lectureplus timberlake1 acids and bases. lectureplus timberlake2 arrhenius acids and bases acids...

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Acids and Bases

Acids and Bases


Arrhenius Acids and Bases

Acids produce H+ in aqueous solutions water

HCl H+(aq) + Cl- (aq)

Bases produce OH- in aqueous solutions

water

NaOH Na+(aq) + OH- (aq)


Acids

Produce H+ (as H3O+) ions in water

Produce a negative ion (-) too

Taste sour

Corrode metals

React with bases to form salts and water


Bases

Produce OH- ions in water

Taste bitter, chalky

Are electrolytes

Feel soapy, slippery

React with acids to form salts and water


Learning Check AB1

Describe the solution in each of the following as: 1) acid 2) base or 3)neutral.

A. ___soda

B. ___soap

C. ___coffee

D. ___ wine

E. ___ water

F. ___ grapefruit


Solution AB1

Describe each solution as:

1) acid 2) base or 3) neutral.

A. _1_ soda

B. _2_ soap

C. _1_ coffee

D. _1_ wine

E. _3_ water

F. _1_ grapefruit


Learning Check AB2

Identify each as characteristic of an A) acid or B) base

____ 1. Sour taste

____ 2. Produces OH- in aqueous solutions

____ 3. Chalky taste

____ 4. Is an electrolyte

____ 5. Produces H+ in aqueous solutions


Solution AB2

Identify each as a characteristic of an A) acid or B) base

_A_ 1. Sour taste

_B_ 2. Produces OH- in aqueous solutions

_B_ 3. Chalky taste

A, B 4. Is an electrolyte

_A_ 5. Produces H+ in aqueous solutions


Some Common Acids

HCl hydrochloric acid

HNO3 nitric acid

H3PO4 phosphoric acid

H2SO4 sulfuric acid

CH3COOH acetic acid


Learning Check AB3

Give the names of the following

A. HBr (aq) 1. bromic acid

2. bromous acid

3. hydrobromic acid

B. H2CO3 1. carbonic acid

2. hydrocarbonic acid

3. carbonous acid


Solution AB3

A. HBr 3. hydrobromic acid

The name of a nonoxy acid begins with the prefix hydro- and ends with -ic acid. In a nonoxy acid, the negative anion end in -ide.

B. H2CO3 1. carbonic acid

The name of an oxyacid is named with the stem of the anion (carbonate) changed to

-ic acid


Some Common Bases

NaOH sodium hydroxide

KOH potassium hydroxide

Ba(OH)2 ________________________

Mg(OH)2 ________________________

Al(OH)3 aluminum hydroxide


Learning Check AB4

Match the formulas with the names:

A. ___ HNO2 1) hydrochloric acid

B. ___ Ca(OH)2 2) sulfuric acid

C. ___ H2SO4 3) sodium hydroxide

D. ___ HCl 4) nitrous acid

E. ___ NaOH 5) calcium hydroxide


Solution AB4

Match the formulas with the names:

A. _4__ HNO2 1) hydrochloric acid

B. _5__ Ca(OH)2 2) sulfuric acid

C. _2__ H2SO4 3) sodium hydroxide

D. _1__ HCl 4) nitrous acid

E. _3__ NaOH 5) calcium hydroxide


Learning Check AB5

Acid, Base Nameor Salt

CaCl2 ______ _________________

KOH ______ _________________

Ba(OH)2 ______ _________________

HBr ______ _________________

H2SO4 ______ __________________


Solution AB5

Acid, Base Nameor Salt

CaCl2 salt calcium chloride

KOH base potassiuim hydroxide

Ba(OH)2 base barium hydroxide

HBr acid hydrobromic acid

H2SO4 acid sulfuric acid


Bronsted-Lowry Acids

Acids are hydrogen ion (H+) donors

Bases are hydrogen ion (H+) acceptors

HCl + H2O H3O+ + Cl-

donor acceptor + -

+ +


Chapter 9Acids and Bases

Acid-Base Neutralization

Buffers

Acid-Base Titration


Neutralization Reactions

When acid and bases with equal amounts of hydrogen ion H+ and hydroxide ions OH- are mixed, the resulting solution is neutral.

