(Answered)-5/2/2016 Week Three Week Three Due: 12:00am on Tuesday, May 10,

Question Details

(Answered)-5/2/2016 Week Three Week Three Due: 12:00am on Tuesday, May 10,

Week 3 Excersices

Tutors,?

Please help my providing answers to the questions in the attached document.?

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Please provide handwritten solutions in a JPEG or PDF document.?

Please let me know if you have any questions.?

5/2/2016

Week Three

Due: 12:00am on Tuesday, May 10, 2016

You will receive no credit for items you complete after the assignment is due. Grading Policy

Exercise 15.7

Part A

Why is there more than one definition of acid?base behavior? Which definition is the right one?

ANSWER:

Essay answers are limited to about 500 words (3800 characters maximum, including spaces).

3785 Character(s) remaining

(none provided)

Exercise 15.34

Part A

Identify each of the following as an acid or a base.

Drag the appropriate items to their respective bins.

ANSWER:

Part B

Write a chemical equation for NaOH(aq) showing how it is an acid or a base according to the Arrhenius definition.

Express your answer as a chemical equation. Identify all of the phases in your answer.

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ANSWER:

Part C

Write a chemical equation for H2 SO 4 (aq) showing how it is an acid or a base according to the Arrhenius definition.

Express your answer as a chemical equation. Identify all of the phases in your answer.

ANSWER:

Part D

Write a chemical equation for HI(aq) showing how it is an acid or a base according to the Arrhenius definition.

Express your answer as a chemical equation. Identify all of the phases in your answer.

ANSWER:

Part E

Write a chemical equation for Ca(OH) 2 (aq) showing how it is an acid or a base according to the Arrhenius definition.

Express your answer as a chemical equation. Identify all of the phases in your answer.

ANSWER:

Exercise 15.36

For each of the following, identify the Bronsted?Lowry acid, the Bronsted?Lowry base, the conjugate acid, and the conjugate base.

Part A

Drag the appropriate labels to their respective targets.

ANSWER:

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Part B

Drag the appropriate labels to their respective targets.

ANSWER:

Part C

Drag the appropriate labels to their respective targets.

ANSWER:

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Part D

Drag the appropriate labels to their respective targets.

ANSWER:

Exercise 15.42

Classify each of the following acids as strong or weak.

Part A

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ANSWER:

strong

weak

Part B

HCHO 2

ANSWER:

strong

weak

Part C

H 2 SO4

ANSWER:

strong

weak

Part D

H 2 CO 3

ANSWER:

strong

weak

Part E

This question will be shown after you complete previous question(s).

Part F

This question will be shown after you complete previous question(s).

Part G

This question will be shown after you complete previous question(s).

Exercise 15.44

Part A

Rank the following solutions in order of decreasing [H3 O

Rank solutions from largest to smallest [H O ] . To rank items as equivalent, overlap them.

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Rank solutions from largest to smallest [H3 O

. To rank items as equivalent, overlap them.

ANSWER:

Exercise 15.124

Identify the Lewis acid and Lewis base from among the reactants in each of the following equations.

Part A

(aq) + 2NH 3 (aq) ? Ag(NH 3 )

(aq)

ANSWER:

is the Lewis base and NH3 is the Lewis acid.

is the Lewis acid and NH3 is the Lewis base.

Part B

AlBr 3 + NH 3 ? H 3 NAlBr 3

ANSWER:

AlBr 3

is the Lewis base and NH 3 is the Lewis acid.

AlBr 3

is the Lewis acid and NH 3 is the Lewis base.

Part C

(aq) + AlCl 3 (aq) ? AlCl 4

(aq)

ANSWER:

AlCl 3

is the Lewis acid and Cl is the Lewis base.

AlCl 3

is the Lewis base and Cl is the Lewis acid.

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Exercise 15.56

Determine the pH of each of the following solutions.

Part A

5.0?10?2 M HI

Express your answer to two decimal places.

ANSWER:

Part B

9.54?10?2 M HClO 4

Express your answer to three decimal places.

ANSWER:

Part C

a solution that is 4.8?10?2 M in HClO 4 and 5.4?10?2 M in HCl

Express your answer to two decimal places.

ANSWER:

Part D

a solution that is 1.11% HCl by mass (Assume a density of 1.01 g/mL for the solution.)

Express your answer to three decimal places.

ANSWER:

Exercise 15.66

Part A

Calculate the pH of a formic acid solution that contains 1.36% formic acid by mass. (Assume a density of 1.01 g/mL for the solution.)

