Concepts Of Acids
Conjugate This!
To Base Or Not To Base
Hydrolysis
Take It To The pH Level
Ka-Boom!
Strong As Is
100

According to Bronsted-Lowry, _____ is a proton donor and _____ is a proton acceptor.

acid

base

17.1.2

100

HCl is a(n) _____. Its conjugate _____ is...

acid

base

Cl-

17.1.6

100

H2O(l)+NH3(aq) ->^2 OH-(aq)+NH4+(aq)

acid donor

base acceptor

conj. base

conj. acid

17.1.3

100

____ ____ occurs when ions produced by the dissociation of a salt react with water to produce ____ or ____.

salt hydrolysis

hydroxide ion

hydronium ion

17.2.31

100

Calculate the pH of a 0.074 M solution of HF. Ka for HF is 

6.5*10^-4

pH=2.16

review sheet 2, question 2

100

Kb= ?/? 

___= Ka*? 

Ka?/? 

Kb= (Kw)/(Ka) 

Kw= Ka*Kb 

Ka(Kw)/(Kb) 

17.2.42-43

100

HCl

hydrochloric acid 

17.1.10

200

A _____ _____ ionizes completely in water. It is present entirely as ions; it is a _____ electrolyte. 

example:HCl

strong acid

strong

17.1.10

200

HNO3 is a(n) _____. Its conjugate _____ is...

acid

base

NO3-

17.1.6

200

CH3COO-(aq)+H2O(l) ->^2 OH-(aq)+CH3COOH(aq)

base acceptor

acid donor

conj. base

conj. acid

17.1.3

200

Consider the solution of sodium cyanide, NaCN.

NaCN(s) -> Na+(aq)+CN-(aq)

A 0.1 M solution NaCN has a pH of 11.1 and is therefore fairly basic. How is this possible?

salt hydrolysis

17.2.30

200

Aniline, C6H5NH2, is used in the manufacture of some perfumes. What is the pH of a 0.200 M solution of aniline at  25^oC ?

Kb= 4.2*10^-10  at  25^oC .

pH= 8.96

17.2.29

200

____ is called the base ionization constant.

Kb

17.2.24

200

HI

hydroiodic acid

17.1.10

300

A ____ ____ is a substance that can accept a pair of electrons whereas a ____ ____ is a substance that can donate a pair of electrons. 

lewis acid

lewis base

17.2.53

300

SO42- is a(n) _____. Its conjugate _____ is...

base

acid

HSO4-

17.1.6

300

What does the word proton refer to in the context of conjugate acids and bases?

it refers to H+

17.1.8

300

Predict whether a 0.10-M solution of each of the following salts will be basic, acidic, or neutral:

a. KClO4

b. (CH3)3NHCl

c. K2C2O4

d. CH3NH3NO3

e. NaHCO3


a. neutral, neither K+ nor ClO4- hydrolyze

b. acidic, (CH3)3NH+ hydrolyzes

c. basic, C2O42- hydrolyzes

d. acidic, CH3NH3+ hydrolyzes

e. basic, HCO3- hydrolyzes 

17.2.38

300

Nitrous acid (HNO2) is a weak acid with a Ka of  4.5*10^-4 . Sodium nitrite (NaNO2) is therefore a strong base. What will be the pH of a solution of 0.065 M sodium nitrite?

pH=8.08

review sheet 2, question 4

300

A weak monoprotic acid is 0.50% ionized in a 1.0 M solution. Calculate the ionization constant of the acid.

Ka= 2.5*10^-5 

17.2.16

300

HBr

hydrobromic acid

17.1.10

400

A _____ _____ ionizes completely in water. It is present entirely as ions; it is a _____ electrolyte.

example: LiOH,NaOH,KOH

strong base

strong

17.1.11

400

H3PO4 is a(n) _____. Its conjugate _____ is...

acid

base

H2PO4-

17.1.6

400

a. the conjugate base of H2O...

b. the conjugate acid of O2-...

c. the conjugate acid of HCO3-...

d. the conjugate base of HSO4-...

a. OH-

b. OH-

c. H2CO3

d. SO42-

17.1.8


400

Will it hydrolyze?

HNO3

HCN

OH-

NH3

no

yes

no

yes

17.2.33

400

Calculate the pH at the titration endpoint, when 35.00 mL of 0.200 M methyl amine (CH3NH2) is titrated by 0.120 M hydrochloric acid. (KCH3NH24.4*10^-4 )

pH = 5.85

review sheet 2, problem 6

400

A 0.015 M solution of a weak acid has a pH of 4.27. What is the Ka for this acid?

Ka1.92*10^-7 

review sheet 2, question 1

400

HNO3

nitric acid

17.1.10

500

A _____ _____ ionizes partly in water. It is present primarily as molecules and partly as ions; it is a _____ electrolyte.

weak acid

weak

17.1.10

500

NHis a(n) _____. Its conjugate _____ is...

base

acid

NH4+

17.1.6

500

To find a conjugate base of a species, ____ a proton from the formula.