NaOH (aq) + HCl(aq) NaCl + H2O

base acid salt water

Ca(OH)2 + 2 HCl CaCl2 + 2H2Obase acid salt water


Neutralization

H3O+ and OH- combine to produce water

H3O+ + OH- 2 H2O

from acid from base neutral

Net ionic equation:

H+ + OH- H2O


Ionic Equations for Neutralization

Write strong acids, bases, and salt as ions

H+ + Cl- + Na+ + OH- Na+ + Cl- + H2O

Cross out matched ions

H+ + Cl- + Na+ + OH- Na+ + Cl- + H2O

Write a net ionic reaction

H+ + OH- H2O


Balancing Neutralization Equations

Write the equation for the neutralization

between magnesium hydroxide and nitric acid.

1. Write the formulas of the acid and base

Mg(OH)2 + HNO3

2. Balance to give equal OH- and H+

Mg(OH)2 + 2 HNO3


3. Write the products:

Mg(OH)2 + 2HNO3 Mg(NO3)2 + H2O

salt water

(metal and nonmetal)

4. Balance products

Mg(OH)2 + 2 HNO3 Mg(NO3)2 + 2 H2O


Learning Check N2

Select the correct group of coefficients for the

following neutralization equations

A. __ HCl + __ Al(OH)3 __AlCl3 + __

H2O

1) 1, 3, 3, 1 2) 3, 1, 1, 1 3) 3, 1, 1 3

B.__ Ba(OH)2 + __H3PO4 __Ba3(PO4)2 + __ H2O

1) 3, 2, 2, 2 2) 3, 3, 1, 6 3) 2, 3, 1, 6


Solution N2

A. 3HCl + 1Al(OH)3 1AlCl3 + 3H2O

B. 3Ba(OH)2 + 2H3PO4 1Ba3(PO4)2 +

6H2O


Learning Check N3

Write a balanced equation and calculate

the mL of 2.00 M H2SO4 required to

neutralize 50.0 mL of 1.00 M KOH?

___H2SO4 + ___KOH ___K2SO4 + H2O

1) 12.5 mL 2) 50.0 mL 3) 200. mL


Solution N3

How many mL of 2.00 M H2SO4 are required to

neutralize 50.0 mL of 1.00 M KOH?

H2SO4 + 2KOH K2SO4 + 2H2O

0.0500 L x 1.00 mole KOH x 1 mole H2SO4 x

1 L 2 mole KOH

1 L x 1000 mL = 12.5 mL

2 mole KOH 1 L


Learning Check N4

A 25 mL sample of phosphoric acid is neutralized by 40. mL of 1.5 M NaOH. What is the molarity of the phosphoric acid solution?

3NaOH + H3PO4 Na3PO4 + 3H2O

1) 0.45 M 2) 0.80 M 3) 7.2 M


Solution S4

0.040 L x 1.5 mole NaOH x 1 mole H3PO4

1 L 3 mole NaOH

x 1 = 0.80 mol/L = 0.80 M

0.025 L


Acids and Bases

Ionization of Water

The pH Scale


Ionization of Water

Occasionally, in water, a H+ is transferred between H2O molecules

. . . . . . . .H:O: + :O:H H:O:H + + :O:H-

. . . . . . . . H H H

water molecules hydronium hydroxide ion (+) ion (-)


Pure Water is Neutral

Pure water contains small, but equal amounts of ions: H3O+ and OH-

H2O + H2O H3O+ + OH-

hydronium hydroxide

ion ion

1 x 10-7 M 1 x 10-7 MH3O+ OH-


Ion Product of Water Kw

[ ] = Molar concentration

Kw = [ H3O+ ] [ OH- ]

