unit 7: acids and bases

Unit 7: Acids and Bases

Acids and Bases: The Basics Acid comes from the Latin word, acidus, which means “sour.”

Ascorbic acid: C6H8O8 – Citrus fruits Acetic acid: CH3COOH – Vinegar Hydrochloric acid: HCl – Toilet bowl cleaners Carbonic acid: H2CO3 - Soda Sulfuric Acid: H2SO4 – Fertilizers

Strength of Acids Strong acid: an acid that dissociates completely in aqueous solution. They are considered strong electrolytes.

Examples: HCl, HNO3, H2SO4, HBr Acids tend to produce H3O+ (Hydronium ion = Hydrogen ion) H3O+ is the same thing as H+

HCl + H2O H3O+ + Cl-

HNO3 + H2O H3O+ + NO3-

H2SO4 + H2O H3O+ + HSO4-

HBr + H2O H3O+ + Br-

Strength of Acids Weak acid: an acid that does not dissociate completely in aqueous solution.

Examples: H3PO4, CH3COOH, H2CO3

H3PO4 + H2O ↔ H3O+ + H2PO4-

CH3COOH + H2O ↔ H3O+ + CH3COO-

H2CO3 + H2O ↔ H3O+ + HCO3-

Strength of Acids

Strength of Bases

Bases have a bitter taste and a slippery feel. Also known as “alkaline” Sodium Hydroxide (NaOH) – drain cleaners Sodium bicarbonate (NaHCO3) – baking soda Potassium carbonate (K2CO3) – ashes

Strength of Bases Strong base: A base that completed

dissociates in water and yields aqueous OH- ions.

Weak bases: A base that does not produce a large number of hydroxide ions (does not dissociate completely).

Strong Bases Weak Bases

NaOH Na+ + OH- NH3 + H2O ↔ NH4+ + OH-

Ca(OH)2 Ca2+ + 2OH-

KOH K+ + OH-

Acids and Bases

Strong acids and strong bases are considered strong electrolytes, because a large concentration of ions are produced.

Bronsted-Lowry: Acid and Bases In the Bronsted-Lowry definition, an acid is any chemical that donates a hydrogen ion, H+ (H3O+), and a base is any chemical that accepts a hydrogen ion.B.A.A.D - “Bases Accept, Acids Donate”

Consider what happens when hydrochloric acid is mixed with water:

HCl donates a H+……resulting in a 3rd hydrogen

bonded to oxygen

Hydrogen ion

H3O+

HCl behaves as an acid (proton donor) and water behaves as a base (proton acceptor). Acids, when dissolved in water, release hydrogen ions.

Ammonia behaves as a base by accepting a H+ from water, which, in this case, behaves as an acid.

Hydroxide ion

Bases tend to increase the concentration of hydroxide ions.

Hydroxide ion

Amphoteric Amphoteric: A substance that is capable of acting as either an acid or a base

It acts as a base when combined with something more strongly acidic than itself. It acts as an acid when combined with something more strongly basic than itself.

Water has the ability to react with itself.

Keep in mind… Acid-base

interactions are almost seen as a behavior. For instance, water can behave as a base and as an acid.

An ammonium ion may donate a H+ back to OH- to reform ammonia and water.

Forward and reverse acid-base reactions proceed simultaneously and can therefore be represented by the double arrow.

Identify the acid or base behavior for each participant in the reaction:H2PO4 + H3O+ ↔ H3PO4 + H2O

Forward: H2PO4

- accepts a H+ to become H3PO4 H2PO4

- behaves as a base H3O+ donates a H+ to become H2O

H3O+ behaves as an acid

Identify the acid or base behavior for each participant in the reaction:H2PO4

- + H3O+ ↔ H3PO4 + H2O

Backwards: H3PO4 donates a H+ to become H2PO4

-

H3PO4 behaves as a acid H2O accepts a H+ to become H3O+

H2O behaves as a base

Conjugate Acid-Base Pairs

In any acid-base equilibrium (↔), it involves the transfer of H+.

