Chemistry Chapters 4-6

Solution

A liquid mixture in which minor component is uniformly distributed with the major solution.

Solvent

Is the part of the solution with the greatest amount of moles.

Solute

The part of the solution with the lesser amount of moles.

Brownian Motion

The motion of a solution’s solvent molecules dispersing the solute throughout the volume of the solution.

Concentration

The amount of solute in a given solution.

Three ways of denoting concentration

• Mass to Mass

• Mole to Volume

• Composition Percentages

Mass to Mass Ratio Equation

Mass of Solute/Mass of total Solution

Denoting Mass to Mass Concentration

(W/W) Ex: .1 W/W Salt (Weight to Weight)

PPM

Part Per Million (A unit used to express very small concentrations of a substance in a larger sample or solution.)

PPB

Parts Per Billion

1 microgram of solute/ 1 gram of solvent

1×10^-9 g Solute

1000 Gram of Solvent

Why can we discount the weight of solute in these “parts per” concentration?

At these concentrations, we can say that the weight of solute does not effect the total weight of the solution.

Molarity

Moles of solute dissolved in liters of solvent.

Molarity’s Units

Mol/L (Moles per Liter) or “M”

Choosing glassware when making a solution.

Uncertainty plays an important role in choosing the type of glassware.

Glassware for storage.

Beaker and Erlenmeyer Flask

Volumetric Flask

A flask that only measures one set measurement and it is very precise and will most likely give the most accurate results.

Why do you need to fully solvate solids before filling to the line when making a solution?

The solid takes up a certain amount of volume, after dissolved it changes the volume.

Last step you should ALWAYS do when making a solution.

Formula for dilutions.

M1V1 = M2V2

M1V1 = M2V2

M1 = Molarity of stock solution. V1 = Volume of stock solution.

M2 = Molarity of dilution solution. V2 = Volume of dilution.

Calibration Curve

• Measurement of concentration at multiple dilutions of stock solution.

• x-y plot is generated (measurement Vs. Concentration)

• Unknown solutions is measures and then using equation from graph concentration is determined.

HCl

Hydrochloric Acid (Strong Acid)

HBr

Hydrobromic Acid (Strong Acid)

HI

Hydroiodic Acid (Strong Acid)

HNO3

Nitric Acid (Strong Acid)

CClO4

Perchloric Acid (Strong Acid)

H2SO4

Sulfuric Acid (Strong Acid)

HClO3

Chloric Acid (Strong Acid)

HIO4

Periodic Acid (Strong Acid)

LiOH

Lithium Hydroxide (Strong Base)

NaOH

Sodium Hydroxide (Strong Base)

KOH

Potassium Hydroxide (Strong Base)

RbOH

Rubidium Hydroxide (Strong Base)

Electrolyte

Salts dissolved in water. They enhance the conductivity of water.

Strong Electrolytes

Complete Dissociation in water.

Weak Electrolyte

Partial Dissociation in water.

Bronsted-Lowry Acid

Acid that donates a proton (H+)

Bronsted_Lowry Base

Base that accepts (H+) protons.

H3O+

Hydronium ion

• It’s formed when a proton (H+) combines with a water molecule (H2O) in aqueous solutions.

Weak Acid

Weak disassociation of proton and counter ion. (Every other Acid not named/ Well for this class.)

Chemical Equilibrium

Dynamic state in a reversible chemical reaction where the forward and reverse reactions occur at equal rates, resulting in constant concentration of reactants and products.

Weak Base

Not a strong grabber of protons. (Exists in an equilibrium state)

General rule for dilutions.

The amount to decrease the concentration of the solution. Dilutions need to be smaller than the target volume.

Conjugated Base of a strong acid.

Always a weak base. This is because strong acids readily donate their protons, and the resulting conjugate base typically more stable and therefore less reactive as a base.

Titrations

Calibration curve but with acids and bases…sort of. Will learn more in analytical chemistry.

Equilibrium Point

The point where (H+) and (OH-) are equal in titration.

Heresy

Insoluble salt

Why are some salts not soluble in water?

The electrostatic force holding things together is greater then water’s ability to pull things apart.

Molecular Equation

Regular standard equation.

Ionic Equation

Everything is broken down into Ions. (So write all the charges of each element.)

Net Ionic Equation

Some Ions/ elements in the equation don’t react to create something. In this equation you simplify the ionic equation and only write the ones that create precipitants.

Spectator Ion

Ions that do not form the precipitate.

Solubility Rules for Common Ionic Compounds in Water

Soluble Compounds

All compounds containing the following ions are soluble:

Cations: Group 1 Ions (Alkali metals and NH4+)

Anions No3- and CH3COO- (Acetate)

Solubility Rules for Common Ionic Compounds in Water

Soluble Compounds (Anions)

Compounds containing the following anions are soluble except as noted:

Cl- Br-, and I-, EXCEPT those of Ag+, Cu+, Hg3+. and Pb2+.