= [ 1 x 10-7 ][ 1 x 10-7 ]

= 1 x 10-14


Acids

Increase H+

HCl (g) + H2O (l) H3O+ (aq) + Cl-

(aq)

More [H3O+] than water > 1 x 10-7M

As H3O+ increases, OH- decreases

[H3O+] > [OH-]H3O+

OH-


Bases

Increase the hydroxide ions (OH-)

H2O

NaOH (s) Na+(aq) + OH- (aq)

More [OH-] than water, [OH-] > 1 x 10-7M

When OH- increases, H3O+ decreases

[OH] > [H3O+]

H3O+OH-


Using Kw

The [OH- ] of a solution is 1.0 x 10- 3 M. What is the

[H3O+]?

Kw = [H3O+ ] [OH- ] = 1.0 x 10-14

[H3O+] = 1.0 x 10-14

[OH-]

[H3O+] = 1.0 x 10-14 = 1.0 x 10-11 M

1.0 x 10- 3


Learning Check pH1

The [H3O+] of lemon juice is 1.0 x 10-3 M.

What is the [OH-] of the solution?

1) 1.0 x 103 M

2) 1.0 x 10-11 M

3) 1.0 x 1011 M


Solution pH1

The [H3O+] of lemon juice is 1.0 x 10- 3 M.

What is the [OH-]?

[OH- ] = 1.0 x 10 -14 = 1.0 x 10-11 M 1.0 x 10 - 3


Using the Calculator

1.0 x 10 -14

4.0 x 10-5

Enter 1.0 EE +/- 14 4.0 EE +/- 5

= 2.5 x 10 -10


Learning Check pH2

The [OH-] of a solution is 5 x 10 -5 M. What is the [H3O+ ] of the solution?

1) 2 x 10- 5 M

2) 1 x 1010 M

3) 2 x 10-10 M


Solution pH2

The [OH-] of a water solution is 5 x 10-5 M.

What is the [H3O+] in the solution?

[ H3O+] = 1.0 x 10 -14

5 x 10- 5

On some calculators:

1.0 EE +/- 14 5 EE +/- 5 = 2 x 10 -10 M


Learning Check pH3

A.The [OH-] when [H3O+ ] of 1 x 10- 4 M

1) 1 x 10-6 M

2) 1 x 10-8 M

3) 1 x 10-10 M

B.The [H3O+] when [OH- ] of 5 x 10-9 M

1) 1 x 10- 6 M

2) 2 x 10- 6 M

3) 2 x 10-7 M


Solution pH3

Kw = [H3O+ ][OH-] = 1.0 x 10 14

A. (3) [OH- ] = 1.0 x 10 -14 = 1.0 x 10 -10

1.0 x 10- 4

B. (2) [H3O+] = 1.0 x 10 -14 = 2 x 10 - 6

5 x 10- 9


pH

Indicates the acidity [H3O+] of the solution

pH = - log [H3O+]

From the French pouvoir hydrogene

(“hydrogen power” or power of

hydrogen)


In the expression for [H3O+]

1 x 10-exponent

the exponent = pH

[H3O+] = 1 x 10-pH M

pH


pH Range

0 1 2 3 4 5 6 7 8 9 10 11 12 13 14

Neutral

[H+]>[OH-] [H+] = [OH-] [OH-]>[H+]

Acidic Basic


Some [H3O+] and pH

[H3O+] pH

1 x 10-5 M 5

1 x 10-9 M 9

1 x 10-11 M 11


pH of Some Common Acids

gastric juice 1.0

lemon juice 2.3

vinegar 2.8

orange juice 3.5

coffee 5.0

milk 6.6


pH of Some Common Bases

blood 7.4

tears 7.4

seawater 8.4

milk of magnesia 10.6

household ammonia11.0


Learning Check pH4

A. The [H3O+] of tomato juice is 1 x 10-4 M.

What is the pH of the solution?

