To make a standard solution of Sodium Carbonate and work out it’s molarity.
Key points about a standard solution
The characteristics of a standard solution are
* Must be obtainable in a highly pure state
* Must be stable to heat and light, both as a solid and in solution.
* Should have a high molar mass
* High solubility in H2O
Equipment/Safety
* Volumetric flask
* Sodium Carbonate powder.
* Spatula
* Deionised water.
* Safety goggles
* Lab coat
* Analytical balance
* Weighing bottle
* Volumetric flaks stopper.
* Small funnel (Burette funnel)
Method of how to make my standard solution of Na2CO3
1. Weigh out approximately between 2.5g and 2.7g of anhydrous Sodium Carbonate powder.
2. Add approximately 50cm3 of deionised water.
3. Stir the water using a glass rod, until the sodium carbonate has dissolved.
4. Transfer the solution to a 250cm3 volumetric flask, using a small funnel.
5. Make up the volume to the 250 mark; add the last drops using a pipette.
6. Replace the stopper and shake the volumetric flask vigour sly.
7. Now calculate the Morality of your solution
Calculations
I am now going to work out the molarity of Na2CO3.
Na2CO3
(23 X 2)+12(16 X 3)
46 +12+48
106
Moles= Mass/R.M.M
0.0241= 2.5555/106
Concentration =Moles /Volume
0.0964M= 0.0241/ 0.25
Conclusion
My aim was to make a standard solution and to work out its molarity
As you can see above I have worked out the molarity.the moarity of my sodium carbonate solution is 0.0964M.
Titration using Na2CO3 and HCl
Aim
The aim of this experiment is to find the end point of Sodium Carbonate and Hydrochloric acid
Equipment/Safety equipment/Chemicals
* HCl
* Sodium Carbonate
* Clamp stand
* Boss
* Small funnel
* Burette
* Pipette
* Two beakers
* White tile
* Methyl Orange
* Conical flask
* Deionised water
Method
1. Pour some sodium carbonate solution into a small beaker.
2. Using pipette filler pipette 10 cm3 of the Sodium Carbonate solution into a conical flask and add three drops of methyl orange.
3. Prepare your burette by rinsing once with distilled water and then with a little of the hydrochloric acid.
4. Fill your burette with HCl and read it to 2 decimal places
5. Titrate the alkali in the flask with the acid until the end point is reached. This is when the colour changes from yellow o orange.
6. Record the initial and final burette readings so you can determine the titre for each titration.
Results
Titration
Initial Reading cm
Final Reading
Titre cm
Rough
1.0
18.10
17.1
1
1.0
17.80
16.8
2
1.0
17.60
16.6
3
1.0
17.70
16.7
4
1.0
17.70
16.6
Average
16.66
Calculations
Number of moles in sodium carbonate
Moles=Volume X Concentration
0.000964 = 0.01 X 0.0964
Number of moles in HCl
2 X 0.00096= 0.001928
Concentration of HCl
Concentration= Mole/Volume
0.116M =0.001928/0.0166
A.S. Level Chemistry