TO find the conjugate acid of a species, ____ a proton to the formula.

remove

add

17.1.8

500

Predict whether a 0.10 M solution of KNO2 will be basic, acidic, or neutral and why?

Ions in solution: K+ and NO2-

K+ is a Group 1A cation, and KOH is a strong base. NO2is the conjugate base of the weak acid HNO2.

The anion hydrolyzes, thus making the solution BASIC.

17.2.36

500

Oxalic acid (H2C2O4) is a diprotic acid with Ka1= 5.9*10^-2 and Ka26.4*10^-5 .What is the pH of the solution of 0.035 M oxalic acid? (can one neglect the second ionization?) 

pH=1.61

review sheet 2, question 3

500

Determine the Kb of the acetate ion (C2H3O2-). The Ka of acetic acid (HC2H3O2) is  1.8*10^-5 .

Kb= 5.6*10^-10 

17.2.44

500

H2SO4

sulfuric acid

17.1.10

600

The larger the value of ____, the ____ the acid.

Ka

stronger

17.2.3

600

C6H5O73- is a(n) _____. Its conjugate _____ is...

base

acid

HC6H5O72-

17.1.6

600

Predict Products:

PO43-(aq)+H2O(l) -> ? 

PO43- is a base because it accepts a proton. (HPO42-) = conjugate acid

H2O is an acid because it donates a proton. (OH-) = conjugate base

PO43-(aq)+H2O(l) -> HPO42-(aq)+OH-(aq)

17.1.9

600

Predict whether a 0.10 M solution of each salt will be basic, acidic, or neutral and why?

a. LiI

b. NH4NO3

a. Ions in solution: Li+ and I-

Li+ is a group 1A cation and LiOH is a strong base. I- is the conjugate base of the strong acid HI. Therefore the solution is neutral because neither hydrolyze. 

b. Ions in solution: NH4+ and NO3-

 NH4is the conjugate acid of the weak base NH3. NO3- is the conjugate base of the strong acid HNO3. Therefore the solution is acidic because the cation will hydrolyze. 

17.2.35

600

You are given 275 mL of a buffer which is 0.25 M in acetic acid and 0.15 M in sodium acetate. To this buffer you add 55 mL of 0.30 M sodium hydroxide. Calculate the pH of the buffer before and after the addition of the sodium hydroxide.

before: pH = 4.52

after: pH = 4.79

review sheet 2, question 5

600

Aspirin (acetylsalicylic acid, HC9H7O4) is a weak acid. It ionizes in water according to the equation: HC9H7O4(aq)+H2O(l) ->^2 H3O+(aq)+C9H7O4-(aq). A 0.10 M aqueous solution of aspirin has a pH of 2.27 at  25^oC . Determine the Ka of aspirin.

 3.0*10^-4 

17.2.15

600

HClO3

chloric acid

17.1.10

700

A _____ _____ ionizes partly in water. It is present primarily as molecules and partly as ions; it is a _____ electrolyte. These are nitrogenous ____ such as NH3.

weak base

weak

bases

17.1.11

700

H2O is a(n) _____. Its conjugate _____ is...

acid and base

base, OH-

acid, H3O+

17.1.6

700

Predict Products:

H2PO4-(aq)+CN-(aq) -> ? 

H2PO4- donates an electron, therefore is an acid. (HPO42-) = conjugate base

CN- accepts an electron, making it a base. (HCN) = conjugate acid

H2PO4-(aq)+CN-(aq) -> HPO42-(aq)+HCN(aq)

17.1.9

700

Write the hydrolysis reactions and K expressions for:

a. (CH3)3NH+

b. C2O42-

c. CH3NH3+

d. HCO3-


a. (CH3)3NH++ H2O ->^2 (CH3)3N+H3O+

Ka=[(CH3)3N][H3O+]/[(CH3)3NH+]

b. C2O42-+H2O ->^2 HC2O4-+OH-

Ka=[HC2O4-][OH-]/[C2O42-]

c. CH3NH3++H2O ->^2 CH3NH2+H3O+

Ka=[CH3NH2][H3O+]/[CH3NH3+]

d. HCO3-+H2O ->^2 H2CO3+OH-

Ka=[H2CO3][OH-]/[HCO3-]

17.2.40

700

What is the pH of a 0.040 M ammonia solution at  25^oC. Kb1.8*10^-5. 

pH=10.93

17.2.28

700

Determine the Kof the methyl ammonium ion (CH3NH3+)

Kof methyl amine (CH3NH2) is  4.4*10^-4 .

Ka= 2.3*10^-11 

17.2.45

700

HClO4

perchloric acid

17.1.10