1. You are provided with:
Determine the number of moles of sodium hydroxide that react with one mole of acid C.
PROCEDURE I
Fill the burette with solution A. Using a pipette and pipette filler, place 25.0cm of solution B into 250 ml
conical flask.
Titrate solution B with solution A using phenolphthalein indicator and record your results in Table 1. Repeat the titration and complete Table 1.
a. Table 1
|
I |
II |
III |
Final burette reading |
|
|
|
nitial burette reading |
|
|
|
Volume of solution A used, cm³ |
|
|
|
(3 marks)
b. Calculate the:
i. average volume of solution A used. (1 mark)
ii. number of moles of solution A in the average volume used. (1 mark)
iii. number of moles of sodium hydroxide (N) in 25.0cm of solution B. (1 mark)
iv. concentration of sodium hydroxide in moles per litre. (1 mark)
PROCEDURE II
Clean the burette and fill it with solution C. Using a pipette and pipette filler, place 25.0cm
of solution B into a 250 ml conical flask.
Titrate solution B with solution C using phenolphthalein indicator and record your results in Table 2. Repeat the titration and complete Table 2.
c. Table 2
|
I |
II |
III |
Final burette reading |
|
|
|
nitial burette reading |
|
|
|
Volume of solution A used, cm³ |
|
|
|
(3 marks)
d. Calculate the:
i. average volume of solution Cused. (1 mark)
ii. concentration in moles per litre, of solution C, given that the relative formula mass of acid C is 210.0. (1 mark)
iii. number of moles of acid C in the average volume used. (1 mark)
e.i. Write the ratio of moles of acid C to moles of sodium hydroxide (N) in the 25.0cm of solution B. (1 mark)
ii. Determine the number of moles of sodium hydroxide that react with one mole of acid C. (1
mark)
2. You are provided with solid D.
You are required to determine the freezing point of solid D.
PROCEDURE
i. Fill a 250 ml beaker with about 200 cm³of tap water and heat the water until it boils.
ii. Place all solid D provided in a dry test tube and insert a thermometer into the solid.
iii. Place the test tube in the boiling water and allow the solid to heat until it all melts.
iv. When the temperature of the melted solid is approximately 90°C, remove the test tube,
wipe the sides with tissue paper and then place the test tube into an empty 250 ml beaker
v. Start the stop watch or clock when the temperature of the melted solid is 85.0°C.
vi. As the solid cools, measure and record its temperature every 30 seconds and complete
Table 3.
a. Table 3
Time S |
0 |
30 |
60 |
90 |
120 |
150 |
180 |
210 |
240 |
270 |
300 |
Temperature°C |
|
|
|
|
|
|
|
|
|
|
|
(4 marks)
b. On the grid provided, plot a graph of temperature (vertical axis) against time. (3
marks)
c. Using the graph in (b), determine the freezing point of solid D. (1 mark)
3. You are provided with solid E. Carry out the following tests and record your observations and inferences in the spaces provided.
a. Place all the solid E in a boiling tube.
Add about 10 cm of dilute nitric(V) acid, warm the mixture and then allow to stand until all the solid dissolves. Add about 10 cm of distilled water to the solution and shake. Retain the solution for tests (b) and (c)
Observations |
Inferences |
(1 marks) |
(1 mark) |
b. Use about 2 cm³ portions of the solution obtained in 3(a) for each of the following tests.
i. To the first portion add 2 or 3 drops of aqueous barium nitrate,
Observations |
Inferences |
(1 marks) |
(1 mark) |
ii. To the second portion add 2 or 3 drops of aqueous lead(II) nitrate.
Observations |
Inferences |
(1 marks) |
(1 mark) |
iii. To the third portion add aqueous sodium hydroxide dropwise until in excess.
Observations |
Inferences |
(1 marks) |
(1 mark) |
iv. Place about 3 cm of aqueous ammonia in a test tube. To the fourth portion, add all
the aqueous ammonia from the test tube dropwise.
Observations |
Inferences |
(1 marks) |
(1 mark) |
c. To the remaining solution of solid in the boiling tube, add all the solid providedn
Shake the mixture for about 2 minutes. Filter the mixture into a boiling tube. Retain the
filtrate for tests (i) and (ii) below.
Observations |
Inferences |
(1 marks) |
(1 mark) |
i. To about 2 cm portion of the filtrate, add aqueous ammonia dropwise until in
excess
Observations |
Inferences |
(1 marks) |
(1 mark) |
ii. To about 2 cm portion of the filtrate add 2 or 3 drops of dilute hydrogen peroxide
solution.
Observations |
Inferences |
(1 marks) |
(1 mark) |
Practical Answers
2021 K.C.S.E Chemistry paper 3
1.a
|
|
24.0 |
|
CT 1 |
|
I |
II |
III |
D1 |
Final burette reading |
|
|
|
A1 |
Initial burette reading |
|
|
|
PA1 |
Volume of solution A used, cm3 |
|
|
|
FA1 |
b. i. Correct working
correct ans (b)(i)
ii. =correct ans (b)(i) x 0.1 (over) 1000 = correct ans (b)(ii)
iii. Ratio A:N b1:1
ans (b) (iii)
iv. =1000 x ans (b)(iii) (over) 25 = ans (b)(iv)
PROCEDURE II
|
|
16.5 |
|
CT1 |
|
I |
II |
III |
D1 |
Final burette reading |
|
|
|
A1 |
Initial burette reading |
|
|
|
PA1 |
Volume of solution |
|
|
|
FA1 |
A used, cm3 |
|
|
|
|
d. i. Correct working
correct ans (d)(i)
ii. =10/210 = 0.0476
iii. =correct ans (d)(i) x 0.0476 (Over) = correct ans (d)(iii)
e. i. ans (d)(iii) : ans(b)(iii)
ii. =ans(b)(iii)/ ans(d)(iii) = ans (e)(ii)
2.Table 3.a
Time, s |
0 |
30 |
60 |
90 |
120 |
150 |
180 |
210 |
240 |
270 |
300 |
Tempe rature, °C |
85.0 |
82.0 |
80.5 |
78.0 |
75.0 |
72.0 |
69.0 |
69.0 |
69.0
|
67.5 |
65.5 |
b.
c. showing
correct reading
3 a.
Observations |
Inferences |
No effervescence |
CO32-/ SO3 2- absent |
No effervescence |
Cu2+ present (1 mark) |
b i
Observations |
Inferences |
No white ppt formed |
SO²4- absent |
ii
Observations |
Inferences |
No yellow ppt formed No white ppt formed |
absent CI-/Br- absent |
iii
Observations |
Inferences |
Blue ppt formed insoluble in excess |
Cu2+ present |
iv
Observations |
Inferences |
Blue ppt formed that dissolves in excess to form a deep blue solution |
Cu2+present |
C.
Observations |
Inferences |
Blue solution changes to green Brown residue Green filtrate Boiling tube becomes warm |
Cu2+ displaced by G/G is more reactive than Cu/G is oxidized by Cu2+ /Cu2+ are reduced b\ G/ Cu2+ are displaced by Fe |
(i)
Observations |
Inferences |
Green ppt formed insoluble in excess |
Fe2+ |
(ii)
Observations |
Inferences |
Green solution changes to brown/Yellow Effervescence |
Fe2+ oxidized to Fe3+ Fe3+ formed |
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