Chapter 3 : Study Of Acids, Bases and Salts - Frank Solutions for Class 10 Chemistry ICSE
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Chapter 3 - Study Of Acids, Bases and Salts Excercise 70
(a) Strong monobasic acids
(b) Weak dibasic acids
(c) Non-volatile acids
(d) Volatile acids
(ii) Nitric acid HNO3
(b) (i) Carbonic acid H2CO3
(ii) Oxalic acid (COOH)2
(c) (i) Sulphuric acid H2SO4
(ii) Hydrogen chloride HCl
(d) (i) Carbonic acid H2CO3
(ii) Acetic acid
(b) Explain, all alkalis are bases but all bases are not alkalis.
(a) Define pH.
(b) State three applications of pH scale.
(a) The pH of a solution is defined as the negative logarithm (base 10) of the hydronium ion concentration present in the solution.
pH = -log10 [H3O+]
(b) The three applications of pH scale are:
It is used to determine the acidic or basic nature of the solution.
It is used to determine hydronium ion concentration present in the solution.
It is used to find out neutrality of the solution.
(b) Explain, why a universal indicator is preferred to acid-base indicators.
(a) An alkali and a base?
(b) An alkali and a metal hydroxide?
(a) Bases in solution
(b) a weak alkali
(c) an acid
Hydroxide ion/ oxide ion and a metallic ion.
(b) A weak alkali furnishes the ions:
Hydroxide ion and metallic ion and molecules of weak alkali./
(c) An acid in a solution furnishes the ions:
Hydronium / Hydrogen ion and a negative ion.
(a) Basic oxide which is soluble in water
(b) A hydroxide which is highly soluble in water.
(c) A basic oxide which is insoluble in water.
(d) A hydroxide which is insoluble in water.
(e) A weak mineral acid.
(f) A base which is not an alkali.
(g) An oxide which is a base.
(h) A hydrogen containing compound which is not an acid.
(f) Ferric hydroxide [Fe (OH)3].
Chapter 3 - Study Of Acids, Bases and Salts Excercise 71
Carbonic acid gives an acid salt but hydrochloric acid does not. Explain.
What do you understand by the strength of an acid? On what factors does the strength of an acid depend?
Strength of an acid measures the ease with which the acid can ionize to produce hydrogen or hydronium ions when dissolved in water. Those acids which can easily ionize to form hydrogen ions are called strong acids while those which can partially ionize to form hydrogen ions are called weak acids.
Strength of an acid depends upon many factors such as:
Molecular structure of the acid
Properties of the solvent
Concept Insight: Bases give pink colour with phenolphthalein because a base will abstract two protons from phenolphthalein and the resulting phenolphthalein ion provides pink colour to the solution.
(a) Copper nitrate
(b) copper carbonate
(c) copper sulphate
(b) How many salts can be obtained from ortho phosphoric acid? Is there any difference in the salts formed by the acid?
(a) MgCO3 from MgCl2
(b) PbCO3 from Pb(NO3)
(c) NaHCO3 from Na2CO3
(iii) Water of crystallization.
(ii) Hygroscopy: It is the phenomenon by which substances absorb moisture from air, but only sufficiently so as to become wet.
(iii) Water of crystallization: It is the fixed amount of water that is present in a crystal as an integral part of its constitution. Hydrated salts are salts having water of crystallisation.
The substances which exhibit deliquescence are called deliquescent.
For example Caustic soda NaOH, Caustic potash KOH.
(b) Give four substances which contain water of crystallization and write their common name.
(b) (i) Na2CO3.10H2O = Washing soda
(ii) MgSO4.7H2O = Epsom salt
(iii) CuSO4.5H2O = Blue vitriol
(iv) ZnSO4.7H2O = White vitriol
Write the reactions of SO2 and oxides of nitrogen which leads to acid rain formation.
Reactions of SO2:
Reactions of oxides of nitrogen:
Fill in the blanks
(a) The word acid comes from latin word acidus meaning _________
(b) Vinegar is the source of ________ acid.
