Acids and Bases

pH < 7 / pOH > 7

proton (H⁺) donors

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

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

blue litmus & neutral litmus

Phenolphthalein

Red litmus

produce H₂

produce H₂O + CO

is about the formation of water

can be good electrolytes

pH > 7 / pOH < 7

proton (H⁺) acceptors

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

-formula for most bases ends with OH

can be good electrolytes

…the concentration of the solution

…salt (+ ion) and water (- ion)

accepts electron pairs to form a covalent bond

donates electron pairs to form a covalent bond

produces/increases hydronium [H₃O⁺] in water

produces/increases hydroxide [OH⁻] in water

H⁺ proton donor

H⁺ proton acceptor

the product of the BL base

the product of the BL acid

any substance that can act as an acid vice versa

leading hydrogen is singular (ex: HCl)

can only donate one hydrogen proton

two leading hydrogen: H₂ (ex: H₂SO₄)

three leading hydrogren: H₃ (ex: H₃PO₄)

can donate >1 hydrogen protons

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

Kw = 1.0x10⁻¹⁴

1.0x10⁻¹⁴ = 1.0x10⁻⁷ x 1.0x10⁻⁷

inverse

pH = -log[H₃O⁺]

pOH = -log[OH⁻]

an expression of the concentration of an acid/base

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

[H₃O⁺] = [OH⁻]

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

the point at which neutralization occurs

the point in a titration when the indicator changes colour

… ionize 100%

… ionize < 100%

… dissociate 100%

…dissociate < 100%

sour

bitter, slippery

formed when an acid interacts with a carbonate

formed when carbonic acid (H₂CO₃) continues to break down