Acid-Base Equilibrium Exam

A 0.100 M solution of calcium formate is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

BS

A 0.100 M solution of lithium perbromate is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

BS

A 0.100 M solution of potassium hypoiodite is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

BS

A 0.100 M solution of rubidium propanoate is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

BS

A 0.100 M solution of sodium chlorite is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

BS

A 0.100 M solution of strontium fluoride is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

BS

A 0.100 M solution of strontium trichloroacetate is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

BS

conjugate base of HCO3-

CO32-

conjugate base of HClO4

ClO4-

an acid increases the _______ when dissolved in H2O

H+

B + H2O <-> BH+ + OH- identify: acid, base, conjugate acid, conjugate base, acid base pairs

H2O B BH+ OH- B/BH+ OH-/H2O

CH3NH2 + H2O <-> Ch3NH3+ + OH- identify: acid, base, conjugate acid, conjugate base, acid base pairs

H2O CH3NH2 CH3NH3+ OH- H2O/OH- CH3NH3+/CH3NH2

[OH] > [H3O]

basic solution

Which of the following equations is representative of a strong base solution? Select one: a. A- + H2O (darrow) OH- + HA b. HA + H2O → H3O+ + A- c. B + H2O → OH- + BH+ d. HA + H2O (darrow) H3O+ + A- e. BH+ + H2O (darrow) H3O+ + B f. B + H2O (darrow) OH- + BH+ g. neutral cations/anions pH = 7.00

c. B + H2O → OH- + BH+

a base can react with a proton (H+) to produce a cation (BH+) called a

conjugate acid

base + proton =

conjugate acid

HA and A- represent a

conjugate acid base pair the only difference between them is 1 proton

B and BH+ represent a

conjugate acid-base pair

acid losing proton=

conjugate base

an acid can dissociate to give a proton (H+) and an anion (A-) called a

conjugate base

The concentration of pure water is approximately ________ M. Select one: a. 83.3 b. 18.02 c. 100 d. 55.6 e. 1.00

d. 55.6

n the gas phase reaction below, NH3 is acting as a(n) ______ base, but not as a(n) _______ base. NH3 + H+ → NH4+ Select one: a. Arrhenius, Lewis b. Lewis, Bronsted-Lowry c. Arrhenius, Bronsted-Lowry d. Lewis, Arrhenius e. Bronsted-Lowry, Lewis

d. Lewis, Arrhenius

What is the conjugate base of OH-? Select one: a. H3O+ b. H2O c. O- d. O2- e. O2

d. O2-

According to the Arrhenius concept, an acid is a substance that _______. Select one: a. autoionization of that solvent b. reacts with the solvent to form the cation formed by c. tastes bitter d. causes and increase in the concentration of H+ in aqueous solutions e. is capable of donating one or more H+ can accept a pair of electrons to form a coordinate covalent bond

d. causes and increase in the concentration of H+ in aqueous solutions

The molar concentration of hydronium ion in pure water at 25oC is ________ . Select one: a. 1.00 x 10-14 b. 7.00 c. 0.00 d. 1.00 e. 1.00 x 10-7

e. 1.00 x 10-7

What is the conjugate acid of HSO4-? Select one: a. OH- b. SO42- c. H3SO4+ d. HSO4+ e. H2SO4

e. H2SO4

Which of the following statements about strong acids is true? Select one: a. Strong acids are very concentrated acids. b. Strong acids produce solutions with a higher pH than weak acids. c. The conjugate base of a strong acid is itself a strong base. d. All acids have H atoms bonded to electronegative oxygen atoms. e. Strong acids are 100% ionized in water.

e. Strong acids are 100% ionized in water.

weak acids (HA)

every acid that isnt a strong acid dissociate less than 100% and are in equilibrium with their conjugate bases and so you must use an ICE box

weak bases (B)

every base that isnt a strong base dissociate less than 100% and are in equilibrium with their conjugate acids and so you must use an ICE box

shortcut for salt solutions?

