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CHEMISTRY: IGCSE > Acids, Bases, and Salts > Flashcards

Acids, Bases, and Salts Flashcards

1
Q

What are the products when an acid
reacts with a metal?

A

acid + metal → salt + hydrogen

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2
Q

What are the products when an acid
reacts with a metal oxide?

A

acid + metal oxide → salt + water

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3
Q

What are the products when an acid
reacts with a metal hydroxide?

A

acid + metal hydroxide → salt + water

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4
Q

What are the products when an acid
reacts with a metal carbonate?

A

acid + metal carbonate → salt + water + carbon dioxide

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5
Q

Why are metal oxides normally bases
rather than alkalis?

A

Metal oxides are normally insoluble.
Alkalis are soluble bases.

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6
Q

What is the name of the salt formed from
magnesium and sulfuric acid?

A

Magnesium sulfate

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7
Q

What is the name of the salt formed from
zinc oxide and nitric acid?

A

Zinc nitrate

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8
Q

What is the name of the salt formed from
calcium carbonate and hydrochloric
acid?

A

Calcium chloride

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9
Q

What color is methyl orange in acid and
alkali?

A

Acid - Red
Alkali - Yellow

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10
Q

What color is blue litmus paper in acid
and alkali?

A

Acid - Turns red
Alkali - Stays blue

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11
Q

What colour is red litmus paper in acid
and alkali?

A

Acid - Stays red
Alkali - Turns blue

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12
Q

What do acids produce in an aqueous
solution?

A

H+ ions

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13
Q

What do bases produce in an aqueous
solution?

A

OH- ions

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14
Q

Define acids and bases in terms of
proton transfer

A

Protons are H+ ions.
Acids are proton donors.
Bases are proton acceptors.

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15
Q

What is the chemical equation for the
the reaction between hydrochloric acid and
ammonia?

A

HCl + NH3 → NH4Cl

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16
Q

What is the chemical equation for the
reaction between sulfuric acid and
sodium hydroxide?

A

H2SO4n+ 2NaOH → Na2SO4 + 2H2O

17
Q

What is the difference between a strong
and weak acid?

A

The strength of the acid refers to the degree of ionisation (or dissociation).
Strong acids are completely ionized in aqueous solutions (lots of H+ ions are released).
Weak acids are only partially ionized in aqueous solutions. (fewer H+ ions released).

18
Q

What is the difference between a strong
and weak base?

A

Strong bases are completely ionised in aqueous solutions (lots of OH- ions are released). Weak bases are only partially ionised in aqueous solutions (fewer OH- ions released).

19
Q

How is the relative acidity and alkalinity of a solution quantified?

A

Using the pH scale

20
Q

How can pH be measured?

A

Universal indicator
pH probe

21
Q

Which pH values describe an acid, alkali and neutral solution?

A

Acid: pH < 7
Neutral: pH = 7
Alkali: pH > 7

22
Q

Why is it important to control acidity in soil?

A

If the soil is too acidic, crops will be unable to grow.

23
Q

How is an acidic oxide formed?

A

An acidic oxide is generally formed when a non-metal reacts with oxygen.
E.g. SO2

24
Q

How is a basic oxide formed?

A

A basic oxide is generally formed when a metal reacts with oxygen.
E.g. CaO

25
Q

What is a neutral oxide?

A

Some non-metallic oxides are neutral. They can’t neutralise acids or bases.
E.g. H2O

26
Q

What is amphoteric oxide?

A

Some metal oxides are amphoteric meaning they can neutralize both acids and bases to form salt and water.
E.g. Al2O3

27
Q

An insoluble base reacts with an acid to form a soluble salt. How can the salt be removed from the solution?

A
  • Add excess base to the acid.
  • Use filter paper and a funnel to remove any unreacted base.
  • Keep in a warm place to evaporate the water. The salt crystals will be left behind.
28
Q

How can a soluble salt be prepared from
an acid and soluble base?

A
  • Use an acid/base titration to find the exact volume of base required for neutralisation of the acid.
  • React the exact quantities of acid and base together without any indicator and collect the solution formed.
  • Leave to dry in a warm place to evaporate the water. The salt crystals can be collected from the evaporating dish.
29
Q

How can an insoluble salt be collected from a reaction mixture?

A

The insoluble salt is a precipitate so can be collected by filtration:

  • Put filter paper in a funnel then place in a conical flask.
  • Pour the reaction mixture into the funnel. Wash the salt with distilled water to wash away any solution.
  • The salt crystals will be collected on the filter paper. Leave this to dry in a warm place before collecting the crystals.
30
Q

What reactants can be used to form the salt magnesium nitrate?

A

Magnesium
Nitric acid

31
Q

Suggest a method that could be used to produce sodium sulfate from sodium hydroxide and hydrochloric acid

A

Titration

32
Q

What colour precipitate forms when sodium hydroxide reacts with calcium ions?

A

White

33
Q

What colour precipitate forms when sodium hydroxide reacts with chromium(III) ions?

A

Green

34
Q

What colour precipitate forms when sodium hydroxide reacts with aluminium ions?

A

White precipitate at first.
Re-dissolves with excess NaOH to form a colourless solution.

35
Q

What colour precipitate forms when sodium hydroxide reacts with copper(II) ions?

A

Blue

36
Q

What colour precipitate forms when sodium hydroxide reacts with iron(II) ions?

A

Green

37
Q

What colour precipitate forms when sodium hydroxide reacts with iron(III) ions?

A

Brown-red

38
Q

What colour precipitate forms when sodium hydroxide reacts with zinc ions?

A

White precipitate at first.
Re-dissolves with excess NaOH to form a colourless solution.

39
Q

Describe how to carry out a flame test

A
  • Clean a nichrome wire using hydrochloric acid.
  • Turn the Bunsen burner onto the blue flame.
  • Dip the wire in the solid substance that you want to test.
  • Place the wire in the flame. Record the colour of the flame.

CHEMISTRY: IGCSE (6 decks)

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