Chemistry X | Acid, Bases and Salts: NCERT Solved Questions

Acid, Bases and Salts: NCERT Solved Questions

Question 1. You have been provided with three test tubes. One of them contains distilled water and the other two contain an acidic solution and a basic solution respectively. If you are given only red litmus paper, how will you identify the contents of each test tube ?


We will dip the red litmus paper in all the test tubes, the test tube in which red litmus changes to blue., contains, basic solution. Now dip the so changed blue litmus paper in other two test tubes, the test tube in which blue litmus changes to red is acidic solution and the third test tube will contain distilled water.

Question 2. Why should curd and sour substances not be kept in brass and copper vessels ?


Curds and other sour substances contain acids which react with brass and copper to form toxic substances which are not suitable for health and consumption. So, it is advisable not to store curds and other sour substances in brass or copper vessels.

Question 3. Which gas is usually liberated when an acid reacts with a metal ? Illustrate with an example. How will you test the presence of the gas ?


Usually hydrogen gas is liberated when an acid reacts with a metal. For example, when zinc granules react with dilute sulphuric acid, zinc, sulphate and hydrogen are produced.

Zn (s) + H2S04 (aq) clip_image002 ZnS04 (aq) + H2 (g)

Hydrogen gas burns with a ‘pop’ sound.

Question 4. A metal compound A reacts with dilute hydrochloric acid to produce effervescence. The gas evolved extinguishes a burning candle. Write a balanced chemical equation for the reaction if one of the compounds formed is calcium chloride.


Metal compound A reacts with dilute hydrochloric acid to form a gas which extinguishes burning candle means produced gas is carbon dioxide. Other product is calcium chloride, so compound A is carbonate or hydrogen carbonate of calcium. We can present the reaction as follows:

Question 5. Why do HCl, HNO3 etc. show acidic character in aqueous solutions while solutions of compounds like C2H5OH and glucose do not show acidic character ?


HCl, HNO3 show acidic character in aqueous solutions because they produce H+ (aq) ions, but solutions of C2H5OH and glucose do not produce H+ ions, so they do not show acidic character.

Question 6. Why does an aqueous solution of an acid conduct electricity ?


An aqueous solution of an acid conduct electricity because in aqueous solution acid produces cations and anions.

Question 7. Why does dry HCl gas not change the colour of dry litmus paper ?


H+ions are responsible for acidic character of HC1 and change of litmus paper. H+ ions are formed in the presence of water only. That’s why, dry HCl gas cannot change the colour of dry litmus paper.

Question 8. While diluting the acid why is it recommended that acid should be added to water and not water to the acid ?


Mixing water and acid is an exothermic reaction. When water is added to acid due to small amount of water, evolved heat will change it to vapour and acid will spill out and may cause injury. So, it is advised to mix acid to water, not water to acid.

Question 9. How is the concentration of hydronium ions (H3O+) affected when a solution of an acid is diluted ?


when a solution of an acid is diluted, the concentration of hydronium ions (H30+) is decreased.

Question 10. How is concentration of hydroxide ions (OH) affect when excess base is dissolved in a solution of sodium hydroxide ?


When excess base is dissolved in a solution of sodium hydroxide concentration of hydroxide ions (OH) is increased.

Question 11. You have two solutions A and B. pH of solution A is 6 and pH of solution B is 8. Which solution has more hydrogen ion concentration ? Which of the above solution is acidic and which one is basic ?


Solution having more hydrogen ion concentration – Solution A.

Acidic solution – Solution A.

Basic solution – Solution B.

Question 12. What effect does the concentration of H+ (aq) have on the acidic nature of the solution ?


Acidic nature of a solution is directly proportional to the H+ (aq) ion concentration. If H+ (aq) ion concentration of one solution is higher than the other, it will be more acidic than the other.

Question 13. Do basic solution also have H+ (aq) ions ? If yes, then why are they basic ?


Yes, basic solution also have H+ (aq) ions. If a solution has H+ (aq) ions and (OH) ions concentration is neutral and when (OH) ions > H+ ions, solution is basic.

