Acid-Base Equilibria Jeopardy Review

Unit 15.1 Jeopardy Review:

Acid-Base Equilibria

SEE SEPARATE WORKSHEET FOR

WORKED OUT ANSWER SOLUTIONS

Question #1

Which of the following is a property of an acid?

a)

Feel like water

b)

Turn litmus paper blue

c)

React vigorously with metals higher on the

activity series

d)

Taste bitter

e)

Conduct electric current

*You may choose more than one option

Answer #1:

a)

Feel like water

c)  React vigorously with metals higher on the

activity series

e) Conduct electric current

Question #2

In a neutralization reaction, strong

acids combine with strong bases so

that the properties of both are lost.

 What are the 2 general products

of a neutralization reaction?

Answer #2:

water + salt

Question #3

Which statement below is true?

a)

An Arrhenius acid accepts hydrogen ions

when dissolved in water.

b)

A Bronsted-Lowry base generates hydroxide

ions when dissolved in water.

c)

A Lewis acid can accept a pair of electrons.

Answer #3:

c) A Lewis acid can accept a pair of electrons.

Question #4

Name two problems with the

Arrhenius definition of acids

and bases.

Answer #4:

•

It is restricted to aqueous solutions.

•

It does not explain why some bases do

not contain OH

 ions (ex: NH

Question #5

Give the name AND formula for the

seven strong acids we discussed in

class.

Answer #5:

Hydrochloric Acid, HCl

Hydrobromic Acid, HBr

Hydroiodic Acid, HI

Chloric Acid, HClO

Perchloric Acid, HClO

Sulfuric Acid, H

SO

Nitric Acid, HNO

Question #6

All of the alkali metals, when

combined with hydroxide, are

considered to be strong bases.

Which three alkaline earth metals are

also classified as strong bases when

combined with hydroxide?

*Give chemical formula of

these bases

Answer #6:

Calcium Hydroxide - Ca(OH)

Strontium Hydroxide - Sr(OH)

Barium Hydroxide - Ba(OH)

Question #7

Name the following acids:

HCN

SO

CO

Answer #7:

HCN – hydrocyanic acid

SO

– sulfurous acid

CO

– carbonic acid

Question #8

Give the formulas for the following

acids:

Acetic acid

Hydrobromic Acid

Phosphorous Acid

Answer #8:

Acetic acid – HC

Hydrobromic Acid – HBr

Phosphorous Acid – H

PO

Question #9

Name this ion:

Answer #9

- hydronium ion

Question #10

What word do we use to describe a

substance that is capable of acting

as either an acid or a base?

Answer #10:

Amphiprotic or amphoteric

Question #11

The stronger an acid or a base,

the ____ its conjugate pair.

Therefore, an acid and its

conjugate base (or a base

and its conjugate acid) have

a(n)  ____ relationship.

Answer #11:

The stronger an acid or a base, the

weaker

 its conjugate acid or

conjugate base.  Therefore, an acid

and its conjugate base or a base

and its conjugate acid have a(n)

inverse

 relationship.

Question #12

Give the conjugate base for the

following Bronsted-Lowry acids:

PH

CH

COO

Answer #12:

PH

OH

CH

COO

2-

Question #13

Give the conjugate acid for the

following Bronsted-Lowry bases:

HSO

CO

2-

Answer #13:

SO

HCO

Question #14

In the reaction below, which

substance is acting as the

conjugate base?

SO

 + NH



HSO

 + NH

Answer #14:

Conjugate base = HSO

Question #15

Write two chemical equations for

the reaction of HSO

 with water:

one in which HSO

 acts as an acid,

and one in which it acts as a base.

Be sure to include states of matter.

Answer #15:

HSO

(aq) + H

O (l)



SO

2-

 (aq) + H

 (aq)

HSO

(aq) + H

O (l)



SO

 (aq) + OH

 (aq)

Question #16

What word do we use to describe

an acid that has more than one

ionizable H atom?

Answer #16:

Polyprotic

Question #17

SO

 is a polyprotic acid.  Show

how this acid can go through

consecutive removals of a

hydrogen ion when added to

water.  Be sure to include states of

matter.