for salt solutions you can ALWAYS USE SHORTCUT

strong bases

group 1 hydroxides: LiOH NaOH KOH RbOH CsOH heavy group 2 hydroxides Ca(OH)2 Sr(OH)2 Ba(OH)2 also 100% dissociation here

polyprotic acids

having more than one acidic proton all weak acids means you will have a Ka1 and Ka2, but Ka1 will always be larger value and you should use Ka1 alone

how to know if you can use SHORTCUT in weak acid and weak base problems

if [HA]0 / Ka > 100 then use shortcut!!! if [B]0 / Kb > 100 then use shortcut!!!

as you dilute, pH ______, % ionization _______ too

increases, increases

[H3O] = [OH]

neutral solution

when acids and bases react, they form water and a salt in a __________________ reaction

neutralization

compare CH4, NH3, H2O, and HF in polarity and acidity

nonpolar CH4 < NH3 < H2O < HF polar neutral CH4 > NH3 > H2O > HF weak acid

large, small charged cations: Na+, K+, Rb+ =

nuetral solutions

review: weak bases

only slightly dissociated B + H2O <-> HB+ + OH- make ICEBOX use Kb if [B]0 / Kb > 100 then use shortcut!!! solve for x = [OH-] pOH= -log[OH-] pH = 14.00 - pOH

review: acidic salts

only slightly hydrolyzed HB+ + H2O <-> H3O+ + B make ICEBOX use Kb of conjugate base to calculate Ka write equi. expression with Ka solve for x using shortcut x = [H3O+] pH = -log[H3O+]

review: basic salts

only slightly hydrolyzed A- + H2O <-> B + OH- make ICEBOX use Ka od conjugate acid to calculate Kb write equi. expression using Kb solve for x using shortcut always= [OH-] pOH= -log[OH-] pH = 14.00 - pOH

acidic salt solutions

pH < 7

neutral salt solutions

pH = 7

? pH of 0.00034 M Ca(OH)2?

pOH= -log(0.00068) = 3.17 pH= 10.83 you double the molarity because of the 2 equivalencies of OH (Ca(OH)2)

basic salt solutions

ph > 7

dative bond

resides between 2 molecules such as AlCl3 and NF3 forming a lewis acid-base complex

acids bases

sour slippery together form salt water as a neutral sol.

a salt derived from _______ and ______ will form an acidic salt solution

strong acid, weak base

a salt derived from _________ and a ________ will form a basic solution

strong base, weak acid

highly polar bonds = ________ acids

stronger

salt hydrolysis

the dissociation of a salt and the reaction of either the anion or cation or both in H2O

oxyacids

the greater the number of oxygen atoms, the greater the acidity

if A- is unstable, then HA is a ______ acid

weak

strong bonds = _______ acids

weak

% ionization

(how much the parent molecule has dissociated and where does the equilibrium lay?) = [H3O+]eq / [HA]0 x 100% = [OH-]eq / [B]0 x 100%

pH

-log[H3O+]

pOH

-log[OH-] to get pH, just subtract pOH from 14

Which one of the following cannot act as a Lewis base? Select one: a. NH3 b. BF3 c. CN- d. Cl- e. H2O

. BF3

7 strong acids

1. HCl 2. HBr 3. HI 4. HClO4 5. HClO3 6. HNO3 7. H2SO4 every other acid will be treated as weak

conjugate bases of STRONG acids DO NOT undergo hydrolysis

1. HCl Cl- - neutral anion 2. HBr Br- - neutral anion 3. HI I - neutral anion 4. HClO4 ClO4- - neutral anion 5. HClO3 ClO3- - neutral anion 6. HNO3 NO3- - neutral anion 7. H2SO4 HSO4- - neutral anion

review: strong acids

100 % dissociated HA + H2O -----> H3O + A- [H3O]eq = [HA]0

all STRONG ACIDS ____________ in water

100% dissociate

review: strong bases

100% dissociated MOH ------> M+ + OH- or M(OH)2 -----> M2+ + 2OH- [OH-]eq = [MOH]0

the neutral anions and neutral cations of the 7 and 8 strong acids and bases can be together to form a salt such as NaCl--- there 7x8= 56 possible combinations and you can recognize them so their pH =

7

.100 M solution of pyridinium nitrate is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

AS

A 0.100 M solution of ammonium bromide is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

AS

A 0.100 M solution of anilinium chlorate is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

AS

A 0.100 M solution of diethylammonium chlorate is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

