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School > Chemistry - Chapter 19 > Flashcards

Chemistry - Chapter 19 Flashcards

1
Q

conjugate acid

A

the ion or molecule formed when a base gains a hydrogen ion

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2
Q

conjugate base

A

the ion or molecule that remains after an acid loses a hydrogen ion

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3
Q

conjugate acid-base pair

A

consists of two ions or molecules related by the loss or gain of one hydrogen ion

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4
Q

amphoteric

give an example

A

a substance that can act as either an acid or a base

ex. HCl = water accepts a proton –> base

NH4 = water donates a proton –> acid

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5
Q

hydronium ion

A

(H3O) the positive ion formed when a water molecule gains a hydrogen ion

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6
Q

Bronsted Lowry Theory

A

where an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor

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7
Q

self-ionization

A

a term describing the reaction in which two water molecules react to produce ions

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8
Q

neutral solution

what is the pH of this solution?

A

an aqueous solution in which the concentrations of hydrogen and hydroxide ions are equal

has a pH of 7.0

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9
Q

ion-product constant for water

A

(Kw) the product of the concentrations of the hydrogen ions and hydroxide ions in water

it is 1 x 10^-14 at 25°C

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10
Q

acidic solution

A

any solution in which the hydrogen-ion concentration is greater than the hydroxide-ion concentration

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11
Q

basic solution

A

any solution in which the hydroxide-ion concentration is greater than the hydrogen-ion concentration

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12
Q

pH

A

number used to denote the hydrogen-ion concentration, or acidity, of a solution

-log[H+] = pH

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13
Q

strong acid

A

an acid that is completely (or almost completely) ionized in an aqueous solution

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14
Q

weak acid

A

an acid that’s only slightly ionized in an aqueous solution

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15
Q

acid dissociation constant

A

(Ka) the ratio of the concentration of the dissociated form of an acid to the undissociated form

stronger acids have larger Ka values than weaker acids

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16
Q

strong base

A

a base that completely dissociates into metal ions and hydroxide ions in aqueous solutions

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17
Q

weak base

A

a base that reacts with water to form the hydroxide ion and the conjugate acid of the base

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18
Q

base dissociation constant

A

(Kb) the ratio of the concentration of the conjugate acid times the concentration of the hydroxide ion to the concentration of the base

19
Q

neutralization reaction

A

a reaction in which an acid and a base react tin an aqueous solution to produce a salt and water

20
Q

titration

A

process used to determine the concentration of a solution (often an acid or base) in which a solution of known concentration (the standard) is added to a measured amount of the solution of unknown concentration until an indicator signals the end point

21
Q

standard solution

A

a solution of known concentration used in carrying out a titration

22
Q

equivalence point

A

the point in a titration where the number of moles of hydrogen-ions equals the number of moles of hydroxide ions

23
Q

end point

A

the point in titration at which the indicator changes color

24
Q

List 3 rate of reaction factors:

A

Temperature

Concentration

Catalyst

25
Q

What is the equilibrium-constant equation?

A

Keq = [D^d} [C^c} / [B^b] [A^a}

26
Q

Arrhenius’s definition of acids and bases? (2)

A

acids are hydrogen containing compounds that ionize to yield hydrogen ions in aqueous solutions

bases are compounds that ionize to yield hydroxide ions in aqueous solutions

27
Q

What is Le Chatelier’s Principle?

A

if a stress is applied to a system in dynamic equilibrium, the system changes in a way that relieves the stress

28
Q

How are [H+] and [OH-] related in an aqueous solution?

A

the product of the hydrogen-ion concentration and the hydroxide-ion concentration equals 1.0 x 10^-14

** ion-product constant for water (Kw)

29
Q

Equation to find the ion-product constant for water (Kw)

A

Kw = [H+] x [OH-] = 1.0 x 10^-14

30
Q

Properties of water molecules (5)

A

highly polar

constantly in motion

+1 H2O molecule = H3O
-1 H2O molecule = [OH-]

Concentration of [H+] and [OH-] ions = 1.0 x 10^-7 M in pure water @ 25°C

31
Q

What is the direction of the shift in equilibrium with the addition or loss of water

A

The equilibrium shifts towards the formation of water

[H+] ^ = v [OH-]

32
Q

What can possibly change when finding the ion-product constant for water? (Kw)

What definitely won’t change?

A

Concentrations may change

Product stays the same

33
Q

basic solutions are also called…?

A

alkaline solutions

34
Q

How do you calculate the acid dissociation constant (Ka)?

A

Ka = [H+][A-] / [HA]

*equilibrium concentrations found with equilibrium constant formula

35
Q

How do you calculate the base dissociation constant (Kb)?

A

Kb = [conjugate acid] x [OH-] / [base]

*equilibrium concentrations found with equilibrium constant formula

36
Q

what do the words concentrated and dilute indicate?

what do they refer to?

A

they indicate how much of an acid or base is dissolved in solution

the number of moles of the acid or base in a given volume

37
Q

how to find the pH of a substance?

A

pH = -log[H+]

38
Q

how to find the [H+] of a substance? (when pH is not a whole number)

A

[H+] = 10^-pH (antilog)

39
Q

low pH =

high pH =

A

more acidic

more basic

40
Q

what is pH often measured with? (2)

A

acid-base indicators or a pH meter

41
Q

how to find [OH-]?

how to find pOH?

A

[OH-] = 10^-pOH

pOH = -log v10[OH-]

42
Q

Since [H+][OH-] = 1.0x10-14…. ?

A

pH + pOH = 14 (@25°C)

43
Q

at what point in a titration does neutralization occur?

A

when the number of moles of hydrogen ions is equal to the number of moles of hydroxide ions

44
Q

define salts

A

ionic compounds consisting of an anion (-) from an acid and a cation (+) from a base

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