1. what are the two equations we have studied so far in this unit? 2. how does a net ionic equation...

1. What are the two equations we have studied so far in this Unit?

2. How does a net ionic equation differ from a molecular equation?

Day 3 1-3

1. Molarity, M or M

a. Most widely-used unit of __________________

b. Formula

concentration

M = # mols of solute # L of solution

D. Dilution is adding more ________ to a solution to reduce the ________________. 1. Used to prepare solutions from

_______________ solutions.

2. Formula

solventconcentration

stock or conc.

VcMc = VdMd

(Volume of Conc.)(M Conc.) = (Volume of Dilute)(M of Dilute sol’n)

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4

First Solutions Lab

A. A solute that forms ions in solution and

conducts ____________ is known as an _____________, while a solute that neither forms ions nor conducts ____________ is known as a ________________.

electricityelectrolyte

electricitynonelectrolyte

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6

B. Ionic compounds and some molecular compounds ____________ in water.

1. Strong electrolytes produce a _______ number of ions.

2. Weak electrolytes produce a _________ number of ions.

dissociate

larger

smaller

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8

C.Most molecular compounds _________ in water and are called _______________.

D. Solubility does not determine if a solute is a strong or weak electrolyte. 1. Acetic acid:

_____ solubility + ______ electrolyte

dispersenonelectrolytes

Only 1% is H+ + C2H3O2- in sol’n, rest is

HC2H3O2high weak

Equilibrium: HC2H3O2(aq) H+(aq) + C2H3O2

-(aq)

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2. Barium hydroxide:

____ solubility + ________ electrolyte

E. Solvation is the surrounding of _______ particles by particles of the ________. Known as ___________ when water is the solvent.

low strong

Not very soluble but

everything that dissolves dissociates

solutesolvent hydration

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ASSIGNMENT :

Page 548 #s 48, 50, 57, 58, 59, 60 (a and b), 61

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F. The Water Welcome Wagon!

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Was the Wicked Witch a good chemistry student?

Did she correctly and scientifically describe

her demise?

HW# 1 due tomorrow14

A. Acids

1. Able to ionize and form ___ in aqueous solutions

2. Often referred to as ________ donors

3. Decrease the concentration of _____ in aqueous solutions

H+

proton

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OH-

4. Monoprotic acids release ____ ___ per molecule of acid.

Ex:

5. Diprotic acids release _____ ___ per molecule of acid.

Ex:

one

H+

HCl, HNO3, HC2H3O2

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two H+

H2SO4H2SO4(aq) HSO4(aq) + H+

(aq)

HSO4(aq) SO-24(aq) + H+

(aq)

Only some of 2nd H+ come off

1st H+ always comes off

6. Strong acids

7. Weak acids

- completely ionize in H2O chloric, hydrobromic, hydrochloric, hydroiodic, nitric, perchloric, sulfuric

- partly ionized in H2O, most acids are weak

acetic, hydrofluoric

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B. Bases

1. Able to ionize and form ____ in aqueous solutions

2. Often referred to as proton __________

3. Decrease the concentration of ___ in aqueous solutions

OH-1

acceptors

H+

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4. Metallic bases are called _____ ___________.

Ex:

5. Nonmetals can also form bases. Ex:

6. Strong bases

7. Weak bases

metal hydroxides

LiOH, NaOH

NH3

- Alkali + heavy alkaline earth metals: LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

19NH3, other metal hydroxides

C. Salts

A salt forms when the __________ of an _____ is replaced by a different _______, generally from a _____. This usually occurs in a ________________ reaction.

Ex:

hydrogenacid cation

baseneutralization

HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)

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A. Metathesis reactions can also be called _______ ______________ reactions.

B.The mixing of 2 solutions will result in a chemical reaction if _____ are _________ from the solution.

double replacement

ions removed

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Metathesis (Exchange) Reactions

• Metathesis comes from a Greek word that means “to transpose.”

AgNO3 (aq) + KCl (aq) AgCl (s) + KNO3 (aq)

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Metathesis (Exchange) Reactions

• Metathesis comes from a Greek word that means “to transpose.”

• It appears the ions in the reactant compounds exchange, or transpose, ions.

AgNO3 (aq) + KCl (aq) AgCl (s) + KNO3 (aq)

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Solution Chemistry

• It is helpful to pay attention to exactly what species are present in a reaction mixture (i.e., solid, liquid, gas, aqueous solution).

• If we are to understand reactivity, we must be aware of just what is changing during the course of a reaction.

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Ions can be removed from solution by any of 3 processes:

1. The formation of an __________ solid, known as a _____________

2. The formation of either a weak

____________ or a ________________

3. The formation of a ____ that bubbles

out of the solution

insolubleprecipitate

electrolyte nonelectrolyte

gas

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Precipitation Reactions

When one mixes ions that form compounds that are insoluble (as could be predicted by the solubility guidelines), a precipitate is formed.

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C. ExamplesWrite the molecular, complete, and net ionic equations

for these reactions that occur in water.

1. Magnesium nitrate and sodium hydroxide

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C. ExamplesWrite the molecular, complete, and net ionic equations for

these reactions that occur in water.

2. Magnesium hydroxide and hydrochloric acid

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C. ExamplesWrite the molecular, complete, and net ionic equations

for these reactions that occur in water.

3. Chromium(II) acetate and nitric acid

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C. ExamplesWrite the molecular, complete, and net ionic equations

for these reactions that occur in water.

4. Iron(II) carbonate and hydrochloric acid

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Locate your lab paper for today!!!