Acids & Salts (Triple) quiz

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

To increase the rate of reaction

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

Question 1 of 21

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

To make the colour of the flame more obvious

To protect the wire from melting

To clean the wire of any unwanted ions

To dissolve insoluble salts

Question 2 of 21

3. When testing a sample for ions, hydrochloric acid and then barium chloride are added to a sample. A white precipitate forms. What ions have been shown to be present?

bromide ions (Br⁻)

carbonate ions (CO₃²⁻)

chloride ions (Cl⁻)

sulfate ions (SO₄²⁻)

Question 3 of 21

4. 7.485 g of a hydrated copper(II) sulphate CuSO₄.xH₂O was heated producing 4.785g of anhydrous copper(II) sulphate. What is the formula of the hydrated salt?

CuSO₄.5H₂O

CuSO₄.4H₂O

CuSO₄.10H₂O

CuSO₄.7H₂O

Question 4 of 21

5. How are potassium ions identified, and what is the result?

Using a flame test. Flame colour is red

Using sodium hydroxide. Precipitate is green

Using sodium hydroxide. Precipitate is blue

Using a flame test. Flame colour is lilac

Question 5 of 21

6. 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) 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.

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) 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.

Question 6 of 21

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

Iron (III), Fe³⁺

Calcium (II), Ca²⁺

Potassium (I), K⁺

Copper (II), Cu²⁺

Question 7 of 21

8. What two observations can be made when a metal reacts with an acid?

Metal floats. Metal melts

Bubbles. Metal disappears.

Bubbles. Metal melts

Metal floats. Metal disappears

Question 8 of 21

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

Titration method

Combustion method

Excess solid method

Precipitation method

Question 9 of 21

10. What is an acid?

An acid is a green solution

An acid is a source of hydrogen ions, H⁺

An acid is a corrosive substance

An acid is a compound that reacts with metals

Question 10 of 21

11. Can a base neutralise an acid?

Only if it is more reactive than hydrogen

Yes

No

Sometimes

Question 11 of 21

12. What is defined as a proton donor?

An ore

A base

An acid

An alkali

Question 12 of 21

13. State the solubility rule for sulfate salts

all sulfates are insoluble, except those of sodium, potassium and ammonium

all sulfates are soluble

all sulfates are insoluble

all sulfates are soluble, except those of lead, barium and calcium

Question 13 of 21

14. 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 14 of 21

15. Is magnesium oxide acidic or basic?

Acidic

Basic

Neutral

Depends on the conditions

Question 15 of 21

16. What is the universal indicator colour of a strongly alkali solution?

Green

Purple

Red

Blue

Question 16 of 21

17. What is the typical range of the pH scale?

1-5

0-10

0-14

1-20

Question 17 of 21

18. Describe the method to prepare a pure dry sample of sodium chloride (soluble salt)

1) Heat hydrochloric acid in a beaker. 2) Add an equal amount of sodium oxide 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 hydrochloric acid in a beaker. 2) Add sodium oxide 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) Pipette 25cm³ of sodium hydroxide into a conical flask. 2) Do not add indicator. 3) (Using titration values)Titrate the known volume hydrochloric acid into conical flask containing alkali. 4) Transfer to an evaporating basin. 5) Heat the solution until a hot saturated solution forms. 6) Allow the solution to cool so that hydrated crystals form. 7) Remove the crystals by filtration and wash with distilled water. 8) Dry by leaving in a warm place.

1) Pipette 25cm³ of sodium hydroxide into a conical flask. 2) Add indicator. 3) (Using titration values)Titrate the known volume hydrochloric acid into conical flask containing alkali. 4) Transfer to an evaporating basin. 5) Heat the solution until a hot saturated solution forms. 6) Allow the solution to cool so that hydrated crystals form. 7) Remove the crystals by filtration and wash with distilled water. 8) Dry by leaving in a warm place.

Question 18 of 21

19. An acid is called a proton _________

An acid is a proton sink

An acid is a proton solvent

An acid is a proton donor

An acid is a proton acceptor

Question 19 of 21

20. In the test of a gas, a lit splint gives a squeaky pop. What is the gas?

Chlorine

Oxygen

Hydrogen

Carbon dioxide

Question 20 of 21

21. State the formula of the silver ion

Ag⁺

Ag⁻

Ag²⁺

Ag²⁻

Question 21 of 21

Acids & Salts (Triple) quiz

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