AS

A 0.100 M solution of hydrazinium iodide is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

AS

A 0.100 M solution of m-nitroanilinium perchlorate is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

AS

A 0.100 M solution of methylammonium nitrate is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

AS

A 0.100 M solution of triethylammonium iodide is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

AS

Kw

= 1.0 x 10^-14 constant value that will not change w stands for water

eq for any basic salt solution and hydrolysis

A- + H2O <-> HA + OH- % hydrolysis = [OH]eq / [A-]0 x 100%

Which of the following equations is representative of a weak base solution? Select one: a. neutral cations/anions pH = 7.00 b. HA + H2O → H3O+ + A- c. HA + H2O (darrow) H3O+ + A- d. B + H2O (darrow) OH- + BH+ e. BH+ + H2O (darrow) H3O+ + B f. A- + H2O (darrow) OH- + HA g. B + H2O → OH- + BH+

B + H2O (darrow) OH- + BH+

weak bases eq for ICEbox

B + H2O <-> HB+ + OH- use Kb always

compare H2O, H2S, H2Se, and H2Te in bond strength and acidity

H2O > H2S > H2Se > H2Te H2O < H2S < H2Se < H2Te

conjugate acid of HSO3-

H2SO3

hydronium ion

H3O+

review: weak acids

HA + H2O <-> H3O +A- only slightly dissociated make ICEBOX use Ka if [HA]0 / Ka > 100 then use shortcut!!! solve for x = [H3O] pH = -log[H3O+]

ICEbox eq for weak acids

HA + H2O <-> H3O+ + A- use this equation to set up ICEbox and always use Ka

HA + H2O <-> H3O+ + A- identify: acid, base, conjugate acid, conjugate base, acid base pairs

HA, H2O, H3O, A HA/A H2O/H3O

eq for any acidic salt solution and hydrolysis

HB+ + H2O <-> H3O+ + B % hydrolysis = [H3O+]eq / [HB+] x 100%

HBrO4 + H2O <-> H3O+ + BrO4- identify: acid, base, conjugate acid, conjugate base, acid base pairs

HBrO4 H2O H3O BrO4 HBrO4/BrO4 H2O/H3O

string acids and bases and their conjugates

HCL (strong acid) has NEUTRAL conjugate base- Cl- NaOH (strong base) has NEUTRAL conjugate acid- Na+

conjugate acid of CO

HCO+

conjugate acid of F-

HF

compare HF, HCl, HBr, and HI in bond strength and acidity

HF > HCl > HBr > HI HF < HCl < HBr < HI

conjugate acid of PO4-3

HPO42-

conjugate base of H2S

HS-

A 0.10 M aqueous solution of ________ will have a pH of 7.0 at 25oC. NaOCl KCl NH4Cl Ca(ClO2)2 Select one: a. NH4Cl b. KCl c. Ca(ClO2)2 d. NaOCl e. KCl and NH4Cl

KCl

The molar solubility of __________ is not affected by the pH of the solution. Select one: a. MnS b. Na3PO4 c. KNO3 d. AlCl3 e. NaF

KNO3

Kb =

Kb = [HB+][OH-] / [B] and get Kb from table

In the reaction BF3 + F- → BF4- BF3 acts as a(n) __________ acid. Select one: a. Arrhenius and Bronsted-Lowry b. Lewis c. Arrhenius d. Bronsted-Lowry e. Arrhenius, Bronsted-Lowry, and Lewis

Lewis

cations of STRONG bases DO NOT undergo hydrolysis

LiOH Li+ (neutral cation) NaOH Na+ (neutral cation) KOH K+ (neutral cation) RbOH Rb+ (neutral cation) CsOH Cs+ (neutral cation) Ca(OH)2 Ca2+ (neutral cation) Sr(OH)2 Sr2+ (neutral cation) Ba(OH)2 Ba2+ (neutral cation)

A 0.100 M solution of cesium iodide is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

NS

A 0.100 M solution of lithium chlorate is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

NS

a base increases the ________ when dissolved in H2O

OH-

conjugate base of PH4+

PH3

A 0.100 M solution of chloric acid is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

SA

A 0.100 M solution of hydrobromic acid is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

SA

A 0.100 M solution of rubidium hydroxide is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

