acid bases salts Flashcards by ppopotamus .

acids & alkalis can dissociate to form

free mobile ions

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ensuring acid is all used up to get ___________ yield

highest

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bronsted-lowry theory
base def: substance that can ___________ a ________ (H+) from another substance

accept, proton

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brontsted-lowry theory
acid def: is _________________ that can __________ a proton (____) to another ________________

substance, donate, H+, substance

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when in same eqn/ paired with acid, water becomes _______

base

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acids only behave like an acid when dissolved in ________; if in organic solvent —___ reaction

water, no

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bases: ______ _________& ______ ________________

metal oxides, metal hydroxides

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alkalis: ________ that are_________ in water & produces ______

bases, soluble, OH-

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common acids:____,_____, CH3CO2H (____________ acid)

HCl, H2SO4, ethanoic

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common alkalis: ______, _____ (aqueous ammonia)

NaOH, NH3

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acids & bases can be classified as strong/weak in terms of their ________of ______________ to give ions in solution

extent, dissociation

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STRONG ACID
def: one which _______________ _________ in solution to give _________ (H+)

dissociates fully, protons

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STRONG ACID
degree of dissociation:

100%

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STRONG ACID
type of arrow used in dissociation eqn:

single arrow (–>)

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STRONG BASE
def:_____________ __________ in solution to give ____________ ions (OH-)

dissociates fully, hydroxide

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strong & weak acids can be _____basic or ___basic

mono, di

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STRONG BASE
degree of dissociation:

100%

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WEAK ACID
def: _____________ ______________ in solution to give ________(H+)

dissociates partially, protons

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WEAK ACID
degree of dissociation:

<100%

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WEAK ACIDS
egs: __________ acids (containing ________) are generally weak acids

organic, -COOH

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WEAK BASE
def: _______________ _____________ in solution to give ____________ ions (OH-)

dissociates partially, hydroxide

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WEAK ACID
type of arrow used:

reversible arrow (⇌)

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WEAK BASE
type of arrow:

reversible arrow (⇌)

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WEAK BASE egs

ammonia (NH3)

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strength of acid: ___________ of _________ (fully/partially) of dissociation of an acid in solution

measure, extent

conc. of acid: ______of ________ of __________________ acid per unit vol.

no., moles, undissociated

strength of acid/base is ________________ of its conc

INDEPENDENT

if a lot of H2O molecules means _____ conc of acid/base

low

HA is generic name for any ______

acid

Power of Hydrogen (pH) def: ___________ ______ to the base ____ of the conc of hydrogen ions in ________

negative log, 10, mol/dm3

pH =

-log[H+]

[H+] =

10^-pH

[ ] means:

conc of thing inside [ ]

larger the pH value (more alkaline), _________ the [H+]

smaller

more acidic means ______ [H+]

at temps of 25 degree celsius, NEUTRAL solution: [H+]___[OH-], pH__7

=, =

at temps of 25 degree celsius, ACIDIC solution: [H+]___[OH-], pH__7

>, <

at temps of 25 degree celsius, ALKALINE solution: [H+]___[OH-], pH__7

<, >

universal indicator: ____________ of dyes that can be used to estimate _____ of a solution by tallying ________ of solution with _______________________________

mixture, pH, colour, universal colour chart

COMMON INDICATORS USED IN TITRATION: SCREENED METHYL ORANGE pH range for colour change: __-__ colour in acidic: colour in alkaline:

- 3, 5 - magenta - green

COMMON INDICATORS: LITMUS pH range at which indicator changes colour: __-__ colour in acidic solution: ____ colour in alkaline solution: ____

- 5, 8 - red - blue

COMMON INDICATORS USED IN TITRATION: METHYL ORANGE pH range for colour change: __-___ colour in acidic: _____ colour in alkaline: _______

- 3, 4.4 - red - yellow

COMMON INDICATORS USED IN TITRATION: THYMOL BLUE pH range for colour change: __-___ colour in acidic: colour in alkaline:

- 8, 9.6 - yellow - blue

PROPERTIES OF ACIDS pH:

less than 7

COMMON INDICATORS USED IN TITRATION: PHENOLPHTALEIN pH range for colour change: __-___ colour in acidic: colour in alkaline:

- 8, 10 - colourless - pink

PROPERTIES OF ACIDS taste:

sour

PROPERTIES OF ACIDS turns ______ blue _______ paper ____ turns ________________________ _________/____

