Acid Base Titrations / Gases

kinetic molecular theory

1. all particles are in constant, random, motion. (collisions with walls cause pressure to be exerted)

2. All collisions between particles are perfectly elastic. (no gain of loss of kinetic energy)

3. The volume of the particles in a gas is negligible. (gases consist of tiny particles)

4. The average kinetic energy of the molecules is its Kelvin temperature. (directly proportional)

5. This theory neglects any inter molecular forces as well. And it is important to not that gases expand to fill their container, solids/liquids do not. And the gases are compressible; solids/liquids are not appreciably compressible.

what is pressure?

Pressure is a measure of the force that a gas exerts on its container. Force is the physical quantity that interferes with inertia. Gravity is the force responsible for the weight.

boyle’s law

volume goes down so pressure goes up (P1V1 = P2V2)

charles’ law

temperature increases so volume increases (V1/T1 = V2/T2)

gay-lussac’s law

temperature increases so pressure increases (P1/T1 = P2/V2)

avogadro’s law

as volume increases so does the number of moles (V1/n1 = V2/n2)

combined gas law

a combo of boyle’s, charle’s, and gay-lussac’s laws (P1V1/T1 = P2V2/T2)

Density w/ equation

d = P(MM)/RT

Molar mass w/ equation

MM = dRT/P

Buret used to

to deliver the second reactant to the flask

Erlenmeyer flask used to

hold the unknown analyte

titrant

substance of known concentration used to determine the unknown concentration of the other substance

analyte

unknown substance

equivalence point

pH at which the amount of acid = amount of base

indicator

compound that changes color based on pH

end point

point at which the indicator changes color