SB

A 0.100 M solution of monochloroacetic acid is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

WA

A 0.100 M solution of magnesium hydroxide is a ___ solution. SA (strong acid; acidic) SB (strong base; basic) WA (weak acid; acidic) WB (weak base; basic) NS (neutral salt; pH = 7) AS (acidic salt; acidic) BS (basic salt; basic)

WB

Which of the following aqueous solutions has the highest [OH-]? Select one: a. a solution with a pH of 3.00 b. pure water c. a solution with a pOH of 12.00 d. a 1.00x10-3 M solution of NH4Cl e. a 1.00x10-3 M solution of HNO3

b. pure water

Ka=

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

Kw =

[H3O+]x[OH-]

Predict which member of each pair produces the more acidic aqueous solution. K+ or Cu2+ Fe2+ or Fe3+ Al3+ or Ga3+ Select one: a. Cu2+, Fe2+, and Al3+ b. K+, Fe2+, and Ga3+ c. Cu2+, Fe3+, and Al3+ d. Cu2+, Fe3+, and Ga3+ e. K+, Fe3+, and Al3+

a. Cu2+, Fe2+, and Al3+

In basic solution, _________. Select one: a. [H3O+] < [OH-] b. [H3O+] > [OH-] c. [H3O+] = [OH-] d. [H3O+] = 0 M e. [H3O+] > 7.00

a. [H3O+] < [OH-]

A Bronsted-Lowry acid is defined as a substance that _________ . Select one: a. acts as a proton donor b. acts as a proton acceptor c. increases [H+] when placed in water d. increases [OH-] when placed in water e. decreases [H+] when placed in water

a. acts as a proton donor

A 0.0035 M aqueous solution of a particular compound has a pH = 2.46. The compound is a ___________ . Select one: a. strong acid b. weak acid c. strong base d. acidic salt e. weak base

a. strong acid

The magnitude of Kw indicates that __________. Select one: a. water autoionizes only to a very small extent b. water autoionizes very quickly c. water autoionizes very slowly d. the autoionization of water is exothermic e. the autoionization of water is endothermic

a. water autoionizes only to a very small extent

[h3O] > [OH]

acidic solution

small, highly charged cations: Al3+, Ga3+, Sn4+ =

acidic solutions

____________ substances can act as an acid or a base

amphoteric substances ex: H2O proton donor or acceptor

bronsted-lowry acids and bases

an acid is a proton donor a base is a proton acceptor

lewis acid

an electron pair acceptor group 13 compounds, transition metal-cations

lewis base

an electron pair donor group 15 compounds, any compound that contains a lone pair of electrons

examples of lewis bases

any single lewis dot structures that have at least 1 pair of lone electrons

salts

are strong electrolytes and undergo 100% dissociation

What is the conjugate acid of OH-? Select one: a. O2- b. H2O c. O2 d. H3O+ e. O-

b. H2O

Which of the following equations is representative of a weak acid solution? Select one: a. A- + H2O (darrow) OH- + HA b. HA + H2O (darrow) H3O+ + A- c. B + H2O (darrow) OH- + BH+ d. BH+ + H2O (darrow) H3O+ + B e. HA + H2O →H3O+ + A- f. B + H2O → OH- + BH+ g. neutral cations/anions pH = 7.00

b. HA + H2O (darrow) H3O+ + A-

An aqueous solution of ____________ will produce a basic solution. Select one: a. NaCl b. Na2SO4 c. KBr d. NH4ClO4 e. NaHSO4

b. Na2SO4

In acidic solution, _________. Select one: a. [H3O+] < [OH-] b. [H3O+] > [OH-] c. [OH-] > 7.00 d. [H3O+] = 0 M e. [H3O+] = [OH-]

b. [H3O+] > [OH-]

A Bronsted-Lowry base is defined as a substance that __________. Select one: a. increases [OH-] when placed in water b. acts as a proton acceptor c. acts as a proton donor d. decreases [H+] when placed in water e. increases [H+] when placed in water

b. acts as a proton acceptor

substance that is capable of acting as both an acid and a base is __________. Select one: a. miscible b. amphoteric c. autosomal d. autocratic e. conjugated

b. amphoteric