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Form 2 Chemistry questions and answers on salts
How would you obtain a sample of pure iodine from a mixture of iodine and lead sulphate?
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1.
Describe how the following reagents can be used to prepare lead sulphate. Solid potassium sulphate, solid lead carbonate, dilute nitric (V) acid and distilled water.
2.
(a) Using dots(.) and crosses (x) to represent electrons draw diagram to represent the bonding in: (i) #NH_3# (ii)#NH_4^(+# (b) State why an ammonia molecule (#NH_3#) can combine with# H^(+# to form #NH_4^(+#(Atomic numbers: N=7 and H=1)
3.
On strong heating of sodium nitrate liberates oxygen gas. In the spaces provided below, draw a labeled diagram of a set-up that could be used for heating sodium nitrate and collecting the oxygen gas liberated.
4.
Explain how you would obtain sodium carbonate from a mixture of lead carbonate and sodium carbonate powders.
5.
When dilute nitric (V) acid was added to a sample of solid C, a colourless gas that formed a white precipitate with limewater was produced. When another sample of solid C was heated strongly in a dry test-tube, there was no observable change. Write the formula of the ions present in C.
6.
Describe how a solid sample of lead (II) Chloride can be prepared using the following reagents; dilute nitric (V) acid, dilute hydrochloric acid and lead carbonate.
7.
Starting with copper metal, describe how a sample of copper (II) carbonate can be prepared.
8.
Use the scheme below to answer the questions that follow. (a) Identify the solids H and J (b) State one commercial use of solid J.
9.
How would you obtain a sample of pure iodine from a mixture of iodine and lead sulphate?
10.
Describe how a solid sample of zinc (II) carbonate can be prepared starting with zinc oxide.
11.
Some sodium chloride was found to be contaminated with copper (II) oxide. Describe how a sample of sodium chloride can be separated from the mixture.
12.
Carbon (IV) oxide can be dissolved in water under pressure to make an acidic solution. (a) What is meant by an acidic solution? (b) Aqueous lead (II) nitrate reacts with the acidic solution to form a precipitate. Write an ionic equation for the reaction.
13.
Study the flow chart below and answer the question that follows. Identify: (a) Solution K (b) Solid L (c) Gas M
14.
Starting with sodium metal, describe how a sample of crystals of sodium hydrogen carbonate may be prepared.
15.
Starting with copper metal, describe how a sample of crystals of copper (II) chloride may be prepared in the laboratory.
16.
When solid B1 was heated, a gas which formed a white precipitate when passed through lime water was produced. The residue was dissolved in dilute nitric (V) acid to form a colourless solution #B_2#. When dilute hydrochloric acid was added to solution #B_2# a white precipitate which dissolved on warming was formed. (a) Write the formula of the; I. Cation in solid #B_1# II. Anion in solid #B_1#
17.
(a) Write an equation to show the effect of heat on the nitrate of: (i) Potassium (ii) Silver (b) The table below gives information about elements A1, A2, A3 and A4 (i) In which period of the periodic table is element A2?. Give a reason (ii) Explain why atomic radius of: I. A1 is greater than that of A2 II. A4 is smaller than its ionic radius. (iii) Select the element which is in the same group as
18.
(a) Distinguish between a deliquescent and hygroscopic substance
19.
Describe how a solid sample of the double salt, ammonium iron (II) sulphate, can be prepared using the following reagents: Aqueous ammonia, sulphuric (VI) acid and iron metal.
20.
Distinguish between the terms deliquescent and efflorescent as used in chemistry.
21.
Write equation to show the effect of heat on each of the following (a) Sodium hydrogen carbonate (b) Silver nitrate (c) Anhydrous iron (II) sulphate
22.
By using aqueous sodium chloride, describe how a student can distinguish calcium ions from lead ions.
23.
(a) Describe one method that can be used to distinguish between sodium sulphate and sodium hydrogen sulphate. (b) Describe how a pure sample of lead (II) sulphate can be prepared in the laboratory starting with lead metal.
24.
When dilute hydrochloric acid was reacted with solid B, a colourless gas which extinguished a burning splint was produced. When an aqueous solution of solid B was tested with a blue litmus paper, the paper turned red/pink. (a) Identify an ion present in solid B (b) Write an ionic equation for the reaction between solid B and dilute hydrochloric acid.
25.
The chart below shows various reactions of aluminium metal. Study it and answer the questions that follow. (a) (i) Other than water, name another reagent that could be R (ii) Write the formula of reagent Q (b) Write an equation for the reaction in step 5
26.
Starting with barium nitrate solution, describe how a pure sample of barium carbonate can be prepared in the laboratory.
27.
The set-up below was used to prepare anhydrous chlorides of a number of elements in a laboratory where no fume cupboard was available. The chlorides were to be collected in flask 1. The following table shows the melting and boiling points of the chlorides that were prepared. (a) Explain why it is necessary to pass dry chlorine through the apparatus before heating each element. (b) Give two reason
28.
When potassium nitrate is heated, it produces potassium nitrite and gas C1. (a) Identify gas C1. (b) Name the type of reaction undergone by potassium nitrate.
29.
The diagram below illustrates a method of preparing salts by direct synthesis (a) This method can be used to prepare either aluminium chloride or iron (III) chloride. Explain why it cannot be used to prepare sodium chloride. (b) Describe how a sample of sodium chloride can be prepared in the laboratory by direct synthesis.
30.
(a) The scheme below shows some of the reaction of solution D. Study it and answer the question that follows. (i) Give a possible cation present in solution D (ii) Write an ionic equation for the reaction in step II (iii) What observations would be made in step V? Give a reason. (iv) Explain why the total volume of hydrogen gas produced in step I was found to be very low although calcium and
31.
A sample of water is suspected to contain sulphate ions. Describe an experiment that can be carried out to determine the presence of sulphate ions.
32.
Potassium nitrate liberates oxygen gas when heated. Draw a diagram of a set-up that shows heating of potassium nitrate and collection of oxygen gas.
33.
You are provided with solid potassium hydrogen carbonate. Describe how a solid sample of potassium nitrate can be prepared.
34.
Starting with copper turnings, describe how a sample of copper (II) Sulphate crystals can be prepared in the laboratory.
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