An acid and a base that only differs in the presence or absence of a H+ are called a conjugate acid-base pair. Every acid has a conjugate base

For example: H2O (acids donate) can become OH-

Every base has a conjugate acid For example, H2O (bases accept) can become H3O+


HNO2 (aq)+ H2O (l)↔ NO2- (aq)+ H3O+

(aq)Acid Base Conjugat

e AcidConjugate Base

donates H+

Accepts H+

HNO2 donates an H+ and becomes its conjugate base, NO2-

H2O accepts an H+ and becomes its conjugate acid, H3O+


HCl + H2O H3O+ + Cl-acid Conjugate

base

base Conjugate acid

Accepts H+

Donates H+

Acid Dissociation

Kelter, Carr, Scott, Chemistry A World of Choices 1999, page 280

HCl

Conjugate baseAcid

Conjugate pair

+

1-

Cl

H


NH3 + H2O NH4+ + OH-

base Conjugate acid

acid Conjugate base

Accepts H+

Donates H+

What is the conjugate base of each of the following acids: Step 1: Remember that acids DONATES an

H+

Step 2: Its conjugate base always has an extra negative charge

HClO4 ClO4

-

H2S HS-

HCO3-

CO32-

What is the conjugate acid of the following bases? Step 1: Remember that all bases ACCEPT

an H+

Step 2: Its conjugate acid always has one LESS negative charge

CN-

HCN H2O

H3O+

HCO3-

H2CO3

Neutralization Reactions

Neutralization reactions occur between an acid and a base. These reactions often produce a salt, created from the positive ion of the base and the negative ion from the acid.

ACID BASE SALTHCN + NaOH NaCN + H2OHNO3 + KOH KNO3 + H2O

Neutralization Reactions

Predict the salt that is produced in the following:2 HCl + Ca(OH)2 ____________ + 2 H2O

HF + NaOH ____________ + H2O

CaCl2

NaFPrevents tooth decay

De-ice roads

What is pH?

What is pH?

In this reaction, a water molecule gains a H+ and the second water molecule must lose a H+.

In pure water, the number of H+ = the number of OH-

The concentration of H+ and OH- each is extremely low – about 1 x 10-7 M

What is pH?

[H3O+][OH-] = Kw [1.0 x 10-7][1.0 x 10-7] = Kw 1.0 x 10-14 = Kw The dissociation constant of water, Kw, means that no matter WHAT is dissolved in water, the product of H+ and OH- always equals 1.0 x 10-14

What is pH?[H3O+][OH-] = Kw = 1.0 x

10-14

Pure Water

[1.0 x 10-7][1.0 x 10-7] = Kw = 1.0 x 10-14

HCl Added [1.0 x 10-5][1.0 x 10-9] = Kw = 1.0 x 10-14

If a small amount of HCl is added to water, it dissociates and increases the H+ from 1.0 x 10-7 to 1.0 x 10-5. Therefore, the OH- concentration decreases so that the product of H+ and OH- is still equal to Kw.

Sample Problem What is the concentration of H+ ions if the concentration of OH- ion is 1.0 x 10-3 M?

[H3O+][OH-] = Kw[H3O+][1.0 x 10-3 M] = 1.0 x 10-14 M[H3O+] =

[H3O+] = 1.0 x 10-11 M

1.0 x 10-

14 M1.0 x 10-3 M

What is pH?

In an acidic solution, [H3O+] > [OH-]

In a basic solution, [H3O+] < [OH-]

In a neutral solution, [H3O+] = [OH-]

Sample Problem

How does adding ammonia, NH3, to water make a basic solution when there are no hydroxide ions in the formula for ammonia?

NH3 + H2O NH4+ + OH-

Ammonia increases the OH- concentration, thereby lowering the H+ concentration.

Because [H+] < [OH-], the solution is basic.

What is pH?

