Acids and bases
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- Created by: Hindleyc
- Created on: 12-04-19 09:50
What is a bronsted-lowry acid
Substance (species) that can donate a proton
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What is a bronsted-lowry base
Substance (species) that can accept a proton
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Acid +metal
Salt and hydrogen
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Acid + metal oxide
salt + water
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Acid +metal hydroxide
salt and water
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Acid +metal carbonate
Salt + water + co2
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Salt=
metal ion + non-metal ion
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Acid salt ion for hydrochloric acid
HCl, Chloride, Cl-
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Acid salt ion for sulphuric
H2SO4, Sulfate, SO4^2-
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Acid salt ion for Nitric acid
HNO3, Nitrate, NO3^-
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Acid salt ion for Phosphoric
H3PO4, Phosphate, PO4^3-
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Acid salt ion for ethanoic
CH3COOH, ethanoate, CH3COO-
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how set out
+Ve first
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what if inorganic then
-ve +Ve
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What from H2CO3
HCO3^-
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What from H2CO3
CO3^2-
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how to determine overall formula of the salt
consider charge on the metal ion
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Group 1,2,3 metals
+1, +2, +3
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What will Transition metals have
Charge indicated in roman numerals eg Cu(||)
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What is a salt
Compound from an acid where H+ is replaced by a metal ion (metal base or oxide)
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H=
+1
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Then what is the rest
opposite
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Dont leave
Charges as neutral overall
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Acid=
proton donor
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Proton=
H+ ion- any substance which dissociates to release H+ ions is classed as an acid
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HCl (Aq)=
H+ + Cl-
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HNO3=
H+ + NO3^-
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H2SO4 (aq)=
2H+ + SO4^2-
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H3PO4=
3H+ + PO4^3- (triprotic)
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What is a monoprotic, mono basic acid
One which only releases one H+ ion eg HCl
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What is a diprotic/dibasic acid
one which release 2H+ ions (H2SO4)
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Base=
Proton acceptor
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Alkali=
still a base but dissolves (soluble) in water to release OH- ions in solution- accepts H+ from acid
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What is classed as a base
Any substance which will accept and bond to an H+ ion is classed as a base
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How do determine which species is an acid/base
Match up and see which is gaining/ losing H
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ite
2
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ide
0
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thiosulfate
s2o3
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Alkali-
soluble base that release OH- ions in solutions (metal hydroxide) always aqueous
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State symbols associated with acid -
aq
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Cation and anion of H2SO4
2H+, SO4^2-
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Cation and anion of HNO3
H+, NO3^-
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Cation and anion of H3PO4
3H+, PO4^3-
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Cation and anion of H2CO3
2H+, CO3^2-
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Cation and anion of H2CrO
2H+, CrO4^2-
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Acid + alkali Full/Ionic equation
Write eqn for reaction, write eqn showing all ions present in solution (only reactants and products that are Aq not S,l,g) Cancel out any species that are on both left and right of eqn and re-write leaving balanced ionic eqn
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Acid + oxides Full/Ionic equation
Write eqn for the reaction- overall (oxide=solid unless stated otherwise), Write showing all ions- only aq affected, cancel out any species on both side and rewrite = balanced ionic eqn
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What does acid base equilibria involve
transfer of protons
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Acid + carbonates Full/Ionic equation
Write eqn for reaction- group 1 carbonates=aq unless stated otherwise, Group 2 solid, Write eqn showing all ions present in solution (Aq), cancel
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Acid + metal Full/Ionic equation
A+M=Salt +H but H+ important role as redox not A-B, 1 write eqn apart from mercury, write showing ions only aq, cancel
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BL acid base reaction
Movement of protons (H+)
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Hydroxide
aq
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what can water act as
Acid or base depending on situation
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Property =
Amphoteric
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What does a conjugate acid-base pair contain
2 species that can be interconverted by transfer or a proton
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What is each acid linked to
a conjugate base on the other side of the eqn
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If you start with one and go to other and first has more H what is it
Acid
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What should you have on each side
Acid and base
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What does the concentration of H+ in aq solution cover
very wide range therefore logarithmic scale
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What is Ph scale used as
Measure of concentration of H+
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How to calculate Ph
Ph=-log[H+]
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The smaller the Ph
the greater the conc of H+ ions
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Diff of 1 on Ph=
x10 difference in [H+]
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0-14
0=strong acid 14=strong base
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Conc strong
Lots of H+ and A-
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Conc weak
Lots of HA and little H+
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Dilute strong
H+ and little A-
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Dilute weak
HA
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Strong and weak
How much dissociates where POE lies left (weak) or right (strong)
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Conc
lots of particles in given volume
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What do strong acids do
Completely dissociate
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Where does POE lie
entirely RHS
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What will the conc of H+ in a monoprotic strong acid be the same as
Conc of the acid
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for
HCl and HNO3 (H+ conc same as original acid)
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What else for
H2SO4, HNO3
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Strong acids
Hydrochloric, sulphuric , nitric, phosphoric,
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Diff b/w strong and conc acid
Fully dissociates and E right, lots of particles in given volume eg acidic
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[H+]=
10^-PH
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What is water
Slightly dissociated
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In all aq solutions and pure water what equilibrium occurs
H2O=H+ (from acid) + OH-(aq)
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What following Kc expression does the equilibrium have
Kc= [H+][OH-]/[H2O]
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What is conc of water
Constant because POE very far left so conc is effectively constant as much bigger than the conc of the ions assume its constant and make a new constant=Kw
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What is Kw
Kc x [H2O] both constant grouped together
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Kw=
[H+(aq)][OH-(aq)]
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What is it
Ionic product of water and at 298k value of Kw for all aq solutions =1x10^-14 mol2dm6
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What can the expression be used for
calculating conc of H+ ions if we know conc of OH- ions and vice versa,
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What does value of Kw alter with and what is it needed in
temp likeKc and Kp, calc PH of strong bases
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Other cards in this set
Card 2
Front
What is a bronsted-lowry base
Back
Substance (species) that can accept a proton
Card 3
Front
Acid +metal
Back
Card 4
Front
Acid + metal oxide
Back
Card 5
Front
Acid +metal hydroxide
Back
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