Reference no: EM132586609

EXERCISE -

1. Select the proper choice from the given multiple choices:

1. What is formed by reaction of non-metal oxide with water?

A. Acid

B. Base

C. Salt

D. Metal

2. Acid + Metal-oxide →?

A. Base + Water

B. Salt + Water

C. Base + Salt

D. Metal + Salt

3. Which gas is produced by reaction of base with metal?

A. Carbon dioxide

B. Dioxygen

C. Dihdrogen

D. Dinitrogen

4. 500 ml aqueous solution is prepared by dissolving 2 moles of HCI in water. What will be the molarity of this solution?

A. 1

B. 2

C. 3

D. 4

5. What is correct for acidic aqueous solution?

A. [H₃O+] = 10^-7 M

B. [H₃O+] > 10^-7 M

C. [H₃O+] < 10^-7 M

D. [H₃O+] < [OH^-]

6. Which of the following solutions is the most basic?

A. pH = 8.2

B. pH = 9.3

C. pH = 11.5

D. pH = 10.6

7. Which statement is incorrect?

A. pH scale was presented by S.P.L Sorensen.

B. pH scale ranges between 0 to 14.

C. pH scale is applicable to only non-aqueous solutions.

D. pH scale is applicable to only aqueous solutions.

8. How is the exact pH of an aqueous solution measured?

A. pH paper

B. Litmus paper

C. pH meter

D. Universal indicator

9. Which of the following substances is an antacid?

A. NaCl

B. Mg(OH)₂

C. HCl

D. H₂SO₄

10. The aqueous solution having pH 11 is how many times less basic than aqueous solution having pH 8?

A. 3

B. 30

C. 300

D. 1000

11. Which of the following is strong acid?

A. Acetic acid

B. Citric acid

C. Nitric acid

D. Oxalic acid

12. What type of substance is NH₃

A. Strong acid

B. Weak acid

C. Strong base

D. Weak base

13. pH + pOH = ?

A. 7

B. 0

C. 14

D. 10

14. Which formula is correct?

A. Mole = Molecular mass / Weight

B. Mole = Weight / Molecular mass

C. Mole = Weight / Litre

D. Mole = Molecular mass / Litre

15. What will be the pH of aqueous solution of NH₄Cl?

A. pH = 7

B. pH > 7

C. pH < 7

D. pH = 0

16. Which of the following solutions will have pH = 2?

A. 0.01 M HCl

B. 0.02 M HCl

C. 0,01M H₂SO₄

D. 0.02M H₂SO₄

17. What will be OH- concentration in aqueous solution having pH = 8?

A. 1 x 10^-8 M

B. 1 x 10^-6 M

C. 8 x 10^-6 M

D. 8 x 10^-8 M

18. If the pH of aqueous solutions A, B, C and D are 1.9, 2.5, 2.1 and 3.0 then what will be the order of acidity ?

A. A < C < B < D

B. D < C < B < A

C. D < B < C < A

D. D > C > B > A

19. Which solution will be basic?

A. [H₃O⁺] =10^-5M

B. [H₃O⁺] =10^-12M

C. [H₃O⁺] =10^-7M

D. [H₃O⁺] =10^-4M

20. Which substance is present in poison of honey bee?

A. Lime

B. Calcium phosphate

C. Mellitin

D. Pepsin.

2. Answer the following questions in brief:

1. Write names of two Arrhenius acids and bases.

2. Write products of reactions of acid with metal.

3. Mention names of four methods of expressing concentration of a solution.

4. Which scientist presented pH scale? Write the formula of pH.

5. Write names of two methods to measure approximate pH of aqueous solution.

6. Mention names of two strong acids and two strong bases.

7. Write names of two weak acids and two weak bases.

8. Give definitions:

i. Arrhenius acid,

ii. Arrenius base,

iii. Bronsted-Lowry acid,

iv. Bronsted-Lowry base,

v. Concentration of solution,

vi. pH of solution,

vii pOH of solution,

viii Strong acid,

ix Weak acid,

X. Strong base,

Xi. Weak base,

xii. Neutralisation reaction,

xiii 1M concentration

9. Mention the formula, name and physical state of the products of following reactions:

1. CO₂(g)+H₂O(l)

2. Li₂O(s) + H₂O(l)

3. H₂SO₄(aq) + 2KOH(aq)

4. 2HCL(aq) +Ca(s)

5 2HNO₃(aq) + CaO(s)

6. 2HCL(aq) + Na₂CO₃(aq)

7. NaOH(aq) + HCl(aq)

8. BaCl₂(aq) + H₂SO₄(aq)

9. Ca(OH)₂(aq) +CO₂(g)

10. HNO₃(aq) + NH₄OH(aq)

11. Na₂SO₄(aq) + Ba(OH)₂(aq)

12. AgNO₃(aq) + NaCl(aq)

3. A. Answer the following questions:

1. Write two chemical properties of acid.

2. Write two chemical properties of base.

3. Write two chemical properties of salt.

4. Deduce pH + pOH = 14

5. Explain the importance of pH in digestion of food.

6. Write chemical equations f four neutralistion reactions.

B. Solve the following problems:

1. Calculate pH of an aqueous solution having H₃+O⁺ concentration equal to 7.9 x 10^-11 M.Which nature, acidic asic or neutral will be possessed by this aqueous solution.

2. Calculate pH of 0.00424 M aqueous solution of KOH.

3. How many times concentrated will be the aqueous solution having pH 11.9 as compared to aqueous solution having pH 8?

4. How will you prepare 500ml aqueous solution of 0.2 M H₂SO₄?

5. How will you prepare 125 ml 0.03 M aqueous solution of KOH.

4. A Answer the following questions in detail:

1. Explain giving example, Arrhenius acid-base theory, Mention the limitations of this theory.

2. Discuss Bronsted-Lowry Acid-base theory.

3. Discuss methods to measure pH of aqueous solution.

B. Solve the following problems:

1. [OH^-] in aqueous solution A is = 4.3 x 10^-M, pH of which solution will be less? Which solution will bemore basic?

2. Calculate the concentration of OH- in aqueous solution having pH value 9.3.

3. 8 gram NaOH is dissolved in water and the aqueous solution is made to 5 litres. Find pH of this solution.

5. A Answer the following question in detail:

1. With reference to PH scale,

I Write formula of pH and pOH

Ii Mention pH and concentration of H₃O⁺ or OH^- in acidic, basic and neutral aqueous solutions.

Iii Mention limitations of pH scale.

2. Explain importance of pH in everyday life.

3. "The aqueous solution of the salt produced by neutralisation of weak acid and strong base possesses basic nature, while aqueous solution of salt produced by neutralisation of weak base and strong acid possesses acidic nature" - Explain.

B. Solve the following problems :

1. pH of aqueous solution of potassium hydroxide at 298 K temperature is 11.65. The initial volume of this solution is made 6 times by addition of water. What will be the pH of the diluted solution?

2. What will be the change in the value of pH if the concentration of aqueous solution of HNO3is increased to 0.05 M from 0.03 M?