(c) Magnesia is used in making __________.
(d) pH scale was introduced by _________ in 1909.
(e) ___________ is the phenomenon by which hydrated salts on exposure to dry air, lose their water of crystallization and crumble to powder.
(a) The word acid comes from the latin word acidus meaning 'sour'.
(b) Vinegar is the source of acetic acid.
(c) Magnesia is used in making refractory bricks.
(d) pH scale was introduced by Sorencen in 1909.
(e) Efflorescence is the phenomenon by which hydrated salts on exposure to dry air lose their water of crystallisation and crumble to powder.
Chapter 3 - Study Of Acids, Bases and Salts Excercise 72
Choose the correct answer from the options given below:
(i) Which of them occurs in solid state?
(a) Citric acid
(b) Formic acid
(c) Acetic acid
(d) Hydrochloric acid
(ii) Benzoic acid is used for/in/as
(a) Baking powder
(b) Food preservative
(iii) Which colour with the universal indicator indicates highly alkaline solution?
(a) Dark red
(iv) Which one is the acidic salt?
(b) Sodium acetate
(c) Calcium chloride
(d) Ammonium acetate
(i) Citric acid
(ii) Food preservative
(iv) Calcium chloride
(i) Increase its pH
(ii) Decrease its pH
If a solution changes the color of litmus from red to blue, what can you say about its pH?
(ii) pH can be decreased by adding an acid such as HCl to it.
If a solution changes colour of litmus from red to blue, it shows that its pH is above 7.
List of substances: Copper, lead, sodium, zinc, copper oxide, lead carbonate, sodium carbonate solution, dilute hydrochloric acid, dilute nitric acid and dilute sulphuric acid.
Salts: (a) zinc sulphate (b) copper sulphate (c) sodium sulphate (d) lead sulphate.
(b) Copper sulphate = Copper oxide and dilute sulphuric acid
(c) Sodium sulphate = Sodium carbonate solution and dilute sulphuric acid
(d) Lead sulphate = Lead carbonate and dilute sulphuric acid
For example: NaHCO3
(ii) What is the pH of pure water?
(iii) A is a soluble acidic oxide; B is a soluble base. Compared to the pH of pure water, what is the pH of (a) a solution of A (b) a solution of B.
(ii) pH of pure water is 7 since it does not have any impurities.
(iii) (a) A soluble oxide of A will have pH less than the pH of pure water i.e. below 7.
(b) A solution of 'B' will have more pH than pure water i.e. above 7.
(i) Water of crystallization.
For example: Sodium carbonate Na2CO3 has 10 molecules of water present as water of crystallization Na2CO3.10H2O
(ii) Anhydrous: Hydrous salt on heating lose their water of crystallization, such salts are then called anhydrous.
For example: Na2CO3.10H2O on losing 10 molecules of water forms Na2CO3.
Chapter 3 - Study Of Acids, Bases and Salts Excercise 73
Answer the following questions below, relating your answers only to salts in the following list:
Sodium chloride, anhydrous calcium chloride, copper sulphate-5-water.
(i) What is the name given to the water in the compound copper sulphate-5-water?
(ii) If copper sulphate-5-water is heated, the water is driven off leaving anhydrous copper sulphate. What is the colour of anhydrous copper sulphate?
(iii) By what means, other than heating, you can dehydrate copper sulphate-5-water and obtain anhydrous copper sulphate?
(iv) Which one of the salts in the given list is deliquescent?
(i) Water of cystallization.
(iv) Sodium chloride.
What is meant by the term weak acid?
Those acids which ionize partially in aqueous solution and thus they contain ions as well as molecules of the acid. Organic acid such as CH3COOH, is a weak acid.
(a) Will liberate ammonia from ammonium sulphate on heating?
(b) Is a strong acid.
(c) Contains molecules as well as ions?
(ii) pH scale.
(b) (i) Outline the steps that would be necessary to convert insoluble lead (II) oxide into insoluble chloride.
