AP Chem Chapter 14-15 Titration, Acids and Bases 2021

What is the name of the point of the curve where pH = pKa?

Halfway point

At what point will [H] = [OH]?

Equivalence point

If a weak acid is titrated with a strong base

What is the definition of a Buffer ?

A solution which contains a weak acid (or weak base) and its conjugate base (or acid)

Given a titration curve, determine the Ka of the acid

anti-log of the negative value of the solution's pH at the halfway point

Why does the titration of a weak acid with a strong base have an equivalence point that is greater than 7?

the acid's conjugate base makes the solution basic

What is the definition of the equivalence point?

The spot on the titration curve where moles of acid = the mole of base . The pH at this point is not necessarily 7

Which indicators would be the most useful when titrating a weak acid with a strong base?

Pink phenolphthalein or thymol blue. Both change colors at pH's between 7.6 and 9. These are the values between which the equivalence

Given an unmarked titration curve, how would you identify the equivalence point?

Isolate the section of the curve where the slope is steepest. Look for the center point

arrhenius acid

they are the acids that dissociate in water to produce H+ ions

arrhenius base

they are the bases that dissociate in water to produce OH- ions

bronsted-lowery acid

acids that are proton donors

they are willing to give up H+

t

bronsted-lowry base

bases that are proton(H+) acceptors

conjugate base

what the acid becomes once the proton(H+) has been donated

conjugate acid

what the base becomes after it accepts the proton(H+)

strong acids

HNO3

HI

HBr

HCl

H2SO4

HClO4

what defines a strong acid

they completely(100%) dissociate in water

what defines a weak acid

acids that only partially dissociate

has a relatively strong conjugate base

strong bases

soluble compounds containing the hydroxide ions

NaOH

KOH

LiOH

RbOH

Mg(OH)2

Ba(OH)2

Ca(OH)2

Sr(OH)2

How # of oxygens on oxyacids affects acid strength

acid strength increases as more oxygens are added to the central Y

increasing the number of electronegative oxygen atoms increases the electrons attraction toward the Y. This will reduce the forces of attraction in the O-H bond making ti easier to remove a H+

Kw

1.0 X 10^-14 at 25 degrees Celsius

how to find pH when given [H3O+]

pH=-log[H3O+]

how to find pOH when given [OH-]

pOH=-log[OH-]

how to find the pH when given the pOH

14-pOH

how to find pOH when given the pH

14-pH

neutral

[H+] = [OH-]

larger Ka value means what

stronger acid because the acid is going more into completion

neutralization SA + SB reaction net ionic equation

H+ + OH- ---> H2O

hydrolysis

states that salts (ionic compounds) can make a solution acidic, basic, or even have no effect on the pH