Click Once to Begin JEOPARDY! Chemistry Final Review Chapters 6.1-6.4 and 6.7 Juliann Frenette.

Click Once to BeginJEOPARDY!Chemistry Final Review

Chapters 6.1-6.4 and 6.7Juliann Frenette

JEOPARDY!

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Vocab. pH SolublityVapor

Pressure

Boiling and

FreezingMisc.

Define strong and weak electrolytes.

Strong electrolytes are ionic compounds that almost completely dissociate into ions

when dissolved in water. Weak electrolytes only partially

dissociate.

Define a solution, solute and solvent.

A solution is composed of the substance that is dissolved. The solute is what is

being dissolved. The solvent is the liquid in which the solute is dissolved.

Write the equations for the 3 main ways to express

concentration: %W/V, molarity and molality.

%W/V= (mass solute/volume)(100)Molarity= moles of solute/L of

solutionMolality= moles of solute/kg of

solvent

State the differences between unsaturated, saturated and

supersaturated.

Unsaturated solutions have room to hold more solute particles and saturated solutions are

holding all the solute particles it can. Supersaturated one are created by heating to increase the amount of solute in the solution then cooled down to a temp. that ordinarily wouln’t allow the solution to hold that much

solute

Explain how well strong and weak electrolytes can conduct

electricity and why that is.

Strong electrolytes conduct electricity better than weak ones because there is a greater sea of

electrons when strong electrolytes are dissolved in

water

What is the equation used to calculate pH?

pH= -log[H+ or H30+]

The normal pH of human blood is 7.4. Human blood is…

Slightly basic

What is the relationship between the concentration of hydronium

ions and pH?

As the concentration of the hydronium ions increases, the pH

decreases.

Strong acids are to strong ________, as weak acids are to

weak _________.

Electrolytes

What is the [H+] of a solution whose pOH = 2.86 ?

  7.24 x 10-12 M

When does a precipitate form?

When two compounds mix to form a product that is

insoluble

True or false? All acetates are soluble

True

Which of the following salts are insoluble?

A: LiClB: NaClC: AgClD: KCl

AgCl

Which is always soluble: Ammonium or Ammonia?

Ammonium

2 KCl(aq) + Pb(NO3)2(aq) → 2 KNO3(?) + PbCl2(?)

2 KCl(aq) + Pb(NO3)2(aq) → 2 KNO3(aq) + PbCl2(s)

Define vapor pressure.

The pressure created by liquid molecules with enough energy

to break them free from the surface and become gas

molecules.

What is the relationship between vapor pressure and temperature?

As temp. increases, the vapor pressure of a liquid increases.

What does vapor pressure have to do with boiling point?

The boiling point is when the vapor pressure of the liquid

and the atmospheric pressure of he surroundings are equal.

A solution always has a vapor pressure that is ______ than that

of the original solvent. Why?

It’s less than the original solvent because there are

fewer solvent molecules on the surface available for

evaporation.

Connect all these terms in a sentence: average kinetic energy, temperature, imfs

and vapor.

When temp. increases, so does the average kinetic energy. When

the average increases, the # of molecules that have the min.

energy needed the break the imfs of the liquid and become vapor

also increases.

What are the equations to calculate boiling point and freezing point and what

do the variable stand for?

Boiling point: T=KB(M) where KB is the boiling point elevation

constant and M is molarity.Freezing point: T=KF(M) where

KF is the freezing point depression constant and M is

molarity.

A substance is at its freezing point when…

The solid phase and liquid phase are in equilibrium.

_______ always have a higher boiling point than a pure ______.

Solutions always have a higher

boiling point than a pure solvent.

What is the normal boiling and freezing point of water in K and

C?

Tb= 373.15 K or 100C TF= 273.15 K or 0C

Explain what happens at the molecular level when a

substance freezes.

Daily Double!!!

At a lower temp., the solid molecules are leaving the

solid phase at a slower rate which can then be matched

by the liquid molecules joining the solid.

What is the pH if the pOH is 4?

10

If 62.0 g of ZnCl2 is added to 0.100 L of water, what is the molarity of the solution (with correct significant digits)?

4.45 M

Given the Kf for water is 1.86°C/m, what will be the

freezing point of a 2.2 m solution of glucose?

-4.09 degrees Celsius

For a 0.262M solution of sucrose in water with a KB of .512

degrees Celsius/Mcalculate the boiling point of the

solution.

.134 degrees Celsius

If the KB for water at sea level is .52 degrees Celsius/M, what is the molarity of it when the boiling

point is raised 100 degrees Kelvin?

.4 M

Final Jeopardy

Click Once to BeginRecite all the Solubility Rules

from memory!