- damp, litmus, red - universal indicator, orange/red

PROPERTIES OF ACIDS can ___________ ______________ (can act as charge carriers as they exist as ________________________ in _____________ solution)

conduct electricity, free mobile ions, acqueous

PROPERTIES OF ALKALIS taste: ________ & feel ________

bitter, soapy

PROPERTIES OF ALKALIS turn ______ red _______ paper _______ turn _____________________________ _____/________

- damp, litmus, blue - universal indicator, blue/violet

PROPERTIES OF ALKALIS pH:

more than 7

PROPERTIES OF ALKALIS can ____________ _____________ (can act as ________ ___________ as they exist as ____________________________ in aqueous solution)

conduct electricity, charge carriers, free mobile ions

in organic solvent, acid exists as a simple molecular compound ( ________ dissociate in organic solvents) —> no ______________________________ to act as _________________ so ____ electrical conductivity

doesn't, free mobile ions, charge carriers, no

neutralisation: reaction between acid and base to form _____ & _______

salt, water

Haber process: industrial method for ______________ of ______________ (a weak base in aqueous medium)

manufacture, ammonia

Haber process is a ____________ reaction

reversible

nature of OXIDE changes from _______ (metal oxides) to _____________ to ________ (non-metal oxides)

basic, amphoteric, acidic

operating conditions for haber process: - ______ pressure of ____ atm (atmospheric press. at sea level) - _______________ temp of ____ °C - _____ __________ - molar ratio of N2:H2 is __:__

- high, 250 - moderate, 450 - iron catalyst - 1:3

grp 13:___ (is _____________)

Al, amphoteric

basic OXIDES can react with ______ to form ______ & _________

acids, salt, water

amphoteric OXIDES can react with ______ ______ ___ ______ to form ______ & ________

both acids & bases, salt, water

acidic OXIDES can react with _______ to form _____& ______

bases, salt, water

grp 1 & 2 r ______ oxides & ______ in nature

metal, basic

BASIC OXIDES: reaction with water they're usually __________ in water but ____________ (_____) & _______________ (_____) are _________ in water to give _________ solution with pH _7

insoluble, sodium oxide (Na2O), potassium oxide (K2O), soluble, alkaline, >

BASIC OXIDES: reaction with water Na2O + H2O —> ________ K2O + H2O —> ________

- 2NaOH (sodium hydroxide) - 2KOH (potassium hydroxide)

BASIC OXIDES: reaction with acids ______ basic oxides can react with acids to give _____ & _______ eg Na2O + 2HCl —> 2NaCl + H2O

metal, salt, water

ACIDIC OXIDES grp ___,___, & ____ r ____________ oxides dat are acidic in nature

14, 15, 16, non-metal

ACIDIC OXIDES: reaction with water non-metal oxides r ______ oxides some acidic oxides _____ dissolve in _______ to form acidic solutions with pH__ 7

- acidic - can, water, <

ACIDIC OXIDES: reaction with water egs: SO2 + H2O —> SO3 + H2O —>

- H2SO3 (sulfurous acid) - H2SO4 (sulfuric acid)

AXIDIC OXIDES: reaction with bases they react with bases to form ______ & _______

salt, water

ACIDIC OXIDES : reaction with bases egs: P4O10 + 12 NaOH —> SO2 + 2NaOH —> SO3 + 2NaOH —>

- 4Na3PO4 (sodium phosphate) + 6H2O - Na2SO3 (sodium sulfite)+ H2O - Na2SO4 (sodium sulfate)+ H2O

ACIDIC OXIDES : reaction with bases egs: silicon dioxide (_____), (giant ___________ struc. with _____________ strong ___________ bonds), reacts with ________________ ____/_________ NaOH at _____ temp to form ________________ SiO2 (s) + 2NaOH (l) ———> ?? molten 350 °C

- SiO2, molecular, numerous, covalent, concentrated hot/molten, high, sodium silicate - Na2SiO3 (l) + H2O (g)

AMPHOTERIC OXIDES: reaction with water _____ react with water

DON'T

AMPHOTERIC OXIDES: reaction with acids & bases react to ______ (______ nature) to form ______ & _______

both, dual, salt, water

AMPHOTERIC OXIDES: reaction with acids & bases egs:

- aluminium oxide - lead(II) oxide - zinc oxide

AMPHOTERIC OXIDES: reaction with ACID eg of reaction:

Al2O3 (acts as basic oxide) + 6HCl —> 2AlCl3 (aluminium chloride)+ 3H2O

AMPHOTERIC OXIDES: reaction with BASE eg of reaction:

