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233/3: Chemistry Practical Question Paper

233/3: Chemistry Practical

Course:Secondary Level

Exam Year:2011

Katulani District Joint Examination 2011
Chemistry Paper 3
233/3
Instruction to candidates:
Answer all questions in the spaces provided.

1. You are provided with solution P and Q.
- Solution P is acidified Potassium Permanganate.
- Solution Q was prepared by dissolving 4.18g of solid Q in distilled water to make 250cm3 of solution.
You are required to determine the number of moles of Q that reacted with one mole of Potassium Permanganate.

PROCEDURE
- Place solution P in a burette. Pipette 25cm3 of solution Q into 250cm3 conical flask.
- Titrate solution Q with solution P until a permanent pink color just appears.
- Record your result in table 1 below. Repeat the above procedure two more times.
a) Table 1
I II III
Final burette reading
Initial burette reading
Volume of Solution P (cm3)
(4mks)
b) Calculate the average volume of solution P used. (1mk)

c) Given that the concentration of solution P is 0.02M, calculate the number of moles of Potassium Permanganate used. (2mks)

d) Calculate the concentration of solution Q in moles per liter. (Relative Molecular Mass of Q is 278. (2mks)

e) Calculate the number of moles of Q.
i) In 25.0 cm3 of solution. (2mks)
ii) Which reacts with one mole of Potassium permanganate? (2mks)

2. You are provided with;
• Aqueous hydrochloric acid - Solution A
• 0.1m Sodium hydroxide – Solution B
• Methyl Orange indicator
You are required to determine the morality of hydrochloric acid – Solution A.

Procedure
1. Using a measuring cylinder (100ml), measure 10 cm3 of A and fill the measuring cylinder with distilled water. Label the dilute acid as A1.
2. Fill the burette with solution A1.
3. Pipette 25cm3 of 0.1M sodium hydroxide – solution B into 250cm3 conical flask; add drops of Methyl orange indicator.
4. Titrate until the indicator just changes color from yellow to pink (red).
5. Record your results in table ii below. Repeat the above procedure two more times

Table II
I II III
Final burette reading
Initial burette reading
Volume of solution A1 used (cm3)

Calculate;
i) Average volume of solution A1 used. (1mk)
ii) Number of moles of sodium hydroxide present in 25cm3 of solution B. (2mks)
iii) Number of moles of solution A1 that reacted with 25cm 3 of solution B. (3mks)
iv) The concentration in moles per liter of solution A1. (2mks)
v) Molarity of solution A. (2mks)

3. a) You are provided with solid V. Carry out the test below. Write your observation and inferences in the space provided.
i) Dissolve solid V in about 20 cm3 of distilled water in a boiling tube. Into 3 separate test tubes, Put 2cm3 portions of the solution and use it for the tests (i) to (iv) below.
Observation Inferences

(1mk)

(1mk)

ii) To the first portion add 2 – 3 drops of lead (ii) Nitrate solution.

Observation Inferences

(1mk)

(1mk)

iii) To the second portion, add Barium Chloride solution (1cm3) followed by 2 cm3 of 2M HCl then shake the mixture.

Observation Inferences

(1mk)

(1mk)

iv) To the third portion, add drops of acidified Potassium permanganate solution P

Observation Inferences

(1mk)

(1mk)

b) You are provided with:
- Solution F containing Barium ions
- Solution G containing Sodium ions

Carry out the tests on solution F, G and V in order to identify the cat ions present in solution V.

Procedure

Clean one end of the glass rod thoroughly. Dip the clean end of the glass rod in solution F. Remove the end and heat it in a non-luminous flame. Note the color of the flame and record it in the table below. Repeat the procedure with solution G and V and complete the table below.

Solution Color of the flame
F

G

V
(3mks)

Identify the cat ion present in solution V. (1mk)

233/3: Chemistry Practical Question Paper

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