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Waec Chemistry Practical Answers 2021 for 21st September 2021
Tuesday, 21st September 2021
- Chemistry 3 (Practical) (Alternative B) 9:30am. –11:30 am.(1stSet)
- Chemistry 3 (Practical) (Alternative B) 12:00noon.–2:00pm.(2ndSet)
EXAM TYPE: Waec 2021
SUBJECT: Chemistry Practical
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WAEC CHEMISTRY PRACTICAL SPECIMENS 2021 AND INSTRUCTIONS TO SCHOOLS
(a) One burette of 50cm³ capacity
(b) One pipette either 20cm³ or 25cm³
All candidates at one center must use a pipette of the same volume. These should be clean and free from grease.
(c) The usual apparatus for titration.
(d) The usual apparatus for reagent for qualitative work including the following with all reagents appropriately labeled.
(i) Dilute sodium hydroxide solution
(ii) Dilute hydrochloric acid
(iii) Dilute trioxonitrate(V) acid
(iv) Barium chloride solution
(v) Acidified potassium dichromate solution
(vi) Aqueous ammonia
(vii) Lime water
(viii) Red and blue litmus papers
(ix) Dilute tetraoxosulphate (VI) acid.
(f) Filtration apparatus
(g) One Beaker
(h) One boiling tube
(i) Four test tubes
(j) Methyl orange as indicator
(k) Glass rod
(l) Wash bottle containing distilled/ diagnosed water
(m) Burning splint
(n) Watch glass
(o) Bunsen burner/ source heat
(q) Mathematical table/Calculator
(3) Each candidate should be supplied the following where n is the candidate’s serial number.
(a) 150cm³ of a solution HCL, in a corked flask or bottle labeled ‘An’. These should be all the same containing 9.0cm³ of concentrated HCL (about 36%) per dm³ of solution.
(b) 150cm³ of NaOH solution in a corked flask or bottle labeled ‘Bn’. These should all be the same containing 4.8g of NaOH per dm³ of solution.
(c) One spatulaful of a uniform mixture of CuSO4 and (NH4)2CO3 in a specimen bottle and corked immediately and labeled ‘Cn’. The components of the mixture should be in ratio 1:1 by mass.
(4) In all cases, more material may be issued if required.
(5) The actual concentration of ‘An’ and ‘Bn’ must be stated in the Supervisor Report Form. The candidate will assume that the concentrations are exactly as stated in the question paper.
(6) It should be noted that schools are not allowed to amend the information provided on the question paper or substitute any substance/solution for those specified in these instructions.
6. An aqueous solution has a pH of 4.0.
(a) (i) What is the hydrogen ion concentration of the solution?
(ii) What effect will it have on litmus paper?
(iii) Which of the following salt solutions would have the same effect on litmus? Give a reason for your answer. NH4Cl(aq); NaCl(aq) ; CH3OON(aq).
(b) (i) Differentiate between a fine chemical and a heavy chemical.
(ii) Name two sources of air pollution.
(iii) Suggest one way of reducing air pollution in cities
8. A substance which ionizes completely into hydroxonium ions is a
A. Strong acid.
B. Strong base.
C. Weak acid.
D. Weak base.
9. Which of the following solutions is able to resist changes in pH when small amounts of an acid or a base is added?
A. Buffer solution
B. Neutral solution
C. Saturated solution
D. Supersaturated solution
10. Protein is a polymer formed from the linkage of
A. Amino acid molecules.
B. Fatty acid molecules.
C. Glucose units.
11. The bond formed betweenand to form the hydroxonium is
12. The minimum amount of energy required for effective collisions between reacting particles is known as
A) Activation energy
B) Bond energy
C) Kinetic energy
D) Potential energy
13. An elementforms the following oxides and This phenomenon illustrates the law of ________
A) Conservation of mass
B) Definite proportion
C) Mass action
D) Multiple proportions
14. How many moles of oxygen would contain
NB: Avogadro’s constant (NA)
15. Which of the following statements about solids is correct?
A) Solid particles are less orderly than those of a liquid
B) Solid have lower densities than liquids
C) Solid particles have greater kinetic energies than those of liquids
D) Solid particles cannot be easily compressed
16. Which of the following apparatus can be used to measure a specific volume of a liquid accurately?
B) Conical flask
C) Measuring cylinder
17. The general gas equationis a combination of
A) Boyle’s and Charles’ laws
B) Boyle’s and Graham’s laws
C) Charles’ and Graham’s laws
D) Dalton’s and Graham’s laws
18. The spreading of the scent of a flower in a garden is an example of ______
A) Brownian motion
D) Tyndal effect
19. Propane and carbon (IV) oxide diffuse at the same rate because [H = 1.00, C = 12.0, O = 16.0]
A) They are both gases
B) Their molecules contain carbon
C) They have the same relative molecular mass
D) Both are denser than air
20. The energy which accompanies the addition of an electron to an isolated gaseous atom is
C) Electron affinity
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(ii)Hydrogen chloride gas(HCl)
To show that hydrogen chloride is extremely soluble in water.
