Acids, Bases, and Salts: Unit 6 Outline

Characteristics of Acids

•Molecular substances that ______in water.

  1. ______difference is less that 1.8
  2. It’s a non-polar covalent molecule
  3. Creates ______in solution

•Acids react with ______metals to create hydrogen gas.

  1. Active metals include, ______.
  2. Cu, Ag, Au, Pt. DO NOT react with acids
  3. Metal + Acid  ______+ H2 (g)

• Affect the color of ______.

•React with bases  more neutral solution of H2O + ______

•Edible acids have a ______taste<don’t try this!>

Arrhenuis Acids

•A solution that yields an ______(a ______) as one of its components in solutions.

•H + Ions are always ______.

•Strong acids have:

  1. 1 H+ proton = 1 ______

•Weak acids have more ______molecules for every H+

Ionization of Acids

•The higher the rate of ionization, the more ______the acid.

•Strong: HCl: nearly ______ionized.

• sulfuric acid(H2SO4) ______ionized.

•Weak: Hydrofluoric acid (HF): ______ions

• Hydrosulfuric acid: ______ions.

Properties of Bases

•______

•Cause ______to turn colors

•Neutralize acids and produce a ______+ H2O

•______taste, ______feel

•Soap in the mouth?

Arrhenuis Bases

•Contribute a OH- (______) in solution.

•OH-, unlike H+, does not attach to other molecules UNLESS it has a ______charge

Ionization of Bases

•Ionize similar to acids, except that Bases tend to be ______compounds.

•The OH- ion is ______, while the metal attached is bonded ______

•Strong Bases: ______(almost 100%)

  1. Weak Bases: Ammonia compounds: ______

Salts

•Ionic compounds that have Ions other than ______and ______.

•SOLID=______

•Conduct ______when molten OR in solution

•Tend to have ______melting points

The Ionization of Water

•Water ionizes itself

•For any sample of water:

• H2O  H3O+ + OH-

•H2O = 1 mole; H3O+ = ______mole and OH- = ______mole

•In 10,000 L of H2O, there would be ______of H2O- one drop from a dropper!

Ionization of Water… continued

•There are ______amount of H3O+ and OH- ions.

•This allows water to:

  1. Be perfectly neutral
  2. Neutralize other substances through self ionization.

• - If an ______ion pops in, the OH- can ______it to a certain extent.

• - Most solutes are combinations of ______and ______, so, water dissolves and separates them.

Ionization of Water… continued

•Kw= OH- x H3O+

•In any sample: ______= 1.0x10-7

• ______=1.0x10-7

•Then Multiply: ______= 1.0x10-14

•Soooooooooooooooooooo… for a solution to be perfectly ______, it must have ______of OH- and H3O+ions.

The pH Scale

•A measure of the ______or ______of a solution, based on the concentration of the ______in solution.

•pH= “pouvoir Hydrogen” = Power of Hydrogen

•The pH of a given solution is: equal to the ______of the Hydrogen Ion ______in a given solution.

  1. ______scale
  2. Small # = ______
  3. Large # = ______

•The p OH scale: OPPOSITE of the pH scale.

  1. pH + p OH = 14; Why?

• Because we want to compare pH to ______—which always has

______

So—[H+] [OH-] = Kw and Kw= 1.0x 0^-14

Another View of Acids and Bases

•Bronsted- Lowry

  1. Acids: ______
  2. Bases: ______

•NH3 + H2O  NH4+ + OH-

  1. Draw Lewis dot structures
  2. ______Acids and Bases
  3. Strengths of acids chart: P.565

More Acids and Bases

•______= Ionization Constant for an acid.

• Strong Acids (HCl, H2SO4, HNO3, etc.) -all of the compound will ______.

  1. Weak Acids all ______at various rates: HC2H3O2 will ionize at lower rate than the strong acids. This affects acid strength.

•______= same thing, except for bases instead of acids.

•The ionization constants tell you the number of moles of the acid (Ka, H+) or base (Kb, OH-) in ______of a ______solution.

•More simply, it’s the ______of a particular ion in solution.

Key Terms

•______, ______(and complete…)

•ALL refer to a compound breaking apart into the ions that make the compound up.

•Simple Reactions:

  1. Adding an acid to a metal will produce?
  2. Adding a base to an acid will produce?

•Any reaction that makes an acid or base from its constituent parts is called Acid (or base) Formation.

  1. H + Cl = HCl.

•Neutralization- An acid + base reacts to produce a salt plus water.

Net Ionic Equations

•Net Ionic Equations*- In some instances, only a few certain elements are involved in a reaction. To ‘simplify’ the equation, all the inactive parts are removed from the equation.

•HCl (aq) + Zn (s)  H2 (g) + ZnCl (aq)

•H changes from a ______to a ______.

• Zinc does the opposite

• But what does the chlorine do?

•We write:

• H+ + Zn0  H20 + Zn +

•Since the Cl stays a ______, we can leave it off for this type of equation.

•Net Ionic Equations only occur in a special type of reaction, called ______

Redox

•Redox is short for ______reaction.

• Redox Reactions are an important part of chemistry.

• Redox Reactions are a result of ______.

•In our example above, electrons are taken from the Zinc, and given to Hydrogen. This makes Zinc an ion, and Hydrogen a free element—the opposite of what they were before the reaction.

• Reduction is the ______of electrons. Why do we call it reduction?

• Oxidation is the ______of electrons.

To remember this:

“LEO says GER”

______= Oxidation;

______= Reduction