SO42- Except those of Ba2+, Ca2+, Hg2 2+, Pb2+, and Sr2+.

Solubility Rules for Common Ionic Compounds in Water

Insoluble Compounds

• All hydroxides except those of group 1 cations and Ca(OH)2, Sr(OH)2, and Ba(OH)2

• All sulfides except those of group 1 cations and NH4+

• All phosphates except those of group1 cations and NH4+

  Most fluorides, though not those of group 1 cations and NH4+.

Water both a…

Bronsted Acid and a Bronsted Base

Saturated Solutions

All salts have a limit of the amount of stuff that can be inside. A saturated solution contains the maximum amount of solute that can be dissolved in a given solvent at a specific temperature and pressure.

Super Saturated Solutions

When a solution contains more salt than the saturation limit.

Oxidation

The loss of electrons OIL Oxidation is Loss

Reduction

The Gain of electrons. RIG Reduction is Gain

Oxidizer

Thing that gains electron(s). (The thing that causes the loss)

Reducer

Thing that loses electron(s).

(Thing that causes the gain)

Real name for the charge state of elements.

The Oxidation States

What does the Oxidation State Signify?

Denotes the number of electrons that element or molecule has lost or gained.

How is a gas more formally defined?

Defined as a compressible fluid.

Characteristics of Gas

1. Fluid as the substance that continually deform (flow) under external fluid.

2. Will conform to the shape of container, but it expands to fill the entire container.

3. Large distance between molecules (0.01% of given space occupied)

   1. Molecules Travel at rapid rates.

STP definition when talking about gases.

0 Degrees Celsius and 1 barr of pressure (o.987 atm)

Pressure Definition

For simplicity we will say that the pressure will be 1 atm. The amount of force divded by a given area. P= F/A also noted as p equal ma/ A. Where m is the mass and a is the acceleration.

Higher altitudes have.. atmospheric pressure.

Less

What is the SI unit for pressure?

Pascal (Pa)

What is a Pascal?

1 Pa = 1 N/m² = 1kg/ms² (m= Meter) (s= Second)

Atm to Pa

1 atm = .101325pa or 101.325kPa

Atm to mm Hg

1 atp pushed Hg up the column 760 mm Hg

Atm to torr

1 torr = 1 mm Hg

Atm to psi

1 atm = 14.7 psi (Pounds of force per square inch)

What is the major assumption in the Gas Laws?

Ideal gas…

What is an ideal gas?

As gas that has no interaction with itself.

Do ideal gases exist in nature?

Noble gases are close, but at high enough temperatures collisions will cause an interaction between atoms. (They do not exist.)

Boyle’s Law relates to what two quantities?

Pressure and Volume are related.

Charles’ law related what two quantites.

Temperature and volume are related.

Avogado’s law relates what two quantities?

Moles and Volume

Amonton’s law relates what two quantities?

Pressure and Temperature.

How are pressure and volume related?

Pressure is inversely proportional to volume meaning as one increases, the other decreases, and vice versa.

This relationship is described by Boyle's Law, which states that for a given amount of gas at constant temperature, the volume of the gas is inversely proportional to its pressure.

P1V1 = P2V2 

What is held constant through Bolye’s law?

Temperature and # of moles.

What explanation is there for these constants during boyle’s law?

The # of collisions between the gas particles and the surface of the container decrease as the volume of the container increase.

Boyle’s Law Equation

P1V1 = P2V2

How are volume and temperature related?

Volume is proportional to the gas’s temperature.

What is held constant through this relationship of volume and temperature?

This relationship is seen when pressure and moles are kept constant.

Why does this relationship of constants apply to how volume and temperature are related?

Temperature is in the constant, the only recourse a system has when the kinetic energy of gas particles (temp) increases, is a corresponding increase in volume.

What is the formula for recalculating Charles’ law after whether V or T change?

V1/T1 = V2/T2

How are moles of gas and volume related?

Moles of gas is proportional to the gas’s volume.

What is held constant in this relatioknship between moles of gas and volume?

The volume and moles are kept constant. W

Why are volume and moles kept constant in Amonton’s Law?

If the kinetic energy of gas molecules (temperature) increases, the number of collisions (pressure) of the gas particles and container will also increase.

What is the formula for recalculating Amonton’s law after either P or T change?

P1/T1 = P2/T2 P = Pressure T = Temperature

What is the ideal gas law?

The combination of the last 4 gas laws to relate P, V, n and T together.

What is the mathematical formula for the ideal gas law?

PV=nRT

What does each letter in the formula PV=nRT mean?

P= Pressure (atm) V= Volume (L) n= Number of mol (mol) R= Ideal gas constant. T= Temperature (K)

What is R

Ideal Gas Constant W

What is the value and unit of R that will be in this class?

R (Ideal Gas Constant) The combination of the constant from the 4 laws, values depends on units that are used.

What is molar volume?

Volume occupied by 1 mol of a gas.