1) - 4 2) 4 3) 8

B. The [OH-] of an ammonia solution is

1 x 10-3 M. What is the pH of the solution?

1) 3 2) 11 3) -11


Solution pH4

A. pH = - log [ 1 x 10-4] = -(- 4) = 4

B. [H3O+] = 1 x 10-11

pH = - log [ 1 x 10- 11] = -(- 11) = 11


Learning Check pH5

The pH of a soap is 10. What is the [H3O+] of the soap

solution?

1) 1 x 10 - 4 M

2) 1 x 1010 M

3) 1 x 10 - 10 M


Solution pH5

The pH of a soap is 10. What is the [H3O+]

of the soap solution?

[H3O+] = 1 x 10-pH M

= 1 x 10-10 M


pH on the Calculator

[H3O+] is 4.5 x 10-6 M

pH = 4.5 x EXP(or EE) 6+/- LOG +/-

= 5.35


Learning Check pH6

A soap solution has a [H3O+] = 2 x 10-8 M. What is the pH of

the solution?

1) 8

2) 7.7

3) 6


Solution pH6

A soap solution has a [H3O+] = 2.0 x 10-

8 M. What is the pH of the solution?

B) 2.0 EE 8 +/- LOG +/- = 7.7


Learning Check pH7

Identify each solution as

1. acidic 2. basic 3. neutral

A. _____ HCl with a pH = 1.5

B. _____ Pancreatic fluid [H+] = 1 x 10-8 M

C. _____ Sprite soft drink pH = 3.0

D. _____ pH = 7.0

E. _____ [OH- ] = 3 x 10-10 M

F. _____ [H+ ] = 5 x 10-12


Solution pH7

Identify each solution as

1. acidic 2. basic 3. neutral

A. _1__ HCl with a pH = 1.5

B. _2__ Pancreatic fluid [H+] = 1 x 10-8 M

C. _1__ Sprite soft drink pH = 3.0

D. _3__ pH = 7.0

E. _1__ [OH-] = 3 x 10-10 M

F. _2__ [H+] = 5 x 10-12


Acid RainUnpolluted rain has a pH of 5.6

Rain with a pH below 5.6 is “acid rain“

CO2 in the air forms carbonic acid

CO2 + H2O H2CO3

Adds to H+ of rain

H2CO3 H+ (aq) + HCO3-(aq)

Formation of acid rain:

1. Emission of sulfur and nitrogen oxides from the burning of fuels expecially coal with high S content, power stations, oil refineries, vehicles as well as bacterial decomposition, and lighting hitting N2

SO2 26 million tons in 1980

NO and NO2 22 million tons in 1980

Mt. St Helens (1980) 400,000 tons SO2

2. Reactions in the atmosphere form SO3

2SO2 + O2 2 SO3

3. Reactions with atmosphere water form acids

SO3 + H2O H2SO4 sulfuric acid

NO + H2O HNO2 nitrous acid

HNO2 + H2O HNO3 nitric acid

4. Effects of Acid Rain

Decline in fish populations in rivers and lasts due to toxic effect of Al leached from soil by acid rain

Extensive fish kills in spring from runoff due to accumulation of large amounts of acid on the snow

Dissolves minerals Mg, Ca, and K from the soil and waxy coatings that protect leaves from bacteria