Answer #17:

SO

 (aq) +  H

O (l)



HSO

 (aq) + H

 (aq)

HSO

 (aq) + H

O (l)



SO

2-

 (aq) + H

 (aq)

Question #18

Calculate the [OH

] concentration

when the [H

] = 5.35 x 10

-11

 M, and

determine if the solution is acidic,

basic or neutral.

Answer #18:

[OH

] = 1.87 x 10

-4

 M; basic

Question #19

A solution has the exact same

[H

] and [OH

].

What is the only possible [H

concentration (molarity) for this

solution?

Would you classify this solution

as acidic, basic or neutral?

Answer #19:

[H

] = [OH

] = 1.0 x 10

-7

 M; neutral

Question #20

A solution has a pOH of 8.87.

What is its [H

]?

Would you classify this solution as

acidic, basic or neutral?

Answer #20:

[H

] = 7.49 x 10

-6

 M; acidic

Question #21

Find the pH of a 0.00476 M

hydrochloric acid solution.

Answer #21:

pH = 2.32

Question #22

Find the pOH of a solution that

contains 3.25 g of H

SO

 dissolved

in 2.75 L of solution.

Answer #22:

pOH = 12.38

Question #23

If the pH = 9.85, what is the

concentration of a solution of

Sr(OH)

Answer #23:

[Sr(OH)

] = 3.54 x 10

-5

Question #24

Calculate the pOH when 12.5 mL

of a 0.015 M Ca(OH)

is

diluted to 0.5 L.

Answer #24:

pOH = 3.12

Question #25

An acid has a

 value that is equal

to 2.5 x 10

-11

Is this acid most likely a strong acid

or a weak acid?  Why?

Answer #25:

A weak acid because for the

 value to be less

than one

, the denominator of the equilibrium-

constant expression must be larger than the

numerator which means that the reactants have

the greater concentrations and that is only

possible when there is a low % ionization like

you would see with a weak acid.

*Strong acids have a

 value greater than one.

Question #26

For a polyprotic acid, the value of

a1

 will always be _____ than

a2

because it is _____ to remove the

first hydrogen ion than it is to

remove the second.

Answer #26:

For a polyprotic acid, the value of

a1

 will always be

larger

 than

a2

because it is

easier

 to remove the

first hydrogen ion than it is to

remove the second.

Question #27

Calculate the pH of a 0.25 M

solution of boric acid (H

BO

).

The

 for boric acid = 7.3 x 10

-10

What is the % ionization of the acid?

Answer #27:

pH = 4.87

% ionization = 0.0054%

Question #28

A 0.11 M solution of ammonia (NH

has a pH of 11.16.

Calculate

 for ammonia.

What percentage of ammonia is

ionized in this solution?

(Hint: ICE Table)

Answer#28:

 for ammonia = 1.8 x 10

-5

% ionization = 1.27%

Final Jeopardy

•

What is another name for the word base?

•

What was Sorenson’s first name in the movie

we watched in class?

•

What is the range for the pH of blood?

•

Rainfall with a pH below ___ is known as acid

rain.

•

Name the 15 items we tested in the

household pH lab.

Final Jeopardy Answer:

Base = alkaline

Soren Sorenson

pH of blood = 7.35 – 7.45

Acid rain is pH below 5.6

Lemon juice, window cleaner, soda, distilled

water, vinegar, vegetable oil, egg whites, borax

solution, bleach, coffee, Gatorade, milk, salsa,

drano, rust dissolver

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Test your knowledge on acid-base equilibria with this interactive Jeopardy review worksheet. Explore properties of acids, neutralization reactions, definitions of acids and bases, and more. See if you can answer the questions correctly and check your solutions for each question.

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Unit 15.1 Jeopardy Review: Acid-Base Equilibria SEE SEPARATE WORKSHEET FOR WORKED OUT ANSWER SOLUTIONS

Question #1 Which of the following is a property of an acid? a) Feel like water b) Turn litmus paper blue c) React vigorously with metals higher on the activity series d) Taste bitter e) Conduct electric current *You may choose more than one option

Answer #1: a) Feel like water c) React vigorously with metals higher on the activity series e) Conduct electric current

Question #2 In a neutralization reaction, strong acids combine with strong bases so that the properties of both are lost. What are the 2 general products of a neutralization reaction?

