# Making a Standard Solution

September 17, 2017 September 1st, 2019 Free Essays Online for College Students

To make a standard solution of Sodium Carbonate and work out it’s molarity.

Key points about a standard solution

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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

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