compositions
the ____ of the solvent and solute determine whether a substance will dissolve
stirring
_____ , temp, and surface area of the dissolveing particles determine how fast the substance wil dissolve
stirring
____ does not influence amount of solute that will dissolve. an insoluble substance remains undissolved regardless of how vigorously or for how long the solvent/solute system is ____
temp
at higher ____ the kinetic energy of water molecules is greater than at loewr temp as the y move faster.
true
more surface area of a solute that is ecposed the faster the rate of dissolving? t/f
kinetic
according to the ____ theory water molcules are in continuous motion
solvate
as ions _____ they dissolve in water
saturated solution
a _____ contains the maximum amount of solute for a given quantity of solvent at a constant temp and pressure. if additional solute is added to this solution it wont dissolve
solubility
the ____ of a substance is the amount of solute that dissolves in a given quanttiy of a solvent at a specificed temperature and pressure to produce a saturated soltion
100g
solubility is often expressed in grams of solute per ______ of solvent
unsaturated solution
a solution that constains less solute than a saturated solution at a given temp and pressure is an _____/ if additional solute is added to it the solute will dissolve until the solution is saturated
miscible
two liquids are ___ if they dissolve in each other in all proportions. in a solution, the liquid that is present in the larger amount is usually considered the solvent.
immiscible
liquids that are insoluble in one another are __
mass
solubility is defined as the mass of solute that dissolves in a give ___ of a solvent at a specified temp
solutes
temp affects the solibity of solid, liquid, and gaseous ___ in a solvent
solibulity increases
the ____ of most solid substances increases as the temp of the solvent ____
ytterbium sulfate
what substance's solubility decreases with temp?
supersaturated solution
a ______ contains mroe solut than it can theoritcally hold at a given temp.
seed crystal
the crystallization of a supernatural solution can be initiaed if a very small crystal called_____ of the solute is added
rock candy
another example of crystallization in a supersaturated solution is the production of ______
crystallize
seed crystals caused the sugar to ____ out of solution onto a string
cold hot
the solubilites of most gases are greater in __ water than __
oxygen
____ becomes less solible in water as the temp of the seolution rises
thermal pollution
when an indsutrial plant takes water from a lake to use for colling and then dumps the resulting heated water back into the lake the temp of the entire lake increases. such a change in temp is kown as ________
you create one by heating the water and then dissolving the substance to its maximum capacity. When the water cools to a normal temp. it will be supersaturated
How does a supersaturated solution form?
temperature -- Generally, an increase in the temperature of the solution increases the solubility of a solid solute. A few solid solutes, however, are less soluble in warmer solutions. For all gases, solubility decreases as the temperature of the solution
Explain the effects of temperature on solid and liquid solutes. Do the same for solutes in the gas phase.
little
changes in pressure have ____ affect o the solubility of solids and liquids
strongly
pressure ____ influeces the solibulity of gases
The solubility of gases in liquids is greatly affected by pressure.It is directly proportional to pressure i.e. increasing pressure increases solubility of gas in water.
The relationship between solubility of gas and pressure was given by Henry in the for
What is the relationship between pressure and solubility for gas solutes.
s1/p1=s2/p2
calculating solubility of a gas
concentration
the ___ of a solution is a measure of the amount of solute that is dissolved in a given quantity of solvent
dilute solution
a ______ is one that contains a small amount of solute
concentrated solution
a ____ contains a large amount of solute
molarity
____ is the number of moles of solute dissolved in one liter of solution
moles of sollute/ liters of solution ( volume)
to calculate molarity of a solution:
molar concentration
molarity is known as
solution concentration= g/mlx mol/gx ml/l=mol/l=M
finding molarity of a solution
moles solute= mol/LxL
finding moles of solute in a solution
lowers same
adding solvent to a concentrated solution ___ the concentration but the total number of moles of solute present remains the ___
solution
diluting a _____ reduces the number of moles of solute per volume but the total number of moles of solute in solution does not change
M1XV1=M2XV2
equation for moles of solute
dilute solution has a small amount of solute in the solvent while concentrated solution has a large amount of solute in the solvent
What is the difference between a concentrated solution and a dilute solution?
volume
concentration of a solution in percent can be expressed in 2 ways: the ratio of ___ fo the solute to the volume of the solution or as the radio of the mass of solute to the mass of the solution?
