10A- acids and bases-Table 1 Flashcards
Define acid
species that donates a proton, H+, during an acid-base reaction
Define acid-base reaction
chemical reaction where a proton, H+, is transferred between two
chemical species
Define alkali
a base that is soluble in water and neutralises acids
Define amphiprotic
species that can either donate or accept a
proton, H+
Define base
species that accepts a proton, H+, during an acid-base reaction and are a
group of substances that neutralise acids
Define Brønsted-Lowry
theory
definition of an acid as a chemical species
which donates a proton, H+,
to a base
Or
describes acid-base properties in terms of proton(H+) transfer
Define corrosive
A highly reactive substance that causes obvious damage to tissue
Define deprotonation
loss of a proton, H+, from an acid
Define diprotic
species that can donate up to two protons, H+, during ionisation
Define hydronium ion
positively charged chemical species with
molecular formula H3O+
Define hydroxide ion
negatively charged chemical species with
molecular formula OH−
Define ionisation
process by which a chemical species gains or loses an electron
to gain an electric charge
Define monoprotic
species that can only donate one proton, H+, during ionisation
Define neutralise
react with an acid or a base to produce water
Define polyprotic
species that donates multiple protons, H+, during ionisation
Define protonated water
alternate name for the hydronium ion, H3O+
Define strength
how readily an acid or base will donate or accept a proton, H+
Define triprotic
species that can donate up to three protons, H+, during ionisation
define caustic
Generally used to describe highly basic substances(looking at internet, looks like it can also be used to describe acids and is interchangeable with corrosive)(Check with choung)
What does the Bronsted-Lowry theory indicate about acids and bases
• An acid is a substance that donates a proton, H+
• A base is a substance that accepts a proton, H+
• An acid-base reaction involves the transfer of a proton from an acid to a base
• Acids and bases are corrosive substances.
What’s the difference between a hydronium ion and a hydroxide ion
Hydroxides is when water loses a hydrogen
Hydronium is when water gains a hydrogen
Is water required in all acid base reaction?
Yes, sometimes its not specified but some have aqueous solutions
Write the balanced equation for the acid-base reaction of hydrochloric acid, HCl, in aqueous solution
HCl(aq) + H2O(l) → H3O+(aq) + Cl−(aq)
How can a compound be both an acid and a base
It can be amphiprotic meaning that it donates and accepts protons in an acid base reaction like water
List some amphiprotic species
Water:H2O
hydrogen sulfate:HSO4-
Bicarbonate:HCO3-
Dihydrogen phosphate:H2PO4-
Hydrogen phosphate:HPO42-
What is giving up a proton known as
Deprotonation
How can we classify types of acids
Monoprotic- only donate one proton
diprotic- donates two H+ ions
triprotic- can donate three H+ ions
polyprotic- can donate a H+ ion more than once
List some monoprotic acids
Nitric acid:HNO3
hydrochloric acid:HCl
ethanoic acid:CH3COOH
ammonium:NH4
List some diprotic acids
Sulfuric acid:H2SO4
carbonic acid:H2CO3
hydrogen sulfide:H2S
selenous acid:H2SeO3
List some triprotic acids
Phosphoric acid:H3PO4
citric acid:C6H8O7
Boric acid:H3BO3
arsenic acid: H3AsO4
What is a strong acid
A strong acid will readily undergo almost complete ionisation when added to water
essentially all acid molecules will donate their protons to form aqueous H+ ions
What is a strong base
A strong base will readily accept H+ ions from an acid
What is a weak acid
Does not readily give up its H+ ion in solution and only partially ionises.
What are weak bases
Bases that don’t readily accept H+ ions
List some strong acids
Sulfuric acid:H2SO4(aq) → HSO4−(aq) + H+(aq)
Hydrochloric acid: HCl(aq) → Cl−(aq) + H+(aq)
Nitric acid: HNO3(aq) → NO3−(aq) + H+(aq)
List some weak acids
Ethanoic acid: CH3COOH(aq) CH3COO−(aq) + H+(aq)
Carbonic acid: H2CO3(aq) HCO3−(aq) + H+(aq)
Ammonium: NH4+(aq) NH3(aq) + H+(aq)
-H3PO4=phosphoric acid
What are some strong bases
O2-
OH-
HPO4 2-
-NaOH=sodium hydroxide
-KOH=potassium hydroxide
-Ca(OH)2=calcium hydroxide
Give an example of a weak base
NH3=Ammonia
NH3(aq) + H2O(l) NH4+(aq) + OH−(aq)
Why do we use harpoon arrows
Harpoon/bidirectional arrows are used to indicate that the reactions don’t go to completion
What compounds create a basic solution
Any compound that more or less completely dissociates to form ions, creates a basic solution
What are some ionic compounds that function as strong bases as they readily dissociate to form OH- ions
NaOH, KOH, Ca(OH)2
act as a strong source of the base OH
Compare strength and concentration
• Strength of an acid/base refers to what proportion of its molecules will donate a H+ ion/accept -> dependent on the identity of it
concentration depends on how many molecules there are to begin with- >Dependent on amount of particles/molecules
What are some
common acids and their uses.
(probs don’t need
to know all but its just nice)
Common acids and
their uses=
-Hydrochloric
acid(HCl)=main component of stomach acid
-Sulfuric
acid(H2SO4)=used in car batteries
-nitric
acid(HNO3)=used to manufacture fertilisers, dyes and explosives
-ethanoic
acid(CH3COOH)=found in vinegar
-Carbonic
acid(H2CO3)=found in carbonated soft drinks
-phosphoric
acid(H3PO4)=used to manufacture fertiliser
-Ammonium(NH4)
What are some characteristics of acids
-all acids taste
sour
-Acids=turn litmus
paper red
-acids=corrosive
-react with bases
-low pH
-acids conduct
electricity in water.
