Acids & Salts (Triple) quiz

1. With universal indicator, what is the pH of a red solution?

0-3

8-10

4-7

12-14

Question 1 of 21

2. 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 2 of 21

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

Yellow

Red

Blue-green

Lilac

Question 3 of 21

4. Write a word equation for the reaction between sodium hydroxide and iron(II) sulfate

sodium hydroxide + iron(II) sulfate → sodium hydroxide + iron (II) sulfate

sodium hydroxide + iron(II) sulfate → iron (II) hydroxide + sodium sulfate

sodium hydroxide + iron(II) sulfate → iron (III) hydroxide + sodium sulfite

sodium hydroxide + iron (II) sulfate → iron (II) hydroxide + sodium sulfite

Question 4 of 21

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

To increase the concentration of the acid

To speed up the reaction

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

To boil the acid

Question 5 of 21

6. Is lead sulfate soluble?

no

slightly

yes

Question 6 of 21

7. What two observations can be made when a metal reacts with an acid?

Metal floats. Metal disappears

Metal floats. Metal melts

Bubbles. Metal disappears.

Bubbles. Metal melts

Question 7 of 21

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

To protect the wire from melting

To clean the wire of any unwanted ions

To dissolve insoluble salts

To make the colour of the flame more obvious

Question 8 of 21

9. What is defined as a proton donor?

An acid

An ore

A base

An alkali

Question 9 of 21

10. Describe the test for oxygen gas

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)

Use a lit splint to see if the gas pops

Question 10 of 21

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

Titration method

Excess solid method

Combustion method

Precipitation method

Question 11 of 21

12. An alkali is called a proton _________

An alkali is a proton acceptor

An alkali is a proton solvent

An alkali is a proton donor

An alkali is a proton sink

Question 12 of 21

13. What is a base?

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

A source of hydroxide ions, OH⁻

A compound that reacts with an acid to form hydrogen

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

Question 13 of 21

14. If nitric acid (HNO₃) produces H⁺ ions, what is formula for the other ion?

NO₃⁻ (nitrate ion)

N⁻ (nitride ion)

N³⁻ (nitride ion)

O²⁻ (oxide ion)

Question 14 of 21

15. 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 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) 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) Filter using filter paper and funnel. 4) Wash with distilled water. 5) Dry by leaving in a warm place.

Question 15 of 21

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

Blue precipitate

White precipitate

Yellow precipitate

Cream precipitate

Question 16 of 21

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

Basic (as metal hydroxides are basic)

Acidic (as metal hydroxides are acidic)

Depends on the conditions

Neutral (as metal hydroxides are neutral)

Question 17 of 21

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

Yellow

Green

Blue

Red

Question 18 of 21

19. 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 19 of 21

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

Question 20 of 21

21. 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

Titration method

Precipitation method

Question 21 of 21

Acids & Salts (Triple) quiz

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