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Chem > C7 - Acids, bases & salts (ionic equations, preparing salts) > Flashcards

C7 - Acids, bases & salts (ionic equations, preparing salts) Flashcards

1
Q

type of bonding in acids & bases & salts

A

acid - covalent - shared pair of e btw non-metals; attraction of protons & e
base - ionic - transfer of e btw metal & non- metal; electrostatic force of attraction btw (+) & (-) ions
salts - ionic

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2
Q

acidic or basic:
-metal oxides
-non- metal oxides

A

-basic
-acidic

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3
Q

what colour does litmus paper turn under acid & alkaline (need to be soluble)

A

-acid - red
base - blue

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4
Q

3 kinds of indicators

A

-universal indicator
-methyl orange solution
-phenolphthalein

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5
Q

base colour for
-universal indicator
-methyl orange solution
-phenolphthalein

A

-universal indicator - blue
-methyl orange solution - yellow
-phenolphthalein - dark pink

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6
Q

acid colour for
-universal indicator
-methyl orange solution
-phenolphthalein

A

-universal indicator - red
-methyl orange solution - red
-phenolphthalein - colourless

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7
Q

3 common acids/ strong acids

A

-hydrochloric acid HCL
-sulfuric acid H2SO4
-nitric acid HNO3

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8
Q

3 common bases/ weak acids

A

-Sodium hydroxide NaOH
-Potassium hydroxide KOH
-Calcium hydroxide Ca (OH)2
-eg. Magnesium hydroxide

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9
Q

2 weak acid & base

A

acid:
-ethanoic acid
-citric acid
base:
-ammonia hydroxide

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10
Q

what is pH

A

-measure of acidity
-1 pH change = 10^1 times [H+ ions]

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11
Q

define strength

A

-how much compound dissociated in a liquid

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12
Q

difference btw strong & weak acids/bases

A

-strong: dissociated fully in water eg. HCl -> H+, Cl-
-weak: dissociated partially in water

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13
Q

define concentration

A

amount of compounds in a given volume

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14
Q

formula for concentration

A

-mass/ volume
- g / (d/c)m3 = g(d/c)m3

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15
Q

difference btw concentration & strength

A

-more con. more H+ ions, more products
-stronger, faster rate of reaction

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16
Q

define alkaline

A

water soluble base

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17
Q

define acid & base

A

acid - proton donners; source of H+ ions
base - proton acceptors; source of OH- ions

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18
Q

why are H+ ions called protons

A

-e is given away
-only neutron & proton in nucleus
-proton had + charge

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19
Q

relationship btw pH & ions

A

-higher the concentration of H+ ions, lower the pH
-higher the concentration of OH- ions, higher the pH

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20
Q

pH of acid, neutral, alkaline

A

acid - <7
neutral - 7
base - >7

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21
Q

pH of metal oxides, hydroxides & carbonates

A

basic

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22
Q

pH of non- metal oxides, hydroxides & carbonates

A

acidic

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23
Q

define solute, solvent, solution

A

solute - substance which dissolved in solvent
solvent - substance which solute dissolves in
solution - mixture of solute & solvent

