WorksheetsPERFORMANCE TASK SCIENCE 1207
Total questions: 50
Worksheet time: 47mins
It describes two liquids that are mutually soluble with each other is called ________________.
imiscible
immiscible
miscible
micible
According to the general rule with regards to miscibility nonpolar solvents dissolve _______________.
a.polar compounds
b.nonpolar compounds
c.nonpolar solvents
d.both b and c
According to this principle when stress is applied to a system at equilibrium, the system shifts to relieve the stress is called ____________.
Hund's Principle
Mendeleev's Principle
Le Chatelier's Principle
Pauli's Exclusion Principle
The following are factors that affect the rate of solution excepts ________________.
agitation
particle size
polarities of solute and solvent
mass of solvent
Also known as the molar concentration of a solution and is the amount of substance in a certain volume of solution is called ______.
molality
molarity
normality
dilution
Also known as molal concentration and is the amount of substance dissolved in a certain mass of solvent is called __________.
molality
molarity
normality
dilution
The symbol used for molality is _________________.
M
m
N
n
The symbol used for normality is ________________.
M
m
N
n
The symbol use for molarity is _________________.
M
m
N
n
The formula used for calculating dilution is _____.
a. C1V1=C2V2
b. M1V1=M2V2
c.L1V1=L2V2
d. both a and b
What is the formula to be used if the given in the problems are no. of moles of solute and molarity?
V= M/n
V= n/M
L=n/M
V= n/m
How do you calculate no. of moles?
divide the mass of solvent to the molar mass of solvent
divide the mass of solute to the molar mass of solute
multiply the mass of solute to the molar mass of solvent
divide the mass of solute to the molar mass of solvent
What is the formula to be used if the mass of solvent and molality are given?
m= kg of solution x molality
n= kg of solution x molarity
n=kg of solvent x molality
n= Liters of solution x molality
What does 10 % by mass of HNO3 solution mean?
10 g solute and 100 g solution
10 kg solute and 100 kg solution
1000 g solute and 1000 kg solution
10 g solute and 90 g
What is the molar mass of HNO3 (Note: round off)
63 g/mol
65 g/mol
67 g/mol
69 g/mol
It refers to the measure of concentration equal to the gram equivalent weight per liter of solution is called __________.
molality
molarity
normality
dilution
Colligative properties are dependent only on ________.
no. of solute particles
no. of solvent particles
identity of the solute particles
identity of the solvent particles
Boiling Point elevation uses the formula ΔTb=i Kb m. What does "i" represents?
Van't Hoff Factor of solute
Vant Hoff Factor of solute
Vant Hoff Factor of solvent
Van't Hoff factor of solvent
The colligative property where there is the diffusion of water from high concentration to low concentration is called _________.
boiling point elevation
freezing point depression
osmotic pressure
vapor pressure
Which among the following is the correct formula for vapor pressure lowering is ____________.
a. ΔP= XB0PA0
b. ΔP= XB PA0
c. P solution= X solvent P solvent
d. both b and c
What is the molarity of 0.500 L NaOH solution if it contains 6.0 g NaOH [NaOH: molar mass: 40.0 g NaOH]
0.3 M NaOH
0.4 M NaOH
0.5 M NaOH
0.6 M NaOH
What is the molarity of 225 mL of a KNO3 solution containing 34.8 g KNO3?
1.51 M KNO3
1.55 M KNO3
1.57 M KNO3
1.59 M KNO3
How many moles of NaCl are in 3.5 L of a 1.5 M solution of NaCl?
5.21 M
5.23 M
5.25 M
5.27 M
If a student has 35.0 g of Fe Cl3 and needs to make a 1.5 molar solution with it, what will the volume of the solution be?
0.25 L
0.27 L
0.28 L
0.29 L
A student pipettes a 100 mL sample of 1.5 M solution of potassium bromide. How many moles of Kbr are contained in the sample?
0.15 mol KBr
0.18 mol KBr
0.19 mol KBr
0.22 mol KBr
Find the molality of a solution that contains 178 grams of CH3OH in 208 g of water.
26.68 m
27.68 m
28.68 m
29.68 m
Calculate the molality of 25.0 grams of KBr dissolved in 750.0 mL pure water.
0.28 m
0.32 m
0.36 m
0.38 m
Find the grams of H2O needed to dissolve 50.0 g of sucrose C12H22O11 to prepare a 1.25 m solution.
