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GCSE Chemistry 1 paper 1 > Acids And Alkalis > Flashcards

Acids And Alkalis Flashcards

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1
Q

What can some acids and alkalis be?

A

Toxic or harmful to the environment

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2
Q

How are hazards associated with handling particular solutions?

A

Identified by international symbols, and they indicate the precautions that need to be taken when handling them

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3
Q

What is the acidity or alkalinity of a solution measured on?

A

Measured on the PH scale

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4
Q

What are solutions with a pH of 7?

A

Neutral

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5
Q

What are acids?

A

Solutions that have a pH lower than 7

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6
Q

What are solutions with a pH higher than 7?

A

Alkalis

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7
Q

The lower the pH the more acidic the solution

A

The higher the pH the more alkaline the solution

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8
Q

How can you find the pH of a solution ?

A

Using indicators

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9
Q

What is universal indicator?

A

A mixture of different indicators and produces a range of colours depending on the pH

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10
Q

In alkaline solutions what colour does litmus, methyl orange, and phenolphthalein turn?

A

Blue, yellow and pink

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11
Q

In acidic solutions what colour does litmus, methyl orange, and phenolphthalein turn?

A

Red, red and colourless

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12
Q

Acids and alkalis are always found in which state symbol So?

A

(Aq) aqueous because water is the base

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13
Q

Which range of numbers will you find on the pH scale?

A

0-14

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14
Q

How do colours of universal indicator reflect the pH numbers?

A

They reflect the pH numbers because the solution turns a specific colour depending on the pH number (so how acidic or alkaline a solution is

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15
Q

Explain how litmus paper, methyl orange and phenolphthalein are affected by acids and alkalis

A

This is affected by the acids and alkalis, because they turn the solution different colours depending wether it is an acid or an alkali

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16
Q

List 3 common acids

A

Hydrochloric acid - HCl
Sulphuric acid - H2SO4
Nitric acid HNO3
Numbers are all small

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17
Q

List 3 common alkalis

A

Sodium hydroxide NaOH
Potassium hydroxide KOH
Calcium hydroxide Ca(OH)2 Number is small

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18
Q

Acids and alkalis can be defined in terms of the ions they produce. Which ions are these?

A

Acids - H➕ ions

Alkalis - OH- ions

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19
Q

In terms of hydrogen ions, how does their concentration affect the pH?

A

The more H➕ ions, the more acidic the solution

20
Q

In terms of hydroxide ions, how does their concentration affect the pH?

A

The more OH- ions, the more alkaline the solution

21
Q

How is concentration calculated?

A

Amount dissolved ➗ volume of solution

Units: trams per decimetre cubed , gdm to the power of -3

22
Q

What is the difference, in terms on concentration of H➕ ions, between a pH 3 and 5?

A

100 H➕ ions (each pH is x10)

23
Q

Complete the sentence: strong acids …………… completely in water while weak acids ……….

A

Dissociate, don’t

24
Q

What are all aqueous solutions?

A

Either acidic, alkaline or neutral

25
Q

Explain why a strong acid could have the same pH as a weak acid

A

If the strong acid is dilute and the weak acid is concentrated, it just depends on the amount of H➕ ions

26
Q

What is a base?

A

Bases are substances that neutralise acids to form a form a salt and water only

27
Q

What is the general reaction for a metal oxide and an acid?

A

(Metal) salt ➕ water

28
Q

How do we name the salts formed from reactions with the 3 most common acids used?

A

Chloride
Nitrate
Sulphate

29
Q

List the steps in making a soluble salt from a neutralisation reaction

A

Go to page 57 in the text book and look ,

30
Q

Explain why the base is added in excess, the acid is warmed and the excess is filtered

A

The base is added in excess so it will all react with the acid and there will be none left
The acid is warmed so the reaction will happen faster
The excess is filtered so it’s just a clear liquid solution

31
Q

What is the difference between a base and an alkali?

A

Many bases are insoluble ( but they can be soluble) alkalis are soluble, and bases that are soluble are alkalis

32
Q

How are group 1 hydroxides different to most metal oxides?

A

Group 1 hydroxides have 1- charge, but group 2 has a 2➕ charge and etc

33
Q

What is the ionic equation that explains why a neutral solution is formed when an acid and an alkali neutralise each other

A

H➕(aq) ➕ OH-(aq) ➡️ H2O(l)

34
Q

Why do we use a titration so to form a dry soluble salt?

A

Easy, reliable way, gets good crystals

35
Q

List the steps in carrying out such a reaction (titration)

A

Add excess oxide to acid
Warm up solution to speed up reaction
Filter to remove the unreacted solid from the solution
Heat up to evaporate water and concentrate salt solution
Leave water to evaporate slowly and for crystallisation to occur

36
Q

What is the general equation for the reaction between metals and acids? Give an example

A

Metal ➕ acid ➡️ metal salt ➕ hydrogen
Lithium ➕ hydrochloric acid ➡️ lithium chloride ➕ hydrogen
2Li ➕ 2HCl ➡️ 2LiCl ➕H2

37
Q

What is a spectator ion?

A

Ions that don’t change during a reaction

38
Q

In terms of half equations, what happens to the H➕ ions! Show the equation

A

The hydrogen ions gain electrons to form hydrogen molecules

2H➕ (aq) ➕ 2e ➡️ H2(g)

39
Q

In terms of half equations, what happens to the metal ions? Give an example

A

Mg(s) ➡️ Mg2➕(aq) ➕ 2e

The magnesium atoms lose 2 electrons. A loss of electrons is an oxidation reaction. A gain of electrons is a reduction

40
Q

Describe the test for hydrogen gas?

A

You put hydrogen gas and cotton wool in the bottom of a tube, then put a lit splint in the, if the gas is present it will pop

41
Q

What is the general equation for the reaction between acids and metal carbonates? Give an example

A

Metal carbonate ➕ acid ➡️ metal salt ➕ water ➕ Carbon dioxide
CuCO3(s) ➕ H2SO4 ➡️ CuSO4(aq) ➕ H2O(l) ➕ CO2(g)

42
Q

Describe the test for carbon dioxide gas?

A

Bubble it through limewater, it will turn limewater from clear and colourless to milky

43
Q

What is a precipitate?

A

An insoluble product formed when solutions of the two soluble reactants are mixed

44
Q

Write a list of the compound that are insoluble in water

A

Most carbonates - silver carbonate, barium carbonate

Most hydroxides - ion hydroxide, zinc hydroxide

45
Q

Describe the steps in the preparation of insoluble salts

A

Go to page 69 in text book and look

GCSE Chemistry 1 paper 1 (8 decks)

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