(ii) Write the balanced equations for the reaction required to convert insoluble lead (II) oxide into insoluble lead chloride.
(iii) If iron reacts with dilute sulphuric acid, what will be the products?
(iv) A solution of iron (III) chloride has a pH less than 7. Is the solution acidic or alkaline?
Chapter 3 - Study Of Acids, Bases and Salts Excercise 74
(i) Iron (II) chloride
(ii) Iron (III) chloride
(iii) Iron (II) sulphate
(iv) Iron (II) sulphide
(b) Write the equations for the laboratory preparation of
(i) sodium sulphate using dilute sulphuric acid.
(ii) lead sulphate using dilute sulphuric acid.
(i) An acid is a compound which, when dissolved in water gives ______ ( hydronium / hydroxide) ions as the only ______ (positive/negative) ions.
(ii) A(n) ______ (acid/basic) salt is one in which the hydrogen of an acid has been partially replaced by a ______ (metal/non-metal).
(ii) Acid, metal.
(i) Iron (II) sulphate from the iron.
(ii) Copper sulphate from copper.
(iii) Lead sulphate from lead nitrate.
(iv) Sodium sulphate from sodium carbonate.
(a) Action of an acid on a metal.
(b) Action of an acid on an oxide or carbonate.
(c) Direct combination.
(d) Neutralization of an alkali by an acid.
(e) Precipitation (double decomposition).
(i) copper(II) chloride.
(ii) iron(III) chloride.
(iii) iron(II) chloride.
(iv) lead (II) chloride.
(v) sodium chloride.
(i) Preparation of copper(II) chloride.
Action of an acid on an oxide or carbonate
(ii) Preparation of iron(III) chloride.
(iii) Preparation of iron (II) chloride.
Action of an acid on a metal
(iv) Preparation of lead (ii) chloride
Precipitation (double decomposition)
(v) Preparation of sodium chloride
Neutralization of an alkali by an acid.
Chapter 3 - Study Of Acids, Bases and Salts Excercise 75
(a) What is the first step that is required to prepare lead sulphate from lead carbonate?
(b) Write the equation for the reaction that will take place when this first step is carried out.
(c) Why is the direct addition of dilute sulphuric acid to lead carbonate an impractical method of preparing lead sulphate?
An acid is a compound which when dissolved in water forms hydronium ions as the only ______ ions.
A base is a compound which if soluble in water contains ______ ions. A base reacts with an acid to form ______ and water only. This type of reaction is known as ______.
(a) Alkaline phenolphthalein solution.
(b) Methyl orange solution.
(c) Neutral litmus solution.
(b) From orange to pink.
(c) From colourless to red.
Ammonia, Ammonium, Carbonate, Carbon dioxide, Hydrogen, Hydronium,
A solution 'X' turns blue litmus red so it must contain (i) ______ ions; another solution 'Y' turns red litmus blue and therefore must contain(ii) ______ ions. When solutions X and Y are mixed together, the products will be a (iii) ______ and ______ (iv) ______. If a piece of magnesium was put into solution X, (v) ______ gas would be evolved.
Chapter 3 - Study Of Acids, Bases and Salts Excercise 76
(i) A salt containing a metal ion surrounded by other ions or molecules.
(ii) A base which is soluble in water.
Carbon dioxide and sulphur dioxide gas can be distinguished by using:
(a) Moist blue litmus paper.
(b) Lime water
(c) Acidified potassium dichromate paper
(d) None of the above.
Solution B is a weak acid.
Solution C is a strong alkali.
(i) Which solution contains solute molecules in addition to water molecules?
(ii) Which solution will give a gelatinous white precipitate with zinc sulphate solution? The precipitate disappears when an excess of the solution is added.
(iii) Which solution could be a solution of glacial acetic acid?
(iv) Give an example of a solution which is a weak alkali.
(ii) Solution A.
(iii) Solution B
(iv) Solution of ammonium hydroxide NH4OH is a weak alkali.
