Acids & Salts (Triple) quiz

1. Describe how you would carry out a flame test

Dissolve solid in acid. Put solution onto wire. Put into an orange flame

Put solid onto a wire. Put into a blue flame

Put solid onto a wire. Put into an orange flame

Dissolve solid in acid. Put solution onto wire. Put into an blue flame

Question 1 of 21

2. What is the universal indicator colour of a pH 7 (neutral) solution?

Green

Purple

Red

Yellow

Question 2 of 21

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

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

To prevent the acid from evaporating

To increase the rate of reaction

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

Question 3 of 21

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

Precipitation method

Crystallisation method

Titration method

Neutralisation method

Question 4 of 21

5. Write the word equation to represent the reaction between nitric acid and copper carbonate

nitric acid + copper carbonate → copper nitrate + carbon dioxide + hydrogen

nitric acid + copper carbonate → copper dinitrate + carbon dioxide

nitric acid + copper carbonate → copper nitrate + carbon dioxide + water

nitric acid + copper carbonate → copper dinitrate + carbon dioxide + hydrogen

Question 5 of 21

6. When testing a sample of lithium bromide, nitric acid and then silver nitrate is added. Describe the result, and name the substance formed.

A cream precipitate of silver bromide

A yellow precipitate of silver iodide

A white precipitate of silver chloride

A white precipitate of silver sulfate

Question 6 of 21

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

Excess solid method

Precipitation method

Combustion method

Titration method

Question 7 of 21

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

Excess solid method

Precipitation method

Titration method

Combustion method

Question 8 of 21

9. 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 9 of 21

10. What is an alkali?

An alkali is a colourless solution

An alkali is a source of hydroxide ions, OH⁻

An alkali is a compound that reacts with metals

An alkali is a corrosive substance

Question 10 of 21

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

Yellow

Lilac

Red

Blue-green

Question 11 of 21

12. An alkali is called a proton _________

An alkali is a proton donor

An alkali is a proton acceptor

An alkali is a proton solvent

An alkali is a proton sink

Question 12 of 21

13. What is the empirical formula of an alcohol with the analysis; 52.2% C, 13.0% H and 34.8% O?

C₂H₆O₂

C₂H₃O

C₂H₆O

CH₆O

Question 13 of 21

14. What is defined as a proton acceptor?

A base

An acid

An ore

An alkali

Question 14 of 21

15. What is an alkali compared to a base?

Alkalis have higher pHs than bases

Both alkalis and bases have pH greater than 7 but only alkalis are corrosive

Alkalis are anything with a pH above 7. Bases are only metal oxides

Alkalis are bases that are soluble in water

Question 15 of 21

16. What is the pH of a weak alkali?

0-3

12-14

8-10

4-7

Question 16 of 21

17. 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) 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) 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 17 of 21

18. State the formula of the hydroxide ion

OH⁺

OH⁻

H₃O⁻

H₃O⁺

Question 18 of 21

19. Describe the test for oxygen gas

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

Use a glowing splint and see if it relights

Question 19 of 21

20. What is a base?

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

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

A compound that reacts with an acid to form hydrogen

A source of hydroxide ions, OH⁻

Question 20 of 21

21. Is lead nitrate soluble?

slightly

no

yes

Question 21 of 21

Acids & Salts (Triple) quiz

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