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DAT GenChem > GenChem10 (Acids and Bases) > Flashcards

GenChem10 (Acids and Bases) Flashcards

1
Q

An indicator which turns red in acidic solution and blue in basic solution

A

Litmus Paper

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2
Q

Defines acids as a species that produces H+ (a proton) in an aqueous solution and a base as a species that produces OH- (a hydroxide ion) in an aqueous solution.

A

Arrhenius Definition

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3
Q

Defines acids as a species that donates protons, and a base as a species that accepts protons.

A

Bronsted-Lowry Definition

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4
Q

Defines an acid as an electron pair acceptor and a base as an electron pair donor.

What are the exceptions?

A

Lewis Definition

BCl3 and AlCl3

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5
Q

Acids formed from anions whose names end in ide have the prefix _____ and the ending ___

A

hydro, ic

hydrofluoric acid - HF
hyrdobromic acid -HBr

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6
Q

Acids formed from oxyanions are called

If the oxyanion ends in -ite, it has more/less oxygen and the acid ends in ______

If an oxyanion ends in -ate, it has more/less oxygen and the acid ends in

A

oxyacids

An oxyanion ending in -ite has less oxygen and the acid ends in -ous.

An oxyanion ending in -ate has more oxygen and the acid ends in -ic

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7
Q 
ClO-
ClO2-
ClO3-
ClO4-
NO2-
NO3-
A 
ClO-Hypocholorite
ClO2- Chlorite
ClO3-Chlorate
ClO4-Perchlorate
NO2-Nitrite
NO3-Nitrate
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8
Q 
HClO
HClO2
HClO3
HClO4
HNO2
HNO3
A 
Hypochlorous acid
Chlorous Acid
Chloric Acid
Perchloric Acid
Nitrous Acid
Nitric Acid
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9
Q

If Ka= 1.8*10^-5, what is pka?

A

slightly less than 5

exactly 4.74

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10
Q

What property do strong acids and bases have?

A

They completely dissociate into there component ions in aqueous solution

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11
Q

Name the strong acids that you should be aware of

A 
HCl
HBr
HI
HNO3
HClO3
HClO4
H2SO4
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12
Q

What is an amphoteric (amphoprotic) compound?

A

It can be an acid or base

ex) HCO3-

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13
Q

The stronger an acid the weaker/stronger the base

A

Weaker the base!

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14
Q

Name the strong bases that you should be aware of.

A

Group I and II metal hydroxides

LiOH
NaOH
KOH
RbOH
CsOH

Ca(OH)2
Sr(OH)2
Ba(OH)2
Magnesium not included because it’s not soluble

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15
Q

What is the equation for Ka?

A

Ka=[H30+][A-]/([HA])

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16
Q

What is the equation for Kb?

A

Kb=[B+][OH-]/[BOH]

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17
Q

A reaction with acids and bases reacting with each other, forming a salt and often water

A

Neutralization Reaction

Ex: HA + BOH —> BA + H2O

18
Q

A reaction in which salt ions react with water to give back an acid or base, also considered the reverse of a neutralization reaction

A

Hydrolysis

19
Q

What are the 4 combinations of strong and weak acids/bases?

A

SA/SB
SA/WB
WA/SB
WA/WB

20
Q

What are the products of a reaction between equal concentrations of a SA and SB?

What is the resulting pH?

Do the resulting ions react with water?

A

Salt and water

pH=7 (neutral)

No

21
Q

What is the product of a reaction between a strong acid and a weak base?

A

Salt, usually no water

22
Q

What happens when HCl reacts with NH3 in aqueous solution?

Why does this occur?

A

NH3 + HCL —> NH4(+) + CL(-)
NH4(+) + H2O —-> NH3 + H3O(+)

The conjugate acid (NH4+) is stronger than the conjugate base (CL-) of the strong acid HCL. NH4 reacts with OH, producing an excess of H+.

23
Q

What is the product of a reaction between an weak acid and a strong base?

A

A basic solution

24
Q

What is the product of a reaction between a weak acid and a weak base?

A

It depends upon the Ka and Kb for the reactants, whichever is higher will cause the solution to be acidic or basic

25
Q

What is the one diprotic strong acid?

How many acid equivalents does it produce?

A

H2SO4

2

26
Q

What is the normality of a concentration of 2M H3PO4?

A

6N

27
Q

What is the equivalent weight of H2SO4 (molecular weight = 98g/mol)

A

49 g; that is, 49 g of H2SO4 releases 1 acid equivalent

28
Q

A species that can act as an acid or a base, depending upon its chemical environment, is called

A

amphoteric or amphiprotic

Ex) Water

29
Q

When water reacts as a base, it behaves as an

When water react with an acid, it behaves as a

A

Acid
H2O + B- —–> NH + OH-

Base
H2O + HA —-> H3O(+) + A-

30
Q

The conjugate base of a polyprotic acid is usually

A

amphoteric

ex) HSO4

31
Q

The hydroxides of certain metals (Al, Zn, Pb, Cr) are

A

Amphoteric

32
Q

A procedure used to determine the molarity of an acid or base. It is accomplished by reacting a known volume of a solution of an unknown concentration with a known volume of a solution of a known concentration

A

Titration

33
Q

In titration, the point at which the acid equivalents equal the base equivalents is known as the

Does this point always occur at pH of 7?

A

Equivalence point

No, only for strong acids/strong base titrations

34
Q

Under what conditions are there several equivalence points?

A

When titrating polyprotic acids or bases

35
Q

Weak organic acids or bases that have different colors in their undissociated and dissociated states. Used in titrations, are in low concentration and don’t alter the equivalence point

A

Indicator

36
Q

The point at which the indicator changes color is called the

This is not the equivalence point, can the volume of the endpoint be used?

A

End point

Because there is very little difference in volume between the equivalence point and the end point (look at the graph on p. 397), and it may be corrected for or ignored.

37
Q

What is the equation to calculate the volume added in a titration using normality?

What is the equation for normality?

What about gram equivalents?

A

VaNa=VbNb

gram equivalents/volume of solution

gram equivalents

38
Q

How is the titration curve of a weak acid using a strong base different from a strong acid using a strong base?

A

The pH is higher at the beginning and the pH changes most significantly early on.

Importantly, the equivalence point is in the basic range.

39
Q

Consists of a mixture of a weak acid and its salt, or a mixture of a weak base and its salt.

A

Buffer Solution

ex: acetic acid (CH3COOH) and its salt (CH3COO-Na+)

ammonia (NH3) and its salt ammonium chloride (NH4+ CL-)

40
Q

What is the equation used to estimate the pH of a solution in the buffer region where the concentrations of the species and its conjugate are present in approximately equal concentrations

For a weak acid buffer solution:
For a weak base buffer solution:

A

pH=pKa + log[conjugate base]/[weak acid]

pH=pKb + log[conjugate acid]/[weak base]

DAT GenChem (11 decks)

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