Acids and Bases

Arrhenius definition of Acid

Acid are any species that dissolves in aqueous solution to produce H+ ions

Arrhenius definition of base

Base are any species that dissolves in aqueous oslution to produce OH ions

Brosted Lowry Acid

H or proton Donor

Bronsted Lowry Base

Proton Acceptor or gains H or proton

Lewis Acid

Any species that accept a pair of electrons Le

Lewis base

any species that donate a pair of electrons

Conjugate Acid

Accept a proton or H +

Conjugate Base

Loses a H or loses proton

What is the relationship between acid and bases

The Stronger the acid the weaker its conjugate base

the weaker the acid the stronger its conjugate base

The hgiher concentration of H + means

more acidic

pH formula

pH = -log [H+]

[H^+] formula

10^-PH

pOH formula

pOH = log [OH^-]

[OH^-] formula is

[OH^-] = 10^-pOH

what does the sum of pH and pOH =

pH + pOH always equals to 14

Ka or dissosicaton Constant of Acid

Ka = H3O+] [Conjugate Acid] / Acid

Kb or Dissosicaiton Constant B

Kb = [HB+][OH-]/ [Base]

What is the dissociation constant of water or Kw

Kw = 1.0 × 10^ -14

pka and pkb measuer what

how storng or how weak the acid or base is

pka equaiton

pka = -log (Ka)

the lower the pka the what

the stronger the acid and ability to donate protons

pkb equaiton

pkb = -log (Kb)

the lower the pkb the stronger the what

the stronger the base

the bigger the Ka and Kb

the stronger the acid or base

Strong Acids vs Weak Acids

Strong acid have Ka > 1

Weak Acids have Ka ««<1

Strong Base vs Weak Base

Strong base is Kb > 1

Weak Base is Kb «< 1

Binary Acids

Binary acids include hydrogen halides like HI HBr HCl and HF

The larger the atomic radius of halide means

the more acidic

Oxoacids

Acids that contain oxygen

The one with more oxygen atoms means it more acidic

Neutralization Reactions

strong acids react wiht a strong base to produce water

M1V1 = M2V2

Salts

the product of a neturalization reaction of acids and bases

How to determine whether a salt is acidic or basic

Break down the salt into respective ions and add a H and OH

if they are strong acid + Strong base = neutral strong acid + weak base is strong acid while strong abse + weak acid is storng acid

Buffers

a solution that resist a change in pH when small amounts of acid or base are added to it

Calculating the pH of a buffer

pH = pka + log [A-]/[HA]

pOH = pkb + log [B-]/HB

Titrations

Titration is experiment used to determine the concentration of an acid or base

how do titrations work

adding an acid/base of a known concentration to determine the unknown concnetration

Analyte is

the unknwon concentration ofa titriation

titrant is

the known concentration

indicator

something that adds to show the color change

strong strong is 7

strong A weak B is below 7

weak A strong B is bigger than 7

Equivalence point

when the solution changes color or when the amount of acid and base euqal

where on the graph is the equivalence point

the steepest part

Equation for equivalence point

NtVt = Na Va

N = Molar mass x n

Half Equivalence point

where the pH = pKa

the midpoint of the buffering region

pH = pKa + log [A-]/HA