HYS - CH10: Acids and Bases

Question 1

general acid base reaction

Answer 1

acid + base –> salt + water

Question 2

arrhenius definition of acids and bases

Answer 2

acids are hydronium ion donors
bases are hydroxide ion donors

doesnt explain all of them and only works with water

Question 3

lewis definition

Answer 3

acids accept an electron pair
basis donate an electron pair

Question 4

bronsted lowry defintion

Answer 4

acids donate a proton
bases accept a proton

Question 5

pH depends on

Answer 5

H+ (acidic) nd OH- (basic)

Question 6

hyrolysis of a salt to form a basic solution example

Answer 6

NaF

Question 7

hydrolysis of a salt to form an acidic solution ex

Answer 7

proton binds to water forming hydronium

Question 8

conjugate acid base pair

Answer 8

exists in a state where it has (acid) or lacks (basic) a proton

Question 9

identify the conjugate acid and base pair and the conjugate base and acid pair

Answer 9

H3PO4 is the acid bc it later donates an proton and looses it to become the conjugate base

H3O+ is the conjugate acid becuase it accepts a proton after being a base

H20 is the base becuase it later accepts a proton when it becomes a conjugate acid

Question 10

ampotheric

Answer 10

act as acid or base

Question 11

Keq, Ka, Kb

Answer 11

help us quantify if reaction goes forward or backwards based

Ka for acids - dissociation constant
Kb for bases - dissociation constant

Question 12

which species are included in equilibrium constant

Answer 12

only aqueous

Question 13

general Kb formula

Answer 13

Question 14

general Ka formula

Answer 14

Question 15

acid base chemistry is centered on interaction with

Answer 15

water

Question 16

Kw at STP

Answer 16

equilibrium constant of water

standard conditions; 25 C and 1 atom
Kw = 1 x 10^-14

Question 17

unit change in Ph causes

Answer 17

10 fold change in acidity

Question 19

if [H30+] is = [OH-] at STP then its
if [H30+] is > [OH-] at STP then its
if [H30+] is < [OH-] at STP then its

Answer 19

if [H30+] is = [OH-] at STP then its neutral
if [H30+] is > [OH-] at STP then its acidic
if [H30+] is < [OH-] at STP then its basic

Question 20

how to find pH (power of hydrogen) and pOH (power of hydroxide)

How to find the pka and the pkb

Answer 20

Question 21

pka + pkb =
ph+ pOH =
Ka*Kb =

Answer 21

Ka*Kb = Kw = 10^14
pka + pkb = 14
ph+ pOH = 14

Question 22

polyprotic acid

Answer 22

A substance capable of donating more than one proton is known as Polyprotic Acid. Diprotic and Triprotic are specific types of polyprotic acid capable of donating two and three protons, respectively.

Question 23

if Ka is large then kb must be
if kb is large then ka must be

Answer 23

if Ka is large then kb must be small
if kb is large then ka must be large

Question 24

strong acid and strong base

Answer 24

ka >1 is strong acid
Kb > 1 is a strong base

Question 26

strong acids and strong bases will _____ dissociate in aqeous solutions

Answer 26

will completely dissociate

dissociation - the breaking up of a compound into simpler constituents that are usually capable of recombining under other conditions.

Question 27

weak acids and weak bases will _____ dissociate in aqeous solutions

Answer 27

will not completely dissociate in aqeous solutions

Question 28

all strong acids

Answer 28

hydrochloric acid (HCl)
hydrobromic acid (HBr)
hydroiodic acid (HI)
sulfuric acid (H2S04)
nitric acid (HNO3)
chloric acid (HClO3)
perchloric acid (HClO4)

Question 29

all strong bases

Answer 29

sodium hydroxide (NaOH)
potassium hydroxide (KOH)
hydroxides formed from group 1 metals
cesium hydroxide (CsOH)
calcium hydroxide (Ca(OH2)
barium hydroxide (Ba(OH)2)
stronium hydroxide (Sr(OH)2)

Question 30

if you but a strong acid in aqeous solution they will___ protons

Answer 30

donate

Question 31

the conjugate cations of the strong bases are considered

Answer 31

inert

Question 32

weak acids and weak bases

Answer 32