Properties of Solutions (Acids + Bases + Buffers + titrations)

Question 1

what is the ionic product of water

Answer 1

1 x 10^-14

Question 2

what is a bronsted-Lowry acid ?

Answer 2

electron acceptor

Question 3

what is a Bronsted-Lowry Base?

Answer 3

electron donor

Question 4

what does amphoteric mean ?

Answer 4

able to act as both an acid and a base.

Question 5

what is an Arrhenius acid?

Answer 5

a species which increases the number of H30+ ions when dissolved in water (pH decreases)

Question 6

what is a Arrhenius base?

Answer 6

a species which increases the number of OH- ions when dissolved in water (pH increases)

Question 7

the Arrhenius acids are limited to …

Answer 7

aqueous solutions

Question 8

the equation for strong acid pH =

Answer 8

-log (c H30+/c standard)

Question 9

in an acid base reaction the equilibrium favours the side with the … this is because…

Answer 9

weaker acid and base, because they are more stable and have lower potential energies.

Question 10

how do we determine the pH of weak acids/bases

Answer 10

first we find the equilibrium constant - in this case known as the Ka (acid dissociation constant)

Question 11

Ka of pure liquids =

Answer 11

1

Question 12

using the Ka we can calculate the …

Answer 12

pKa

Question 13

for weak acids the equilibrium lies far to the…

Answer 13

left

Question 14

what does HA stand for

Answer 14

the acid which dissociates into the conjugate acid (A-)

Question 14

what should you do after writing the equation for finding the Ka of weak acids?

Answer 14

create the initial and equilibrium table.

Question 14

what’s the first step for finding the pH of weak acids

Answer 14

finding the Ka (equation sheet)

Question 14

after finding x in the pH weak acid calculations, how do you find the pH?

Answer 14

pH = -logx

Question 14

pKa + pKb =

Answer 14

pKw = 14

Question 14

Ka x Kb =

Answer 14

Kw

Question 14

what is the inductive effect?

Answer 14

occurs when electron-withdrawing or electron-donating groups in a molecule cause a change in electron density. this causes the pH to change.

Question 14

the ___ resonance forms the ____ stable the anion and hence the stronger the acid

Answer 14

more, more

Question 14

what makes up a buffer solution?

Answer 14

mix of either a weak acid or base and its corresponding salt.

Question 15

the Henderson-hasselbalch help to determine the pH of what?

Answer 15

buffer solutions

Question 16

what is the first step of finding buffer pH of the weak acid and strong base titration?

Answer 16

calculating the initial moles of the reactants

Question 17

what is the second step finding buffer pH of the weak acid and strong base titration?

Answer 17

calculating the final moles of the weak acid and its conjugate base

Question 18

final moles of the weak acid =

Answer 18

initial moles of weak acid - initial moles of strong base

Question 19

final moles of conjugate base =

Answer 19

initial moles of strong base

Question 20

what is the 3rd step of find the buffer pH of a weak acid and strong base titration?

Answer 20

using the buffer pH equation

Question 21

how do you find the pKa from the Ka

Answer 21

pKa = -log(Ka)

Question 22

what is the equivalence point?

Answer 22

when the same volume of the acid and base have been used in the titration

Question 23

what is the halfway point

Answer 23

when half the volume of weak acid (in the burette) is added to the base.

Question 24

what is a lewis base

Answer 24

an electron pair donor

Question 25

what is a lewis acid

Answer 25

an electron pair acceptor

Question 26

what does association mean ?

Answer 26

the addition of two or more substances together to form a larger entity

Question 27

what is the Kw of water ?

Answer 27

1 x 10 -14