Chemistry JAMB, WAEC, NECO AND NABTEB Official Past Questions

 All your burette readings (initial and final), as well as the size of your pipette, must be recorded but no account of experimental procedure is required. All calculations must be done in your answer book.

A is a solution containing 6.3g dm\(^{-3}\) of impure ethanoic acid. B is 0.10mol. dm\(^{-3}\) sodium hydroxide sodium hydroxide solution.

(a) Put A into the burette and titrate with 20.0cm\(^3\) or 25.0cm\(^3\) portions of B using phenolphthalein as indicator. Record the volume of your pipette Record the volume of your pipette. Tabulate your burette readings and calculate the volume of A used.

(b) From your result and the information provided, calculate the

(i) concentration of solution A in mol.dm\(^{-3}\) 

(ii) Concentration of solution A in dm\(^{-3}\) and hence the percentage purity of the ethanoic acid,

(iii) Volume of solution A that would neutralize a solution containing 0.005 mole of sodium hydroxide. The equation for the reaction is;

H\(_2\)C\(_2\)O\(_{4(aq)}\) + 2NaOH\(_{(aq)}\) \(\to\) Na\(_2\)C\(_2\)O\(_{(aq)}\) + 2H\(_2\)O\(_{(l)}\) [H = 1; C = 12. O = 16]

(c)(i) What would be the colour of methylorange indicator in solution B?

(ii) Give the reason why methylorange is not a suitable indicator for titration. 

Credit will be given for strict adherence to instructions, for observations precisely recorded, and for accurate inferences. All tests, observations, and inferences must be clearly entered in your answer book, in ink at the time they are made.

C is a mixture of two simple salts. Carry out the following exercises on C. Record your observations and identify any gases evolved. State the conclusion you draw from the result

(a)(i) Put all C in a boiling tube or beaker and add about 10cm\(^{3}\) of distilled water Stir the mixture thoroughly and tilter Keep both the residue and the filtrate

(ii) Test the filtrate with litmus paper.

(b) Divide the filtrate of two portions

(i) To the first portion of the filtrate. add about 2cm\(^3\) of dilute trioxonitrate (v) acid and then silver trioxonitrate (v) solution

(ii) To the second portion of the filtrate, add sodium hydroxide solution in drops until it is in excess.

(c) Put half of the residue in a test tube and heat strongly. Allow to cool

(d)(i) Put the remaining half of the residue in a test tube and add about 2cm\(^3\) of dilute hydrochloric acid.

(ii) To the resulting solution from (d(i)) above, add aqueous ammonia in drops until it is in excess.

(a) Use the following reaction scheme to answer Questions;(i) – (iii) below;

(i) Give one suitable procedure for carrying out each of reactions 1, 2, and 3 separately in the laboratory

(ii) State the gases produced along with lead (lI) Oxide in reaction 1.

(iii) What is the colour of lead (II) tetraoxosulphate (VI)?

(b) When a drop of concentrated trioxonitrate (V) acid was added to potassium iodide solution, a violet-colored gas was evolved?

(i) What is the name of the gas evolved?

(ii) State the functions of concentrated trioxonitrate (V) acid in the reaction.

(iii) What would be observed if starch solution were added to the reaction mixture?

(a)(i) Explain what is meant by saturated solution

(ii) Describe in outline, a suitable procedure for preparing a saturated solution of sodium trioxonitrate(V) at 30°C.

(ii) State two techniques that can be used to recover crystals of sodium trioxonitrate(V) from its saturated solution.

(b) 1.0dm\(^3\) of an aqueous solution at 90°C contains 404g of potassium trioxonitrate(V) and 245g of potassium trioxochlorate (V).

(i) Determine which of the two salts will separate out when the solution is cooled to 60°C. N = 14. O = 16, CI = 35.5, K = 39; Solubility of KNO\(_3\) in water at 60\(^o\)C = 5.14 mol.dm\(^{-3}\), Solubility of KCIO\(_3\) in water at 60°C = 1.61 mol.dm\(^{-3}\)

(ii) Calculate the mass of salt that will separate out at 60°C

(c)(i) List two salts which cause hardness of water.

(ii) Explain why temporary hardness of water result in the furring of kettle.
 

(a) List three properties of a system that is in a state of chemical equilibrium.

(b) Consider reaction represented by the following equation: 3H\(_{2(g)}\) + N\(_{2(g)}\) \(\rightleftharpoons\) 2NH\(_{3(g)}\); H = 92KJ

(i) Explain the effect of increasing the temperature of the reaction on the yield of ammonia

(ii) Uses of energy profile diagram to illustrate the effect of a positive catalyst on the rate of either the forward reaction or the reverse reaction.

(c) In the extraction of aluminium from bauxite:

(i) outline the procedure used for purifying the ore;

(ii) write equation for the reaction at each electrode, during the electrolysis of the pure alumina;

(iii) state the function of molten cryolite in the electrolytic cell for the extraction.

(a)(i) What is isomerism?

(ii) Name the alkanol that is isomeric with methoxymethane (CH\(_3\)OCH\(_3\)).

(b)(i) Outline the laboratory:preparation of ethylethanoate. (Diagrams not required)

(ii) Write the structural formula of ethylethancqte

(iii) State two physical properties of ethylethanoate.

