Acids and Bases NotesUnit 11 Page 1

Learning Target:I can name ionic compounds containing acids, and bases, using (IUPAC) nomenclature rules.

I can write the chemical formulas of acids and bases.Criteria for Success:

I can identify an acid as a binary acid or an oxyacid.I can name common binary acids, oxyacids, and bases given their chemical formula.

I can write the formula for common binary acids, oxyacids, and bases given their chemical name.

Binary Acid Nomenclature1. The name of a binary acid begins with the prefix ___________________.2. The _______ of the name of the second element follows this prefix.3. The name then ends with the suffix ___________.

Oxyacid Nomenclature1. An _________________ is an acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal.

a. Nomenclature for oxyacids typically follow the name of the __________________________ ion involved in the acid formula.

Name of oxyacid Name of polyatomic anionPrefix Suffix Prefix Suffixhypo- -ous hypo- -iteNone -ous None -iteNone -ic None -ateper- -ic per- -ate

b. This chart can be summed up with a memory trick! Think of the terrible acid disease, ___________________.

Base Nomenclature

1. Name bases using the same _____________ nomenclature rules you always have! (Ex: LiOH, KOH, etc.)a. The only common base that will not be named this way is ___________ , ______________________.

Acids and BasesUnit 11 Page 2

Content Objective:I can explain the process of chemical equilibrium as a dynamic, reversible state in which rates of opposing

processes are equal.

Criteria for Success:I can identify that in many classes of reactions, it is important to consider both the forward and reverse reaction.

I can define and interpret the equilibrium constant, K.

NotesA. Dynamic Equilibrium

1. Many chemical reactions are ____________.

2. Double arrows (⇋) indicate that the reaction is _______________.

3. At equilibrium, both ____________ and ____________ are present.

4. Dynamic equilibrium is reached when the forward and backward reactions continue at the same ____________ , and the concentrations of the reactants and products are ____________.

Constant concentration of reactants and products does not necessarily mean identical concentrations of reactants and products. In fact, they are very rarely the same numerical value. All concentrations being constant (not changing) is not the same thing as concentrations being equal (all having the same value). This is a common misconception and one that you must not have.

B. Graphical Representation of Dynamic EquilibriumH2(g) + I2(g) ⇌ 2 HI(g)

Product-Favored Reaction Reactant-Favored Reaction

C. Quantitative Treatment 1. The equilibrium ____________, K, relates the concentrations of ____________ and ____________ at equilibrium at a given temperature. For the general reaction:

aA + bB ⇋ cC + dDThe equilibrium constant expression, K, is expressed as

i. ____________ molar concentrations are in the numerator. ii. ____________ molar concentrations are in the denominator. iii. Each concentration is raised to the power of its stoichiometric coefficient in the ________ equation. iv. Pure solids and pure liquids (e.g., water) are _______ placed into the expression. v. This expression for the equilibrium constant is also known as the law of ___________ __________.vi. There are NO __________ for equilibrium constant K (They cancel out).

D. What Does the Equilibrium Constant Mean? 1. If K > 1, then the ____________ formation is favored— equilibrium concentrations of products are large.

2. If K < 1, then the ____________ formation is favored— equilibrium concentrations of reactants are large.

3. If K = 1, the formation of reactants and products are ____________ favored — equilibrium concentrations of reactants and products are approximately the same.

Acids and BasesUnit 11 Page 4

Objective:I can define acids and bases according to Arrhenius’s theory.

I can distinguish between degrees of dissociation for strong and weak acids and basesCriteria for Success:

I can define acid and base according to Arrhenius’s theoryI can explain the differences between strong and weak acids and bases.

Arrhenius Acids and Bases

A. An Arrhenius _________ is a chemical compound that increases the concentration of ________________ ions (H+1), in

aqueous solution. The hydrogen ions are attracted to the water molecules in an aqueous solution and form

_________________________ ions (H3O+1).

B. An Arrhenius _________ is a chemical compound that increases the concentration of ________________ ions (OH-1), in

aqueous solution.

Strength of Acids and Bases

A. A strong acid is one that ionizes completely in an aqueous solution. __________________ ions and _____________ are

formed in solution.

HCl(aq) + H2O(l) → H3O+1(aq) + Cl-1(aq)

1. Strong acids are strong __________________________.

2. Because strong acids _________________ dissociate in solution, they have Ka values _______________ than 1.

B. A weak acid is one that does not dissociate completely in an aqueous solution. In aqueous solution, both the

dissociation and the reverse reaction occur at the same time. ____________________ ions and _________ are formed in the

forward reaction but in the reverse reaction dissolved acid molecules and water are produced.

