Buffers/Solubility/Titration

[H+] is defined by what two factors

the value of Ka and the raton [HA]/[A^-]

what is a buffer

a weak acid and a conjugate base

the pH=-log ka + log [conjugate base]/[conjugate acid]

henderson-hasselbach

low pH= ?

high concentration

a strong acid titrated with a strong base = ?

neutral pH (7)

a weak acid titrated with a strong base = ?

neutral point will be a little greater than 7 if theyre the same concentration

the initial pH increases as….

Ka(equilibrium) increases

the weaker your acid the …

higher the equivalence point

the two factors that contribute to acid behavior

1. adding an oxygen atom attached to a carbon atom in a carbyl group which stabilizes the conjugate base

2. residence: conjugate base of the carboxylic acid (carboxylate anion)

a solution is in contact with an undissolved solid

saturated solution

lewis acid goes …

toward water molecules

An Arrhenius Acid produces what in an aqueous solution

H+ ions

In the reaction below, name the conjugate base of the strong acid

 

HNO_3(aq) + NH_3(g) NO₃^-_(aq)+ NH₄⁺ _(aq)

NO-3

In the reaction below, name the conjugate acid of the weak base

 

HNO₃ + NH₃ NO₃^- + NH₄⁺

NH4^+

At the equivalence point the number of moles of acid will equal the number of moles of the base that is added to neutralize the acid. True or False

True

A buffer consists of a strong acid and its conjugate base. True or False

False

Does a weak acid have a small or large Ka value

small

Which expression correctly expresses the solubility product constant for Ag₃PO₄ in water? 

[Ag⁺]³[PO₄^3-]