Chapter 6 Problems

6-29, 6-31, 6-39, 6.41, 6-42, 6-48,

Outline Equilibrium of Acids and Bases

Bronsted-Lowry Acids/Bases Define strong Define weak

pH of pure water at 25oC Define Ka and Kb Relationship b/w Ka and Kb

Chapter 8 – Activity Relationship with K

Acids and Bases & EquilibriumEquilibrium

Section 6-7

Strong Bronsted-Lowry Acid

A strong Bronsted-Lowry Acid is one that donates all of its acidic protons to water molecules in aqueous solution. (Water is base – electron donor or the proton acceptor).

Strong Bronsted-Lowry Base

Accepts protons from water molecules to form an amount of hydroxide ion, OH-, equivalent to the amount of base added.

Question

Can you think of a salt that when dissolved in water is not an acid nor a base?

Weak Bronsted-Lowry acid

One that DOES not donate all of its acidic protons to water molecules in aqueous solution.

Example?

Weak Bronsted-Lowry base

Does NOT accept an amount of protons equivalent to the amount of base added, so the hydroxide ion in a weak base solution is not equivalent to the concentration of base added.

example:

Common Classes of Weak Acids and Bases

Weak Acids

Weak Bases

Question: Question: Calculate the Concentration of H+ and OH- in Pure

water at 250C.

Equilibrium and Equilibrium and WaterWater

EXAMPLE: Calculate the Concentration of H+ and OH- in Pure water at 250C.

H2O H+ + OH-

KW=

Kw =

EXAMPLE: Calculate the Concentration of H+ and OH- in Pure water at 250C.

H2O H+ + OH-

KW=

Kw =

Example

What is the concentration of OH- in a solution of water that is 1.0 x 10-3 M in [H+] (@ 25 oC)?

Kw = [H+][OH-]

1.0 x 10-14 = [1 x 10-3][OH-]

1.0 x 10-11 = [OH-]

“From now on, assume the temperature to be 25oC unless otherwise stated.”

pH

~ -3 -----> ~ +16pH + pOH = - log Kw = pKw = 14.00

Weak Acids and Bases

HA H+ + A-

HA + H2O(l) H3O+ + A-

Ka

Weak Acids and Bases

B + H2O BH+ + OH-Kb

Relation Between KRelation Between Kaa and and KKbb

Relation between Ka and Kb

Consider Ammonia and its conjugate acid.

NH3 + H2O NH4+ + OH-

Kb

NH4+ + H2O NH3 + H3O+

Ka

Example

The Ka for acetic acid is 1.75 x 10-5. Find Kb for its conjugate base.

Example Calculate the hydroxide ion concentration in

a 0.0100 M sodium hypochlorite solution.OCl- + H2O HOCl + OH-

The acid dissociation constant = 3.0 x 10-8

][

]][[

OCl

OHHOClKb

1st Insurance Problem

Challenge on page 120Challenge on page 120

Chapter 8

ActivityActivity

Write out the equilibrium constant for the following expression

Fe3+ + SCN- Fe(SCN)2+

Q: What happens to K when we add, say KNO3 ?

]][[

])([3

2

SCNFe

SCNFeK

K decreases when an inert salt is added!!! Why?

Keq

8-1 Effect of Ionic Strength 8-1 Effect of Ionic Strength on Solubility of Saltson Solubility of Salts

Consider a saturated solution of Hg2(IO3)2 in ‘pure water’. Calculate the concentration of mercurous ions.

Hg2(IO3)2(s) Hg22+ + 2IO3

- Ksp=1.3x10-18

A seemingly strange effectseemingly strange effect is observed when a salt such as KNO3 is added. As more KNO3 is added to the solution, more

solid dissolves until [Hg22+] increases to 1.0 x 10-6 M. Why?

1823

22 103.1]][[ IOHgK sp

IICCEE

somesome -- - --x-x +x+x +2x+2xsome-xsome-x +x+x +2x+2x

182 103.1]2][[ xxK sp7109.6][ x

Increased solubility

Why? LeChatelier’s Principle?

Complex Ion?

?

The potassium hydrogen tartrate example

K+-O

O

OH

OH

O

OH

potassium hydrogen tartrate

Alright, what do we mean by Ionic strength?

Ionic strength is dependent on the number of ions in solution and their charge.

Ionic strength () = ½ (c1z12+ c2z2

2 + …)

Or Ionic strength (m) = ½ cizi2

Examples Calculate the ionic strength of (a) 0.1 M

solution of KNO3 and (b) a 0.1 M solution of

Na2SO4 (c) a mixture containing 0.1 M KNO3

and 0.1 M Na2SO4.() = ½ (c1z1

2+ c2z22 + …)

Alright, that’s great but how does it affect the equilibrium constant?

Activity = Ac = [C]c

AND

bB

baA

a

dD

dcC

c

bB

aA

dD

cC

BA

DC

AA

AAK

][][

][][

Relationship between activity and ionic strength

x

x

xz

3.31

51.0log

2

Debye-Huckel Equation

2 comments

= ionic strength of solution = activity coefficientZ = Charge on the species x = effective diameter of ion (nm)

(1)What happens to when approaches zero?(2)Most singly charged ions have an effective radius of about 0.3 nm

Anyway … we generally don’t need to calculate – can get it from a table

Activity coefficients are Activity coefficients are related to the hydrated related to the hydrated radius of atoms in radius of atoms in moleculesmolecules

Relationship between and

Back to our original problem

Consider a saturated solution of Hg2(IO3)2 in ‘pure water’. Calculate the concentration of mercurous ions.

Hg2(IO3)2(s) Hg22+ + 2IO3

- Ksp=1.3x10-18

Back to our original problem

Consider a saturated solution of Hg2(IO3)2 in ‘pure water’. Calculate the concentration of mercurous ions.

Hg2(IO3)2(s) Hg22+ + 2IO3

- Ksp=1.3x10-18

In 0.1 M KNO3 - how much Hg22+ will be dissolved?

Back to our original problem

Consider a saturated solution of Hg2(IO3)2 in ‘pure water’. Calculate the concentration of mercurous ions.

Hg2(IO3)2(s) Hg22+ + 2IO3

- Ksp=1.3x10-18