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Chem > Chap 8 - Acids, bases & salts, ionic equations, preparing salts > Flashcards

Chap 8 - Acids, bases & salts, ionic equations, preparing salts Flashcards

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1
Q

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

A

-acid - red
base - blue

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2
Q

3 kinds of indicators

A

-universal indicator
-methyl orange solution
-phenolphthalein

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3
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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4
Q

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

A

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

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5
Q

3 common acids/ strong acids

A

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

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6
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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7
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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8
Q

what is pH

A

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

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9
Q

define strength

A

-how much compound dissociated in a liquid

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10
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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11
Q

define alkaline

A

water soluble base

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12
Q

define acid & base

A

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

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13
Q

define concentration

A

amount of compounds in a given volume

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14
Q

pH of acid, neutral, alkaline

A

acid - <7
neutral - 7
base - >7

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15
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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16
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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17
Q

why are H+ ions called protons

A

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

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18
Q

formula for concentration

A

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

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19
Q

define metalloids

A

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

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20
Q

pH of metal oxides, hydroxides & carbonates

A

basic

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21
Q

pH of non- metal oxides, hydroxides & carbonates

A

acidic

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22
Q

define amphoteric & eg.

A

-substance can react as basic & acidic
-Zinc & Aluminum oxides

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23
Q

define neutral oxides & eg.

A

-substances that don’t react with acids or bases
-eg. carbon monoxide CO, dinitrogen oxide N2O

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24
Q

define corrosive

A

break down of substance

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25
Q

ammonia & ammonium ion symbol

A

ammonia - NH3 - alkaline
ammonium ion - NH4+

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26
Q

note: reactions with acids & bases usually happens in water - so aqueous

A
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27
Q

neutralization reaction

A

acid + base -> neutral salt + water

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28
Q

what type of salts are ammonium salts

A

weak adics

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29
Q

define spectator ion

A

ion which charge remains same in reaction

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30
Q

how to do ionic equations

A

-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

31
Q

is neutralization a redox reaction, why

A

no, oxidations states aren’t changed

32
Q

note: oxidation state & charge is same except for polyatomic ions

A
33
Q

requirement for metals to react with acid

A

-metal must be more reactive than hydrogen to react with acid & displace Hydrogen

34
Q

2 weak acid & base

A

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

35
Q

3 ways to make salt

A

-titration - soluble acid & base
-excess solid method - insoluble base/ metal + acid ( 1 of reactant is insoluble)
-precipitation method - insoluble salt

36
Q

titration process

A

-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

37
Q

excess solid method

A

-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

38
Q

why is substance put in excess for excess solid method

A

so all acid particles react

39
Q

what to add if want to decolourise solution

A

-add decolourising charcoal

40
Q

precipitation method

A

-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

41
Q

what is 1 mole equal to

A

-1 mole = 6.02 x 10^23
-no. molecules in a mole

42
Q

moles formmula

A

atomic mass/ atomic no.

43
Q

where is neutralization used in & what bases used

A

neutralize acidic soil to grow plants
eg. CaO, Ca(OH)2, CaCO3

44
Q

how is ammonia gas created using ammonium chloride

A

-thermal decomposition
-heat ammonium chloride NH4Cl

45
Q

define thermal decomposition reaction

A

when heating 1 reactant gives many products

46
Q

are they soluble:
1 -all G1 compounds, sodium, potassium, ammonium salts
2 -all nitrates
3 -all chlorides
4 -all sulfates
5 - all hydroxides & carbonates

A

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

47
Q

insoluble compounds:

A

-silver & lead chloride
-calcium, barium & lead sulfates
-all hydroxides & carbonates except sodium, potassium & ammonium

48
Q

how to decide which method to make salt

A

-is salt soluble?
-yes
-are reactants soluble?
-yes; titration
-no; excess solid method
-no; precipitation

49
Q

reactions with acids

A

-metal (solid) + acid
-metal oxide + acid
-metal hydroxide + acid
-meta carbonate + acid

50
Q

reaction with bases

A

-acid + base
-base + ammonium salt - salt + ammonia (g) + water

51
Q

gas tests:
-hydrogen
-oxygen
-carbon dioxide
-ammonia (alkaline)
-chlorine

A

-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

52
Q

define cations & anions

A

cations - positively charged metal ions
anions - negatively charged non - metal ions

53
Q

test for cations: flame test (colour of flame)
-lithium
-sodium
-potassium
-calcium
-copper

A

-lithium - red
-sodium - yellow
-potassium - purple
-calcium - orange
-copper - green

54
Q

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+ )

A

-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

55
Q

note: precipitate short form - ppt
define ppt

A

solid insoluble product

56
Q

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+ )

A

-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

57
Q

test for anions:
-carbonate CO3 ( 2- )
-chloride Cl ( - )
-bromide Br ( - )
-iodide I ( - )
-nitrate NO3 ( - )
-sulfate SO4 ( 2- )
-sulfite SO3 ( 2- )

A

-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 & Br(NO3)2 (aq), forms white ppt
-sulfite - add dilute HCl, warm & gently, SO2 produced turns acidified potassium manganate purple to colourless

58
Q

define anhydrous

A

-contains no water

58
Q

note: rinse ppt. in distilled water to make sample pure

A
59
Q

what are hydrated salts

A

-salts containing water
-written as: salt formula. (no.) H2O

60
Q

are all salts neutral

A

-mostly
-unless: strong acid/ base + weak acid/ base

61
Q

note: not all metals react with acids
give eg.

A

-Au, Ag, Cu, Pt

61
Q

how to find density of element

A

-look at atomic mass of element

62
Q

formula for ethanol

A

C2H6O

62
Q

difference btw concentration & strength

A

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

62
Q

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

A
63
Q

define standard solution

A

-solution containing an accurately known concentrations of an element/ compound

64
Q

uses of lighted splint to find H2, O2, CO2

A

H2 - sqeuaky pop
O2 - splint will relight
CO2 - light in splint will die

64
Q

how to find concentration, mass / volume of compound added

A

-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 ____

65
Q

note: gold, silver, copper, platinum doesn’t react with dilute acids because they’re lower than H2 in reactivity series

A
66
Q

note: to know which reactant to put in excess, check states of products & if you can separate them later

A
67
Q

note: to find evidence that solution contains a compound, find tests for the specific elements in the compound

A
68
Q

note: CaO (lime), Ca(OH)2 (slaked lime), CaCO3 (limestone) can be used to neutralise acidic soil

A
69
Q

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

A

-basic
-acidic

Chem (10 decks)

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