CH110

Chapter 16 Notes

Solubility was introduced in Chapter 4 with the formation of precipitates

LeChatelier's Principle tells us that formation of a solid from aqueous reactants drives a reaction in the forward direction

Using what we learned in Chapter 14 on equilibrium constants, we can discuss how soluble something is

Ex- BaSO₄(s) in eq. with Ba²⁺(aq) + SO₄^2-(aq)

The equilibrium constant (or solubility product constant here), K_sp = 1.1x10^-10 at 25^oC

....not very soluble, which is why it can be taken prior to being X-rayed

K_sp's are influenced by a complex set of factors

Given K_sp, you can calculate an ion concentration and vice versa

Common Ion Effect revisited

LeChatelier's Principle re-revisited

Reaction (or Ion Product) quotient, Q_ip

Comparing Q_ip to K_sp tells whether precipitation will occur

For Q_ip > K_sp, precipitation of the supersaturated solution should occur

For Q_ip < K_sp, precipitation of the unsaturated solution cannot occur

For Q_ip = K_sp, the solution is saturated

Selective precipitation

Example 16.10 on page 707

pH effect

What is the effect if an ion is a conjugate acid or base?

Complex ions

Why is toothpaste fluoridated?

Qualitative analysis

Identity not amount (quantitative analysis)

A series of solubility tests can identify an unknown

Be informed! Read Chapter 25!!!

Air and water- composition and pollution

Smog and ozone

Global warming

Algae blooms

Acid rain and limestone

Nitrogen cycle

Carbon cycle

Poisons

Carcinogens

Corrosives

Heavy metals

Nerve gas

Oxygen transport blockers