Acid-Base Equilibria

Question 1

tastes sour and causes dyes to change colour

Answer 1

Acids

Question 2

tastes bitter and feels soapy

Answer 2

Base

Question 3

increases [H+] when dissolved in solution

Answer 3

Arrhenius Acid

Question 4

increases [OH-] when dissolved in solution

Answer 4

Arrhenius Base

Question 5

H+ donor; donates a proton

Answer 5

Bronsted-Lowry Acid

Question 6

H+ acceptor; accepts a proton

Answer 6

Bronsted-Lowry Base

Question 7

two formulas that differ by H+

Answer 7

Conjugate Acid-Base Pair

Question 8

Conjugate ___ of a/an ___ has one fewer H+

Answer 8

base; acid

Question 9

Conjugate ___ of a/an ___ has one more H+

Answer 9

acid; base

Question 10

substance is one which can both donate and accept protons/hydrogen ions

Answer 10

Amphiprotic

Question 11

substances has reactions as both acid and base

Answer 11

Amphoteric

Question 12

All ____ substances are ____, but not all ____ substances are ____.

Answer 12

amphiprotic; amphoteric; amphoteric; amphiprotic

Question 13

in water, few molecules act as bases and few act as acids

Answer 13

autoionization of water

Question 14

Ion Product Constant (Kw)

Answer 14

Kw) = 1.0×10^(-14)

Question 15

[H+] and [OH-] if a solution is neutral

Answer 15

[H+] = [OH-]

Question 16

[H+] and [OH-] if a solution is acidic

Answer 16

[H+] > [OH-]

Question 17

[H+] and [OH-] if a solution is basic

Answer 17

[H+] < [OH-]

Question 18

formula for calculating pH

Answer 18

pH = -log[H+]

Question 19

formula for calculating [H+]

Answer 19

[H+] = 10^(-pH)

Question 20

formula for calculating pOH

Answer 20

pOH = -log[OH-]

Question 21

formula for calculating [OH-]

Answer 21

[OH-] = 10^(-pOH)

Question 22

relationship between pH and pOH

Answer 22

[H+][OH-] = 1.0×10^(-14)

pH + pOH = 14.00

Question 23

uses electrodes to indicate small changes in voltage to detect pH for accurate measurements

Answer 23

pH meter

Question 24

give less accurate, but quick measurements; compound that has one colour in its acid form and another in its basic form

Answer 24

indicators

Question 25

What are the common strong acids?

Answer 25

HCl, HBr, HI, HNO3, HClO3, HClO4, H2SO4

Question 26

donates only one proton ex: HCl, HBr, HI, HNO3, HClO3, HClO4

Answer 26

monoprotic

Question 27

donates two protons ex: H2SO4

Answer 27

diprotic

Question 28

What are the common strong bases?

Answer 28

KOH, NaOH, Ba(OH)2, CsOH, Sr(OH)2, LiOH

Question 29

strongest acid that can exist in an aqueous solution

Answer 29

H3O+

Question 30

strongest base that can exist in an aqueous solution

Answer 30

OH-

Question 31

formula for percent ionization

Answer 31

[H+]eq/[HA]initial × 100

Question 32

Relationship between KA and Kb

Answer 32

Ka × Kb = 1.0×10^(-14)

Question 33

shift in equilibrium causes by the addition of a compound having an ion in common with the dissolved substance

Answer 33

the common ion effect

Question 34

resist a change in pH when small amounts of a strong base or strong acid is added

Answer 34

buffer solutions

Question 35

Henderson-Hasselbalch Equation

Answer 35

pH = pKa + log([A-]/[HA]) [A-]/[HA] = antilog(pH-pKa) *pKa = -log(Ka)

Question 36

technique used to determine the concentration of an unknown solution

Answer 36

Titration

Question 37

solution of a known concentration which is added to another solution whose concentration has to be determined

Answer 37

Titrant

Question 38

solution whose concentration has to be determined

Answer 38

Analyte or Titrand

Question 39

point at which the amount of titrant added is enough to completely neutralise analyte solution; moles of base is equal to the moles of acids and the solution only contains salt and water

Answer 39

equivalent point

Question 40

substance (weak acid or weak base) that is added to the analyte solution and changes colour at or near the equivalence point

Answer 40

indicator

Question 41

point at which indicator changes colour in an acid-base titration

Answer 41

end point

Question 42

equivalence point of strong acid and strong base titration

Answer 42

pH = 7

Question 43

equivalence point of weak acid and strong base

Answer 43

pH > 7

Question 44

equivalence point of strong acid and weak base titration

Answer 44

pH < 7