Express your answer to two decimal places.

ANSWER:

Exercise 15.76

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Part A

Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka

2.0?10?5.

1.3?10?3.

0.18.

Express your answer to two decimal places.

ANSWER:

Part B

Find the percent dissociation of this solution.

Express your answer using two significant figures.

ANSWER:

Part C

Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka

Express your answer to two decimal places.

ANSWER:

Part D

Find the percent dissociation of this solution.

Express your answer using two significant figures.

ANSWER:

Part E

Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka

Express your answer to two decimal places.

ANSWER:

Part F

Find the percent dissociation of this solution.

Express your answer using two significant figures.

ANSWER:

Exercise 15.90

Amphetamine (C H N) is a weak base with a pK of 4.2.

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Week Three

Amphetamine (C 9 H13 N) is a weak base with a pKb of 4.2.

Part A

Calculate the pH of a solution containing an amphetamine concentration of 250 mg/L .

Express your answer to one decimal place.

ANSWER:

Exercise 15.100

Part A

Determine whether each of the following salts will form a solution that is acidic, basic, or pH ?neutral.

Drag the appropriate items to their respective bins.

ANSWER:

Exercise 15.108

Write chemical equations and corresponding equilibrium expressions for each of the two ionization steps of carbonic acid.

Part A

Write chemical equations for first ionization step of carbonic acid.

Express your answer as a chemical equation. Identify all of the phases in your answer.

ANSWER:

Part B

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This question will be shown after you complete previous question(s).

Part C

Write chemical equations for second ionization step of carbonic acid.

Express your answer as a chemical equation. Identify all of the phases in your answer.

ANSWER:

Part D

This question will be shown after you complete previous question(s).

Exercise 15.13

Part A

Choose an equation for the autoionization of water and an expression for the ion product constant for water (Kw ).

ANSWER:

Kw =

[H3 O

[OH

Kw = [H 3 O

Kw =

[OH

[H3 O

+ [OH[OH

Part B

What is the value of Kw at 25 ? C ?

ANSWER:

Kw = 1.0 ? 10

Kw = 1.8 ? 10

Kw = 1.0 ? 10

Kw = 1.8 ? 10

?14

?16

?10

Exercise 15.17

In most solutions containing a strong or weak acid, the autoionization of water can be neglected when calculating [H3 O + ] .

Part A

Explain why this is so.

ANSWER:

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Essay answers are limited to about 500 words (3800 characters maximum, including spaces).

3785 Character(s) remaining

(none provided)

Exercise 15.48

Part A

Calculate [H3 O

in the following aqueous solution at 25 ? C : [OH

1.8?10?9 M .

2.6?10?2 M .

6.1?10?12 M .

Express your answer using two significant figures.

ANSWER:

[H 3 O

Part B

Classify the solution as acidic or basic.

ANSWER:

acidic

basic

Part C

Calculate [H3 O

in the following aqueous solution at 25 ? C : [OH

Express your answer using two significant figures.

ANSWER:

[H 3 O

Part D

Classify the solution as acidic or basic.

ANSWER:

acidic

basic

Part E

Calculate [H3 O

in the following aqueous solution at 25 ? C : [OH

Express your answer using two significant figures.

ANSWER:

[H 3 O

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Part F

Classify the solution as acidic or basic.

ANSWER:

acidic

basic

Exercise 15.50

Calculate [H3 O

and [OH

for each of the following solutions.

Part A

pH =

8.58

Express your answer using two significant figures. Enter your answers numerically separated by a comma.

ANSWER:

[H 3 O

, [OH

Part B

pH =

11.20

Express your answer using two significant figures. Enter your answers numerically separated by a comma.

ANSWER:

[H 3 O

, [OH? ] =

Part C

pH =

2.82

Express your answer using two significant figures. Enter your answers numerically separated by a comma.

ANSWER:

[H 3 O

, [OH? ] =

Exercise 15.54

The value of Kw increases with increasing temperature.

Part A

Is the autoionization of water endothermic or exothermic?

ANSWER:

endothermic

exothermic

Exercise 16.8

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Part A

What factors influence the effectiveness of a buffer? What are the characteristics of an effective buffer?

ANSWER:

Essay answers are limited to about 500 words (3800 characters maximum, including spaces).

3785 Character(s) remaining

(none provided)

Exercise 16.11

Part A

The pH at the equivalence point of the titration of a strong acid with a strong base is 7.0. However, the pH at the equivalence point of the titration of a

weak acid with a strong base is above 7.0. Why?