HCN(aq) + H2O(l) ⇋ H3O+1(aq) + CN-1(aq)

1. Weak acids are poor _________________________.

2. Because weak acids do ______ completely dissociate in solution, they have Ka values ________ than 1.

C. A strong base is one that dissociates completely in an aqueous solution. __________________ ions and _____________ are

formed in solution.

NaOH(s) + H2O(l) → Na+1(aq) + (OH)-1(aq)

1. Strong bases are strong __________________________.

2. Because strong bases _________________ dissociate in solution, they have Kb values ____________ than 1.

D. A weak base is one that does not dissociate completely in an aqueous solution. In aqueous solution, both the

dissociation and the reverse reaction occur at the same time. ____________________ ions and _________ are formed in the

forward reaction but in the reverse reaction dissolved base molecules and water are produced.

NH3(aq) + H2O(l) ⇋ (NH4)+1(aq) + (OH)-1(aq)

1. Weak bases are poor _________________________.

2. Because weak bases do _______ completely dissociate in solution, they have Kb values _________ than 1.

Acids and BasesUnit 11 Page 5

Learning Target:I can define acids and bases according to Brønsted-Lowry theory.

Criteria for Success:I can define a Brønsted-Lowry acid as a proton donor.

I can define a Brønsted-Lowry base as a proton acceptor.I can define and explain the concept of a Brønsted-Lowry conjugate acid-base pair.

I can identify Brønsted-Lowry acid-base pairs in aqueous acid-base reactions.

Brønsted-Lowry Acids and Bases

A. A Brønsted-Lowry ________________ is a molecule or ion that is a ___________________ donor.

1. Because _______ is a proton, all acids defined as an Arrhenius acid are also defined as a Brønsted-Lowry

acid.

B. A Brønsted-Lowry ________________ is a molecule or ion that is a ____________________ acceptor.

C. In a Brønsted-Lowry __________________________ reaction, protons are transferred from one reactant (the acid) to

another (the base).

Conjugate Acids and Bases

A. The species that remains after a Brønsted-Lowry acid has given up a proton is the __________________________

_______________ of that acid.

HF(aq) + H2O(l) ⇋ F-1(aq) + H3O+1(aq)

B. The species that is formed when a Brønsted-Lowry base gains a proton is the _____________________ ____________ of

that base.

HF(aq) + H2O(l) ⇋ F-1(aq) + H3O+1(aq)

C. In general, Brønsted-Lowry acid-base reactions are ______________________ systems meaning that both the

_____________________ and _____________________ reactions occur.

1. The extent of the reaction depends on the relative _____________________ of the acids and bases involved.

a. The ___________________ an acid is, the ___________________ its conjugate base.

b. The ___________________ a base is, the ____________________ its conjugate acid.

2. The favored direction of the reaction is the one in which the ____________________ acid and the

_____________________ base are produced.

a. You will need to use a reference chart with K values.

Example 1:

HClO4(aq) + H2O(l) ? H3O+1(aq) + ClO4-1(aq)

Example 2:

CH3COOH(aq) + H2O(l) ? H3O+1(aq) + CH3COO-1(aq)

D. Any species that can react as either an acid or a base is described as _____________________.

(______________ is a good example).

Self-Ionization of WaterUnit 11 Page 6

Learning Target:I can describe the self-ionization of water and describe a solution in terms of concentrations of H1+ and OH1-.

Criteria for Success:I can describe the self-ionization of water.

I can define the ionization constant of water, Kw.I can describe a solution in terms of [H1+] and [OH1-].I can calculate H1+ and OH1- concentration using Kw.

Self-Ionization of Water

A. In the _______________________________ of water, a _____________________ molecule produces a __________________________ ion,

H1+, and a ___________________________ ion, OH1-.

H2O(l) H1+(aq) + OH1-(aq)

1. Conductivity measurements show that concentrations of H1+ and OH1- in pure water are each only

_______________________ of water at 25°C.

2. To represent __________________________ in moles per liter (M), the formula of the particular ion is enclosed

in brackets, [ ]. Examples: ______________ and ______________.