Question 14. Under what soil conditions do you think a farmer would spread or treat the soil of his fields with quick lime (calcium oxide) or slaked lime (calcium hydroxide) or chalk (calcium carbonate).


Quick lime, slaked lime and chalk are basic in nature, so soil should be treated using these substances when the soil is acidic in nature

Question 15. What is the common name of compound CaOCl2 ?


The common name of compound CaOCl2 is bleaching powder.

Question 16. Name the substance which on treatment with chlorine yields bleaching powder ?


Dry slaked lime.

Question 17. Name the sodium compound which is used for softening of hard water.


Washing soda (sodium carbonate) is used for softening of hard water.

Question 18. What will happen if the solution of sodium hydrogen carbonate is heated ? Give the equation of the reaction involved.


On heating NaHCO3 changes to Na2CO3

NaHCO3clip_image002[1] Na2CO3 + H20 + CO2

Question 19. Write an equation to show the reaction between plaster of Paris and water.


CaSO4. clip_image005 H20 + 1clip_image005[1] H20 clip_image002[2] CaS04. 2H20

Objective Questions

Question 20. A solution turns red litmus blue, its pH is likely to be

(a) 1

(b) 4

(c) 5

(d) 10

Answer: (d)

Question 21. A solution reacts with crushed egg shells to give a gas that turns lime water milky, the soultion contains.

(a) NaCl

(b) HCl

(c) LiCl

(d) KCl.

Answer: (d)

Question 22. 10 mL of a solution of NaOH is found to be completely neutralised by 8 mL of a given solution of HCl. If take 20 mL of same solution of NaOH, the amount of HCl solution (the same solution as before) required neutralise it will be

(a) 4 mL

(b) 8 mL

(c) 12 mL

(d) 16 mL.

Answer: (d)

Question 23. Which one of the following types of medicines is used for treating indigestion ?

(a) Antibiotic

(b) Analgesic

(c) Antacid

(d) Antiseptic.

Answer: (c)

Question 24. Write word equations and then balanced equation when

(a) Dilute sulphuric acid reacts with zinc granules

(b) Dilute hydrchloric acid reacts with magnesium ribbon

(c) Dilute sulphuric acid reacts with aluminium powder

(d) Dilute hydrochloric acid reacts with iron filings



(a) Zinc (s) + Sulphuric acid (aq) clip_image002[3] Zinc sulphate (aq) + Hydrogen (g)

Zn (s) + H2S04 (aq) clip_image002[4] ZnS04 (aq) + H2 (g)

(b) Magnesium (s) + Hydrochloric acid (aq) —> Magnesium chloride (aq) + Hydrogen (g)

Mg (s) + 2HC1 (aq) clip_image002[5] MgCl2 (aq) + H2 (g)

(c) Aluminium (s) + Sulphuric acid (aq) clip_image002[6]Aluminium sulphate (aq) + Hydrogen (g)

2A1 (s) + 3H2S04 (aq) clip_image002[7]A12(S04)3 (aq) + 3H2 (g)

(d) Iron (s) + Hydrochloric acid (aq) clip_image002[8] Iron chloride (aq) + Hydrogen (g)

2Fe (s) + 6HC1 (aq) clip_image002[9]2FeCl3 (aq) + 3H2 (g)

Question 25. With the help of a chemical reaction explain how a soda-acid fire extinguisher helps in putting out a fire.


In soda-acid fire extinguisher, which contains a solution of sodium hydrogen carbonate surrounding a glass bottle containing sulphuric acid.

In case of fire, the knob (provided at the top of extinguisher) is pressed, thereby bottle breaks and the two solutions come in contact, thereby liberating carbon dioxide gas.

2 NaHCO3 + H2SO4clip_image013Na2SO4 + 2 H2O + 2 CO2

The liberated carbon dioxide forces a stream of effervescing liquid on the fire. In this way, carbon dioxide surrounds the combustible substances and cut­off the supply of air, thereby it assists to put out the fire.


Question 27. Why does distilled water not conduct electricity whereas rain water does.


