unit 7 vocab

Question 1

equilibrium constant (K)

Answer 1

the relative concentrations of the reactants and products in a reaction at equilibrium

Question 2

dynamic equilibrium

Answer 2

the point at which the rate of the reverse reaction or process equals the rate of the forward reaction of process

Question 3

law of mass action equation

Answer 3

K equals concentration of products over concentrations of reactants. the concentrations are raised to the power of their coefficients

Question 4

law of mass action

Answer 4

law regarding the relationship between the balanced chemical equation and the expression of the equilibrium constant

Question 5

Kc

Answer 5

equilibrium constant with respect to concentration (M)

Question 6

Kp

Answer 6

equilibrium constant with respect to the partial pressures of the gas (atmospheres)

Question 7

concentration of ideal gas A

Answer 7

number of moles of A divided by its volume in litres

Question 8

ICE table

Answer 8

initial, change, equilibrium

Question 9

equilibrium

Answer 9

state where the forward and reverse rates of reaction are equal, and the concentration of products and reactants don’t change

Question 10

what happens to K when the reaction is reversed?

Answer 10

K is inverted

Question 11

K overall =

Answer 11

the product of K for the individual reactions

Question 12

reaction quotient (Q)

Answer 12

the same concept as equilibrium constant, just at any point of the reaction

Question 13

le chatlier’s principle

Answer 13

when a chemical system at equilibrium is disturbed the system shifts in a direction that minimizes the disturbance, aka it bounces back to an equilibrium

Question 14

decreasing volume shifts a reaction..

Answer 14

to the side with fewer moles of gas

Question 15

increasing volume shifts a reaction..

Answer 15

to the side with more moles of gas

Question 16

in an EXOthermic reaction, increased temp shifts it..

Answer 16

towards reactants, and K decreases

Question 17

in an EXOthermic reaction, decreased temp shifts it..

Answer 17

towards products, and K increases

Question 18

in an ENDOthermic reaction, increased temp shifts it..

Answer 18

towards products, and K increases

Question 19

in an ENDOthermic reaction, decreased temp shifts it..

Answer 19

towards reactants, and K decreases

Question 20

when Q>K, then…

Answer 20

the reaction shifts to consume more products

Question 21

when Q<K, then…

Answer 21

the reaction shifts to consume more reactants

Question 22

buffer

Answer 22

resists pH change by neutralizing the added acid or base. contains significant amounts of a weak acid and its conjugate base, or a weak base and its conjugate acid

Question 23

common ion effect

Answer 23

the tendency for a common ion to decrease the solubility of an ionic compound or decrease the ionization of a weak acid or weak base

Question 24

If pH<pKa…

Answer 24

then the buffer has more acid than base

Question 25

buffer capacity

Answer 25

the amount of acid or base that can be added to a buffer without causing a large pH change. goes up with higher absolute concentrations of the buffer

Question 26

molar solubility

Answer 26

solubility in moles per liter

Question 27

how to calculate solubility wit Ksp

Answer 27

1) write Ksp expresssion in terms of x 2) substitute in the value of Ksp, then solve for x 3) convert to grams

Question 28

selective precipitation

Answer 28

a process involving the addition of a reagent to a solution. The reagent forms a precipitate with one of the dissolved ions but not the others

Question 29

complex ion

Answer 29

an ion containing a central metal ion bound to one or more ligands

Question 30

ligand

Answer 30

neutral molecule or ion that acts as a lewis base with the central metal ion in a complex ion

Question 31

formation constant (Kf)

Answer 31

the equilibrium constant associated with reactions for the formation of complex ions