Work-Sheet on Acids, Bases and Salts

work-sheet on Acids, bases and salts

1. Fill in the blanks:

i) The insoluble base obtained when sodium hydroxide reactswith iron (III) chloride is ------.

ii) The negative logarithm (to the base 10) of the hydrogen ion concentration expressed in moles /litre is known as ------

iii) ------indicators can differentiate between the acidic or basic solutions of different Ph values.

iv) ------is the process due to which the (H+)ions of an acid react completely or combine with the (OH-) ions of a base to form salt and water only.

v) FeCl3 is stored in air tight bottles because it is a ------substance.

1. Name the following:

i) A base which is soluble in water.

ii) A base which is amphoteric in nature.

iii) Two bases which are not alkalis.

iv) The property of spontaneously giving up of water of crystallisation to the atomsphere.

v) A salt which does not contain water of crystallisation.

vi) An insoluble metal sulphate .

vii) A basic oxide which is soluble in water.

viii) An alkali which is deliquescent in nature.

1. Name the method used for the preparation of the following salts from the list given below:

i) Sodium nitrate ii) Iron(III) Chloride iii) Lead chloride iv) Zinc sulphate v) sodium hydrogen sulphate

List : a) simple displacement b) Neutraliation c) Decomposition by acid d) Double decomposition e) Direct synthesis

Q1. Define acid.What do you understand by the statement ' acetic acid is a monobasic acid'?

Q2. Name the acidic anhydride of the following acids:i) sulphurous acid ii) carbonic acid iii) Phosphoric acid

Q3. What do you understand by an alkali? Give two examples of i) Strong alkali ii) weak alkali

Q4.Name a substance which changes the blue colour of copper sulphate crystals to white.

Q5. Anhydrous hydrogen chloride is not an acid but its aqueous solution is a strong acid.Explain.

Q6. Carbonic acid gives an acid salt but hydrochloric acid does not.Explain.

Q7. The pH value of pure water is 7.Compare the pH values of sulphur dioxide solution and ammonium solution with that of pure water.

Q8. Name : i) Two bases which are not alkali

ii) A normal salt and acid salt of same acid.

iii) A salt insoluble in cold water but soluble in hot water.

Q9. Identify the cation in each of the following cases :

i) Sodium hydroxide solution when added to the solution 'A' gives reddish brown ppt.

ii) Ammonium hydroxide added to solution 'B' gives white ppt which dissolves in excess NH4OH .

iii) Sodium hydroxide solution added to 'C' produces white ppt .which remains insoluble in excess.

iv) Ammonium hydroxide solution when added to solution E gives bluish white ppt.which dissolves in excess to produce a deep blue solution.

Q10. How does ammonium hydroxide help in distinguishing :

i) Iron (II) chloride and iron (III) chloride

ii) Zinc nitrate and lead nitrate

iii) Lead hydroxide and zinc hydroxide

Q11. What are the colours of the precipitates when ammonium hydroxide is added to the following soluitions ?

i) Iron (II) chloride

ii) Lead nitrate

iii) Zinc nitrate

iv) Copper nitrate

v) Iron(III)Chloride

Q12. I) Name the common acid- base indicators.

ii) Name two salts whose aqueous solutions on mixing will form a precipitate of silver chloride.

iii) Name the procedure used to prepare a sodium salt such as sodium sulphate.

Q13. Explain the following:

i) Lime water is bitter while lime juice is sour in taste.

ii) Dilute sulphuric acid is a stronger acid as compared to concentrated sulphuric acid.

iii) On exposure to air,Glauber’s salt loses weight whilequicklime gains weight .

iv) Common salt (containing traces of magnesium chloride ) becomes sticky during the rainy season.

v) Conc .sulphuric acid becomes becomes dilute when exposed to air.

Q14. Write balanced equations for the following reactions:

I) Lead sulphate from leadnitrate solution and dilute sulphuric acid.

ii) Lead chloride from lead nitrate solution and sodium chloride solution.

iii) Ammonium sulphate from ammonia and dilute sulphuric acid .

iv) Sodium chloride from sodium carbonate solution and dilute hydrochloric acid.

v) Sodium aluminate from aluminium oxide and sodium hydroxide.

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10th Chemistry

Mole – concept Numericals

1. A) An organic compound with vapour density =94 contains C= 12.67 % ,H = 2.13 % and Br = 85.11 % .Find the molecular formula .( C = 12, H =1,Br=80)

B) Calculate the mass of i) 1022 atoms of sulphur.

ii) 0.1 mole of CO2.(S= 32, C=12,O=16)and Avogadro’s number = 6x10 23

1. What percentage of water is present in Washing soda crystals.

1. 2C4H10 + 13 O2 --- 8CO2 + 10H2O , Calculate :

i) How many moles of oxygen would be needed for the complete combustion of 5.8 g of butane?

ii) What volume of CO2 would be formed at s.t.p at the same time?

1. The reduction of iron(III) oxide by carbon monoxide takes place:

Fe2O3 + 3CO - 2Fe + 3CO2

What is the mass of 22.5 cm3 of CO?

1. Short answers:

i) The number of oxygen atoms in 1 molecule of ozone =------

ii) 0.2 moles of water weighs =------

iii) Atomic weight of Chlorine is 35.5 .Its vapour density is =------

iv) Empirical formula of hexane is =------

v) Volume at s.t.p occupied by 16 g of oxygen is = ------

vi) 44.8 litres of nitrogen contain ------moles.

vii) 3.2 g of SO2 contain------moles .

viii) Weight of 5.6 litres of CO2 is =------

ix) The volume occupied by 1 mole of a gas at stp is =------