Acids & Salts (Triple) quiz

1. Describe an experiment to prepare a pure, dry sample of an insoluble salt, starting from two soluble reactants

1) Mix the two salt solutions together in a beaker. 2) Stir with glass rod. 3) Pour away the liquid 4) Wash with distilled water. 5) Dry by leaving in a warm place.

1) Mix the two salt solutions together in a beaker. 2) Stir with glass rod. 3) Pour away the liquid 4) Wash with one of the original solutions. 5) Dry by leaving in a warm place.

1) Mix the two salt solutions together in a beaker. 2) Stir with glass rod. 3) Filter using filter paper and funnel. 4) Wash with distilled water. 5) Dry by leaving in a warm place.

1) Mix the two salt solutions together in a beaker. 2) Stir with glass rod. 3) Filter using filter paper and funnel 4) Wash with one of the original solutions. 5) Dry by leaving in a warm place.

Question 1 of 21

2. What is defined as a proton acceptor?

An acid

An alkali

An ore

A base

Question 2 of 21

3. Describe how you would test for carbonate ions (CO₃²⁻) and what is the result if they are present?

Add dilute HCl, followed by barium chloride (BaCl₂) and see if a white precipitate forms

Flame test. Flame colour is lilac

Add nitric acid and see if carbon dioxide bubbles form

Add nitric acid and silver nitrate and see if a precipitate forms

Question 3 of 21

4. A pure, dry sample of a soluble salt can be prepared starting from an acid and alkali. What are the two stages of this method called?

Titration then crystallisation

Combustion then crystallisation

Neutralisation then filtration

Neutralisation then precipitation

Question 4 of 21

5. nitric acid + calcium carbonate →

nitric acid + calcium carbonate → calcium dinitrate + carbon dioxide + hydrogen

nitric acid + calcium carbonate → calcium nitrate + carbon dioxide + hydrogen

nitric acid + calcium carbonate → calcium nitrate + carbon dioxide + water

nitric acid + calcium carbonate → calcium dinitrate + carbon dioxide

Question 5 of 21

6. With universal indicator, what is the pH of a blue solution?

12-14

4-7

0-3

8-10

Question 6 of 21

7. Write a word equation for the reaction between sodium hydroxide and iron(II) sulfate

sodium hydroxide + iron (II) sulfate → iron (II) hydroxide + sodium sulfite

sodium hydroxide + iron(II) sulfate → iron (III) hydroxide + sodium sulfite

sodium hydroxide + iron(II) sulfate → iron (II) hydroxide + sodium sulfate

sodium hydroxide + iron(II) sulfate → sodium hydroxide + iron (II) sulfate

Question 7 of 21

8. When preparing hydrated copper(II) sulfate crystals starting from copper(II) oxide, why is an excess of copper (II) oxide added?

To ensure there is enough solid left for the impurities to be filtered out

To prevent the acid from evaporating

To ensure all the acid has reacted so there is no acid left

To increase the rate of reaction

Question 8 of 21

9. In a flame test, a lilac colour is seen. Give the formula of the cation which is present.

Cu²⁺

K⁺

Li⁺

Na⁺

Question 9 of 21

10. What method would be followed to prepare a sample of pure, dry lead (II) sulfate?

Titration method

Combustion method

Precipitation method

Excess solid method

Question 10 of 21

11. Is iron (III) hydroxide acidic or basic?

Depends on the conditions

Neutral (as metal hydroxides are neutral)

Basic (as metal hydroxides are basic)

Acidic (as metal hydroxides are acidic)

Question 11 of 21

12. Describe the test for chlorine gas

Turns damp red litmus paper blue

Burns with a squeaky pop

Relights a glowing splint

Turns moist litmus paper white (bleaches)

Question 12 of 21

13. Work out the empirical formula of an oxide of chlorine contains 7.1 g of chlorine and 1.6 g of oxygen.

Cl₄O₂

Cl₂O

Cl₂O₂

Cl₄O

Question 13 of 21

14. Describe the method to prepare a pure dry sample of copper sulfate (soluble salt)

1) Heat acid in a beaker. 2) Add an equal amount of base and stir with glass rod. 3) Filter the mixture using filter paper and funnel. 4) Heat the filtered solution (filtrate) until a hot saturated solution forms. 5) Allow the solution to cool so that hydrated crystals form. 6) Remove the crystals by filtration and wash with distilled water. 7) Dry by leaving in a warm place.

1) Heat acid in a beaker. 2) Add base until excess and stir with glass rod. 3) Filter the mixture using filter paper and funnel. 4) Heat the filtered solution (filtrate) until a hot saturated solution forms. 5) Allow the solution to cool so that hydrated crystals form. 6) Remove the crystals by filtration and wash with distilled water. 7) Dry by leaving in a warm place.

1) Heat acid in a beaker. 2) Add an equal amount of base and stir with glass rod. 3) Filter the mixture using filter paper and funnel. 4) Heat the filtered solution (filtrate) until a hot saturated solution forms. 5) Filter and wash with distilled water. 7) Dry by leaving in a warm place.

1) Heat acid in a beaker. 2) Add base until excess and stir with glass rod. 3) Filter the mixture using filter paper and funnel. 4) Heat the filtered solution (filtrate) until a hot saturated solution forms. 5) Filter and wash with distilled water. 7) Dry by leaving in a warm place.

Question 14 of 21

15. An alkali is called a proton _________

An alkali is a proton acceptor

An alkali is a proton solvent

An alkali is a proton sink

An alkali is a proton donor

Question 15 of 21

16. Describe how you would carry out a flame test

Put solid onto a wire. Put into an orange flame

Put solid onto a wire. Put into a blue flame

Dissolve solid in acid. Put solution onto wire. Put into an blue flame

Dissolve solid in acid. Put solution onto wire. Put into an orange flame

Question 16 of 21

17. Is sodium carbonate soluble?

slightly

no

yes

Question 17 of 21

18. State the formula for the iron (II) ion

Fe²⁺

Fe⁺

Fe²⁻

Fe⁻

Question 18 of 21

19. What is a base?

A substance which can neutralise an acid, forming salt and water only

A compound that reacts with an acid to form hydrogen

A source of hydroxide ions, OH⁻

An unreactive form of an alkali that is used to store it

Question 19 of 21

20. What is the universal indicator colour of a pH 4-6 solution?

Red

Green

Purple

Yellow

Question 20 of 21

21. What is an acid?

An acid is a compound that reacts with metals

An acid is a corrosive substance

An acid is a green solution

An acid is a source of hydrogen ions, H⁺

Question 21 of 21

Acids & Salts (Triple) quiz

Related Posts:

Share This Story, Choose Your Platform!