8.1 acids and bases

what’s an arrhenius acid

a substance that produces H+ protons when dissolved in water

what’s an arrhenius base

a substance that produces OH- ions when dissolved in water

what is a bronsted-lowry acid

a proton donor

what is a bronsted-lowry base

a proton acceptor

what is formed when HCL donates a proton to water

H3O+ + Cl-

What’s the significance of using a single arrow for HCL+H2O → H3O+ + Cl-

it’s irreversible because HCL is a strong acid

why can only one hydrogen be donated from CH3CH2OOH

only the hydrogen bonded to the electronegative oxygen can dissociate

CH3CH2COOH forms what when water is added

H3O+ + CH3CH2COO-

How does NH3 act as a bronsted-lowry base

it accepts a proton from water to form NH4+

NH3+H2O forms what

NH4+ + OH-

why can organic molecules with nitrogen act as bases

nitrogen has a lone pair that can accept a proton

what does amphiprotic mean

a substance that can donate or accept a proton

why is water amphiprotic

it can accept a proton to form H3O+ or donate a proton to form OH-

What’s an example of another amphiprotic substance

HCO3-

What’s a conjugate acid

the species formed after a base accepts a proton

What’s a conjugate base

the species formed after an acid donates a proton

what’s the conjugate acid in HX+Y→HY++X-

HY+

what’s the conjugate base in HX+Y→HY++X-

X-

Conjugate pairs when H2S reacts with water (H2S+H2O→H3O++HS-)

H2S/HS- and H3O+/H2S

what’s the rule about conjugate bases and acids

the conjugate base has one fewer H+ than the acid

what determines acid/base strength

the degree of dissociation in water

what makes an acid strong

when it dissociates 100% in water

name 3 common strong acids

HCl, HNO3, H2SO4

what are strong bases

metal hydroxides that dissociate completely

two examples of strong bases

NaOH and KOH

what makes an acid weak

when it partially dissociates in water

two examples of weak bases

CH3COOH and H2CO3

relationship between acid strength and conjugate base strength

strong acids have weak conjugate bases

what’s the self ionization of water

H2O+H2O<>H3O++OH-

what’s the ion product constant for water (Kw)

[H3O+][OH-]

value of Kw (constant for water) at 25 degrees Celsius

1.0×10^-14

in pure water at 25 degrees celsius what’s the molarity of [H3O+] and [OH-]

both are 1.0×10^-7 M

What happens if [H3O+] increases in the self ionization of water

[OH-] decrease to maintain kw at 1.0×10^-14

Why does adding solute not change Kw

Kw is temperature-dependent only, not concentration-dependent

4 strongest acids from the chart

HCl, H2SO4, HNO3, H3O+

4 weak acids from the chart

HF, CH3COOH, H2CO3, H2S

3 strongest bases from the chart

O²-, OH-, and S²-

3 weakest bases from the chart

HCO3-,NH3,F-