(c) When gas oil which consists of larger hydrocarbons was subjected to high temperature and pressure, the following reaction occurred.

C\(_{17}\)H\(_{36(l)}\) \(\to\) 3C\(_2\)H\(_{4(g)}\) + C\(_3\)H\(_{6(g)}\) + Q\(_{(l)}\)

(i) What name is given to the process indicated above?

(ii) State the importance of the process to the petroleum industry.

(iii) Find the formula of the product which Q represents in the equation above.

(iv) Mention one type of chemical industry that utilizes ethene as raw material.

(d) Consider the following compounds: CH\(_3\) — (CH\(_2\))\(_2\) —CH\(_3\); C\(_6\)H\(_5\) —CH = CH\(_2\); CH=C — CH\(_3\). State which of them:

(i) is used as a domestic fuel;

(ii) is an aromatic compound,

(iii) participates in such situation but not addition reactions;

(iv) would react with two moles of hydrogen per mole.

(a)(i) List the three types of particles present in atoms.

(ii) name the element which does not contain all the three particles in its atom. Mention the particle that is not present.

(b) Give the reason why:

(i) the relative atomic masses of some elements are not whole number;

(ii) relative atomic masses are used instead of the actual masses of atoms in grams;

(iii) metals are good conductors of electricity.

(c)(i) Name the type of bond present in the oxonium ion,

(ii) State one effect of the existence of intermolecular hydrogen bonding on the physical properties of ethanol.

(d)(i) Explain what is meant by water of crystallization.

(ii) When 5.0g of a compound Y was heated to constant mass, 1.8g of water vapour was given off. Determine the number of molecules of water of crystallization in one molecule of Y, given that the molar mass of its anhydrous form is 160g. [H = 1, 0 = 16]

(a) List two differences between solids and liquids.

(b) The graph below is the heating curve for a solid X. Use the graph to answer Questions (i) — (iii) below.

(i) What is the melting point of X?

(ii) If the vapour of X is cooled, at what temperature will it start to condense?

(iii) (I) As X is heated, state what happens to the: I. frequency of collision of molecules of X;

(II) value of the entropy of the system.

(a) Mention one process apart from respiration, which increases the amount of carbon (IV) oxide in the atmosphere.

(b)(i) State one use of sodium hydrogentrioxocarbonate (IV).

(ii) Write an equation to show the action of heat on sodium hydrogentrioxocarbonate(IV).

(a) What is the change in oxidation state of chromium in the reaction represented by the following equation?

3SO\(_2\) + Cr\(_2\)O\(^2_{-7}\) + 2H\(^+\)  -> 3SO\(_4^{2-}\) + 2Cr\(^{3+}\) + H\(_2\)O

(b) Use the half equations given below to deduce the equation for the reaction between iron(II) ions and heptaoxodichromate (VI) ions in acidic solution.

Fe\(^{2+}\)  –> Fe\(^{3+}\) + e\(^-\)

Cr\(_2\)O\(^{2-}_7\) + 14H\(^+\) + 6e\(^-\) —-> 2Cr\(^{3+}\) + 7H\(_2\)O.

(a) Mention the chemical substance manufactured starting from each of the foirownc sets of materials:

(i) sugar and yeast;

(ii) ammonia, air and water;

(iii) vegetable oil and caustic alkali.

(b) State one air pollutant generated during the manufacture of fertilizers.

(a) Name the device used for producing an electric current from a chemical

(b) Copy and complete the table below.

(a) State the type of reaction involved in the conversion of:

(i) proteins.to amino acids:

(ii) ethanol to ethene;

(iii) benzene to bromobenzene

(b) Write an equation to show that ethene reasts with hydrogen in the presence of finely divided nickel.

(a)(i) Sketch a graph to illustrate Charles’ law.

(ii) A gas occupies 500 cm\(^{ 3}\) at 2TC. calculate its volume at 40°C constant pressure.

(b) List two gases that are used as refrigerant

(a)(i) Explain the term pH

(ii) If sodium hydroxide solution were added to a solution of a strong acid, what would happen to the pH of the solution?

(b) Give one example of each of the following:

(i) acidic oxide

(ii) acid salt.

What name is given to each of the following? The

(a) irregular random movement of smoke particles in air.

(b) existence of an element in various forms in the same physical-state

(c) disintegration of atomic nuclei, accompanied with radiation emission.

(d) conversion of a solid difitrunto vapour without melting.

(a) State three reasons why air is classified as a mixture.

(b) List two methods that can be used to separate a mixture of iodine crystals and iron filings.

What is the amount (in mole) of hydrogen gas that would be produced if 0.6 mole of hydrochloric acid reacted with excess zinc according to the following equation? Zn_(s) + 2HCI_(aq) → ZnCI_2(aq) + H_2(g)

What is the amount (in mole) of hydrogen gas that would be produced if 0.6 mole of hydrochloric acid reacted with excess zinc according to the following equation? Zn_(s) + 2HCI_(aq) → ZnCI_2(aq) + H_2(g)

The following salts dissolve readily in cold water except

Copper (ll) tetraoxosulphate (VI) is often added to swimming pools because it