0.10 g H2O
0.12 g H2O
0.15 g H2O
0.18 g H2O
In reading the volume of a liquid we are using the __________.
a. low meniscus
b. high meniscus
c. moderate meniscus
d. both a and b
If 0.750 L of a 5.00 M solution of copper nitrate, Cu(NO3)2, is diluted to a volume of 1.80 L by adding water, what is the molarity of the resulting diluted solution?
2.04 M
2.08 M
3.2 M
4.2 M
A solution is prepared from 17.0 g NaCl dissolved insufficient water to give 150.0 mL of solution. What is the molality of the solution?
1.94 m
2.94 m
3.94 m
4.94 m
Calculate the moles and mass of solute in 250.0 mL of 1.50 M KCl?
0.375 mol, 30.0 g
0.375 mol, 28.0 g
0.475 mol, 28.0 g
0.375 mol, 48.0 g
Calculate what volume of the solution is required to obtain 0.250 mol of each solute given the molarity of 0.250 M AlCl3.
1 L
2 L
3 L
4 L
Calculate the no. of moles of 28 g glucose C6H12O6 in 300 g of water?
0.16 mole
0.18 mole
0.20 mole
0.22 mole
Molarity is also known as ________.
molar concentration
molal concentration
normality concentration
dilution
What is the molality of a solution in which 15.0 grams of iodine gas is dissolved in 500 g of alcohol?
0.12 m
0.14 m
0.15 m
0.18 m
What is the molality of the solution in which 3.0 moles of sodium chloride are dissolved into 1.5 kg of water?
2 m
3 m
4 m
5 m
What is the molality of a solution in which 0.145 mol carbon dioxide is dissolved in 591 g of water?
0.25 m
0.27 m
0.29 m
0.31 m
How many moles at ethanol, C2H6O are needed to prepare a 4 m solution using 0.800 kg of water
3.2 mole
3.5 mole
3.8 mole
3.9 mole
Osmosis flow to a semi-permeable membrane from high concentration to low concentration. High concentration refers to ________.
diluted solution
concentrated solution
water
solute
What is the normality of a solution that contains 50 g of H2SO4 dissolved in 15 L?
0.068 N
0.702 N
0.705 N
0.707 N
A mass of CaCl2 , when dissolved in 100.00 g of water, gives an expected freezing point of -5.0°C. What mass of glucose would give the same result?
49 g glucose
47 g glucose
45 g glucose
42 g glucose
Calculate the molarity of 4 molar solution of glycerin with a denisty of 6g/ cm3 of C3H8O3.
0.810 mol/kg
1.710 mol/kg
0.910 mol/kg
0.710 mol/kg
Concentrated sulfuric acid is a solution with a density of 1.94 g/mL and containing 95 % H2SO4 by mass. What is the molarity of this acid?
18.81 mol/ L
21.81 mol/ L
20.81 mol/ L
19.81 mol/ L
A solution of copper (II) acetate Cu(CH3CO2)2 is used as a green dye for textiles. We want to prepare a 0.150 M solution of copper (II) acetate, starting with 40.0 g of Cu(CH3CO2)2. What should be the total volume of the solution?
1.0 L
1.47 L
1.67 L
1.27 L
If 0.750 L of a 5.00 M solution of Copper nitrate, Cu (NO3) 2 is diluted to a volume of 1.80 L by adding water, what is the molarity of the resulting diluted solution?
2.08 M
3.08 M
4.08 M
5.08 M
Automotive antifreeze consists of ethylene glycol, C2H6O2 , a nonvolatile nonelectrolyte. Calculate the boiling point and freezing point of a 25.0 mass percent solution of ethylene glycol in water.
boiling point = 102.72 °C
freezing point = -9.87 °C
boiling point = 104.72 °C
freezing point = -7.87 °C
boiling point = 100.72 °C
freezing point = -9.87 °C
boiling point = 102.72 °C
freezing point = -5.87 °C
Calculate the freezing point of a solution containing 0.600 kg of CH3Cl3 and 42.0 g of eucalyptol C10H8O18, a fragrant substance found in the leaves of eucalyptus tree. Kf for CHCl3 is 4.68 OC/molal and normal freezing point is -63.5 oC.
-65.61 oC
-68.62 oC
-72.61 oC
-82.61 oC
Calculate the molarity of a solution of HNO3 that is 35 % by mass and has a density of 1.21 g/mL.
6.72 mol HNO3/ L
6.74 mol HNO3/ L
6.78 mol HNO3/ L
7.71 mol HNO3/ L
The mass % of AlCl3 in water is 15 %. The density of the solution is 1.17 g/mL. What is the M of the solution?
1.28 M
1.30 M
1.32 M
1.34 M
