Acids and Bases

Question 1

Strong Acids

Answer 1

HCl H2SO4 HNO3 HI HBr HClO4 HClO3

Question 2

Strong Base

Answer 2

All oxides and hydroxides of group 1 and 2

Question 3

Conjugate Acids and Bases

Answer 3

• A strong acid will have a weak conjugate base - A strong base will have a weak conjugate acid -> Most of the time, a weak base will have a weak conjugate acid

Question 4

Polyprotic Acids

Answer 4

Can donate more than one hydrogen ion in an acid-base reaction

Question 5

Arrhenious Theory

Answer 5

-> An acid is a substance that produces H+ in solution -> A base is a substance that produces OH- in solution -> According to the Arrhenius theory, acids are substances that produce H+ when dissolved in water -> and bases are substances that produce OH- when dissolved in water.

Question 6

Bronsted Lowry Theory

Answer 6

-> An acid is a proton (H+) donor -> A base is a proton (H+) acceptor -> Amphoteric substances can react as acids or bases -> Strong acids (for example, HCl, H2SO4) and strong bases(for example, NaOH) are essentially completely ionised(acids) or dissociated(bases) into ions in aqueous solution. Strong acids have a high H- concentration. Strong bases have a higher OH- ion concentration -> For weak acids (for example, CH3COOH, H3PO4) and weak bases (for example, NH3) only a small proportion of the molecules are ionised in aqueous solution. For acids there is a low hydrogen ion concentration, for bases there is a low hydroxide ion concentration

Question 7

Basic Salts

Answer 7

• > Form OH- -> The formation of the OH- makes it basic
• a negative ion that is the conjugate base of a weak acid undergoes hydrolysis to form OH- ions.
• this is what makes it basic
• weak acid + strong base -> weak base + ion
• weak base + H2O -> OH- + acid

Question 8

Acidic Salts

Answer 8

• > Form H3O -> The formation of the H3O makes it acidic
• a positive ion that is the conjugate acid of a weak base form H3O
• strong acid + weak base -> weak acid + ion
• > weak acid + H2O -> H3O + base

Question 9

Buffers

Answer 9

• Solutions which resist change in pH when little acids / bases are added
• > consists of weak acid + conjugate base
• > weak base + conjugate acid

Question 10

Buffer Capacity

Answer 10

• depend on two conditions:
• > Relative concentration of buffer capacity, where concentration of acid and its conjugate base are EQUAL
• > Concentration of the conjugate pair, more of the conjugate pair increases the amount it can react w/ acids and bases

Question 11

Primary Standard

Answer 11

-> Pure -> Known Formula -> Not react w/ surroundings -> Have a high molar mass -> Maintain constant concentration over time

Question 12

Primary standards for acid-bases

Answer 12

-> anhydrous sodium carbonate,Na2CO3, -> oxalic acid, H2C2O4·2H2O, -> potassium hydrogenphthalate,KHC8H4O4.

Question 13

Equivalence Points

Answer 13

The point during a reaction at which stoichiometric amounts of the reactants have been mixed

• > Acid: Strong, Base: Strong, pH equiv. = 7, indicator: phenolphthalein
• > colour change: colourless to pink
• > Acid: Weak, Base: Weak, pH Equiv: 7, Indicator: Phenolphthalein
• > Colour change: colourless to pink
• > Acid: Strong, Base: Weak, pH: Acidic, Indicator: Methyl Orange,
• > Colour Change: Red to Yellow
• > Acid: Weak, Base: Strong, pH: Basic, Indicator: Phenolphthalein,
• > Colour Change: colourless to pink

Question 14

Multiprotic Acids

Answer 14

H2CO3 (weak acid) –> HCO3- (Weak base) —> CO32- (Weak base)

H2SO4 (Strong acid) –> HSO4- (weak acid) –> SO42- (neutral)

H3PO4 (Weak acid) –> H2PO4 (weak acid) –> HPO42- (weak base) -> PO43- (weak base)

Question 15

Weak Bases

Answer 15

Metal Phosphates

Metal Carbonates

Ammonia

Metal Hydrogen Carbonates