ANSWER:

Essay answers are limited to about 500 words (3800 characters maximum, including spaces).

3785 Character(s) remaining

(none provided)

Exercise 16.28

A formic acid solution has a pH of 3.25.

Part A

Which of the following substances will raise the pH of the solution upon addition?

Check all that apply.

ANSWER:

KCl

NaBr

HCl

NaCHO 2

Part B

This question will be shown after you complete previous question(s).

Exercise 16.32

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Part A

Calculate the percent ionization of a 0.14 M formic acid solution inpure water.

Express your answer using two significant figures.

ANSWER:

Part B

Calculate the percent ionization of a 0.14 M formic acid solution in a solution containing 0.11 M potassium formate.

Express your answer using two significant figures.

ANSWER:

Part C

Explain the difference in percent ionization in the two solutions.

ANSWER:

Essay answers are limited to about 500 words (3800 characters maximum, including spaces).

3785 Character(s) remaining

(none provided)

Exercise 16.42

Calculate the pH of the solution that results from each of the following mixtures.

Part A

160.0 mL of 0.27 M HF with 230.0 mL of 0.31 M NaF

Express your answer using two decimal places.

ANSWER:

Part B

170.0 mL of 0.11 M C 2 H5 NH 2 with 270.0 mL of 0.22 M C 2 H5 NH 3 Cl

Express your answer using two decimal places.

ANSWER:

Exercise 16.50

For each of the following solutions, calculate the initial pH and the final pH after adding 0.010 mol of NaOH .

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Part A

For 200.0 mL of pure water, calculate the initial pH and the final pH after adding 0.010 mol of NaOH .

Express your answers using two decimal places separated by a comma.

ANSWER:

pH initial

, pHf inal =

Part B

For 200.0 mL of a buffer solution that is 0.240 M in HCHO2 and 0.310 M in KCHO 2 , calculate the initial pH and the final pH after adding 0.010

mol of NaOH .

Express your answers using two decimal places separated by a comma.

ANSWER:

pH initial

, pHf inal =

Part C

For 200.0 mL of a buffer solution that is 0.315 M in CH3 CH2 NH 2 and 0.285 M in CH3 CH2 NH 3 Cl , calculate the initial pH and the final pH after

adding 0.010 mol of NaOH .

Express your answers using two decimal places separated by a comma.

ANSWER:

pH initial

, pHf inal =

Exercise 16.62

Two 28.0 mL samples, one 0.100 M

these two titrations.

HCl

and the other 0.100 M

, were titrated with 0.200 M

KOH

. Answer each of the following questions regarding

Part A

What is the volume of added base at the equivalence point for HCl ?

ANSWER:

Part B

What is the volume of added base at the equivalence point for HF?

ANSWER:

Part C

Predict whether the pH at the equivalence point for each titration will be acidic, basic, or neutral.

ANSWER:

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neutral for HF, and basic for HCl

neutral for HCl , and acidic for HF

neutral for HCl , and basic for HF

neutral for HF, and acidic for HCl

neutral for both

Part D

Predict which titration curve will have the lowest initial pH .

ANSWER:

curve

HCl

curve

Exercise 16.64

The graphs below labeled (a) and (b) show, the titration curves for two equal?volume samples of bases, one weak and one strong. Both titrations were

carried out with the same concentration of strong acid.

Part A

What is the approximate pH at the equivalence point of (a) curve?

Express your answer as a whole number.

ANSWER:

Part B

What is the approximate pH at the equivalence point of (b) curve?

Express your answer as a whole number.

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ANSWER:

Part C

Which curve corresponds to the titration of the strong base and which one to the weak base?

ANSWER:

Graph (a) represents a strong base and graph (b) represents a weak base.

Graph (b) represents a strong base and graph (a) represents a weak base.

Exercise 16.68

A 20.0?mL sample of 0.125 M HNO 3 is titrated with 0.150 M

NaOH

Part A

Calculate the pH for at least five different points throughout the titration curve and make a sketch of the curve.

ANSWER:

Exercise 16.78

A 0.446?g sample of an unknown monoprotic acid was titrated with 0.105 M

KOH

and the resulting titration curve is shown in the figure.

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Part A

Determine the molar mass of the acid.

Express your answer using two significant figures.

ANSWER:

g/mol

Part B

Determine pKa of the acid.