Rain water dissolves atmospheric carbon dioxide to form carbonic acid (H2C03) which forms H+ions and due to presence of H+ ions, rain water conducts electricity, but a distilled water cannot.

Question 28. Why do acids do not show acidic behaviour in the absence of water?


Acids show acidic behaviour when they form H+ (aq) ions which are not formed in the absence of water.

Question 29. Five solutions A, B, C, D and E when tested with universal indicator showed pH as 4, 1, 11, 7 and 9 respectively. Which solution is:

(a) neutral ?

(b) strongly alkaline ?

(c) strongly acidic ?

(d) weakly acidic ? weakly alkaline ?

(f) arrange the pH in increasing order of hydrogen ion concentration.


Solution Showing pH

(a) Neutral 7

(b) Strongly alkaline: 11

(c) Strongly acidic: 1

(d) Weakly acidic: 4

(e) Weakly alkaline: 9

(f) pH in increasing order of hydrogen ion concentration: 11 <9<7<4< 1.

Question 30. Equal lengths of magnesium ribbons are taken in test tubes A and B. Hydrochloric acid (HCl) is added to tube A while acetic acid (CH3COOH) is added to test tube B. In which test tube will the fizzing occur more vigorously and why ?


The fizzing will occur more vigorously in test tube A because HCl is a strong acid and it produces more number of H+ ions.

Question 31. Fresh milk has a pH of 6. How do you think the pH will change as it turns into curd ? Explain your Answer


When milk changes to curd its pH will decrease due to the formation lactic acid.

Question 32. A milkman adds a small amount of baking soda to fresh milk.

(a) Why does he shift the pH of the fresh milk from 6 to slightly alkaline ?

(b) Why does the milk take a long time to set as curd.


(a) Addition of baking soda (alkaline in nature) makes milk more alkaline, i.e., pH of milk increase about

(b) The pH required for fermentation of milk is about 5-6 and we know that on addition of baking sour milk makes it alkaline {i.e., pH>7). Hence, milk takes a long time to set as curd.

Question 33. Plaster of Paris should be stored in moisture-proof container. Explain why ?


Plaster of Paris changes to a hard substance reacting with water. That’s why, it is stored in a moisture- proof container.

Question 34. What is a neutralization reaction ? Give two examples.


Neutraliztion is the interaction of an acid and base with the formation of salt
Example :

HCl (aq) + NaOH (aq) clip_image002[10] NaCl (aq) + H20 (I)

H2S04 (aq) + Ca (OH)2 (aq) clip_image002[11] CaS04 (aq) + 2H20 (I)

Question 33. Give two important uses of washing soda and baking soda.


Uses of washing soda :

(i) It is used in the manufacture of soap, glass and paper.

(ii) It is used in the production of sodium compound.

Uses of baking soda :

(i) It is an important ingredient of baking powder.

(ii) It is also used as antacid.


Chemistry IX | Matter-Its Nature and Behaviour: Mole Concept | Part 3

Matter-Its Nature and Behaviour: Mole Concept


Atomic Mass

· The average relative mass of an atom of an element as compared to the mass of an atom of carbon (C12) taken as 12. In other words atomic mass is a number which expresses as to how many times an atom of the element is heavier than 1/12th of the mass of carbon atom. Therefore,

· Atomic mass = clip_image002

Average Atomic Mass

· It has been found that majority of the elements occur as several isotopes. Isotopes are the different atoms of the same element possessing different atomic masses but same atomic number. The atomic mass of each isotope is determined separately and then combined according to the ratio of their proportions of occurrence. This is known as average atomic mass. E.g., Boron occurs in nature in the form of two isotopes B10, B11 with atomic mass 10 and 11 in the ratio of 1 : 4 respectively. Therefore Average atomic mass of carbon

= clip_image004

= clip_image006

Gram Atomic Mass

· The atomic mass of an element expressed in grams is the gram atomic mass or it is also called gram atom e.g. the atomic mass of oxygen is 16 amu, therefore gram atomic mass of oxygen is 16g.