Corrodes metals, textiles, paper and leather


Sources of Acid Rain

Power stations

Oil refineries

Coal with high S content

Car and truck emissions

Bacterial decomposition, and lighting

hitting N2


SO2 26 million tons in 1980

NO and NO2 22 million tons in 1980

Mt. St Helens (1980) 400,000 tons SO2

Reactions with oxygen in air form SO3

2SO2 + O2 2 SO3

Reactions with water in air form acids

SO3 + H2O H2SO4 sulfuric acid

NO + H2O HNO2 nitrous acid

HNO2 + H2O HNO3 nitric acid


Effects of Acid Rain

Leaches Al from soil, which kills fish

Fish kills in spring from runoff due to

accumulation of large amounts of acid in

snow

Dissolves waxy coatings that protect leaves

from bacteria

Corrodes metals, textiles, paper and leather


Chapter 9Acids and Bases

Strengths of Acids and Bases

Making Dilutions


Strengths of Acids and Bases

Strong acids completely ionize (100%) in

aqueous solutions

HCl + H2O H3O+ + Cl- (100 % ions)

Strong bases completely (100%) dissociate into ions in aqueous solutions.

NaOH Na+ (aq) + OH-(aq) (100 % ions)


NH3, A Bronsted-Lowry Base

When NH3 reacts with water, most of the reactants remain dissolved as molecules, but a few NH3 reacts with water to form NH4

+ and hydroxide ion.

NH3 + H2O NH4+(aq) + OH- (aq)

acceptor donor

+ +


Strong and Weak Acids and Bases

Strong acids

HCl, HNO3 , H2SO4

Most other acids are weak.

Strong bases

NaOH, KOH, and Ca(OH)2

Most other bases are weak.


Learning Check SW1

Identify each of the following as a

1) strong acid or base 2) weak acid

3) weak base

A. ___ HCl (aq)

B. ___ NH3(aq)

C. ___ NaOH (aq)

D. ___ H2CO3 (aq)


Solution SW1

Identify each of the following as a

1) strong acid or base 2) weak acid

3) weak base

A. _1__ HCl (aq)

B. _3__ NH3(aq)

C. _1__ NaOH (aq)

D. _2__ H2CO3 (aq)


Antacids

Used to neutralize stomach acid (HCl)

Many contain one or more weak bases

Alka-Seltzer: NaHCO3, citric acid, and aspirin

Di-gel: CaCO3 and Mg(OH)2

Gelusil: Al(OH)3 and Mg(OH)2

Maalox: Al(OH)3 and Mg(OH)2

Mylanta: Al(OH)3 and Mg(OH)2


More Antacids

Milk of Magnesia: Mg(OH)2

Rolaids: AlNa(OH)2CO3

aluminum sodium dihydroxy carbonate

Tums: CaCO3

Tempo: CaCO3, Al(OH)3, Mg(OH)2


Dilutions

Add water Volume increases. New concentration is less than initial


Concentration of A Diluted Solution

A 25 mL sample of a 6.0 M KOH is diluted by adding 75 mL of water. Calculate the new concentration of the KOH solution.

Moles KOH = 0.025 L x 6.0 moles = 0.15 moles

1 L

New volume = 25 mL + 75 mL = 100. mL = 0.100 L

New molarity = 0.15 moles = 1.5 M

0.100 L


Learning Check SW 2

A 125 mL sample of a 3.0 M HCl is diluted by adding 250 mL of water. The new concentration of the HCl solution is

1) 8.0 M

2) 1.5 M

3) 1.0 M


Solution SW 2

3) 1.0 M

moles HCl = 0.250 L x 3.0 moles = 0.75 mole 1 L

new M = 0.75 mole 1.0 M HCl 0.750 L(new volume)


Learning Check SW 3

A 50.0 mL sample of 15% sucrose solution is diluted by adding 200. mL of water. The new concentration of the sucrose solution is

1) 3.0 %

2) 7.5 %

3) 10. %


Learning Check SW 3

A 50.0 mL sample of 15% sucrose solution is diluted by adding 200. mL of water. The new concentration of the sucrose solution is

1) 3.0 %

g sucrose = 50.0 mL x 15 g sucrose = 7.5 g

100 mL

new % = 7.5 g sucrose = 3.0 % sucrose

250 mL

(new volume)

lectureplus timberlake1 acids and bases. lectureplus timberlake2 arrhenius acids and bases acids...

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