Fill a round-bottomed fask with dry hydrogen chloride through a tube A and air through another tube B. Add a few drops of water through B and close the tubes. Invert the flask into a trough of water containing blue litmus solution. The water turns red.
(i)Pollution of water bodies by chemical waste
(ii)Pollution of the air
(iii)Radioactive particles are released
(i)Coal gas=> important gaseous fuel
(ii)Coke => used as a reducing agent
(ii)Addition of caustic soda.
(i)Hard water contains dissolved minerals and therefore tastes better.
(ii)The calcium salts in hard water help animals to build strong teeth and bones.
CLICK HERE FOR THE IMAGE
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Draw the diagram
I. Activation Energy = (210 – 100)KJ = 110K
II. Hp – HR = ΔH
54 – 100 = -46KJ
Q2(g) + R2(g) –> 2QR(g)
The heat content of the reactant is higher than that of the product.
E7 – 1s² 2S² 2P³
F9 – 1s² 2S² 2P⁵
G12 – 1S² 2S² 2P⁶ 3S²
H13 – 1S² 2s² 2P⁶ 3S² 3P¹
I. G and H
Isotopy is the existence of an element in more than one physical form with the same atomic number but different atomic masses.
CLICK HERE FOR THE IMAGE
They are isomers
A – Trans 1,2 dichloroethane
B – Cis 1,2 dichloroethane
They contain the same functional group the single bond. The only difference is the polarity(physical property)
The Cis – polar compound while Trans-1, -di chloroethane is non polar
(i) Temperature remains constant during boiling
(ii) There is change of state during boiling
I – It will increase the boiling point of water.
II – It will reduce the boiling point of water.
Boiling occurs at a specific temperature While Evaporation occurs at almost all temperatures.
An unsaturated solution is one that contains less than the maximum amount of solute that can dissolve at a given temperature While A saturated solution is one that contains maximum of solute that can be dissolved in it at that temperature.
(i) By increasing the temperature of the solution.
(ii) By increasing the amount of the solute.
Mole is a standard scientific unit for measuring large quantities of very small entities such as atoms, molecules, or other specified particles
MgO(s)+2HCl(aq) —> MgCl(aq)+H2O(l)
From the equation of reaction; 1 mole of MgO = 2 moles of HCl
Hence n = cv/100
where c = 0.1moldm-³; v = 25.0cm³
No of mole of HCl = n = 0.1×25/1000
= 2.5 x 10-³ moles
Hence the no of moles ofMgO required = 2.5/2 x10-³
But n = m/M = reacting mass/ Molar mass —> m = nM = 1.25×10-³ x 40
= 50 x 10-³ = 0.05g of MgO.
(i) They are malleable
(ii) They are ductile
(iii) They are good conductors of heat and electricity
Faraday’s first law of electrolysis states that the mass(m) of an element discharged during electrolysis is directly proportional to the quantity of electricity(Q) passing through it.
(i) Strong electrolytes conduct large currents while Weak electrolytes do not conduct current readily.
(ii) Strong electrolytes ionize completely while weak electrolytes ionize only slightly.
Ethyne burns in air to give a smoky and luminous flame (complete combustion)
If an organic compound contains carbon atoms joined by double or triple covalent bonds. The compound is said to be an unsaturated hydrocarbon.
CH3COOH(aq) + CH3OH(aq) <–> CH3COOCH3(l) + H2O(l)
By removing the main product continuously
Number of moles of Zn dust = Mass/molars mass = 3.75/65 =0.0077
Reacting mole ratio of Zn to H2 is 1:1
:’ No of moles of H2 produced =0.0677 moles
1 mole = 6.02×10²³ molecules
0.0577moles of hydrogen produces
Or 3.47×10²² molecules
Zinc (from + 2 to + 4)
(i)Each spectral line is caused by an electron
(ii)Electron can exist only in circular orbit of definite quantum energy.
It could not account for the spectrum at note complicated atoms
(i)Temperature of the reacting system
(ii)Pressure of the reacting system
(iii)Concentration of the reacting system
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