Acids & Salts (Triple) quiz

1. Describe the test for ammonia gas

Burns with a squeaky pop

Relights a glowing splint

Turns damp red litmus paper blue

Turns limewater cloudy

Question 1 of 21

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

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

To increase the rate of reaction

To prevent the acid from evaporating

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

Question 2 of 21

3. What is defined as a proton donor?

An acid

A base

An ore

An alkali

Question 3 of 21

4. 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) 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) 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.

Question 4 of 21

5. 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

Neutralisation then precipitation

Combustion then crystallisation

Neutralisation then filtration

Question 5 of 21

6. Is sodium hydroxide soluble?

no

slightly

yes

Question 6 of 21

7. When testing a sample for ions, hydrochloric acid and then barium chloride are added to a sample. A white precipitate forms. What is the name of that precipitate?

barium bromide

barium sulfate

barium chloride

barium carbonate

Question 7 of 21

8. What is the universal indicator colour of a pH 0-3 solution?

Yellow

Green

Red

Purple

Question 8 of 21

9. If sulfuric acid (H₂SO₄) produces 2H⁺, what must the other ion be?

SO₄²⁻ (sulfate ion)

S²⁻ (sulfide ion)

O²⁻ (oxide ion)

S²⁺ (sulfide ion)

Question 9 of 21

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

Excess solid method

Precipitation method

Combustion method

Titration method

Question 10 of 21

11. acid + base →

acid + base → salt + water + carbon dioxide

acid + base → salt + water

acid + base → salt + hydrogen + oxygen

acid + base → salt + hydrogen

Question 11 of 21

12. Is ammonia acidic or basic?

Basic

Acidic

Depends on the conditions

Neutral

Question 12 of 21

13. An alkali is called a proton _________

An alkali is a proton sink

An alkali is a proton solvent

An alkali is a proton donor

An alkali is a proton acceptor

Question 13 of 21

14. What is the pH of a weak alkali?

12-14

4-7

8-10

0-3

Question 14 of 21

15. What is the empirical formula of a compound in which 0.48 g of carbon combines with 0.08 g of hydrogen and 0.64 g of oxygen?

CH₂O

CH₄O

C₂H₄O₂

C₄H₂O

Question 15 of 21

16. When NaOH is added to a sample, a brown precipitate forms. What cation was present in the sample?

Iron (III), Fe³⁺

Iron (II), Fe²⁺

Calcium (II), Ca²⁺

Potassium (I), K⁺

Question 16 of 21

17. In a flame test, why is hydrochloric acid used?

To make the colour of the flame more obvious

To clean the wire of any unwanted ions

To dissolve insoluble salts

To protect the wire from melting

Question 17 of 21

18. Can a base neutralise an acid?

Yes

Sometimes

Only if it is more reactive than hydrogen

No

Question 18 of 21

19. How are sodium ions identified, and what is the result?

Using a flame test. Flame colour is yellow

Using sodium hydroxide. Precipitate is blue

Using sodium hydroxide. Precipitate is green

Using a flame test. Flame colour is red

Question 19 of 21

20. What is an acid?

An acid is a corrosive substance

An acid is a source of hydrogen ions, H⁺

An acid is a compound that reacts with metals

An acid is a green solution

Question 20 of 21

21. 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) 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) 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 one of the original solutions. 5) Dry by leaving in a warm place.

Question 21 of 21

Acids & Salts (Triple) quiz

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