Chapter 3 - Study Of Acids, Bases and Salts Excercise 77
Select the correct answer from the choices a,b,c and d which are given.
Write only the letter corresponding to the correct answer.
(i) A particular solution contains molecules and ions of the solute so it is a
(a) Weak acid
(b) Strong acid
(c) Strong base
(d) Salt solution
(ii) An organic weak acid is
(a) Formic acid
(b) Sulphuric acid
(c) Sulphuric base
(d) Hydrochloric acid
(iii) An example of a complex salt is
(a) Zinc sulphate
(b) Solution hydrogen sulphate
(c) Iron(II) ammonium sulphate
(d) Tetramine copper (II) sulphate
Write the equation for the following reaction:
Magnesium sulphate solution is mixed with barium chloride solution.
Give the equation for the preparation of each of the following salts from the starting material given.
(i) Copper sulphate from copper (II) oxide
(ii) Iron (III) Chloride from Iron
(iii) Potassium sulphate from potassium hydroxide solution
(iv) Lead chloride from lead carbonate (two equations)
Solution A is a sodium hydroxide solution. Solution B is a weak acid. Solution C is dilute sulphuric acid. Which solution will.
(i) Liberate sulphur dioxide from sodium sulphite
(ii) Give a white precipitate with zinc sulphate solution,
(iii) Contain solute molecules and ions?
(i) C = Dilute sulphuric acid
(ii) A = Sodium hydroxide
(iii) B = Weak acid
What happen to the crystals of washing soda when exposed to air? Name the phenomenon exhibited.
When crystals of washing soda are exposed to air, it loses its water of crystallisation and the phenomenon is known as efflorescence.
Name the method used for 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
(a) Simple displacement
(c) Decomposition by acid
(d) Double decomposition
(e) Direct synthesis
(i) (B) Neutralisation
(ii) (E) Direct synthesis
(iii) (D) Double decomposition
(iv) (A) Simple displacement
(v) (C) Decomposition by acid
From the list given below, select the word(s) required to correctly complete blanks (i) to (v) in the following passage. The words from the list are to be used only once. Write the answers as (a) (i), (ii) (iii) and so on. Do not copy the passage
Ammonia, ammonium, carbonate, carbon dioxide, hydrogen, hydronium,hydroxide,precipitate,salt,water
(a) A solution M turns blue litmus red, so it must contain (i) _______ ions; another, solution O turns red litmus blue and hence, must contain (ii)__________ ions
(b) When Solutions M and O are mixed together, the products will be (iii) ________ and (iv) ________
(c) If a piece of magnesium was put into a solution M.(v) _________________Gas would be evolved
Chapter 3 - Study Of Acids, Bases and Salts Excercise 78
State what would you observe when :
(a) Washing soda crystals are exposed to the atmosphere.
(b) The salt ferric chloride is exposed to the atmosphere.
(a) When washing soda (Na2CO3.10H2O) is exposed to air, it loses 9 molecules of water to form a monohydrate.
(b) It absorbs moisture from the atmosphere and becomes moist and ultimately dissolves in the absorbed water, forming a saturated solution.
Match the salts given in Column I with their method of preparation given in Column II:
(i) P(NO3)2 from PbO
(ii) MgCl2 from Mg
(iii) FeCl3 from Fe
(iv) NaNO3 from NaOH
(v) ZnCO3 from ZnSO4
(A) Simple displacement
(i) P(NO3)2 from PbO
(ii) MgCl2 from Mg
(iii) FeCl3 from Fe
(iv) NaNO3 from NaOH
(v) ZnCO3 from ZnSO4
(F) Simple displacement
Fill in the blank from the choices given in bracket:
(a) When a metallic oxide is dissolved in water, the solution formed has a high concentration of ___________ ions. (H+,H3O+,OH-)
(a) When a metallic oxide is dissolved in water, the solution formed has a high concentration of OH⁻ ions.
To increase the pH value of neutral solution, we should add
(a) An acid
(b) An acid salt
(c) An alkali
(d) A salt
(b) (c) An alkali
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