Acids & Salts (Triple) quiz

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

Blue

Green

Red

Yellow

Question 1 of 21

2. Describe the observations of the reaction of aluminium and dilute hydrochloric acid

fizzing, metal disappears, metal floats, lilac flame seen

no reaction

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

fizzing and metal disappears

Question 2 of 21

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

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) 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) 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. An acid is called a proton _________

An acid is a proton donor

An acid is a proton sink

An acid is a proton solvent

An acid is a proton acceptor

Question 4 of 21

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

Excess solid method

Combustion method

Precipitation method

Titration method

Question 5 of 21

6. Can a base neutralise an acid?

Yes

No

Sometimes

Only if it is more reactive than hydrogen

Question 6 of 21

7. If copper chloride has the formula CuCl₂, what is the formula of the copper ion?

Cu²⁺

Cu⁻

Cu⁺

Cu²⁻

Question 7 of 21

8. Is magnesium oxide acidic or basic?

Neutral

Depends on the conditions

Acidic

Basic

Question 8 of 21

9. In the test for sulfate ions, what result shows they are present?

bubbles form

A white precipitate is formed

cream precipitate

limewater goes cloudy

Question 9 of 21

10. 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 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

To increase the rate of reaction

Question 10 of 21

11. Is iron sulfate soluble?

yes

no

slightly

Question 11 of 21

12. What is the pH of a weak acid?

0-3

4-6

8-10

12-14

Question 12 of 21

13. In a flame test, a orange-red colour is seen. Give the formula of the cation which is present.

K⁺

Li⁺

Na⁺

Ca²⁺

Question 13 of 21

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

Copper (II), Cu²⁺

Iron (III), Fe³⁺

Iron (II), Fe²⁺

Calcium (II), Ca²⁺

Question 14 of 21

15. State the steps for calculating empirical formula

1) Aᵣ/mass. 2) divide by the smallest. 3) Give the ratio has a whole number. 4) State final empirial formula

1) Aᵣ/mass. 2) divide by the largest. 3) Give the ratio has a whole number. 4) State final empirial formula

1) mass/Aᵣ. 2) divide by the largest. 3) Give the ratio has a whole number. 4) State final empirial formula

1) mass/Aᵣ. 2) divide by the smallest. 3) Give the ratio has a whole number. 4) State final empirial formula

Question 15 of 21

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

To clean the wire of any unwanted ions

To dissolve insoluble salts

To protect the wire from melting

To make the colour of the flame more obvious

Question 16 of 21

17. 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 17 of 21

18. In the test of a gas, a glowing splint relights. What is the gas?

Chlorine

Carbon dioxide

Hydrogen

Oxygen

Question 18 of 21

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

Combustion method

Excess solid method

Titration method

Precipitation method

Question 19 of 21

20. What is defined as a proton donor?

A base

An acid

An alkali

An ore

Question 20 of 21

21. What is an acid?

An acid is a corrosive substance

An acid is a compound that reacts with metals

An acid is a source of hydrogen ions, H⁺

An acid is a green solution

Question 21 of 21

Acids & Salts (Triple) quiz

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