CHEMISTRY SEMESTER B COMPLETE
DETAILED CASE STUDY
l 1. Which solution would be least likely to carry an electric current? - C6H12O6
Which pair of compounds is immiscible? - water and toluene
Agitation prevents settling in a(n) - suspension
The substance dissolved in a homogeneous mixture is the
____________________________. - solute
Which type of mixture contains the smallest particles? - solutions
Henry's law relates - pressure to gas-liquid solubility.
When the energy released by the formation of solvent-solute attractions is greater than the energy
absorbed by overcoming solute-solute and solvent-solvent attractions, the dissolving process - has a
negative enthalpy of solution.
Effervescence is the - escape of a gas from a gas-liquid solution.
A substance that does not dissolve in a polar solvent is probably
____________________________. - nonpolar
All of the following are heterogeneous mixtures except - tap water.
,Under which conditions is more CO2 dissolved in a carbonated beverage? - in an unopened bottle in the
refrigerator
Raising the temperature of a solvent causes solvent-solvent collisions to become - more frequent and
more energetic.
In a solution at equilibrium, - the rate of dissolution and the rate of crystallization are equal.
In 100 mL of cold water, 35 g of NaCl will dissolve, but 70 g will not. This observation implies that -
solubility depends on the amounts of solute and solvent present.
To carry an electric current, a solution must contain
____________________________. - ions
NaOH solution contains 1.90 mol of NaOH (molar mass = 40.00 g/mol), and its concentration is 0.555 M.
What is its volume? ___________L - 3.42
Molecules whose water solutions can carry electric current - ionize in water
A dissolved solute that does not form ions is a ____________. - nonelectrolyte
Which of the following does not increase the rate at which a solid dissolves in water? - using large pieces
of the solid
What is the concentration of a 100. mL aqueous solution that contains 1.00 g KCl (molar mass = 74.55
g/mol)? Give your answer to the nearest thousandth Molar. Give only the number. - 0.134
What mass of NaCl (molar mass = 58.44 g/mol) is needed to make a 1.50 m solution using 300. g of
solvent? - 26.3 g NaCl
, The solubility of CuCl2(s) would ____________________________ with increasing solvent temperature.
- increase
Unit 2 - Test 2
Substances which change color in the presence of acids or bases are called _____. - indicators
The top industrial chemical produced in the United States for many years has been - sulfuric acid
Which is not a property of water that is a result of its hydrogen bonding? - Water has an unusually high
freezing point.
Complete the following table, which deals with pH, [H+],acidity, neutrality and basicity.
pH
[H+]
Solution is:
<7
(a)
(b)
(c)
DETAILED CASE STUDY
l 1. Which solution would be least likely to carry an electric current? - C6H12O6
Which pair of compounds is immiscible? - water and toluene
Agitation prevents settling in a(n) - suspension
The substance dissolved in a homogeneous mixture is the
____________________________. - solute
Which type of mixture contains the smallest particles? - solutions
Henry's law relates - pressure to gas-liquid solubility.
When the energy released by the formation of solvent-solute attractions is greater than the energy
absorbed by overcoming solute-solute and solvent-solvent attractions, the dissolving process - has a
negative enthalpy of solution.
Effervescence is the - escape of a gas from a gas-liquid solution.
A substance that does not dissolve in a polar solvent is probably
____________________________. - nonpolar
All of the following are heterogeneous mixtures except - tap water.
,Under which conditions is more CO2 dissolved in a carbonated beverage? - in an unopened bottle in the
refrigerator
Raising the temperature of a solvent causes solvent-solvent collisions to become - more frequent and
more energetic.
In a solution at equilibrium, - the rate of dissolution and the rate of crystallization are equal.
In 100 mL of cold water, 35 g of NaCl will dissolve, but 70 g will not. This observation implies that -
solubility depends on the amounts of solute and solvent present.
To carry an electric current, a solution must contain
____________________________. - ions
NaOH solution contains 1.90 mol of NaOH (molar mass = 40.00 g/mol), and its concentration is 0.555 M.
What is its volume? ___________L - 3.42
Molecules whose water solutions can carry electric current - ionize in water
A dissolved solute that does not form ions is a ____________. - nonelectrolyte
Which of the following does not increase the rate at which a solid dissolves in water? - using large pieces
of the solid
What is the concentration of a 100. mL aqueous solution that contains 1.00 g KCl (molar mass = 74.55
g/mol)? Give your answer to the nearest thousandth Molar. Give only the number. - 0.134
What mass of NaCl (molar mass = 58.44 g/mol) is needed to make a 1.50 m solution using 300. g of
solvent? - 26.3 g NaCl
, The solubility of CuCl2(s) would ____________________________ with increasing solvent temperature.
- increase
Unit 2 - Test 2
Substances which change color in the presence of acids or bases are called _____. - indicators
The top industrial chemical produced in the United States for many years has been - sulfuric acid
Which is not a property of water that is a result of its hydrogen bonding? - Water has an unusually high
freezing point.
Complete the following table, which deals with pH, [H+],acidity, neutrality and basicity.
pH
[H+]
Solution is:
<7
(a)
(b)
(c)
