IB Chemistry Acids and Bases

Hydrochloric Acid

HCl, strong acid

Nitric Acid

HNO3, Strong acid

Sulphuric Acid

H2SO4, strong acid

phosphoric acid

H3PO4, weaker acid

Ethanoic Acid

CH3COOH, weak acid

Carbonic Acid

H2CO3, weak acid

Sodium Hydroxide

NaOH, strong base

Potassium Hydroxide

KOH, strong base

Calcium Hydroxide

Ca(OH)2, weaker base

Barium Hydroxide

Ba(OH)2, weaker base

Ammonia

NH3, weak base

Alkalies are...

bases that dissolve in water

An Acid is defined as

a proton donor (or a hydrogen ion donor as hydrogen ion consists of only one proton)

A base is defined as

a proton acceptor

Ionization

when an acid is placed in water, the acid gives up its H+ ion forming hydronium ions (H3O+)

Reaction of acids with water

H3O+

Reaction of Base with water

OH-

Conjuctive acid-base pair

the acid and base that are related by the exchanging of a hydrogen ion

Conjugate base

when an acid loses a proton, the species produced is referred to as the conjunctive base

Polyprotic species

acids capable of donating more than 1 hydrogen ion

monoprotic acid

can donate only 1 hydrogen ion

diprotic acid

can donate 2 hydrogen ions thus 2 reactions will occur

triptoproic acid

can donate 3 hydrogen ions

Amphiprotic

can act as either a base or an acid. e.g. HSO4-, HCO3-, H2O

Properties of acids

Sour taste

blue litmus red

corrosive

molecular in structure

conduct electricity

Acid + Metal

Salt + Hydrogen Gas

Acid + Metal hydroxides

Salt + Water

Acid + Metal Oxides

Salt + Water

Acid + Metal Carbonates

Salt + Water + Carbon Dioxide

Acid + Metal Hydrogen Carbonates

Salt + Water + Carbon Dioxide

Acid pH

Less than 7

Base pH

Greater than 7

positive ion

goes first

Base properties (taste, litmus, Feel, Conductivity)

taste bitter

turn red litmus blue

feel slippery

conducts electricity

Base + Acid

Salt + Water

Ammonia + Acid

Ammonium Salt

Ionic equations

separate into ions and cancel

A good indicator

gives a distinct colour change

Neutral pH

=7

Calculating pH

-log10 (H+)

Calculating H+

10^-pH

if the pH changes by 1

then the concentration changes by a factor of 10

H3O+ x OH- =

10^-14

H+ x OH- =

10^-14

Concentration =

Number of mol divided by Volume

distinguishing between strong and weak acids

conductivity

pH

Rate of reaction (metal carbonate + Acid)

Acid Rain pH

less than 5.6