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Federal (FBISE) · Chapter test · Free

10th Class Chemistry Chapter 6 Test06. Salts

30 marks · 40 minutes · 21 questions. Covers: 06. Salts.

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10th Class Chemistry Chapter 6 Test

10th Class · Chemistry · Federal (FBISE)

Name: ____________Roll No: ________Class/Section: ________Date: ________Total marks: 30Time: 40 minutes

Q1. Multiple choice questions (Attempt all · 10 × 1 = 10)

  1. Which insoluble base reacts with H₂SO₄ to produce copper(II) sulphate?
    1. CaCO₃
    2. CuO
    3. NaOH
    4. Zn
  2. Which of the following methods is used to prepare a salt by titration?
    1. Acid + Metal
    2. Acid + Insoluble Base
    3. Acid + Insoluble Carbonate
    4. Acid + Alkali
  3. Which of the following is insoluble in water?
    1. Potassium nitrate (KNO₃)
    2. Calcium carbonate (CaCO₃)
    3. Ammonium chloride (NH₄Cl)
    4. Sodium sulphate (Na₂SO₄)
  4. Which property is due to the lattice stiffness of salts?
    1. Flexibility
    2. Malleability
    3. Hardness and brittleness
    4. Elasticity
  5. Salts are formed through:
    1. Covalent bonding
    2. Electrostatic attraction
    3. Hydrogen bonding
    4. Metallic bonding
  6. Which of the following is a general solubility rule for chlorides?
    1. All chlorides are insoluble.
    2. All chlorides are soluble.
    3. Chlorides are soluble except lead and silver chlorides.
    4. Chlorides are soluble except sodium and potassium chlorides.
  7. In preparation with excess metal (Zn + H₂SO₄), what gas is released?
    1. Oxygen
    2. Hydrogen
    3. Carbon dioxide
    4. Chlorine
  8. When pressure is applied to ionic compounds, they break due to:
    1. Attraction between like charges
    2. Repulsion between like charges
    3. Weak hydrogen bonds
    4. Metallic forces
  9. What happens to the ions in a salt when it is dissolved in water?
    1. They form a gas.
    2. They become fixed in place.
    3. They become mobile.
    4. They form a solid.
  10. Which ion is commonly found in soluble nitrates?
    1. NH4+{NH_4^+}
    2. NO3−NO_3^-
    3. Cl−Cl^-
    4. CH32−CH_{32}^-

Q2. Short questions (Attempt any 6 of 8 · 6 × 2 = 12)

  1. Which salts are always soluble according to solubility rules?
  2. What happens to the ions in an ionic compound when it dissolves in water?
  3. Write the reaction between HCl and NaOH leading to the formation of NaCl.
  4. What is the effect of lattice stiffness on ionic compounds?
  5. Why are salts usually solids at STP?
  6. Which indicator is used when preparing NaCl by titration?
  7. Which type of force holds the ions together in salts?
  8. Which rule applies to all nitrate salts?

Q3. Long questions (Attempt any 2 of 3 · 2 × 4 = 8)

  1. Discuss the properties of salts that make them solid at STP and have high melting points.
  2. Explain the methods of preparing salts using excess metal, insoluble base, and insoluble carbonate with examples.
  3. Explain the process of formation of salts with example.