3. In water at 25°C, [H1+]=______________________ and [OH1-]=______________________.

4. The mathematical _________________________ of [H1+] and [OH1-] remains constant in water and aqueous

solutions at constant ___________________________. This is known as the ___________________________

_______________________ of water, Kw.

Kw = [H1+] [OH1-]

5. At 25°C, which is within ordinary range of room temperature, the following relationship is valid and you

can assume these conditions unless otherwise stated:

Kw = [H1+] [OH1-]= (1.0x10-7M) (1.0x10-7M) = __________________________

6. It is important to note that Kw increases with increasing _________________________.

Neutral, Acidic, and Basic Solutions

A. Important relationships involving acidic, neutral, and basic solutions are summarized below:

Acidic: [H1+] ________ [OH1-]

Neutral: [H1+] ________ [OH1-]

Basic: [H1+] ________ [OH1-]

Calculating [H1+] and [OH1-]

A. Use __________ to calculate concentration of unknown ion. Assume 25°C.

→←

B. Notice that in order for __________ to remain constant an _________________ in either [H1+] or [OH1-] causes a

_________________ in the other ion.

pH ScaleUnit 11 Page 7

Learning Target:I can define pH and use the hydrogen or hydroxide ion concentrations to calculate the pH of a solution.

Criteria for Success:I can define pH.

I can explain and use the pH scale.I can calculate pH given [H1+] or [OH1-]

The pH ScaleA. Expressing acidity or basicity in terms of _______ or _______ can be cumbersome because the values tend to be very _________. ____________ make these values easier to work with.

1. The letters pH stand for the French words pouvoir hydrogène, meaning _____________ ___________.

2. The _____ of a solution is defined as the ______________ of the common ________________ of the _______________ ion concentration, [H1+].

-log[H1+] = pH 10-pH=[H1+]

3. Remember that the values of [H1+]and [OH1-] are related by ______.

4. Like pH, pOH represents the _________________and relative _______________ of a base.

5. pOH can either be calculated the __________ way _____ is calculated or by using the following formula:

pH + pOH= 14

Modeling pH and Concentration

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

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

[H1+]

pH

Solution General Condition At 25°C

Neutral [H1+] = [OH1-] [H1+] = 1x10-7MpH=7.0 [OH1-]= 1x10-7M

Acidic[H1+] > [OH1-] pH < 7.0

[H1+] > 1x10-7M [OH1-] < 1x10-7M

Basic[H1+] < [OH1-] pH >7.0

[H1+] < 1x10-7M [OH1-] > 1x10-7M

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

10-14 10-13 10-12 10-11 10-10 10-9 10-8 10-7 10-6 10-5 10-4 10-3 10-2 10-1 1Acids and Bases

Unit 11 Page 8

Learning Target:I can understand acid-base reactions and predict products in acid base reactions that form water.

Criteria for Success:I can define neutralization.

I can predict the products in a neutralization reaction.I can explain how to carry out an acid-base titration.

I can calculate the concentration of a solution from titration data.

Neutralization

A. In aqueous solutions, _____________________________ is the reaction of hydrogen ions, H+1, and hydroxide ions, OH-1 to

form water molecules.

1. A ____________________ is also produced. It is an ionic compound composed of a ___________________ from a

base and an _________________________ from an acid.

2. Neutralization reactions are examples of ______________________ replacement reactions.

General Neutralization Reaction

HX(aq) + MOH(aq) → MX(aq) + H2O(l)

Titration

A. A ___________________________ is the controlled addition and measurement of the amount of a solution of

________________ ________________________ (titrant) required to react completely with a measured amount of a solution of

_______________________ ___________________________.

1. The point at which the two solutions used in a titration are present in stoichiometrically equivalent

amounts is the __________________________ point.

a. In the neutralization of a ________________ acid with a ________________ base, the equivalence point

occurs at approximate pH of ________.

b. The equivalence point does NOT always occur at a pH of 7 (You will learn more AP CHEM!)

2. The point at which the indicator changes color in a titration is known as the ____________________.

a. Ideally, the indicator that is chosen for the titration will have an endpoint that is close to the

equivalence point as a visual indication of the point at which the stoichiometric equivalent has been

added.

Molarity and Titration

A. Steps for Determining Molarity of Unknown

1. Start with the ___________________ equation for the ___________________ reaction, and determine the

stoichiometric relationship between the acid and base.

2. Determine the __________________ of acid (or base) from the __________________ (standardized) solution used

during the titration.

3. Determine the ___________________ of solute of the ____________________ solutions used during the titration

using the stoichiometric ratio from the balanced equation.

[OH1-]

pOH

4. Determine the _____________________ of the unknown solution using the number of moles determined from

above and the original volume of the unknown.