Acids & Salts (Triple) quiz

1. Is iron (III) hydroxide acidic or basic?

Basic (as metal hydroxides are basic)

Neutral (as metal hydroxides are neutral)

Depends on the conditions

Acidic (as metal hydroxides are acidic)

Question 1 of 21

2. 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 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) 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.

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.

Question 3 of 21

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

Titration method

Combustion method

Precipitation method

Excess solid method

Question 4 of 21

5. What is defined as a proton donor?

An ore

A base

An acid

An alkali

Question 5 of 21

6. Give the name of the green precipitate formed when sodium hydroxide is added to a solution containing Fe²⁺

iron (II) hydroxide

iron (III) oxide

iron (III) hydroxide

iron (II) oxide

Question 6 of 21

7. Describe the test for carbon dioxide gas

Turns moist litmus paper white (bleaches)

Relights a glowing splint

Turns damp red litmus paper blue

Bubble the gas through limewater and see if it goes cloudy

Question 7 of 21

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

Combustion method

Titration method

Precipitation method

Excess solid method

Question 8 of 21

9. Describe the observations of the reaction of calcium carbonate and dilute hydrochloric acid

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

fizzing, solid disappears, solid floats, lilac flame seen

no reaction

fizzing and solid disappears

Question 9 of 21

10. Can a base neutralise an acid?

Yes

Only if it is more reactive than hydrogen

Sometimes

No

Question 10 of 21

11. What is an acid?

An acid is a compound that reacts with metals

An acid is a corrosive substance

An acid is a green solution

An acid is a source of hydrogen ions, H⁺

Question 11 of 21

12. An alkali is called a proton _________

An alkali is a proton sink

An alkali is a proton acceptor

An alkali is a proton solvent

An alkali is a proton donor

Question 12 of 21

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

Cream precipitate

White precipitate

Blue precipitate

Yellow precipitate

Question 13 of 21

14. State the solubility rule for sodium, potassium and ammonium salts

all common sodium, potassium and ammonium salts are insoluble except nitrates

all common sodium, potassium and ammonium salts are insoluble

all common sodium, potassium and ammonium salts are soluble except carbonates and hydroxides

all common sodium, potassium and ammonium salts are soluble

Question 14 of 21

15. 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?

CuSO₄.7H₂O

CuSO₄.10H₂O

CuSO₄.4H₂O

CuSO₄.5H₂O

Question 15 of 21

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

Neutralisation method

Crystallisation method

Titration method

Precipitation method

Question 16 of 21

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

Na⁺

K⁺

Li⁺

Cu²⁺

Question 17 of 21

18. 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 18 of 21

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

Red

Purple

Yellow

Green

Question 19 of 21

20. With universal indicator, what is the pH of a blue solution?

4-7

12-14

8-10

0-3

Question 20 of 21

21. State the formula of the carbonate ion

C⁴⁻

CO₃²⁻

C⁴⁺

CO₃²⁺

Question 21 of 21

Acids & Salts (Triple) quiz

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