Al2O3 (acts as acidic oxide) + 2NaOH + 3H2O —> 2NaAl(OH)4 (hydrated sodium aluminate)

neutral oxides: ______ react with acids & bases pH__7

- don't - =

egs of neutral oxides

- carbon monoxide (CO) - water - nitric oxide (NO) - nitrous oxide (N2O)

salts r ______ ___________(eg NaCl)

ionic compounds

salts contain _______ ________ & ___________ ________

metal cation & non-metal anion

salts taht contain water of crystallisation are

hydrated

naming of hydrated salts eg: hydrated sodium carbonate (Na2Co3 · 10H2O) LHS is _____ RHS is water of crystallisation, in this case there’s ___ moles of water of crystallisation for every mole of Na2CO3

- salt - 10

salts that don't contain water of crystallisation are

anhydrous

water molecules _____________ bind to ions in salt crystals —> water bonded _____________ within crystal known as ____________________________

chemically, chemically, water of crystallisation

water of crystallisation can be driven off by __________ (energy to ______ chem bonds) crystals strongly to form _____________ salts (might also have colour _________)

heating, break, anhydrous, change

SOLUBILITY OF SALTS salts with grp 1 cations: ____ soluble in water

ALL

SOLUBILITY OF SALTS ammonium salts:____ soluble in water

ALL

SOLUBILITY OF SALTS - chloride salts: ____________________, _____________________________ INSOLUBLE in water, all other r _____________ - btw their halides (grp ___) are insoluble except for _________

- lead (II) chloride (PbCl2), silver chloride (AgCl), soluble - 17, flourides

SOLUBILITY OF SALTS nitrate salts: _____ soluble in water

ALL

SOLUBILITY OF SALTS sulfate salts: _____________________, _________________________, _____________________ INSOLUBLE in water, all other r ___________

calcium sulfate (CaSO4), lead (II) sulfate (PbSO4), barium sulfate (BaSO4), soluble

SOLUBILITY OF SALTS carbonate salts: _____________________, ______________________________ SOLUBLE, all others _______________

grp 1 carbonates, ammonium carbonate: (NH4)2CO3, insoluble

SOLUBILITY OF SALTS oxides & hydroxides: _____________ & ___________ __________, all others ____________

grp 1 oxides & hydroxides, soluble, insoluble

ALL SOLUBLE SALTS

- all grp 1 cations - all ammonium salts - all nitrate salts - chlorides except lead & silver chlorides - sulfates except Ca, Pb & Ba sulfates - grp 1 carbonates - ammonium carbonate, (NH4)2CO3 - grp 1 oxides & hydroxides

ALL INSOLUBLE SALTS

- lead (II) & silver chloride - lead (II) & silver halides (except flourides) - calcium, lead (II) & barium sulfates - carbonates except grp 1 & ammonium carbonate - oxides & hydroxides except grp 1 oxides & hydroxides

reactivity series most ------------------------------------>least reactive

K, Na, Ca, Mg, Al, Zn, Fe, Pb, H, Cu, Ag, Au

reactivity series everything above H: everything after H:

- reacts with acid - doesn't react with acid

reactivity series: ____, ____, ____ don't react with acids ____ ain't corrosive ____ & ____ r jewellery

Cu, Ag, Au Cu, Ag, Au

reactivity series: K vs Na K has more _______ -->electrons ___________ _______ --> ___________________ forces of attraction ___________ --> electrons _________ _______ --> _______ __________

shells, further away, elecrostatic, weaker, easily lost, more reacive

ACID-METAL reaction when _________ metal (located above H in reactivity series) reacts with ________ acid, ______ & ________________ r formed

reactive, dilute, salt, hydrogen gas

ACID-METAL reaction less reactive metals _________ H in reactivity series eg _______, _________ & ______ metal ______ react with dilute acids

below, Cu, Ag, Au, don't

ACID-METAL reaction simple formula:

acid + metal —> salt + hydrogen gas

ACID-METAL reaction extremely reactive metals eg _______ metals: __________, _____________ react ___________ & _____________ with dilute acids

grp 1, sodium, potassium, violently, explosively

ACID-(HYDROGEN)CARBONATE reaction when (hydrogen)/carbonate reacts with acid, _____, ________ & ________________ r formed

salt, water, carbon dioxide gas

ACID-(HYDROGEN)CARBONATE reaction simple formula

(hydrogen)/carbonate + acid —> salt + water + carbon dioxide gas

ACID-BASE reaction (neutralisation) simple formula

acid + base —> salt + water

ACID-BASE reaction (________________) egs of bases: ______ oxides & hydroxides, ____________ when acid reacts with base, _____ & ________ r formed

