Acid Base Chemistry Ka and Kb + Titrations (lecture 2 + 3)

Unit 2

weack acids and bases

partly dissociate in anqueous solutions

conjugate base

the chemical species that remains after an acid has donated a proton (H+) (ex: in HCl-, Cl- is whats left over after H+ is donated)

conjugate acid

hemical species that is formed when a base accepts a proton H+)

if H3O > OH- then the solution is

acidic

if H3O < OH- then the solution is

basi

the larger the Ka means

smaller Pka and stronger acid

the larger the Kb

smaller Pkb and stronger base

relationship between Kw, Kb, and Ka

Kw= KbKa, thus the stronger the acid the weaker the conjugate base

ka x kb =

kw = 10^-14

what do buffers always have

a conjugate and a weak base/acid

buffer eqatuon for weak base and conjugate acid

OH-= kb(cb/ca) (c= concentration aka amount)

what unit of measurement must C be

concentraion must be in Molarity

net ionic equation for strong acid strong base

H+ (aq) + OH- (aq) —> H2O (l)

net ionic equation for strong acid and weak base

H+ (aq) + B(aq) —> HB+ (aq) (HB= weak base)

net ionic equation for when strong acid and weak base but the base is an anion

H+ (aq) + A-(aq) —> HA+ (aq) OR H+ (aq) + HCOO-(aq) —> HCOOH(aq

net ionic equation for weak acid and strong base

HA (aq) + OH- (aq) —→ A- + H2O (l)

what does A- mean

conjugate base

net ionic equation for weack acid and weak base

both reactants partially dissociate and react to form a salt (doesnt really neutralize

what is a titration

lab method used to find the exact concentration of a solution. It works by slowly adding solution of an acid to solution of a base (or vice versa) until the neutrilization reaction is complete

analyte

the solution with an unknown concentration that you are trying to measure in a titration

titrant

titrant is the solution with a known concentration that is slowly added to the analyte during a titration.

what is a titrantion curve used to determine

the amount needed for acid & base to netralize (point of equilivance) and Ph og the solution at that equilivance point

how to solve for titrations

RICE table and determie limiting reagent

strong acids and strong base titrantion curves have equilivance point at

pH= 7 ALWAYS

weak base and strong acids titrantion curves have equilivance point at

pH <7

what is the buffer region

tha pH range where the Ph of a soltion remains static. usually happens at the half equilivce point (Ph=pka of the weak acid 

what is buffer capacity

how mch of a strong acid or base can be added to a buffer solution before the vuffer is lost

weak acid and strong base  titrantion curves have equilivance point at

pH>7

weak acid and weak base  titrantion curves have equilivance point at

pH above or below 6