Acids and Bases

Advanced Chemistry - Kunka; test 5/5

Acids

pH < 7 / pOH > 7

proton (H⁺) donors

acids are…

…compounds that release hydronium ions \[H₃O⁺\] when dissolved in water

\-formula for most acids begin with H (ex: HCl)

acid effect indic: red

blue litmus & neutral litmus

acid effect indic: clear

Phenolphthalein

acid effect indic: no change

Red litmus

acids + active metals

produce H₂

acids + carbonates

produce H₂O + CO

net ionic equation

is about the formation of water

acids ionize

can be good electrolytes

Bases

pH > 7 / pOH < 7

proton (H⁺) acceptors

bases are…

… compounds that give off hydroxide ions \[OH⁻\] when dissolved in water

\-formula for most bases ends with OH

bases dissociate

can be good electrolytes

amount / % / degree determines…

…the concentration of the solution

Neutralization reactions produce…

…salt (+ ion) and water (- ion)

Lewis acid

accepts electron pairs to form a covalent bond

Lewis base

donates electron pairs to form a covalent bond

Arrhenius acid

produces/increases hydronium \[H₃O⁺\] in water

Arrhenius base

produces/increases hydroxide \[OH⁻\] in water

Bronsted-Lowry acid

H⁺ proton donor

Bronsted-Lowry base

H⁺ proton acceptor

(BL) conjugate acid

the product of the BL base

(BL) conjugate base

the product of the BL acid

amphoteric

any substance that can act as an acid vice versa

Monoprotic acids

leading hydrogen is singular (ex: HCl)

can only donate one hydrogen proton

Diprotic acids

two leading hydrogen: H₂ (ex: H₂SO₄)

Triprotic acids

three leading hydrogren: H₃ (ex: H₃PO₄)

polyprotic acids

can donate >1 hydrogen protons

steps of ionization

if there are multiple hydrogren (polyprotic acids) the hydrogens will be given away in steps

Ionization Constant of Water

Kw = 1.0x10⁻¹⁴

K=\[H₃O⁺\] x \[OH⁻\]

1\.0x10⁻¹⁴ = 1.0x10⁻⁷ x 1.0x10⁻⁷

H₃O⁺ and OH⁻ have an ______ relationship

inverse

log expression of acid concentration

pH = -log\[H₃O⁺\]

log expression of base concentration

pOH = -log\[OH⁻\]

pH / pOH

an expression of the concentration of an acid/base

titration

technique used to determine the concentration of an unknown acid or base by neutralizing it with a known acid or base

Neutralization

\[H₃O⁺\] = \[OH⁻\]

\#H x M x V = #OH x M x V

equivalence point

the point at which neutralization occurs

end point

the point in a titration when the indicator changes colour

strong acids…

… ionize 100%

weak acids…

… ionize < 100%

strong bases…

… dissociate 100%

weak bases…

…dissociate < 100%

acids taste…

sour

bases taste __ and feel ___

bitter, slippery

carbonic acid: H₂CO₃

formed when an acid interacts with a carbonate

H₂O and CO₂

formed when carbonic acid (H₂CO₃) continues to break down