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24
Q

define metalloids

A

-non- metals with metallic properties
eg. boron, silicon

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25
define amphoteric & eg.
-substance can react as basic & acidic -Zinc & Aluminum oxides
26
define neutral oxides & eg.
-substances that don't react with acids or bases -eg. carbon monoxide CO, dinitrogen oxide N2O
27
define corrosive
break down of substance
28
note: reactions with acids & bases usually happens in water - so aqueous
29
requirement for metals to react with acid
-metal must be more reactive than hydrogen to react with acid & displace Hydrogen
30
neutralization reaction
acid + base -> neutral salt + water
31
is neutralization a redox reaction, why
no, oxidations states aren't changed
32
where is neutralization used in & what bases used
neutralize acidic soil to grow plants eg. CaO, Ca(OH)2, CaCO3
33
define thermal decomposition reaction
when heating 1 reactant gives many products
34
ammonia & ammonium ion symbol
ammonia - NH3 - alkaline ammonium ion - NH4+
35
what type of salts are ammonium salts
weak adics
36
how is ammonia gas created using ammonium chloride
-thermal decomposition -heat ammonium chloride NH4Cl
37
define spectator ion
ion which charge remains same in reaction
38
how to do ionic equations
-must in aqueous -solid, liquid & gas are 0 chagre unless aqueous -single elements are 0 charge -water is 0 charge -balance equation -cancel spectator ions -balance charges
39
note: oxidation state & charge is same except for polyatomic ions
40
3 ways to make salt
-titration - soluble acid & base -excess solid method - insoluble base/ metal + acid ( 1 of reactant is insoluble) -precipitation method - insoluble salt
41
how to decide which method to make salt
-is salt soluble? -yes -are reactants soluble? -yes; titration -no; excess solid method -no; precipitation
42
titration process
-add acid to burette -add acid to alkaline until indicator changes colour & calculate volume of acid added -transfer solution to evaporating basin & heat to evaporate water -uses burette & pipette
43
excess solid method
-Heat acid & react it with excess metal/ base/ carbonate -filter mixture to remove excess solid -heat filtrate to evaporate until crystals form eg. H2SO4 & CuO
44
why is substance put in excess for excess solid method
so all acid particles react
45
what to add if want to decolourise solution
-add decolourising charcoal
46
precipitation method
-2 soluble solutions are mixed -filter the precipitate -wash salt with distilled water -filter again to deionize salt -heat it eg, NaCl + AgNo3 - white precipitate, KI + AgNO3 - yellow ppt
47
what is 1 mole equal to
-1 mole = 6.02 x 10^23 -no. molecules in a mole
48
are they soluble: 1 -all G1 compounds, sodium, potassium, ammonium salts 2 -all nitrates 3 -all chlorides 4 -all sulfates 5 - all hydroxides & carbonates
1 - soluble 2 - soluble 3- all soluble except silver & lead chloride 4 - all soluble except calcium, barium & lead 5 - all insoluble except sodium, potassium & ammonium
49
insoluble compounds:
-silver & lead chloride -calcium, barium & lead sulfates -all hydroxides & carbonates except sodium, potassium & ammonium
50
reactions with acids
-metal (solid) + acid -> salt + hydrogen -metal oxide + acid -> salt + water -metal hydroxide + acid -> salt + water -meta carbonate + acid -> salt + water + carbon dioxide -base + acid -> neutral salt + water
51
reaction with bases
-acid + base -base + ammonium salt - salt + ammonia (g) + water
52
gas tests: -hydrogen -oxygen -carbon dioxide -ammonia (alkaline) -chlorine
-hydrogen - lit splint combusts with squeaky pop -oxygen - glowing splint will relight -carbon dioxide - limewater turn cloudy -ammonia - damp red litmus paper turns blue, has pungent smell -chlorine - damp blue litmus paper turns red before bleaching it white
53
define cations & anions
cations - positively charged metal ions anions - negatively charged non - metal ions
54
test for cations: flame test (colour of flame) -lithium -sodium -calcium -potassium -copper
-lithium - red -sodium - yellow -calcium - orange -potassium - lilac -copper - green
55
test for aqueous cations: reacting with NaOH (aq) in detail (all gives ppt except NH4) -ammonium ion ( + ) -aluminum ion ( 3+ ) -zinc ion (2+ ) -calcium ion (2+ ) -copper ion (2+ ) -chromium ion ( 3+ ) -iron (II) ion (2+ ) -iron (III) ion (3+ )
-ammonium ion - ammonium salt + base = damp red litmus paper turns blue -aluminum ion - white ppt, soluble in excess giving colourless solution -zinc ion - white ppt, soluble in excess giving colourless solution -calcium ion - white ppt, insoluble in excess -copper ion - light blue ppt, insoluble in excess -chromium ion - green ppt, soluble in excess -iron (II) ion - green ppt, insoluble in excess -iron (III) ion - red - brown ppt, insoluble in excess
56
note: precipitate short form - ppt define ppt
solid insoluble product
57
test for aqueous cations: reacting with NH3 (aq) -ammonium ion ( + ) -aluminum ion ( 3+ ) -zinc ion (2+ ) -calcium ion (2+ ) -copper ion (2+ ) -chromium ion ( 3+ ) -iron (II) ion (2+ ) -iron (III) ion (3+ )
-ammonium ion - nothing -aluminum ion - white ppt, insoluble in excess -zinc ion - white ppt, soluble in excess giving colourless solution -calcium ion - no ppt or slightly white -copper ion - light blue ppt, soluble in excess a giving dark blue solution -chromium ion - grey - green ppt, insoluble in excess -iron (II) ion - green ppt, insoluble in excess -iron (III) ion - red - brown ppt, insoluble in excess
58
test for anions: -carbonate CO3 ( 2- ) -chloride Cl ( - ) -bromide Br ( - ) -iodide I ( - ) -nitrate NO3 ( - ) -sulfate SO4 ( 2- ) -sulfite SO3 ( 2- )
-carbonate - add dilute HCl - CO2 produced makes limewater cloudy -chloride - add HNO3 & AgNO3 (aq), forms white ppt -bromide Br - add HNO3 & AgNO3 (aq), forms cream ppt -iodide - add HNO3 & AgNO3 (aq), forms yellow ppt -nitrate - add NaOH (aq) & Al, NH3 produced makes damp red litmus paper blue -sulfate - add HNO3 & Ba(NO3)2 (aq), forms white ppt -sulfite - add dilute HCl, warm & gently, SO2 produced turns acidified potassium manganate purple to colourless
59
note: rinse ppt. in distilled water to make sample pure
60
what are hydrated salts
-salts containing water -written as: salt formula. (no.) H2O
61
note: not all metals react with acids give eg.
-Au, Ag, Cu, Pt
62
note: -acids can't react with acids, bases can't react with bases -neutral compound/ noble gases don't react -reactions with acids & bases usually happens in water - so aqueous, unless with metal (solid) + acid or ppt is formed -no colour = colourless -sugar is neutral -CO2 is an acidic oxide -CO3 is a weak base -H2 is flammable -carbonic acid H2CO3 -all lead salts are insoluble -iodide compounds are usually yellow -any metal compounds except transition metal compounds are white (including ppt.) -oxides are formed with steam, OH are formed with water -Chlorine is acidic -when I2 element is heat, sublimation happens, turns into a purple vapor -copper compounds are blue usually -to get hydrated salt, wash then heat
63
define standard solution
-solution containing an accurately known concentrations of an element/ compound
64
uses of lighted splint to find H2, O2, CO2
H2 - sqeuaky pop O2 - splint will relight CO2 - light in splint will die
65
how to find concentration, mass / volume of compound added
-formula -write which part you have -find the remaining part for reactant 1 -write balanced formula for reaction -find ratio of reactants -multiply as needed -find the missing part of the equation for reactant 2 -[ compound formula ] = concentration of ____
66
note: gold, silver, copper, platinum doesn't react with dilute acids because they're lower than H2 in reactivity series
67
note: to know which reactant to put in excess, check states of products & if you can separate them later
68
note: to find evidence that solution contains a compound, find tests for the specific elements in the compound
69
note: CaO (lime), Ca(OH)2 (slaked lime), CaCO3 (limestone) can be used to neutralise acidic soil

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