- neutralisation - metal, ammonia - salt & water

ACID-BASE reaction (neutralisation) when ammonia (weak ______) reacts with acid, _____ ______ is formed

base, only salt

ACID-AMMONIA reaction (_________________) simple formula

- neutralisation - acid + ammonia (NH3) —> salt ONLY

ALKALI-AMMONIUM SALT reactions when ammonium ______ warmed in presence of alkali, _____, _______ & ____________ _____ r formed

salt, salt, water, ammonia gas

ALKALI-AMMONIUM SALT reactions simple formula

ammonium salt(NH4+) + base (alkali) — (warmed)—> salt+ water + ammonia gas (NH3)

PRECIPITATION reactions forms ___________ salts (know from solubility table) thru _________ of 2 _________ (_____________) reagents

insoluble, mixing, soluble, aqueous

PRECIPITATION reactions when aqueous solution that contains ________ of an insoluble salt is _______ with an aqueous solution containing _______ of that salt, the _____________ salt will _______________ out of ___________

anion, mixed, cation, insoluble, precipitate, mixture

PRECIPITATION reactions to get the__________ salt: _______ _____ excess liquid into beaker, then the ___________ is the salt

insoluble, filter out, residue

prep of salts - soluble salt usually prepared from reactions with ______ - insoluble salt usually prepared by _________________________ ( _________ of 2 __________ salts)

- acids - precipitation method, mixing, soluble

reactions with acids: if salt to be prepared is ___________ in water while reactants ____________, salt can be prepared thru reaction of acid with excess _______/ ______ (insoluble)/ ______________ (insoluble)

insoluble, soluble, metal, base, carbonate

reaction of ACID & EXCESS METAL - metal + acid—> _____ + _____________ _____ - to produce salt that’s soluble in water, excess metal is use such that acid is _____________ used up (acid is ___________ reagent) - ___________ _____ escapes so only soluble salt & excess metal remains & they can be separated thru ______________

- salt, hydrogen gas - completely, limiting - hydrogen gas, filtration

reaction of ACID & EXCESS METAL (acid + metal —> salt + hydrogen gas) this method unsuitable for: - _____ ____________ metals eg Na & K cus they react ____________ with acids - metals ________ ____ in reactivity series eg _______ & __________ as they don’t react with dilute acids

- very reactive, violently - below H, copper, silver

reaction of ACID & EXCESS METAL experiment steps - add ________ metal to ________ acid in beaker & _____ constantly till ____ ______ metal __________ in acid - ______ to separate ________ metal —> salt collected as _________ & metal collected as __________ - heat _________ to evaporate water to _______________ salt solution to obtain ______________ solution of salt - on __________, metal _________ will form - ______ to get metal as _________ & wash it with abt __ _____ (cus salt is ___________—>can’t use too much water) of _____ distilled water to remove _____________ - dry ________ by pressing them between layers of ______ paper

- excess, dilute, stir, no more, dissolves - filter, excess, filtrate, residue - filtrate, concentrate, saturated - cooling, crystals - filter, residue, 1 drop, soluble, cold, impurities - crystals, filter

reaction of ACID + EXCESS INSOLUBLE BASE reaction between base (metal ______/ ___________) and acid acid + base (____________) —> _____ + _______

-oxides, hydroxides - insoluble, salt, water

reaction of ACID + EXCESS INSOLUBLE BASE experiment steps - add _______ base to acid in beaker & _____ constantly till ___ _____ base _________ in acid - ______ to separate _______ base from ___________ solution of salt, which is collected as _________ & base collected as ___________ - _____ the _________ to _____________ water to _______________ salt solution to get _______________ solution of salt - on __________, salt _________ forms - ________ to obtain salt _________ as _________ & wash them with abt __ _____ (salt is _____________) of ______ distilled water to remove ______________ - dry _________ by pressing them between layers of _______ paper

- excess, stir, no more, dissolves - filter, excess, aqueous, filtrate, residue - heat, filtrate, evaporate, concentrate, saturated - cooling, crystals - filter, crystals, residue, 1 drop, soluble, cold, impurities - crystals, filter

reaction of ACID + EXCESS INSOLUBLE CARBONATE carbonate (____________) + acid —> _____ + _________ + __________________

insoluble, salt, water, carbon dioxide gas

reaction of ACID + EXCESS INSOLUBLE CARBONATE experiment steps - add ________ carbonate to acid & _____ constantly till ___ ______ carbonate __________ in acid - ______ to separate ________ carbonate from ___________ solution of salt, which is collected as _________ & carbonate as ____________ - _____ the ________ to evaporate water to ______________ salt solution to get a ______________ solution of salt - on _________, salt ________ forms - ______ to obtain ________ as ____________ & wash them with abt __ _____ of ______ distilled water to remove ______________ - dry ________ by __________ them in between layers of _______ paper

