Dissolving
Solubility
Molarity
Dilution
Colligative Properties
100

In a solution, the substance that is being dissolved is the ____.

What is a Solute?

100

The limit of solubility of a solution. Beyond this no more solute dissolves. 

Saturated solution

100

The solution concentration expressed in terms of mol/L

Molarity

100
When diluting a solution this does not change
What is the number of moles
100

Give at least 2 colligative properties

What are vapor pressure lowering, boiling point elevation, and freezing point depression?

200
An increase in temperature will cause the solubility of gases to _______(increase, decrease, stay the same) in a solution

Decrease

200

A solution that is unstable due to high amount of solute causing crystals to form.

What is a supersaturated solution

200

The Molarity 15.0 L solution with 2.0mol of HCl.

What is 0.13 M

200
The concentration of a 5 mL of 2.0 mol/L solution after being diluted to 400mL
What is 0.0250 mol/L
200

This affects the colligative properties of solution and NOT the identity of the solute.

What is the number of solute particles?

300

This is the substance that dissolves the solute in solutions.

What is the solvent?

300

The type of  solution that has 30 grams of KNO3 dissolved in 100mL of water ( the solubility of KNO3 is 90g/100mL)

What is unsaturated

300

What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution? M=mol/Liter

3M

300

The volume of 6.00 M HCl needed to make 319 mL of 6.80M HCl is ____.


362 mL

300

A salt is dissolved in water, which has a boiling point of 100°C. The boiling point of the solution will be

greater than 100 °C

400
the separation of ions when an ionic compound is dissolved in water
What is dissociation
400
Causes the solubility of gases to decrease and the solubility of liquids to increase
What is an increase in temperature
400
The number of moles present in a 400mL solution with a concentration of 0.157 mol/L
What is 0.0628 moles
400

How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr?

50 mL

400

When the boiling point of the solution is higher than the pure solvent

Boiling point elevation

500

What factors affect the solubility of solutes  in a solution (Give 2) 

Pressure, Temperature, Amount of Solvent

500

A type of solute that exists as ions in solution and can conduct electricity. 

Electrolyte

500

What mass of Na2SO4 is needed to make 2.5 L of 2.0M solution? (Na = 23 g; S = 32 g; O = 16 g)


710 g

500

If 2.0 mL of 6.0M HCl is used to make a 500.0-mL aqueous solution, what is the molarity of the dilute solution?

0.024 M

500

A solution containing 0.1 mol of cane sugar (C12H22O11) in .500 kg of water froze at 0.374°C. (freezing point of pure water is 0°C) Calculate the freezing point depression constant (Kf) of the solvent. Change in temp.=Kf x (mol/kg solvent)x n 

1.87 °C/m

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