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Chemistry > Acids > Flashcards

Acids Flashcards

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1
Q

Which ions make aqueous solutions acidic?

A

Hydrogen ions (H^+)

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2
Q

Which ions make aqueous solutions alkaline?

A

Hydroxide ions (OH^-)

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3
Q

What is the pH scale?

A

The pH scale ranges from pH 0 to pH 14
and measures the acidity or alkalinity of
a solution.

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4
Q

What are pH ranges for acids and alkalis? What the

pH of a neutral solution?

A

Acid - Less than pH 7 (pH 1 is strongest).

Neutral - pH 7.

Alkali - Greater than pH 7 (pH 14 is strongest).

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5
Q

What can be used to measure pH?

A

Universal indicator

pH probe

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6
Q

What colour is phenolphthalein in acid, neutral and alkali?

A

Acid - Colourless
Neutral- colourless
Alkali - Pink

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7
Q

What colour is methyl orange in an acid, neutral and an

alkali?

A

Acid - Red
Neutral- Yellow
Alkali - Yellow

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8
Q

What colour is blue litmus paper in an acid and an

alkali?

A

Acid - Turns red

Alkali - Stays blue

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9
Q

What colour is red litmus paper in an

acid and an alkali?

A

Acid - Stays red

Alkali - Turns blue

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10
Q

Suggest a problem with using universal indicator to

test the pH of a solution

A

The colour of the solution is matched to a pH
colour chart. This is quite subjective as people
may disagree with which colour the solution
matches.

It doesn’t provide an exact pH value.

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11
Q

Acid X has a pH of 1. What can you say about the

concentration of hydrogen ions in acid X?

A

There is a high concentration of hydrogen
ions in the acid, making it a strong acid.

The lower the pH of the acid, the higher the
concentration of H^+
ions.

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12
Q

Alkali Y has a pH of 8.5. What can you say about the

concentration of hydroxide ions in alkali Y?

A

There is a low concentration of hydroxide ions in
the alkali, making it a weak alkali.

The lower the pH of the alkali, the lower the
concentration of OH^- ions.

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13
Q

If pH decreases by one unit, what happens to the

concentration hydrogen ions?

A

The hydrogen ion concentration

increases by a factor of 10.

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14
Q

What is a neutralisation reaction?

During an acid-alkali neutralisation reaction, what happens?

A

A neutralisation reaction is a reaction between an
acid and a base.

In an acid-alkali neutralisation reaction, H+
ions from the acid react with OH- ions from the alkali
to form water.

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15
Q

What is the ionic equation for a neutralisation

reaction?

A

H+ (aq) + OH^- (aq) → H2O(l)

check google if unsure

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16
Q

What do the terms concentrated and dilute mean
when talking about acid? Is this the same as strong/
weak acids?

A

Concentrated acids have more moles of acid per unit
volume of water than dilute acids.

The concentration of an acid is not the same as strength.
Strength refers to whether the acid has completely
dissociates in water or not.

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17
Q

An acid only partially dissociates in water. What can

be said about the strength of the acid?

A

Weak acid

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18
Q

What is a base?

A

Any substance that reacts with an acid to

form salt and water only.

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19
Q

True or false?

‘Alkalis are insoluble bases’

A

FALSE

Alkalis are soluble bases.

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20
Q

What are the products when an acid reacts with a

metal?

A

Salt and hydrogen

acid + metal → salt + hydrogen

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21
Q

What are the products when an acid reacts with a

metal oxide?

A

Salt and water

acid + metal oxide → salt + water

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22
Q

What are the products when an acid reacts with a

metal hydroxide?

A

Salt and water

acid + metal hydroxide → salt + water

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23
Q

What are the products when an acid reacts with a

metal carbonate?

A

Salt, water and carbon dioxide

Acid + metal carbonate→ salt + water + carbon
dioxide

24
Q

Why are metal oxides normally bases rather than

alkalis?

A

Metal oxides are normally insoluble.

Alkalis are soluble.

25
Q

What is the name of the salt formed from

magnesium and sulfuric acid?

A

Magnesium sulfate

26
Q

What is the name of the salt formed from zinc oxide

and nitric acid?

A

Zinc nitrate

27
Q

What is the name of the salt formed from calcium

carbonate and hydrochloric acid?

A

Calcium chloride

28
Q

Describe the chemical test for hydrogen

A

Insert a lit splint into a test tube of gas.

A‘squeaky pop’ will be heard if hydrogen
is present.

29
Q

Describe the chemical test for carbon dioxide

A

Bubble the gas through limewater
(calcium hydroxide).

Limewater turns cloudy if carbon dioxide
is present.

30
Q

When a soluble salt is prepared from an acid and an
insoluble reactant, why is excess of the insoluble
reactant added?

A

To ensure all the acid reacts.

