Acid/Base Chemistry

yeah good luck

Arrhenius acid

Increases the concentration of H⁺ (as H₃O⁺) ions in water, acts as an electrolyte, and has a pH less than 7. It will react with bases to form a salt and water. It will react with certain metals to create H₂ gas and with carbonates/bicarbonates to produce CO₂ gas. It turns blue litmus paper to red.

Arrhenius base

Increases the concentration of OH^- ions in water, acts as an electrolyte, and has a pH greater than 7. It will react with acids to form a salt and water. It turns red litmus paper to blue.

Common acids to know

HCl hydrochloric acid

HNO₃ nitric acid

H₂SO₄ sulfuric acid

H₃PO₄ phosphoric acid

Polyatomic ions to know

OH^- hydroxide

NO₃^- nitrate

HCO₃^- hydrogen carbonate

CO₃^2- carbonate

SO₄^2- sulfate

PO₄^3- phosphate

NH₄⁺ ammonium

Bronsted-lowry acid

a neutral molecule or ion that donates a proton (H⁺)

Bronsted-lowry base

a neutral molecule or ion that accepts a proton (H⁺)

HA + :B → HB⁺ + :A^-

Conjugate base

the species that remains after the acid has given away its proton

HCl → Cl^-

Conjugate acid

the species that remains after the base has accepted the proton

e.g. OH^- → H₂O

Amphiprotic

Can act as a bronsted-lowry acid or base by donating or accepting a proton

Amphoteric

Can act as an acid or base by any definition

Lewis acid

an electron pair acceptor

Lewis base

an electron pair donator

All ___ acids are ___ acids, but not the reverse

All bronsted-lowry acids are lewis acids, but not the reverse

pH + pOH = ?

14

pH = ?

-log[H⁺]

pOH = ?

-log[OH^-]

A 1x unit change is a __ change in pH

10x

titration equation

1/coefficient of A in the balanced equation x [H⁺] x volume of A = 1/coefficient of B in the balanced equation x [OH^-] x volume of B

How do weak and strong acids differ?

Strong acids dissociate completely in water. The reaction is not reversible. It’s the opposite for weak acids.

Strong acids to know

HCl, HBr, HI, HNO₃, H₂SO₄, NH₄⁺

Strong bases to know

anything in Group 1 + OH^-

A strong base makes a…

A weak conjugate acid. This will hydrolyze water to form a basic solution

Na⁺ + H₂O → OH^- + HNa

A strong acid makes a…

Weak conjugate base. This will hydrolyze water to form an acidic solution

Cl^- + H₂O → H⁺ + ClOH

Buffer solution

a solution that resists a change in pH. Can be formed by a weak acid and its conjugate base (base ___) or a weak base and its conjugate acid (base ___)

To make a buffer solution…

1) A weak acids/base and its conjugate

2) A weak acids/base and enough of a strong acid/base to partially neutralize the weak acid (leaving a large amount of its conjugate)

Henderson-Hasselback equation

pH = pK_a + log([A^-]/[HA])

(when the original equation is HA → H⁺ + A^-, you can get pK_a from the data booklet)