Q1 = 11MKS
Q2 = 14MKS
Q1. You are provided with:
Solution A: Potassium Chromate VI
Solution B: 0.1mNa2SO3
You are required to determine the number of moles dichromate VI ions (Cr2O2-7) in one litre of solution.
PROCEDURE
Fill the burette with solution B. Pipette 25cm3 of solution A and transfer it into conical flask. Titrate until a permanent green colour is obtained. Record your results in table below and repeat the procedure to fill the table.
I | II | III | |
Find burette readings | |||
Initial burette readings | |||
Volume of solution B (cm3) |
- Determine the average volume of solution B. (5mks)
- Calculate the number of moles of solution B. (2mks)
- Given that the ionic equation for the reaction between dichromate ion and sulphate is;
Cr2O2-7(aq) + 3SO2-3(aq) + 8H+(aq) → 2Cr3+(aq) + SO2-4(aq) + 4H2O(l)
Calculate;- Number of moles of dichromate IV ion in 25cm3 (2mks)
- Moles of dichromate ion one litre of solution.
Q2. You are provided with substance E, carry out the tests below and write your observations and inferences in the space provided.
- Describe the appearance of substance E.
Observation inferences - Place one third of substance E in the test tube. Heat it strongly.
Observation inferences - Place remaining amount of E in boiling tube. Add about 10cm3 of distilled water and shake well. Retain the mixture for tests in d) below.
Observation inferences - Use about 2cm3 potion of the mixture obtained in (c) for tests (i) to (iv)
- Add 2 to 3 drops of lead (ii) Nitrate to the mixture.
Observation inferences - Add 2 to 3 drops of barium Nitrate to second portion of the mixture.
Observation inferences - Add five drops of dilute nitric (v) acid to the mixture in (ii) above
Observation inferences - To the last portion, add few then excess drops of sodium hydroxide.
Observation inferences
- Add 2 to 3 drops of lead (ii) Nitrate to the mixture.
- Give the formula of cat ion and anion present in substance E.
Cat ion
Anion
CONFIDENTIAL
In addition of apparatus formed in lab, each student is expected to have;
- 100cm3 of solution A
- 100cm3 of solution B
- 0.5g of solid E
- Burette
- Pipette
- 2 conical flask
- test tubes in rack
- boiling tube holder
- Test tube holder
- Distilled water in wash bottle.
Access
- 0.5 mBa (NO3)2 solution and dropper.
- 2M NaOH solution and dropper.
- Source of heat.
- 0.1MPb (NO3)2 solution and dropper.
- 2MHNO3 solution and dropper.
- Solution A is acidified 0.01MK2CrO7.
- Solution B is 0.1MNa2SO3.
- Solution E is about 0.5g of MgSO4.H2O.
NOTE:
Solution A is prepared by dissolving 2.94g of K2CrO7 in 200cm3 of 2M H2SO4 then adding distilled water to 1l of solution.
MARKING SCHEME
Q1 = 11MKS
Q2 = 14MKS
Q1. You are provided with:
Solution A: Potassium Chromate Vi
Solution B : 0.1mNa2SO3
You are required to determine the number of moles dichromate VI ions (Cr2O2-7) in one litre of solution.
PROCEDURE
Fill the burette with solution B. Pipette 25cm3 of solution A and transfer it into conical flask. Titrate until a permanent green colour is obtained. Record your results in table below and repeat the procedure to fill the table.
I | II | III | |
Find burette readings | 8.0 | 15.5 | 23.0 |
Initial burette readings | 0.0 | 8.0 | 15.5 |
Volume of solution B (cm3) | 8.0 | 7.5 | 7.5 |
- Determine the average volume of solution B. (5mks)
7.5 + 7.5 = 7.5cm3
2
CT√
D√
PA√
A± 0.1√
±0.2√
FA√ - Calculate the number of moles of solution B. (2mks)
1.0 x 7.5
1000
= 0.00075moles - Given that the ionic equation for the reaction between dichromate ion and sulphate is;
Cr2O2-7(aq) + 3SO2-3(aq) + 8H+(aq) → 2Cr3+(aq) + SO2-4(aq) + 4H2O(l)
Calculate;- Number of moles of dichromate IV ion in 25cm3 (2mks)
0.00075
3
= 0.00025 moles - Moles of dichromate ion one litre of solution.
0.00025 x 1000
25
= 0.01moles/litre
- Number of moles of dichromate IV ion in 25cm3 (2mks)
Q2. You are provided with substance E, carry out the tests below and write your observations and inferences in the space provided.
- Describe the appearance of substance E.
- White crystalline solid// colourless crystalline solid.
- Place one third of substance E in the test tube. Heat it strongly.
Observation inferences Colourless vapor on condenses on cover plots Hydrate salt// contains water of crystallization - Place remaining amount of E in boiling tube. Add about 10cm3 of distilled water and shake well. Retain the mixture for tests in d) below.
Observation inferences Solid dissolved forming colorless Solution soluble salt
Absence of Fe2+, Fe3+,Cu2+ - Use about 2cm3 potion of the mixture obtained in (c) for tests (i) to (iv)
- Add 2 to 3 drops of lead (ii) Nitrate to the mixture.
Observation inferences White precipitate SO42-
SO32- Present All=1√
CO32- 3=√
Cl- 2 or 1 = 0 - Add 2 to 3 drops of barium Nitrate to second portion of the mixture.
Observation inferences White precipitate SO42-
SO32- All=1√
CO32- 2=√
1 = 0 - Add five drops of dilute nitric (v) acid to the mixture in (ii) above
Observation inferences White precipitate present SO42- confirmed - To the last portion, add few then excess drops of sodium hydroxide.
Observation inferences Observation inferences
White precipitate present
Insoluble in excess√Mg2+ √ present
- Add 2 to 3 drops of lead (ii) Nitrate to the mixture.
- Give the formula of cation and anion present in substance E.
Cat ion - Mg2+
Anion - SO42
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