31
Q

When a soluble salt is prepared from an acid and an
insoluble reactant, how and why is the excess
reactant removed?

A

By filtration.

It is removed to leave a pure solution of the
salt.

32
Q

What method must be used to prepare a salt from an

acid and a soluble reactant? Why?

A

Titration

This is used to prepare a salt from an acid and a soluble reactant. Since both the reactants are soluble, a titration
allows you to combine the reactants exactly
and avoid adding an excess of either reactant
as this would be hard to remove.

33
Q

Name the method that could be used to prepare a
sample of soluble copper sulfate from insoluble
copper oxide and sulfuric acid?

A

Filtration

34
Q

What 3 steps are required when producing a pure

dry salt from an acid and alkali?

A

Complete a titration to find the volume of acid that reacts
exactly with a set volume of alkali.

Use the results from the titration to mix the acid and alkali in
the correct proportions.

Evaporate the water from the solution, leaving pure dry salt
crystals.

35
Q

Describe how to carry out an acid-alkali titration

A
  1. Use a pipette to add a measured volume of acid to the conical flask
  2. Then add a few drops of indicator.
  3. Place on a white tile.
  4. Fill the burette with the alkali
  5. Note the initial volume.
  6. Add the alkali to the conical flask.
  7. First complete a rough trial to find the end point (the point at which the indicator first changes colour).
  8. Repeat, adding the alkali drop by drop near the end point and swirling the flask constantly to mix.
  9. Record the final volume in the burette. Repeat until you have concordant results.
36
Q

Most common chlorides are soluble.

What are the two exceptions?

A

Silver chloride and lead chloride are

insoluble.

37
Q

True or false?

‘All nitrates are soluble’

A

TRUE

38
Q

Fill in the gap: ‘All common sodium, potassium and

ammonium salts are _____ ’

A

Soluble

39
Q

Most common sulfates are soluble. What are the

three exceptions?

A

Lead sulfate, calcium sulfate and barium

sulfate are insoluble

40
Q

Most common carbonates and hydroxides are

insoluble. What are the three exceptions?

A

The carbonate / hydroxides of sodium

potassium and ammonium are soluble.

41
Q

What salt is produced when lead reacts with sulfuric

acid? Will a precipitate form?

A

Lead sulfate

A precipitate will form because lead
sulfate is insoluble.

42
Q

How could you prepare a pure, dry sample of an insoluble salt?

A
  1. Mix the two solutions required to form the salt.
  2. Filter the mixture using filter paper.
  3. The residue on the filter paper is the insoluble
    salt.
  4. Wash the salt with distilled water and leave to dry.
43
Q

What is the chemical symbol for hydrochloric acid?

A

HCl

44
Q

What is the chemical notation for sodium hydroxide?

A

NaOH

45
Q

What colour is litmus paper in a neutral solution?

A

Purple

46
Q

What is the formula of sulfuric acid

A

H2SO4

47
Q

What is the formula of Nitric Acid

A

HNO3

48
Q

When​ ​an​ ​acid​ ​is​ ​in​ ​solution,​ ​a​ ​higher​ ​concentration​ ​of​ ​___​​ ​ions​ ​means​ ​that​ ​the solution​ ​is​ ​more​ ​_____,​ ​thus​ ​having​ ​a​ ​______​ ​pH

A

H​+

acidic

Lower

49
Q

When​ ​an​ ​_____​ ​is​ ​in​ ​a​ ​solution,​ ​a​ ​higher​ ​concentration​ ​of​ ​OH​-​​ ​ions​ ​means​ ​that​ ​the solution​ ​is​ ​more​ ​______,​ ​thus​ ​having​ ​a​ ​______​ ​pH

A

alkali

alkaline

higher

50
Q

What is dissassociation?

A

Dissociation​ ​is​ ​where​ ​an​ ​acid breaks​ ​down​ ​to​ ​release​ ​H​+​​ ​ions​ ​in​ ​solution

Stronger​ ​an​ ​acid,​ ​greater​ ​the​ ​dissociation,​ ​the​ ​more​ ​H​+​​ ​ions​ ​released,​ ​the​ ​lower
the​ ​pH​

51
Q

Give some examples of strong acids?

A

hydrochloric,​ ​nitric​ ​and​ ​sulfuric​ ​acids

52
Q

Give some examples of weak acids?

A

ethanoic,​ ​citric​ ​and​ ​carbonic​ ​acids

53
Q

acid​ ​+​ ​base​ ​→​ ​______​ ​+​ ​_____

A

Salt + water

54
Q

What is the IUPAC rules for naming salts?

A

1) Metal e.g. Lithium

2) Acid e.g. Sulfate

55
Q

How do you make an insoluble salt?

A

Soluble salt + Soluble salt —> Insoluble salt + Soluble salt

Chemistry (30 decks)

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