oat chem unit 10

hello people today we will be talking about the effects of the cosmic hand

arrhenius acids/bases

• Acid: any species that dissolves in aqueous solution to produce H⁺ ions.

• Base: any species that dissolves in aqueous solution to produce OH^- ions.

bronsted lowry aids/bases

• Acid: any species that acts as a proton donor

• Base: any species that acts as a proton acceptor

lewis acids/bases

• Acid: any species that accepts a pair of electrons

• Base: any species that donates a pair of electrons

conjugate acids and bases

• The stronger a base or acid is, the weaker its conjugate is.

• The weaker a base or acid is, the stronger its conjugate is.

pH and pOH

power of H or OH, on a scale of 0-14 to describe the acidity or alkalinity of a solution.

• Higher concentration of H⁺ = lower pH.

• pH = -log[H⁺]

• [H⁺] = 10^-pH

• pOH = -log[OH^-]

• [OH^-] = 10^-pOH

• pH + pOH = 14

dissociation constant

the extent at which a particular substance dissociates into ions.

• K_a = [H⁺][A^-] / [HA] ← acid dissociation constant

• K_b = [HB⁺][OH^-] / [B] ← base dissociation constant

• K_w = 1 x 10^-14 ← water dissociation constant

• K_w = K_aK_b

pKa and pKb

measures how strong or weak an acid or base is.

• pKa = -log(K_a) ← lower pKa = stronger acid

• pKb = -log(K_b) ← lower pKb = stronger base

strong acids/bases

have a K_a or K_b > 1, and dissociate completely in water

weak acids/bases

have a K_a or K_b < 1, and dissociate partially in water

binary acids

includes hydrogen halides like HI, HBr, HCl, and HF. A larger atomic radius means hydrogen can dissociate easier, so HI is the strongest and HF is the weakest.

oxoacids

acids that contain oxygen. More oxygen atoms = more acidic. A more electronegative central atom = more acidic.

neutralization reaction

strong base reacts with strong acid to produce water.

• Example: HCl + LiOH → LiCl + H₂O.

• M₁V₁ = M₂V₂

salts

the product of a neutralization reaction between acids and bases.

• HCl + LiOH → LiCl + H₂O. ← LiCl is the salt.

• A strong acid and a weak base make an acidic salt.

• A weak acid and a strong base make a basic salt.

buffer

A solution that resists a change in pH when small amounts of acid or base are added to it. It works best when a weak acid and base are equal in concentration.

6 ways to make a buffer

• 1:1 ratio of weak acid + salt

• 1:1 ratio of acidic salt and weak base

• 1:2 ratio of strong acid + basic salt

• 1:2 ratio of strong acid and weak base

• 2:1 ratio of acidic salt and strong base

• 2:1 ratio of weak acid + strong base

henderson hasselbach equation

• Used to calculate pH of a buffer

• pH = pK_a + log([A^-]/[HA])

titration

Experiment used to determine the unknown concentration of an acid or base.

equivalence point

Point in a titration in which the amount of titrant added is just enough to neutralize the analyte solution. It is the steepest part of a titration curve

• N_tV_t = N_aV_a

• N = M * n

half equivalence point

The midpoint of the buffering region where pH = pK_a.

polyvalent acids/bases

can donate or accept more than one H⁺ ion. Their titration curves can feature multiple buffering regions and multiple equivalence points.

acidic boner

you stuff your doodle wang into a bottle of orange juice and swish it around to mix it