Acid/base equilibria

What are the 2 definitions for acids and bases

1. Bronsted-Lowry

2. Lewis Acid

What is a Bronsted-Lowry acid

A species that donates an H+

What will result from Brronsted-Lowry acids

a conjugate base

What is a Bronsted-Lowry base

A species that accepts an H+

What do Bronsted-Lowry acids form

a conjugate acid

What is a Lewis acid

a species that accepts electron pairs

What is a Lewis base

a species that donates electron pairs

What does the pH of a solution depend on

The concentration of H+ in a solution

What happens to the pH of a solution when you add acid (ex HCl)

it decreases

What happens to the pH of a solution when you add base (ex: NaOH)

it increases

What is a buffer

an aqueous solution that resists change in pH upon addition of acid or base

What makes up buffer solution

a pair of weak acid with its conjugate base or a weak base with its conjugate acid

What is the equilibrium constant equation

What is the equation for pH

What 2 components make an effective buffer

1. a large number of weak acid and its conjugate base in comparison to the number of moles a strong acid or base has

2. a ratio of [HA]:[A-] that ranges from 10:1 to 1:10

What is Ka

the acid ionization constant

What is the equation for Ka

What does a high Ka indicate as far as dissociation

100% dissociation

the stronger the acid the __ the conjugate base

weaker

What is the conjugate base of HCl and is it weak or strong

Cl- is the conjugate base and it is weak

a lower Ka indicates what about an acid

it is a weak acid because it does not dissociate as well

What is the name of this ion: H3O+

hydronium

What is the name of this ion: H3O+

hydroxide

What is Kw

the autoionization constant

What is the equation for Kw

What is the concentration of [H3O+] in pure water

1×10^-7M

What is the concentration of [OH-] in pure water

1×10^-7M

what number represents Kw

1×10^-14

When does neutrality exist

when [OH-] = [H3O+]

What is the pH equation

Wha is the pOH equation

What is this molecule called: HCl

hydrochloric acid

What is this molecule called: HBr

hydrobromic acid

What is this molecule called: HI

hydroiodic acid

What is this molecule called: HNO3

nitric acid

What is this molecule called: HClO4

perchloric acid

What is this molecule called: H2SO4

sulfuric acid

what will form from the complete dissociation of a strong base in water

OH- ions

Which group(s) on the periodic table contain strong bases

group 1 and group 2

What is the equation for pKa

What happens to Ka as pKa increases

Ka decreases

What happens to Ka as pKa decreases

Ka increases

What is the relationship between pKa and Ka valutes

They are inversely proportional. So as pKa increases, Ka decreases, and vice versa

The lower the pKa the ___ the pH

lower

lower pKa indicates a more (acidic/basic) solution

acidic

stronger acids have a ___ Ka

larger

weaker acids have a ___ Ka

smalelr

what is Kb

the base dissociation constant

what is the equation for Kb

The higher the Kb the ___ the base

stronger

The lower the Kb the ___ the base

weaker

What is the pKb equation

The stronger the acid the ___ the conjugate base

weaker

what determines if a salt solution will be acidic or basic

whether or not the cation or anion reacts with water

What are the 6 strong acids

1. HCl

2. HBr

3. HI

4. HClO4

5. HNO3

6. H2SO4

What are the 8 strong bases

1. LiOH

2. NaOH

3. KOH

4. RbOH

5. CsOH

6. Ca(OH)2

7. Sr(OH)2

8. Ba(OH)2

Is the solution basic or acidic: Neither the cation nor the solution basic or acidic anion reacts with water

It’s neutral

Is the solution basic or acidic: The cation does not react with water, but the anion does

basic

Is the solution basic or acidic: The cation reacts with water, but the anion does not

acidic

Is the solution basic or acidic: Both the cation and anion react with water

Can be acidic, basic, or neutral

Is NaCl acidic or basic

HA IT’S NEUTRAL

Is Ba(CHCOO)2 acidic or neutral

basic

Is NH4NO3 acidic or basic

acidic

Will anion hydrolysis result in increased or decreased pH

increase. it will become more basic

Will cation hydrolysis result in increased or decrease pH

decrease. it will become ore acidic

Ka > Kb =

acidic

Ka = Kb =

neutral

Ka < Kb

basic

in terms of ka and kb, what does Kw =

Kw = (Ka) (Kb)

What is a buffer

a solution that resists change in pH

What is the Henderson-Hasselbach equation

When do we use the Henderson-Hasselbach equation

When calculating pH of buffer solutions