Molecular Mass

· Molecular mass of a compound is defined as the weight of a molecule of the compound relative to a carbon atom, the atomic weight of which is supposed to be equal to 12.

Molecular mass of H2SO4 =

2 clip_image008 atomic mass of hydrogen + atomic mass

of sulphur + 4clip_image008[1] atomic mass of oxygen

= 2 clip_image008[2]1 + 32 + 4 clip_image008[3] 16 = 98

Gram Molecular Mass

· Molecular mass of a substance expressed in grams is called gram molecular mass. It is also known as gram molecule. e.g., molecular mass of N2 is 28 and its gram molecular mass is 28 gm.

Determination of the molecular weight

(i) By using Graham’s law of diffusion


r1 and r2 are the rates of diffusion of gases having molecular weights M1 and M2 respectively.

(ii) Victor Meyer’s method

V.D. = clip_image016 (Approx).

m grams of substance displaces x mL of air at NTP.

Equivalent Mass

  • An equivalent mass of a substance is defined as the amount of it which combines with 1 mole of hydrogen atoms or replaces the same number of hydrogen atoms in a chemical reaction. The equivalent mass of a substance expressed in grams is called gram equivalent. e.g., in the compounds like H2O, NH3, CH4, one mole of hydrogen combine with clip_image018 mole of O, clip_image020 mole of N and clip_image022 mole of C respectively Hence

Equivalent mass of O = clip_image024

Equivalent mass of N = clip_image026

Equivalent mass of C = clip_image028

Relation between Atomic weight, Equivalent weight and Valency

Equivalent weight = clip_image030

E = clip_image032

e.g., equivalent mass of H2SO4 is clip_image034 = 49

For Bases

E = clip_image036

For Ca(OH)2, E = clip_image038

For Salts

E = clip_image040

cations or anions

For Oxides

E = clip_image043

· In a redox reaction equivalent mass depend upon the number of electrons taking part in the reaction

E = clip_image045

Where n factor is total change in oxidation number of element in molecule

Determination of Equivalent weight

(i) Hydrogen displacement method :

Eq. wt. of the metal

= clip_image047

(ii) Oxide formation method :

Eq. wt. of element = clip_image049

where w1 = weight of element

w2 = weight of chloride

(iii) Chloride formation method :

Eq. weight of the element = clip_image051

where m1 = weight of element

m2 = weight of chloride

(iv) Metal displacement method : A more electropositive metal ‘B’ displaces less electropositive metal ‘A; from its salt solution.

clip_image053= clip_image055


· A mole is the amount of substance that contains as many particles as are present in 12 g of carbon – 12 isotope.

· ‘Mole may also be defined as “the amount of a substance in grams which contains 6.023 x 1023 units of that substance.

· 6.023 x 1023 particles of a substance weight equal to the molecular weigh of that substance in grams, therefore, 1 mole is the gram molecular weight of a substance :

Number of mole = clip_image057

= clip_image059

= clip_image061

Gram Molar Volume

· The volume occupied by 1 mole of a substance is called gram molar volume of the substance. The gram molar volume of perfect gas is 22.4 liters at STP or NTP. N.T.P. clip_image063 Normal temperature and pressure S.T.P. clip_image063[1] Standard temperature and pressure e.g., volume of 1 mole of H2 at STP = 22.4 L

STP = 22.4 L

Volume of clip_image022[1] mole of H2,

= clip_image067 = 5.6 L

Vapour Density

· Vapour density of a gas is the ratio of the mass of a certain volume of the gas to the mass of equal volume of hydrogen, measured under same conditions of temperature and pressure.

Vapour density = clip_image069

Molecular weight = 2 clip_image008[4] vapour density

Atomic weight = 2 clip_image008[5] clip_image073

Knowledge Update

– Equivalent weight of CO2, SO2 and SO3 is equal to clip_image075.

– Equivalent weight of acidic salt = clip_image077

– Mole wt. = 2 clip_image008[6] vapour density

Mole = clip_image080

Atomic wt. clip_image008[7] specific heat = 6.4 (approx)