percent
another way to expess concentration of a solution is as a ___(mass/mass) which is the number of grams of solute in 100 grams of solution
solution solute
the mass of solvent equals the mass of the ___ minus the mass of the ____
colligative property
a property that depends upon the number of solute particles in the solution and not upon their identity is called
vapor pressure lowering, boiling point elevation, freezing point depression
three important colligative properties of solutions are?
vapor
________pressure is the pressure exerted by a vapor that is in dynamic equilibrium with its liquid in a closed system
solution
a ____ that contains a solute that is not easily vaporized always has a lower vapor pressure than the pure solvent
throughout
in an aqueous solution of sodium chloride, sodium ions and chloride ions are disprsered _______ the liquid water
shells of water of solvation
both within the liquid and at the surface, the ions are surrounded by layers of associated water molecules or ______
reduce
the formation of these shells of water of solvation ___ the number of solvent molecules that have enough kinetic energy to escape as vapor.solution has a lower vapor pressure than the pure solvent would have at the same temperature.
Either the boiling point elevation or the freezing point depressionis a colligative property, meaning that the property depends on the molar concentration of the solute but not on its identity.
Is the identity of the solute important in determining how low a solvent's vapor pressure will go?
ionic solutes
______ that dissociate such as sodium chloride and calcium chloride have greater effects on the vapor pressure than does a nondissociating solute such as glucose
decrease number
the _____ in a sollutions vapor pressure is proportioanl to the ____ of particles the solute makes in solution
orderly
when a substance freezes, the particles of the solid take on an _____ pattern
solute
the presence of a ____ in water disrupts the formation of this patter because of the shells of water of solvation
kinetic withdrawn
as a result more _____ energy must be ____ from a solutan than from the pure solvent to cause the solution to solidify
pure solvent
the freezing point of a solution is lower than the freezing point of the ____
freezing point depression
the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent is the ?
number indentity
the magnitude of the freezing point depression is proportional to the ____ of solute particles dissolved in the solvent and does not depende upon their ____
1000g
the addition of 1 mol of solute particles of ______ of water lowers the freezing point by -1.86C
-1.86C
if you add 1 mol (180g) of glucose to 1000g of water the solution freezes at ?
solution
the melted ice forms a ___ with a lower freezing point than that of pure water
boiling point
the _____ of a substnace is the temp at which the vapor pressure of the liquid phase equals atmospheric pressure
decreases
adding a nonvolatile solute to a liquid solvent ___ the vapor pressure of the solvent
added
because the decrease in vapor pressure, additional kinetic energy must be ____ to raise the vapor pressure of the liquid phase of the solution to atmospheric pressure and initate boiling
higher
the boiling point of a solution is __ than the boiling point of the pure solvent
boiling point elevation
the difference in temp between the boiling point of a solution and the boiling point of the pure solvent is the ___
concentration
the boiling point elevation depends on the _____ of particles not on their identity
additional kinetic energy
it takes _______ for the solvent particles to overcome the attractive forces that keep them in the liquid
solute
the presence of ____ elevates the boiling point of the solvent
boilint point elevation number
the magnitude of the ______ is proportioanl to the ____ of solute particles dissolved in the solvent
0.512C
the boiling point of water increases by ______ for every mole of particles that the solute forms when dissolved in 1000g of water
When you add a soluble solute to a pure solvent the vapor pressure is lowered. This happens because there are solute molecules located throughout the solution. Some of the solute molecules are at the surface where vaporization occurs. When that is the cas
Explain what happens at the molecular level that accounts for the lowering of a solvent's vapor pressure when a solute is added.
Freezing-point depression describes the phenomenon that the freezing point of a liquid (a solvent) is depressed when another compound is added, meaning that a solution has a lower freezing point than a pure solvent.
Give a molecular explanation for the freezing-point depression of a solvent when a solute is added.
Solute changes the boiling point of the solvent. In fact when solute is added in a solvent then after adding the solute the boiling point of the solution increases. For example, if salt is added in water then the boiling point of water will increase from
Give a molecular explanation for a solvent's boiling point elevation which result from the addition of solute.
This question is aimed at the van 't Hoff factor, a value associated with how much a substance ionizes in solution. Glucose is a molecular compound and does not ionize at all. Its van 't Hoff factor is equal to 1 NaCl ionizes full in solution, yielding tw
Of the following three solutes, which would lower water's freezing point the most: glucose, sodium chloride, calcium chloride? Which would lower water's vapor pressure the most? Which would elevate water's boiling point the most? Give an explanation for e