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Chemistry GCSE > C8 ACIDS AND ALKALIS > Flashcards

C8 ACIDS AND ALKALIS Flashcards

(59 cards)

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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

Study These Flashcards
A

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

25
acids and their anions
sulfuric acid - sulfate nitric acid - nitrate hydrochloric acid - chloride
26
reaction of metal oxides with acid
metal oxide + acid - salt + water e.g magnesium oxide + hydrochloric acid - magnesium chloride
27
preparing soluble salts
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
bases and alkalis
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
common alkalis
sodium hydroxide , NaOH potassium hydroxide , KOH calcium hydroxide , Ca(OH)2
30
reaction of alkalis with acids
acid + alkali - salt + water eg. sodium hydroxide nitric acid - sodium nitrate + water NaOH(aq) + HNO3(aq) - NaNO3(aq) + H2O(L)
31
balancing equations
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
acid and alkali ions
acids produced hydrogens ions H+, alkalis produced hydroxide ions , OH-
33
ions and neutralisation
the H+ ion and OH- ion react together to form H2O (water)
34
producing a salt by neutralisation
the salt is produced from the ions left over once the H+ and OH- ions have reacted together
35
burette
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
pipette
a piece of glassware used to very accurately measure a fixed amount of liquid
37
titration
a method used to find out exactly how much acid is needed to neutralise an alkali
38
titration metod
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
titration indicators
use indicators with a sharp colour change - such as phenolphthalein - rather than a gradual one such as universal
40
reaction of acid with metals
metal + acid - salt + hydrogen
41
metal and acid observations
bubbles of hydrogen metal dissloves warms up
42
ionic equation
a chemical equation that shows changes to the ions in a reaction
43
ionic equation for magnesium and acid
mg+2H+ -> MG2+ +H2
44
Spectator ion
an ion that does not change during a chemical reaction
45
half equations
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
half equation examples
mg -> MG2+ +2e 2H+ +2e- - H2 combine to give: MG + 2H+ - MG2+ +H2
47
reaction of metal carbonates with acid
carbonate + acid -> salt + water + carbon dioxide
48
carbonate and acid observations
bubbles of CO2 gas | solid carbonate dissolves
49
carbonate and acid ionic equation
2H+ +CO3'2- - H20 +CO2
50
soluble
when a substance can be dissolved by a liquid
51
insoluble
when a substance cannot be dissolved by a liquid
52
soluble in water
``` all common sodium potassium and ammonium salts all nitrates most chlorides most sulfates ```
53
insoluble in water
sliver and lead chlorides lead, barium and calcium sulfates most carbonates most hydroxides
54
precipitate
a solid (insoluble) product formed by mixing two solutions. turns the solution cloudy
55
precipitate reaction
a reaction that produces a solid precipitate by mixing two solutions
56
predicting precipitate
when mixing two solutions, swap the names of the salts around to find the possible products. if one is insoluble a precipitate forms
57
predicting equations
AB + YX - AX + YB eg sodium chloride + sliver nitrate - silver chloride + sodium
58
precipitation ionic equations
only include the ions that make that solid precipitate
59
to prepare insoluble salts
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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