The pH scale is a numeric scale used to describe acidity.

pH = -(log[H3O+])

Consider a neutral solution, [H+] = 1.0 x 10-7 M

pH = -(log [1.0 x 10-7])pH = -(-7)pH = 7

What is pH? Acidic solutions have greater H+

concentrations, which lowers its pH.

Acidic solutions: pH < 7

Consider [H+] = 1.0 x 10-4 M

pH = -(log [H+])pH = -(log [1.0 x 10-4 M])

pH = -(-4)pH = 4

What is pH? Basic solutions have pH

values > 7, because its H+ concentrations are less.

Consider [H+] = 1.0 x 10-8 M

pH = -(log [H+])pH = -(log [1.0 x 10-8 M])

pH = -(-8)pH = 8

What is pH?

Rainwater is Acid & Ocean Water is Basic

Rainwater is Acidic: pH 5-6

The source of this acidity is carbon dioxide, the same gas that gives fizz to soda pop. There are 760 billion tons of CO2 in the atmosphere that undergo this reaction:

CO2 (g) + H2O (l) H2CO3 (aq)Carbonic acid

Carbonic acid lowers the pH, accelerating the erosion of land and historical artifacts.

What is classified as ACID RAIN? Acid rain: rain that has a pH < 5.

Source: Airborne pollutants that are absorbed by atmospheric moisture, most commonly – sulfur dioxide. Sulfur dioxide is readily convert to sulfur trioxide…

2 SO2 (g) + O2 (g) 2 SO3 (g) …which reacts with water to form sulfuric acid.

SO3 (g) + H2O (l) H2SO4 (aq) Acid rain affects vegetation and ecosystems.

ACID RAIN CYCLE

Impact of Acid Rain: Midwest

Midwest: The ground contains calcium carbonate (basic), which often neutralizes the acid rain before much damage is done.

Liming In order to rains the pH of acidified

lakes and rivers by adding calcium carbonate – a process called liming.

Long-term solution: Prevent the sulfur dioxide and other pollutants from entering the atmosphere in the first place. Shift fossil fuels to nuclear and solar

energy

Impact of Acid Rain: Northeast

Northeast: The ground contains LITTLE CaCO3. The effect of acid rain on lakes and rivers accumulate.

Buffer Solutions Resist Change in pH

Buffer solution

Buffer solution: any solution that resists change in pH (1) neutralizes any added base (2) neutralizes any added acid

This does not mean that the pH remains unchanged, it just resists LARGE changes in pH

Example of Buffers Blood: optimal pH of 7.35 to 7.45

Primary buffer system combines (1) carbonic acid and (2) sodium bicarbonate

Carbon dioxide in the blood stream reacts with water to produce carbonic acid

CO2 + H2O H2CO3 We fine-tune the levels of carbonic acid in our

blood by breathing!

Aspirin overdose: Alkalosis Aspirin (acetylsalicylic acid) is an acid

chemical that when taken in large amounts can overwhelm the blood buffering system, dropping the blood pH.

Symptom: Hyperventilate Exhaling at excessive rates is your body’s attempt

to lower the concentration of carbonic acid. Alkalosis: suddenly raising your blood pH can be

life-threatening Acidosis: (if the breathing rate is too slow)

suddenly lowering your blood pH (increased H3O+ concentration)

Alkalosis

If our breathing becomes too fast (hyperventilation)…

Carbon dioxide is removed from the blood too quickly.

This accelerates the rate of degradation of carbonic acid into carbon dioxide and water.The lower level of carbonic acid encourages the combination of hydrogen ions andbicarbonate ions to make more carbonic acid. The final result is a fall in blood H1+

levels that raises blood pH which can result in over-excitability or death.


Acidosis

If breathing becomes too slow (hypoventilation)…

…free up acid, pH of blood drops, with associated health risks such as depressionof the central nervous system or death.

The normal pH of blood is between 7.2 – 7.4. This pH is maintained by the bicarbonate ion and other buffers.


unit 7: acids and bases

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