Acids & Salts (Triple) quiz

1. Describe the test for oxygen gas

Use a lit splint to see if the gas pops

Bubble the gas through limewater and see if it goes cloudy

Use a glowing splint and see if it relights

Turns moist litmus paper white (bleaches)

Question 1 of 21

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

To dissolve insoluble salts

To make the colour of the flame more obvious

To protect the wire from melting

To clean the wire of any unwanted ions

Question 2 of 21

3. 1.170 g of CoCl₂.xH₂O gave a residue of 0.641 g on heating. Find x.

5

7

6

3

Question 3 of 21

4. What is defined as a proton donor?

An acid

An ore

A base

An alkali

Question 4 of 21

5. What scale typically ranges between 0 and 14?

A burette

Litmus

pH scale

Logarithmic scale

Question 5 of 21

6. Is magnesium oxide acidic or basic?

Depends on the conditions

Acidic

Neutral

Basic

Question 6 of 21

7. Can a base neutralise an acid?

Only if it is more reactive than hydrogen

Sometimes

Yes

No

Question 7 of 21

8. Describe the observations of the reaction of magnesium and dilute sulfuric acid

fizzing, metal moves around, metal melts, metal disappears and metal floats

fizzing, metal disappears, metal floats, lilac flame seen

fizzing and metal disappears

no reaction

Question 8 of 21

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

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 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 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.

Question 9 of 21

10. State the formula of the carbonate ion

CO₃²⁻

C⁴⁺

C⁴⁻

CO₃²⁺

Question 10 of 21

11. Is ammonium nitrate soluble?

yes

slightly

no

Question 11 of 21

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

Using sodium hydroxide. Precipitate is blue

Using a flame test. Flame colour is red

Using sodium hydroxide. Precipitate is green

Using a flame test. Flame colour is lilac

Question 12 of 21

13. A pure, dry sample of an insoluble salt can be prepared starting with two soluble reactants. What is this method called?

Neutralisation method

Titration method

Crystallisation method

Precipitation method

Question 13 of 21

14. An acid is called a proton _________

An acid is a proton solvent

An acid is a proton donor

An acid is a proton acceptor

An acid is a proton sink

Question 14 of 21

15. When testing for halide or sulfate ions, why is acid added added first?

To increase the rate of reaction

To dissolve insoluble salts

To act as a catalyst

To remove any carbonate ions

Question 15 of 21

16. 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 16 of 21

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

Iron (III), Fe³⁺

Copper (II), Cu²⁺

Calcium (II), Ca²⁺

Iron (II), Fe²⁺

Question 17 of 21

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

Excess solid method

Combustion method

Precipitation method

Titration method

Question 18 of 21

19. 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 19 of 21

20. What is an alkali?

An alkali is a colourless solution

An alkali is a source of hydroxide ions, OH⁻

An alkali is a corrosive substance

An alkali is a compound that reacts with metals

Question 20 of 21

21. What is the universal indicator colour of a pH 8-10 solution?

Blue

Red

Yellow

Green

Question 21 of 21

Acids & Salts (Triple) quiz

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