College Chem 1/2 ch. 4

what is the bond angle for water?

104.5

Aqueous Chemistry

Chemistry of solutions with water as the solvent.

Why is water special?

its structure. Has a bent bong angle of 104.5

most solids that get dissolved are what?

salts

hydration

The process of the oppositely charged particles being attracted to one another and the salt “falling apart”

Solubility

how likely a substance is to dissolve in water.

solute

the substance that gets dissolved in the liquid (usually starts as the solid)

Solvent

the substance that does the dissolving, Usually water

electrolyte

a substance that produces an electrically conducting solution when dissolved in water or melted, due to the separation of the substance into positively and negatively charged particles called ions

strong electrolyte

lots of ions present, so the salt breaks apart into ions completely

weak electrolytes

Some but not all of the salts dissolve

Nonelectrolyte

a solid does not break up into ions in solution

what can be strong electrolytes?

soluble salts, strong Acids strong bases

what can be weak electrolytes?

most popular, acetic acid (HC₂H₃O₂) and ammonia (NH₃)

what can be nonelectrolytes?

anything without an OH

Molarity=?

Moles of Solute/ Liters of solvent

stock

is a strongly concentrated solution whose concentration is accurately known and is typically going to be diluted

Dilution

Taking a portion of your standard/stock solution, and diluting it down

dilution equation=

M1 V1= M2 V2 (M=Molarity of solution, V= volume of solution)

What are the three types of chemical reactions?

Precipitate, Acid/base, & Oxidation

precipitate

When two solutions are mixed an insoluble substance forms, (cannot be charged), usually a double replacement

what will form form a precipitate reaction?

A cation and an anion only

What forms in an acid base reaction?

water and a salt

molecular equations

Shows the salts combined.  (We’re used to these.)

Complete ionic equation

The individual ions, not the molecules , are shown in the equation.  What is actually occurring in the reaction

Net ionic equation

spectator ions are not shown.  Only the ions that participate in the rxn.

Arrhenius’s definitions

Acid ~ produces H⁺ (a proton) in water. (HCl), Base ~ produces OH^- ions in water. (NaOH)

Volumetric analysis

a technique for determining the amount of a certain substance.

Titration

delivery through a buret of a measured volume of a solution of a known concentration (titrant) into a solution being analyzed (analyte). 

equivilance point

the point in the titration where enough titrant has been added to react exactly with the analyte.

3 Requirements for Titrations

k

HI

Hydroiodic acid

HBr

Hydrobromic acid

HCl

Hydrochloric acid

HNO3

Nitric acid

H2SO4

sulfuric acid

HClO4

perchloric acid

LiOH

Lithium Hydroxide

NaOH

sodium Hydroxide

KOH

potassium Hydroxide

RbOH

rubidium hydroxide

CsOH

Cesium Hydroxide

Be(OH)2

Beryllium hydroxide

Mg(OH)2

magnesium hydroxide

Ca(OH)2

calcium hydroxide

Sr(OH)2

strontium hydroxide

Ba(OH)2

Barium hydroxide