04/22

Question 1

what is advanced equilibria

Answer 1

it is equilibria that involves more than a single reaction where the concentrations of the products or reactants are reliant on each other

Question 2

what is the difference between a weak acid and a strong acid

Answer 2

a weak acid partially dissociates, some of the HX is still present in solution

a strong acid dissociates completely, none of the HX is present in the solution

Question 3

if we have a small ka, what does it mean?

Answer 3

it means our acid is very weak and not good at making H30+

Question 4

if we have a large ka, what does it mean?

Answer 4

it means our acid is very strong and good at making H3O+

Question 5

what is the difference between weak bases and strong bases

Answer 5

strong bases dissociate completely to give OH

weak bases do not dissociate completely (Some XOH is left)

Question 6

what is true about conjugate acid base pairs and equilibrium constants

Answer 6

ka*kb=kw

if we know one we can find the other

Question 7

what is kw at 25 C

Answer 7

1x10^-14

Question 8

if our dissociative ions form strong acids or bases when dissolved in water, would that actually happen and contribute to the PH?

Answer 8

no, it is unstable to form a strong acid or base and equilibrium favors the formation of weak acids/bases

Question 9

when are ions recognizable as conjugate acids or bases?

Answer 9

when they form weak acids or bases in water

Question 10

conjugate bases of weak acids form what types of solutions

Answer 10

basic solutions

Question 11

conjugate acids of weak bases form what types of solutions

Answer 11

acidic solutions

Question 12

how will NaBr affect the PH when dissolved in water

Answer 12

neutral no change

Na is the conjugate to a strong base
Br is the conjugate to a strong acid

Question 13

how will NH4Cl affect pH when dissolved in water

Answer 13

NH4 is the conjugate acid to a weak base —> acidic

Cl is the conjugate base to a strong acid—> neutral

the pH will be acidic

Question 14

how will K2HPO4 effect pH

Answer 14

the solution will be basic

K is the conjugate to a strong base, so it is neutral

the HPO4 is the conjugate to a weak acid and forms hydroxide so it will be basic

Question 15

how will KCH3COO affect PH?

Answer 15

it will be basic

Question 16

when we add an “inert” salt to a not very soluble salt, what happens to the solubility of the salt

Answer 16

it increases the solubility

Question 17

why does adding an inert salt increase the solubility?

Answer 17

it increases the ionic strength of a solution which increases the charge on the ionic atmosphere.

The ionic atmosphere decreases the attraction between the ions in the salt (Ca2+ and SO4^2-) which increases the solubility

Question 18

what interaction is being described by adding ions to a solution with an insoluble salt?

Answer 18

its an electrostatic interaction

Question 19

what is the ionic atmosphere

Answer 19

it is the region of net positive or negative charge around a cation or anion in a solution

Question 20

in a solution with an inert salt, an anion is surrounded by

Answer 20

excess cations

Question 21

in a solution with an inert salt, a cation is surrounded by

Answer 21

excess anions

Question 22

when you have a greater ionic strength, what happens to the charge in the atmosphere

Answer 22

it is higher

Question 23

what is ionic strength

Answer 23

it is u and is a measure of the total concentration of ions in a solution

Question 24

if you have a highly charged ion, what is the influence on u

Answer 24

it has a higher influence lol

Question 25

why do we not include H30 and Oh in the ion strength calculation

Answer 25

if we have a neautral solution, they have a negligible affect on the strength

Question 26

is a solution of CaCl in water, what ions are present and which do we care about

Answer 26

Ca, Cl, H+ and Oh- are in the solution but H and OH are neglible and do not contribute to the ionic strength sufficiently enough to be considered