Acids and Bases

Arrhenius definition of acid

a substance that dissociates in water/splits apart to make H+/H3O+ or Oh- ions

Degree of Acidity

measured in pH
lower on scale = more acidic
higher on scale = more basic/alkaline
scale = logarithmic ^10

properties of acids

- reactive w metals

- turns litmus paper red

- clear - look like water

- conducts electricity bc of H+

- corrosive (hurt skin)

- sour

Arrhenius definition of base

a substance that dissociates in water to form OH- ions (metal in the front)

Degree of basicity

measured in pH
lower on scale = more acidic
higher on scale = more basic/alkaline
scale = logarithmic ^10

properties of bases

- bitter

- turns litmus paper blue

- slippery

- corrosive

- clear

- conducts electricity

water equilibrium K

1 x 10^-7

water equilibrium in acids

1 x 10^-14= [H3O+][OH-]

dilute

having a small amount of solute in a given amount of solvent
- measured in Molarity, M (moles solute/liter solution)

concentrated

having a large amount of solute in a given amount of solvent
- measured in Molarity, M (moles solute/liter solution)

weak

small amount of the acid or base solute dissociates (separate)

strong

nearly all the acid or base solute dissociates (separate)

strong base

ionic substances that contain OH in formula - fully dissociate but have very low solubility in water

strong acid (H2SO4)

is a polyprotic acid, do not double bc does not fully break apart

strong acid def

Has a K much greater than one (equilibrium constant)

weak acid def

has a K much smaller than 1 (equilibrium constant)

bronsted lowry acid

donates H+

bronsted lowry base

receives H+

Titration

how many drops of acid will neutralize a base/ drops of base to acid:
M=mol/L
Xa x Ma x Va = XbMbVb
# of H+ in f # of OH - in formula
think balancing scale

buffer

resists change in pH by containing weak acid + conjugate base of weak base + conjugate acid (ex blood - can neutralize H+ and OH-

polyprotic acid/base

has more than one H+ or OH - so account for in titration