Acids & Salts (Triple) quiz

1. Describe the test for oxygen gas

Use a glowing splint and see if it relights

Turns moist litmus paper white (bleaches)

Bubble the gas through limewater and see if it goes cloudy

Use a lit splint to see if the gas pops

Question 1 of 21

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

Calcium (II), Ca²⁺

Iron (III), Fe³⁺

Iron (II), Fe²⁺

Potassium (I), K⁺

Question 2 of 21

3. When preparing hydrated copper(II) sulfate crystals starting from copper(II) oxide, why is the acid gently heated?

To speed up the reaction

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

To increase the concentration of the acid

To boil the acid

Question 3 of 21

4. How are lithium ions identified, and what is the result?

Using sodium hydroxide. Precipitate is green

Using sodium hydroxide. Precipitate is blue

Using a flame test. Flame colour is red

Using a flame test. Flame colour is green

Question 4 of 21

5. Is magnesium oxide acidic or basic?

Neutral

Basic

Acidic

Depends on the conditions

Question 5 of 21

6. What is the pH of a strong alkali?

4-7

0-3

8-10

11-14

Question 6 of 21

7. hydrochloric acid + magnesium →

hydrochloric acid + magnesium → magnesium chloride + hydrogen

hydrochloric acid + magnesium → magnesium chloride + water

hydrochloric acid + magnesium → magnesium hydrochloride + hydrogen

hydrochloric acid + magnesium → magnesium hydrochloride + water

Question 7 of 21

8. In the test for carbonate ions, what result shows they are present?

cream precipitate

limewater goes cloudy

white precipitate

bubbles form

Question 8 of 21

9. What is an alkali?

An alkali is a source of hydroxide ions, OH⁻

An alkali is a compound that reacts with metals

An alkali is a corrosive substance

An alkali is a colourless solution

Question 9 of 21

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

Precipitation method

Combustion method

Titration method

Excess solid method

Question 10 of 21

11. Is zinc sulfate soluble?

slightly

yes

no

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) 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) 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.

Question 12 of 21

13. Describe how you would carry out a flame test

Put solid onto a wire. Put into an orange flame

Dissolve solid in acid. Put solution onto 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

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) 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.

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 acid is called a proton _________

An acid is a proton donor

An acid is a proton sink

An acid is a proton acceptor

An acid is a proton solvent

Question 15 of 21

16. State the formula of the hydroxide ion

OH⁻

H₃O⁻

OH⁺

H₃O⁺

Question 16 of 21

17. What is a base?

A compound that reacts with an acid to form hydrogen

A source of hydroxide ions, OH⁻

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

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

Question 17 of 21

18. 1.170 g of CoCl₂.xH₂O gave a residue of 0.641 g on heating. Find x.

3

6

5

7

Question 18 of 21

19. What is the universal indicator colour of a weakly alkali solution?

Green

Red

Blue

Yellow

Question 19 of 21

20. 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 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.

Question 20 of 21

21. What is defined as a proton donor?

An alkali

A base

An acid

An ore

Question 21 of 21

Acids & Salts (Triple) quiz

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