physical chemistry

MSOP 1014 - the science of medicines

define molarity

moles of solute dissolved in 1L of solution

define normality

gram equivalent weight of solute dissolved in 1L of solution

define molality

moles of solute per kilogram of solvent

mole fraction

moles of solute / total number of moles

define milliequivalent (mEQ)

concentration of an ion in solution

what is a molecular equation?

an equation with reactants and products written as molecular substances

what is a complete ionic equation?

an equation where soluble ionic compounds are written as separate ions

what is a net ionic equation?

an equation where soluble ionic compounds are written as separate ions and spectator ions are cancelled

define an electrolye

a substance that dissociates into ions

define a non-electrolyte

a substance that does not dissociate into ions

what is a hydronium ion?

H3O+

define an acid according to the arrhenius theory

a substance that releases H+ into water

define a base according to the arrhenius theory

a substance that releases OH- into water

what is the exception to the arrhenius theory?

NaHCO3 (is a base though does not release H+)

what is an acid according to the bronsted-lowry theory?

a substance that donates a proton

what is a base according to the bronsted-lowry theory?

a substance that accepts a proton

what is an amphoteric substance?

a substance that can act either as an acid or a base

what is self-ionisation?

when a molecule reacts with itself to give ions

what is the ionic product of water (Kw)?

[H3O+][OH-]

give the value of Kw at 25C

1×10^-14

give the value of Kw at 37C

2.5×10^-14

what happens to [H+] ([H3O+]) with acids and bases according to bronsted-lowry?

acids increase concentration, bases decrease concentration

give the equation for pH by hydronium ion concentration (for a strong acid)

pH = -log10[H3O+]

give the equation for hydronium ion concentration by pH value

[H3O+] = 10^-pH

give the equation for pOH by hydroxide ion concentration (for a strong base)

pOH = -log10[OH-]

the higher the Ka value, the ___ the acid

stronger

the lower the pKa value, the ___ the acid

stronger

[H3O+][OH-] = …

Kw

pH + pOH = …

pKw

the higher the Kb value, the ___ the base

stronger

the lower the pKb value, the ___ the base

stronger

which of these is the correct equation for the equilibrium constant (Kc)?

B

which of these is the correct equation for the acid dissociation constant (Ka)?

B

which of these is the correct equation for the base dissociation constant (Kb)?

B

what is the bronsted-lowry definition of a polyprotic acid?

an acid that can donate more than one proton

Ka x Kb = …

Kw

pKa x pKb = …

pKw

which of these is the correct equation for the pH of a weak acid using the initial molarity of the weak acid

A

which of these is the correct equation for the pH of a weak base using the initial molarity of the weak base

B

what salt is formed from a weak base and a strong acid?

an acidic salt

what salt is formed from a weak acid and a strong base?

a basic salt

what salt is formed from a strong acid and a strong base?

a neutral salt

what salt is formed from a weak acid and a weak base?

a neutral salt

what is meant by %ionisation

ratio of the concentration of ionised molecules to the concentration of all molecules in solution

which of these is the correct equation for the percentage ionisation of a weak acid?

which of these is the correct equation for the percentage ionisation of a weak acid