AP Chemistry: Chapter 8 Acids and Bases

3 Deck Combination

In the Acid-Base Theory, what is an acid?

A proton/H= ion donor

In the Acid-Base Theory, what is a base?

A proton/H+ acceptor

What is the species formed when a proton is added to a base

A conjugate acid

what is the species formed when a proton is removed from an acid

a conjugate base

What is the name of a species that can either accept or donate a proton?

Amphiprotic

What makes a species amphiprotic?

Has an H+ ion, but can also accept H+

What is H2O

amphiprotic

what is HCO3-

Amphiprotic

what is H2SO4

amphiprotic

what is H2PO4

amphiprotic

What is HPO4 2-

amphiprotic

what is the conjugate base of nitric acid

NO3-

What is the conjugate acid of cyanide

HCN

what is the conjugate base of bicarbonate

CO3 2-

what is the conjugate acid of bicarbonate

H2CO3

What is the ion product constant of water

1.0 × 10^-14

What makes a solution neutral

[H+] = [OH-]

if [H+] > 1.0 × 10^-7 M, then [OH] is ___ 1.0 × 10^-7

[OH] < 1.0 × 10^-7 M

if [H+] > 1.0 × 10^-7 M, then the solution is _______

acidic

if [H+] < 1.0 × 10^-7 then [OH] is ___ 1.0 × 10^-7 M

[OH] > 1.0 × 10^-7 M

if [H+] < 1.0 × 10^-7, then the solution is _______

basic

What is Kw = to

[H+][OH-]

The higher the pH, the ________ acidic the solution

less acidic

the lower the pH, the _______ acidic the solution

more

What is pH = to

-log(H+)

To get to [H+] from pH, what do you do?

10^-pH, or 10^-pOH

To get from pOH to pH

14 - pOH = pH

what is HCl

strong acid

what is HBr

strong acid

what is HI

strong acid

What is HClO4

strong acid

what is HNO3

strong acid

what is H2SO4

strong acid

what is LiOH

strong base

what is NaOH

strong base

what is KOH

strong base

what is Ca(OH)2

strong base

what is Sr(OH)2

strong base

what is Ba(OH)2

strong base

what is H3PO4

weak acid

what is HNO2

weak acid

what is CH3COOH

weak acid

what is H2SO3

weak acid

what is NH3

weak base

what is C5H5N

weak base

What is CH3NH2

weak base

what is the formula for nitric acid

HNO3

What is the formula for barium hydroxide

Ba(OH)2

how can you measure pH

pH meter, indicators, or pH paper

we can predict that solutions with transition metal cations are _____

acidic

stronger weak acids have a ____ kA in comparison to weaker weak acids

higher

stronger weak acids have a _______ Pka in comparison to weaker weak acids

lower

weaker acids have a ________ k in comparison to stronger acids

lower

weaker acids have a _______ Pka in comparison to stronger acids

higher

what does % ionization depend on

Ka value, initital concentration of the acid

the higher the starting concentration of an acid, the _________ % ionization

lower

the lower the starting concentration of an acid, the ______ % ionization

higher

the “-x” can be ignored in an ice diagram if % ionization is __________

less than 5%

how to calculate % ionization

[H+] divided by starting [acid] x 100

in a diprotic weak acid, what happens to the conjugate acid from step 1?

it becomes the acid of step 2

what is the equation for [H+] of a diprotic acid

the square root of (Ka1 x [acid])

what is the equation for the concentration of a base for a diprotic acid

[B] = Ka2

What kind of anion would make a compound neutral

anions of strong acids/spectator ions

what kind of cation would make a compound neutral

group I and II cations

what anion would make a compound basic

conjugate bases of weak acids

what cation would make a compound basic

none

what anion would make a compound acidic

amphiprotic acids

what kind of cation would make a compound acidic

the conjugate acids of weak bases, or transition metal cations (ex. NH3)

A has a KB of 1, B has a KB of 2, which is a stronger base?

B

A has a PKb of 1, B has a PKB of 2, which is a stronger base?

A

How to calculate pOH?

-log([OH-]

how to calculate pH from pOH

14 - (-log[OH-])

how strong/weak is the conjugate base of a stronger acid

very weak

what is the relationship between the strength of acids and the strength of their conjugate bases

inverse (one goes up the other goes down)

what is a salt

an ionic solid containing a cation other than H+ and an anion other than OH or O2-

What happens when a salt dissolves in water?

the cation and anion seperate from one another

in a salt, what does it mean if Ka > Kb

the salt is acidic

in a salt, what does it mean if Ka < Kb?

the salt is basic

how to determine whether an amprotic compound is acidic or basic

see if the Ka or Kb is higher

what does a lewis acid do

accepts an electron pair

what does a lewis base do

donates an electron pair

how to determine the [H+] in water if given the [OH-]

1.01 × 10^-14 = [H+][OH-]

what is the formula for acetic acid

HC2H3O2

how to calculate the Ka of a weak acid

[H+][B-]/[HB]

how to calculate PKa if given molarity of reactant

set up ice diagram, solve for x (x2/[]), calc Ka ([A][B-]/[HB]), calc pKa (-log(ka))

how to solve for pKA from Ka

-log(Ka)

what makes an acid stronger/weaker

longer bonds to H (increasing atomic radius), or more polar bonds to H

practice question: is NaI acidic, basic, or neutral?

neutral

practice question: is LiH2PO4 acidic, basic, or neutral?

acidic

practice question: is KOH acidic, basic, or neutral?

basic

practice question: is Cr(NO3)3 acidic, basic, or neutral?

acidic

practice question: is KNO2 acidic, basic, or neutral?

acidic

practice question: is NaCN acidic, basic, or neutral?

basic

practice question: is FeCl3 acidic, basic, or neutral?

acidic

This acid is an H+ donor. It’s named after two famous chemists.

Brønsted-Lowry acid

Note: This is also an Arrhenius acid.

This base is an H+ receiver. It’s also named after two famous chemists.

Brønsted-Lowry base

This base is an OH- donor. It’s named after one famous chemist.

Arrhenius base

This acid only donates one proton (H+) when it dissociates.

Monoprotic acid

What is the opposite of a monoprotic acid? What is its main property?

Polyprotic acid; gives more than one H+ in solution

True or False? Water itself auto-ionizes through the reaction below without any real effect on pH.

2H₂O_(l) ⇌ H₃O⁺_(aq) + OH^-_(aq)

True