Answer #2: water + salt

Question #3 Which statement below is true? a) An Arrhenius acid accepts hydrogen ions when dissolved in water. b) A Bronsted-Lowry base generates hydroxide ions when dissolved in water. c) A Lewis acid can accept a pair of electrons.

Answer #3: c) A Lewis acid can accept a pair of electrons.

Question #4 Name two problems with the Arrhenius definition of acids and bases.

Answer #4: It is restricted to aqueous solutions. It does not explain why some bases do not contain OH-ions (ex: NH3)

Question #5 Give the name AND formula for the seven strong acids we discussed in class.

Answer #5: Hydrochloric Acid, HCl Hydrobromic Acid, HBr Hydroiodic Acid, HI Chloric Acid, HClO3 Perchloric Acid, HClO4 Sulfuric Acid, H2SO4 Nitric Acid, HNO3

Question #6 All of the alkali metals, when combined with hydroxide, are considered to be strong bases. Which three alkaline earth metals are also classified as strong bases when combined with hydroxide? *Give chemical formula of these bases

Answer #6: Calcium Hydroxide - Ca(OH)2 Strontium Hydroxide - Sr(OH)2 Barium Hydroxide - Ba(OH)2

Question #7 Name the following acids: HCN H2SO3 H2CO3

Answer #7: HCN hydrocyanic acid H2SO3 sulfurous acid H2CO3 carbonic acid

Question #8 Give the formulas for the following acids: Acetic acid Hydrobromic Acid Phosphorous Acid

Answer #8: Acetic acid HC2H3O2 Hydrobromic Acid HBr Phosphorous Acid H3PO3

Question #9 Name this ion: H3O+

Answer #9 H3O+ - hydronium ion

Question #10 What word do we use to describe a substance that is capable of acting as either an acid or a base?

Answer #10: Amphiprotic or amphoteric

Question #11 The stronger an acid or a base, the ____ its conjugate pair. Therefore, an acid and its conjugate base (or a base and its conjugate acid) have a(n) ____ relationship.

Answer #11: The stronger an acid or a base, the weaker its conjugate acid or conjugate base. Therefore, an acid and its conjugate base or a base and its conjugate acid have a(n) inverse relationship.

Question #12 Give the conjugate base for the following Bronsted-Lowry acids: PH4+ H2O CH3COO-

Answer #12: PH3 OH- CH2COO2-

Question #13 Give the conjugate acid for the following Bronsted-Lowry bases: HSO4- H2O CO32-

Answer #13: H2SO4 H3O+ HCO3-

Question #14 In the reaction below, which substance is acting as the conjugate base? H2SO4+ NH3 HSO4-+ NH4+

Answer #14: Conjugate base = HSO4-

Question #15 Write two chemical equations for the reaction of HSO3-with water: one in which HSO3-acts as an acid, and one in which it acts as a base. Be sure to include states of matter.

Answer #15: HSO3-(aq) + H2O (l) SO32-(aq) + H3O+(aq) HSO3-(aq) + H2O (l) H2SO3(aq) + OH-(aq)

Question #16 What word do we use to describe an acid that has more than one ionizable H atom?

Answer #16: Polyprotic

Question #17 H2SO4is a polyprotic acid. Show how this acid can go through consecutive removals of a hydrogen ion when added to water. Be sure to include states of matter.

Answer #17: H2SO4(aq) + H2O (l) HSO4-(aq) + H3O+(aq) HSO4-(aq) + H2O (l) SO42-(aq) + H3O+(aq)

Question #18 Calculate the [OH-] concentration when the [H+] = 5.35 x 10-11M, and determine if the solution is acidic, basic or neutral.

Answer #18: [OH-] = 1.87 x 10-4M; basic

Question #19 A solution has the exact same [H+] and [OH-]. What is the only possible [H+] concentration (molarity) for this solution? Would you classify this solution as acidic, basic or neutral?