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Chemistry GCSE > C8 ACIDS AND ALKALIS > Flashcards

C8 ACIDS AND ALKALIS Flashcards

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1
Q

pH scale

A

A scale running from 0-14 that measures how acid or alkaline a solution is

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2
Q

Acid

A

A solution with a pH less than 7

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3
Q

Alkali

A

A substance with pH greater than 7

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4
Q

Neutral

A

A substance with a pH equal to 7

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5
Q

Indicator

A

A substance that changes colour depending on the pH

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6
Q

Common indicators

A

Litmus:red in acid, blue in alkali
Methyl orange: red in acid, orange alkali
Phenolphthalein: colourless in acid, pink in alkali

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7
Q

Universal indicator

A

A mixture of serval indicators that is red in strong acids, green when neutral and purple in strong alkali

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8
Q

Acids and ions

A

Acids dissolve in water to produce an excess of hydrogen ions H+

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9
Q

Alkalis and ions

A

Alkalis dissolve in water to produce an excess of hydroxide ions OH-

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10
Q

Hydrochloric acid

A

Formula: HCL
hydrogen ions formed: 1
Anion formed: chloride CL-

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11
Q

nitric acid

A

formula : HNO3
hydrogen ions formed: 1
anion formed: nitrate, NO3

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12
Q

sulfuric acid

A

formula: H2SO4
hydrogen ions formed: 2
anion formed: sulfate, SO42-

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13
Q

ions and pH

A

the higher the hydrogen ion concentration the lower the pH the higher the hydroxide ion concentration , the higher the pH

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14
Q

concentrated solution

A

a solution with a large amount of solute dissolved in a given volume

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15
Q

dilute solution

A

a solution with a small amount of solute dissolved in a given volume

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16
Q

pH and hydrogen ion concentration

A

every step down the pH scale is a ten-fold increase in hydrogen ion concentration and vice versa
pH 3 to 1 = 100 times increase
ph 4 to 7 = 1000 times decrease

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17
Q

dissociation

A

when an acid dissolves in water, it splits up into positive hydrogen ions and negative anions

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18
Q

strong acids

A

acids that dissociate fully when dissolved in water, every single molecule splits up

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19
Q

weak acids

A

acids that do not fully dissociate when dissolved in water, only some molecules split up

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20
Q

acid examples

A

strong : hydrochloric, sulfuric

weak : ethanoic

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21
Q

properties of strong acids

A

strong acids react more quickly than weak acids because there are more hydrogen ions available for reactions

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22
Q

base

A

a substance that neutralises an acid to form a salt and water

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23
Q

salt

A

a compound formed from the metal cation of a base and the non-metal anion of an alkali

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24
Q

naming salts

A

two part names . first part = the metal from the base , second part = the anion from the acid

25
Q

acids and their anions

A

sulfuric acid - sulfate
nitric acid - nitrate
hydrochloric acid - chloride

26
Q

reaction of metal oxides with acid

A

metal oxide + acid - salt + water

e.g magnesium oxide + hydrochloric acid - magnesium chloride

27
Q

preparing soluble salts

A

gently warm a beaker of acid
add a spatula of metal oxide and stir until dissolved
repeat until it no longer dissolves
filter to remove excess oxide
allow water to evaporate to produce pure crystals

28
Q

bases and alkalis

A

a base is a substrate that neutralises an acid to form a salt and water. an alkali is a base that is soluble in water

29
Q

common alkalis

A

sodium hydroxide , NaOH
potassium hydroxide , KOH
calcium hydroxide , Ca(OH)2

30
Q

reaction of alkalis with acids

A

acid + alkali - salt + water

eg.
sodium hydroxide nitric acid - sodium nitrate + water
NaOH(aq) + HNO3(aq) - NaNO3(aq) + H2O(L)

31
Q

balancing equations

A

use a tally chart to keep track of the number of atoms on each side.
change the coefficients (the big numbers) to add more of things that are missing
DO NOT TOUCH THE LITTLE NUMBERS

32
Q

acid and alkali ions

A

acids produced hydrogens ions H+, alkalis produced hydroxide ions , OH-

33
Q

ions and neutralisation

A

the H+ ion and OH- ion react together to form H2O (water)

34
Q

producing a salt by neutralisation

A

the salt is produced from the ions left over once the H+ and OH- ions have reacted together

35
Q

burette

A

a tall glass tube with 0.1cm3 markings on it and a tap at the bottom used for accurately adding variable amounts of liquid

36
Q

pipette

A

a piece of glassware used to very accurately measure a fixed amount of liquid

37
Q

titration

A

a method used to find out exactly how much acid is needed to neutralise an alkali

38
Q

titration metod

A

add alkali to beaker with a pipette
add an alkali to the beaker
gradually add acid from a burette
note how much has been added at the point of neutralisation

39
Q

titration indicators

A

use indicators with a sharp colour change - such as phenolphthalein - rather than a gradual one such as universal

40
Q

reaction of acid with metals

A

metal + acid - salt + hydrogen

41
Q

metal and acid observations

A

bubbles of hydrogen
metal dissloves
warms up

42
Q

ionic equation

A

a chemical equation that shows changes to the ions in a reaction

43
Q

ionic equation for magnesium and acid

A

mg+2H+ -> MG2+ +H2

44
Q

Spectator ion

A

an ion that does not change during a chemical reaction

45
Q

half equations

A

an equation that shows what happens to just one of the ions during chemical reaction. two half equations combine to give the overall ionic equation

46
Q

half equation examples

A

mg -> MG2+ +2e
2H+ +2e- - H2

combine to give:
MG + 2H+ - MG2+ +H2

47
Q

reaction of metal carbonates with acid

A

carbonate + acid -> salt + water + carbon dioxide

48
Q

carbonate and acid observations

A

bubbles of CO2 gas

solid carbonate dissolves

49
Q

carbonate and acid ionic equation

A

2H+ +CO3’2- - H20 +CO2

50
Q

soluble

A

when a substance can be dissolved by a liquid

51
Q

insoluble

A

when a substance cannot be dissolved by a liquid

52
Q

soluble in water

A 
all common sodium
potassium and ammonium salts
all nitrates 
most chlorides 
most sulfates
53
Q

insoluble in water

A

sliver and lead chlorides
lead, barium and calcium sulfates
most carbonates
most hydroxides

54
Q

precipitate

A

a solid (insoluble) product formed by mixing two solutions. turns the solution cloudy

55
Q

precipitate reaction

A

a reaction that produces a solid precipitate by mixing two solutions

56
Q

predicting precipitate

A

when mixing two solutions, swap the names of the salts around to find the possible products. if one is insoluble a precipitate forms

57
Q

predicting equations

A

AB + YX - AX + YB

eg
sodium chloride + sliver nitrate - silver chloride + sodium

58
Q

precipitation ionic equations

A

only include the ions that make that solid precipitate

59
Q

to prepare insoluble salts

A

mix your two solutions
filter the mixture
wash the residue by pouring distilled water through the filter
leave somewhere warm to dry

Chemistry GCSE (8 decks)

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