Acids & Salts (Triple) quiz

1. 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?

CuSO₄.4H₂O

CuSO₄.7H₂O

CuSO₄.10H₂O

CuSO₄.5H₂O

Question 1 of 21

2. acid + metal →

acid + metal → salt + water

acid + metal → salt + hydrogen + oxygen

acid + metal → salt + hydrogen

acid + metal → salt + water + carbon dioxide

Question 2 of 21

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

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.

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) 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) 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.

Question 3 of 21

4. Can a base neutralise an acid?

Only if it is more reactive than hydrogen

Sometimes

Yes

No

Question 4 of 21

5. With universal indicator, what is the pH of a yellow solution?

0-3

8-10

12-14

4-6

Question 5 of 21

6. State the formula of the carbonate ion

C⁴⁺

C⁴⁻

CO₃²⁻

CO₃²⁺

Question 6 of 21

7. When NaOH is added to a sample, the resultant gas turns damp red litmus paper blue. What cation was present in the sample?

Copper (II), Cu²⁺

Calcium (II), Ca²⁺

Potassium (I), K⁺

Ammonium, NH₄⁺

Question 7 of 21

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

To dissolve insoluble salts

To make the colour of the flame more obvious

To clean the wire of any unwanted ions

To protect the wire from melting

Question 8 of 21

9. An alkali is called a proton _________

An alkali is a proton sink

An alkali is a proton solvent

An alkali is a proton acceptor

An alkali is a proton donor

Question 9 of 21

10. In the flame test for copper (II) ions what colour is the result?

Blue-green

Lilac

Red

Yellow

Question 10 of 21

11. What is an alkali?

An alkali is a corrosive substance

An alkali is a compound that reacts with metals

An alkali is a colourless solution

An alkali is a source of hydroxide ions, OH⁻

Question 11 of 21

12. 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 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) 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 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.

Question 12 of 21

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

To prevent the acid from evaporating

To increase the rate of reaction

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

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

Question 13 of 21

14. Nitric acid and silver nitrate are added to a solution containing iodide ions. Describe the result.

Cream precipitate

Yellow precipitate

White precipitate

Blue precipitate

Question 14 of 21

15. Describe the test for oxygen gas

Bubble the gas through limewater and see if it goes cloudy

Turns moist litmus paper white (bleaches)

Use a lit splint to see if the gas pops

Use a glowing splint and see if it relights

Question 15 of 21

16. Is ammonia acidic or basic?

Neutral

Acidic

Basic

Depends on the conditions

Question 16 of 21

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

Combustion method

Excess solid method

Precipitation method

Titration method

Question 17 of 21

18. A pure, dry sample of a soluble salt can be prepared starting with an insoluble reactant. What is this method called?

Precipitation method

Titration method

Excess solid method

Combustion method

Question 18 of 21

19. Is sodium carbonate soluble?

no

yes

slightly

Question 19 of 21

20. What is defined as a proton donor?

An alkali

An ore

A base

An acid

Question 20 of 21

21. What is the universal indicator colour of a weakly acid solution?

Red

Blue

Green

Yellow

Question 21 of 21

Acids & Salts (Triple) quiz

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