What are some
common bases and their uses
Common bases and
their uses=
-sodium
hydroxide(NaOH)=used in drain and oven cleaners
-Ammonia(HN3)=used
in household cleaners, fertilisers and explosives.
-calcium
hydroxide(Ca(OH)2)=used in garden lime to adjust soil pH.
-magnesium
hydroxide(Mg(OH)2)=key ingredient in some antacids
-sodium
carbonate(Na2CO3)=used to manufacture washing powder.
-Oxide
-Potassium
hydroxide
What are sone
characteristics of acids
-all bases taste
bitter
-Bases=litmus to
blue
-react with acids
-high pH
-corrosive(known
as caustic for bases)
-feel slippery
What is a
proton/hydrogen ion in a solution represented by
:hydronium
ion(H3O+)
:hydrogen ion(H+)
What is the
difference between caustic and corrosive
Caustic
and corrosive both mean A
highly reactive substance that causes obvious damage to tissue
A
difference between corrosive and caustic is that caustic is utilised
generally to describe bases, where as corrosive is used to describe acids.
What
arrow is used to show a reaction with a strong acid
or base
-Full
arow → is used to show a
reaction with a strong acid or base
What
arrow is used to show a reaction with a weak acid or
base
-Equilibrium Arrow ⇌ is used to
show a reaction with a weak base or acid
How can you
determine if a molecule is amphiprotic
-all amphiprotic
species have a negative charge=this allows it to give a charge, as well as
except a charge
-All amphiprotic
species also have 1 or 2 extra hydrogens that it is able to donate.
Difference between
strong acids/bases and weak acids/bases
Strong
acids/bases= will ionise readily= virtually no unreacted acid molecules
Weak
acids/bases=will ionise a small proportion= large number of unreacted acid
molecules
Define
strength(adj.), in terms of strength of an acid or base
-strength(adj.)=Tendency to dissociate
-in context of
acids and bases= ‘strong’ and ‘weak’= refer to the relative tendency to
accept or donate protons.
Define
concentration(adj.)
-concentration(adj.)=the amount of acid or
base ions dissolved in a solvent
Difference between
concentration and strength of an acid
:strenght
and concentration are two separate properties=
-strength=refers to a substances willingness
to ionise
-concentration=refers to how much of a
substance is present within a solution
What will happen
to a
1)strong dilute
solution
2)strong
concentrated solution
3)weak dilute
solution
4)weak
concentrated solution
1)strong
dilute solution=will fully ionise
2)strong
concentrated solution=will fully ionise
3)weak
dilute solution=no reacted ions
4)weak
concentrated solution=unionised
What is=
-HCl’s conjugate
-waters conjugate
HCl(aq){acid}+H2O(l){base}
→ H3O+(aq) + Cl-(aq)
-HCl’s conjugate
base is a chloride ion
-waters conjugate
acid is hydronium ion
What is=
-NH3’s conjugate
-H2O’s conjugate
NH3(aq){acid} +
H2O(l){base} → NH4+(aq) + OH-(aq)
-NH3’s conjugate
base is ammonium ion
-H2O’s conjugate
acid is hydroxide ion
What is a
conjugate
-Oxford
dictionary=(of an acid or base) related to the corresponding base or acid by
loss or gain of a proton.
-In acid and base
conjugate pair=the acid always has one hydrogen extra in comparison to its
base conjugate.
-In base and acid
conjugate pair=the base always has one hydrogen less in comparison to its
acid conjugate.
-Explanation of
conjugate acid and base=
A
conjugate acid isthe product that is different from a base by
one proton.
Examples of conjugate acids include water (base) reacting with an acid to
form the hydronium ion (conjugate acid), and ammonia (base) reacting with an
acid to form the ammonium ion (conjugate acid).
Are the conjugate
bases of strong acids always weak or always strong.
Conjugate bases of
all strong acids will be weak
-I don’t think
this is the same pattern for weak bases, weak acids and strong bases. This
only occurs for the conjugate bases of strong acids.(check with Choung but
this is what vid says)
Patterns I have
noticed in determining whether a base is strong or weak and whether and acid
is strong or weak, but this may not be always true(FELIX OBSERVES)
Strong acids=
:Generally have
extra H, and are not carboxylic, and some have hydroxyl groups(sulfuric acid)
:they are
generally covalently bonded molecules
Weak acids=
:Generally
carboxylic acids
:Generally
covalently bonded molecules
Strong bases=
:Have ionic bonded
hydroxides
:generally ionic
Weak bases=
:Just missing a
hydrogen
:Hydrogen
ionically attracted with weak base
:e.g. Is ammonia
What are the
functional groups acids normally have, but this may not be always true(FELIX
OBSERVES)
Acids generally
have=
:carboxyl group
:hydroxyl group
:has hydrogens
What are the
functional groups bases normally have, but this may not be always true(FELIX
OBSERVES)
Bases generally
have=
:hydroxyl groups
:carbonate
:or can fit in
hydrogens
What is the
difference between hydroxyl and hydroxy(I THINK .THIS IS FROM INTERNET)
Hydroxyl refers to
the hydroxyl radical (OH-) only while the functional group OH is called
hydroxy group.
