mark?
Results: Standardisation of hydrochloric acid with sodium carbonate
Complete the following calculations using your provided sample data.
Part 1: Preparation of an approximately 0.05 mol/L standard solution of sodium carbonate
Weighings (g) 

Weight weighing bottle + Na_{2}CO_{3} 

Weight weighing bottle  Na_{2}CO_{3} 

Difference = Weight Na_{2}CO_{3} 

Calculate the specific concentration of sodium carbonate solution.
Concentration of standard sodium carbonate solution
mol L^{1} 
Part 2: Titration of hydrochloric acid against sodium carbonate
Titrations
Burette Readings (mL) 
Rough Titration 
Accurate Titrations Place an asterisk (*) next to your concordant results 

Final 






Initial 






Titre 






Mean titre volume of your concordant results 
mL 
Mean titre volume of concordant results:______________mL
1. Complete the boxes below with the names of chemical species present in each solution, and the quantities and units you know. For the unknown value put in a question mark.
Determining the concentration of hydrochloric acid
1. Write the balanced chemical equation for the titration reaction.
2. For which component in the titration are all values known? This is our known solution.
3. For which component in the titration are some values missing? This is our unknown solution.
4. For the known solution, what volume has been used and what is its concentration?
5. Determine the number of moles of the known compound.
6. At the endpoint, what is the molar ratio between HCl and Na_{2}CO_{3}?
7. At the endpoint, how many moles of the unknown solution are present?
8. What was the volume of the unknown solution that you used?
9. Using your answers to Questions 7 and 8, what is the concentration of the unknown solution?
Uncertainty calculation
Hint! If you are having trouble with uncertainty calculations, refer to the Snapshot video on Blackboard or to the information provided on Page 13 (Principles of Measurement) of your laboratory manual.
Apparatus Used 
Value 
Absolute Uncertainty 
Relative (%) Uncertainty 
Balance for standard solution (g) 



Volumetric flask for standard solution (mL) 



Bulb pipette for titration (mL) 



Burette for titration (mL) 



Total % uncertainty 

Remember that the final absolute uncertainty is determined by the equation:
Concentration of hydrochloric acid (with associated uncertainty)
± mol L^{1} 
WITH SOLUTION AND EXPLANATION
DONT PLAGIARIZE...