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Chemistry - IGCSE > Ch - 11 (Acids and Bases) > Flashcards

Ch - 11 (Acids and Bases) Flashcards

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1
Q

What happens when acids are added to water?

A

Form positively charged hydrogen ions. (H+)

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2
Q

What makes a solution acidic?

A

Presence of H+ ions.

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3
Q

Give a word equation of acids reacting with metals?

A

Acid + Metal –> Salt + Hydrogen

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4
Q

Which metals in the reactivity series will react with dilute acids?

A

Metals above hydrogen

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5
Q

What can act as bases?

A
  • Metal oxides
  • Hydroxides (alkalis)
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6
Q

Give a word equation of acid reacting with base.

A

Acid + base –> Salt + water

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7
Q

Give an equation of the acid reacting with a metal carbonate.

A

Acid+ metal –> salt + carbon dioxide + water

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8
Q

What is one common indicator?

A

Litmus extracted from lichens

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9
Q

What are synthetic indicators?

A

Organic compounds that are sensitive to changes in acidity and appear different colours in acids and alkalis.

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10
Q

What are 2 synthetic indicators frequently used in acid - alkali titrations?

A

Thymolphthalein and methyl orange

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11
Q

What are synthetic indicators used for?

A

To show the endpoint in titrations as they have a very sharp change of colour when an acid has been neutralised by an alkali or vice versa.

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12
Q

Is litmus suitable for tritration? why or why not?

A

colour change is not so sharp, colour in neutral solution makes it difficult

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13
Q

What pH does a base have?

A

Above 7

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14
Q

What is a base?

A

water soluble referred to as an alkali

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15
Q

In basic (alkaline) what colour do the following change into:
- red litmus paper
- methyl orange
-thymolphthalein

A
  • red litmus paper: blue
  • methyl orange: yellow
    -thymolphthalein: blue
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16
Q

What form are bases of metals?

A

Oxides or hydroxides

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17
Q

What happens when alkalis are added to water?

A

Form negative (OH-) ions

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18
Q

What makes a solution an alkali?

A

Presence of OH- ions

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19
Q

Give a word equation of what happens when acid reacts with bases?

A

Acid + base –> salt + water

20
Q

What happens when acids are added to water?

A

Form positively charged H+ ions (acidic)

21
Q

What happens when alkalis are added to water?

A

Forms negative OH- ions (alkali)

22
Q

When does a neutralisation reaction take place?

A

When acid reacts with an alkali

23
Q

What happens when substances react together in a neutralisation reaction?

A

H+ ions reacts with OH- ions to produce water

24
Q

What is the net ionic equation of acid - alkali neautralisation reaction?

A

H+ + OH- –> H2O

25
Q

What is the pH of all acids?

A

Below 7

26
Q

What is the pH of all alkalis?

A

Above 7

27
Q

What does it mean when we have more hydrogen ions?

A

Stronger the acid but lower the pH

28
Q

What does it mean when we have a stronger concentration of hydroxide ions?

A

Higher pH

29
Q

How is the Ph scale calibrated?

A

Logarithmic, change of 1 on the scale represents a change in concentration by a factor of 10

30
Q

Define a universal indicator.

A

A universal indicator is a mixture of different indicators which is used to measure pH.

31
Q

Define acids

A
  • Proton donors
  • Produce H+ protons
32
Q

Define bases.

A
  • Proton acceptor
33
Q

How can an acid be weak or strong?

A

depending on how many H+ ions they produce

34
Q

What happens to strong acids?

A

Completely dissociate (ionise) in water, producing very low pH

35
Q

What are examples of strong acids?

A

Hydrochloric acid, Sulfuric acids, nitric acid

36
Q

What is an example of a weak acid?

A

Ethanoic acid (CH3COOH) - Vinegar

37
Q

What happens to weak acids in water?

A

Partially dissociate (ionise) in water and produce pH value closer to the middle lf pH scale below 7

38
Q

What does a concentrated solution mean?

A

An acid that contains a higher no. of acid molecules

39
Q

Define oxides.

A

Compounds made from one or more atoms of oxygen combined with another element.

40
Q

How can oxides be classified?

A

Based on their acid - base characteristic.

41
Q

What are the difference in properties of acidic and basic oxides?

A
  • Difference in their pH depends on the bonding with a metal or non - metal
  • Metallic character of the element influences the acidic or basic behaviour
42
Q

What are properties of acidic oxides?

A
  • Non - metal combines with oxygen
  • React with bases to form salt and water
  • When dissolved in H2O, they produce an acidic solution with low pH

Example - CO2, SO2, NO2

43
Q

What are the properties of basic oxides?

A
  • Metal element combines with oxygen
  • React with acids to form salt and water
  • When dissolved in H2O, they produce a basic solution with a High pH.

Example: CuO, CaO

44
Q

what are neutral oxides?

A
  • Do not react with acids or bases
  • Example: N2O, NO and CO
45
Q

Define amphoteric oxides.

A
  • Curious group of oxides tht behave both acidic and basic, depending on reactant being an acid or base
46
Q

What are properties of an amphoteric oxide?

A
  • Salt and water is formed
  • common example: ZnO, Al2O3
  • Hydroxides are also amphoteric

Chemistry - IGCSE (24 decks)

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