- excess, stir, no more, dissolves - filter, excess, aqueous, filtrate, residue - heat, filtrate, concentrate, saturated - cooling, crystals - filter, crystals, residue, 1 drop, cold, impurities - crystals, pressing, filter

reaction of acid + SOLUBLE base/ carbonate but since it’s soluble there won’t be any remaining ___________ residue to show that reaction is complete, so use ____________: determines _______ vol. of alkali that reacts with known amt of acid in presence of an _____________

insoluble, titration, exact, indicator

alkalis are a

soluble base

when acids react with metal, metal will be _______ --> ___________, so must be in _________

solid, insoluble, excess

reaction of acid + SOLUBLE base/ carbonate - part a: get the vol of base needed for __________________ with use of an _______________ - part b: prepare salt __________ use of an ____________ (cus it might _____________ salt —> salt not _____)

- neutralisation, indicator - without, indicator, contaminate, pure

reaction of acid + SOLUBLE base/ carbonate TITRATION - fill __________ with dilute _______ & record reading (1st reading) - _________ ______cm3 of dilute ______ into a _____cm3 ________ _______ - add 1-2 drops of _____________ to acid & see og colour - add dilute base from _________ (____________ near end-point), til end-point colour ________ observed - record final _________ reading (2nd reading) - record amt of base needed for __________ neutralisation (1st reading - 2nd reading)

- burette, base - pipette, 25, acid, 250 conical flask - indicator - burette, drop-wise, change - burette - complete

reaction of acid + SOLUBLE base/ carbonate preparation of salt __________ use of indicator' - _________ _____cm3 of dilute ______ into _____cm3 beaker - add (_________________________)cm3 of dilute ______ (from __________) to acid - ______ reaction mixture in beaker to evaporate off water —> get a ____________ solution - let solution _____ ______ slowly & __________ of salt start to form (might need ice bath) - _______ off _________ (as __________) - wash them with ______ amt of ______ distilled water to remove ___________ - dry them between layers of ______ paper

- without - pipette, 25, acid, 250 - 1st reading - 2nd reading, base, burette - heat, saturated - cool down, crystals - filter crystals, residue - little, cold, impurities - filter

IONIC PRECIPITATION REACTION (for insoluble salts) have to choose 2 suitable _______ ____________ that when combined results in ______________ of wanted salt (need to ___________ any solid starting material to get __________ solution first)

ionic compounds, precipitate, dissolve, aqueous

IONIC PRECIPITATION REACTION (for insoluble salts) basically, take the salt, find ______ eqn of it, then choose 2 ______ ___________(each as 1 part of the salt) that can react with each other to give that salt & another compound but can ignore that

ionic, ionic compounds,

IONIC PRECIPITATION REACTION (for insoluble salts) experiment steps - using ___________ ____________, add certain vol of 1 of the _______ ____________ into small beaker - add ________ amts of the other ______ ___________ & _____ till ___ ______ ______________ forms - ______ mixture to get insoluble salt as __________ - wash ______________ with ______ amt of ___________ water to remove any ______________ - dry it between layers of ______ paper

- measuring cylinder, ionic compounds - excess, ionic compound, stir, no more precipitate - filter, residue - precipitate, small, de-ionised, impurities - filter

IONIC PRECIPITATION REACTION (for insoluble salts) BUT STARTING MATERIAL’S INSOLUBLE - stage 1: convert it to a _________ ______ BY: adding ________ insoluble starting material to dilute ______ ______ (always convert to that) to form soluble salt & stir till ___ ______ insoluble starting material _____________. then _______ mixture to obtain ___________ _____ as filtrate - stage 2: mix solutions of soluble salt (from stage 1 filtrate) & another ______ ___________ (basically the steps from b4: 2 soluble solutions)

- soluble salt, excess, nitric acid, no more, dissolves, filter, soluble salt - ionic compound

IONIC PRECIPITATION REACTION (for insoluble salts) BUT STARTING MATERIAL’S INSOLUBLE insoluble staring material can’t be added directly to other solution to make insoluble salt cus reaction would form an __________ compound that ______ surface of ____________ ____________ _____________, preventing it from __________ _________ with the other ionic compound in the other solution —> ____ ______ of insoluble salt

insoluble, coats, insoluble starting material, further reacting, low yield