ANSWER:

12.0

2.0

4.0

8.0

Exercise 16.82

Phenolphthalein has a pKa of 9.7 and is colorless in its acid form and pink in its basic form.

Part A

For pH

2.1 calculate [In ? ]/[HIn] .

Express your answer using two significant figures.

ANSWER:

[In

/[HIn]

Part B

Predict the color of a phenolphthalein solution.

ANSWER:

colorless

pink

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Part C

For pH

5.0 calculate [In

/[HIn]

Express your answer using two significant figures.

ANSWER:

[In

/[HIn]

Part D

Predict the color of a phenolphthalein solution.

ANSWER:

colorless

pink

Part E

For pH

7.9 calculate [In

/[HIn]

Express your answer using two significant figures.

ANSWER:

[In

/[HIn]

Part F

Predict the color of a phenolphthalein solution.

ANSWER:

colorless

pink

Part G

For pH

11.5 calculate [In

/[HIn]

Express your answer using two significant figures.

ANSWER:

[In

/[HIn]

Part H

Predict the color of a phenolphthalein solution.

ANSWER:

colorless

pink

Exercise 16.86

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Part A

Write a balanced equation for the dissolution of CaCO 3 .

Express your answer as a chemical equation. Identify all of the phases in your answer.

ANSWER:

Part B

Write an expression for Ksp for the dissolution of CaCO 3 .

ANSWER:

Ksp = [Ca

K sp =

[CO

[Ca

[CaCO 3 ]

[CO 3

[CaCO 3 ]

K sp =

[Ca2+ ][CO 3

K sp =

[CaCO 3 ]

K sp =

[CO

[Ca

[CO 3

[CaCO 3 ]

Ksp = [Ca

[CO

Part C

Write a balanced equation for the dissolution of PbCl2 .

Express your answer as a chemical equation. Identify all of the phases in your answer.

ANSWER:

Part D

Write an expression for Ksp for the dissolution of PbCl2 .

ANSWER:

K sp =

[Pb

[PbCl 2 ]

[Cl

[PbCl 2 ]

Ksp = [Pb

K sp =

[Pb

[Cl

[PbCl 2 ]

K sp =

[Pb

Ksp = [Pb

[Cl

[Cl[Cl

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Part E

Write a balanced equation for the dissolution of AgI .

Express your answer as a chemical equation. Identify all of the phases in your answer.

ANSWER:

Part F

Write an expression for Ksp for the dissolution of AgI .

ANSWER:

Ksp = [Ag

K sp =

[Ag

K sp =

[AgI]

[Ag + ][I

Ksp = [Ag

K sp =

[Ag

[AgI]

Ksp = [Ag

Exercise 16.90

Part A

Use the molar solubility 1.08 ? 10 ?5

in pure water to calculate Ksp for BaCrO 4 .

in pure water to calculate Ksp for Ag 2 SO3 .

in pure water to calculate Ksp for Pd(SCN) 2 .

ANSWER:

Ksp

Part B

Use the molar solubility 1.55 ? 10 ?5

ANSWER:

Ksp

Part C

Use the molar solubility 2.22 ? 10 ?8

ANSWER:

Ksp

Exercise 16.96

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Week Three

Calculate the molar solubility of CuX

(Ksp = 1.27 ? 10

?36

)

in each of the following.

Part A

pure water

Express your answer using three significant figures.

ANSWER:

Part B

0.28 M CuCl 2

Express your answer using two significant figures.

ANSWER:

Part C

0.19 M Na 2 X

Express your answer using two significant figures.

ANSWER:

Exercise 16.100

Part A

Determine whether or not Hg 2 Br 2 will be more soluble in acidic solution than in pure water.

ANSWER:

will be more soluble

will not be more soluble

Part B

This question will be shown after you complete previous question(s).

Part C

Determine whether or not Mg(OH)2 will be more soluble in acidic solution than in pure water.

ANSWER:

will be more soluble

will not be more soluble

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Part D

This question will be shown after you complete previous question(s).

Part E

Determine whether or not CaCO 3 will be more soluble in acidic solution than in pure water.

ANSWER:

will be more soluble

will not be more soluble

Part F

This question will be shown after you complete previous question(s).

Part G

Determine whether or not AgI will be more soluble in acidic solution than in pure water.

ANSWER:

will be more soluble

will not be more soluble

Part H

This question will be shown after you complete previous question(s).

Score Summary:

Your score on this assignment is 0.0%.

You received 0 out of a possible total of 4.16 points.

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