The equation for molarity is
Moles of solute / Liter of solution
Moles of solute/ Moles of solution
Moles of solution/ Liters of solute
Liter of solution/ Moles of solute
Moles of a component over the total moles of the solution is known as?
Molality
Molarity
Mass percent
Mole Fraction
Mass of component/ total mass solution x 100 is mass percent.
CH3COOH is more soluble in which of these solutions?
H2O
CH3COOH
C6H6 is nonpolar and soluble in water.
What is the molarity of a solution made by dissolving 2.335 grams of H2SO4 in enough water to make 50 mL of solution?
.476 M
.764 M
6.47 M
7.46 M
How many mL of .200 m HCL solution are needed to obtain 0.0500 moles of HCL?
.250 mL
250 mL
4 mL
.400 mL
What is the mole fraction of methanol if 32.0 grams of methanol (CH3OH) is dissolved in 90 grams of water?
.166
.452
.998
4.99
Which one of the following can be used as a solvent for hexane (C6H14)?
Methanol (CH3OH)
Benzene (C6H6)
Liquid ammonia
Water
What is the mass percent of a saline solution made by dissolving 1 mole of NaCl (mm = 58.45 g) in 1 liter of water total?
5.84%
5.52%
5.00%
11.34%
The NaCl concentration of seawater is 3.5% by mass. What is its molarity if the density of seawater is 1.025 g/mL?
6.14 m
.614 m
.416 m
1.46 m
Molality is the moles of solute/kg of solvent.
What is the molality of a solution made by dissolving 1.45 grams of sucrose C12H22O11 in 30 mL of water?
14.1 M
.141 m
.141 M
1.41 m
The density of a 45.0 mass % solution of ethanol (C2H5OH) in water is 0.873 g/mL. What is the molarity of the solution?
8.53 M
9.77 M
15.5 M
0.515 M
What is the mole fraction of HCl in a 4.50 m aqueous HCl solution?
3.87
0.222
0.0750
0.0811
What is the mass percent concentration of a saline solution prepared by dissolving 1.00 mol of Na2SO4 in 1.00 L of water?
12.4%
57%
6%
The density at 20 ∘C of a 0.828 M solution of acetic acid in water is 1.0052 g/mL. The molar mass of acetic acid, CH3CO2H, is 60.05 g/mol. What is the molality of the solution? Molality = m
The molality of a solution prepared by dissolving 22.5 g of H2SO4 in 1.80 L of water m = m
The mole fraction of each component of a solution prepared by dissolving 2.05 g of nicotine, C10H14N2, in 88.0 g of CH2Cl2 XC10H14N2 , XCH2Cl2 = ,
The density of a 16.0 mass % solution of sulfuric acid in water is 1.1094 g/mL at 25.0 ∘C. What is the molarity of the solution?
148.18 M
2.12 M
1.81M
167.4 M
A 0.944 M solution of glucose, C6H12O6, in water, has a density of 1.0624 g/mL at 20∘C. What is the concentration of this solution in the following units? What is the mole fraction? What is the mass percent? What is the molality?
Mole Fraction = 1.87×10−2
Mole Fraction = 1.10×10−4
Mass Percent = 37.0 mass %
Mass Percent = 16.0 mass %
Molality = 1.06 m
Molality = 3.04 m
Which of the following conditions will increase the solubility of a gas?
Low temperature and low pressure
Low temperature and high pressure
High temperature and low pressure
High temperature and high pressure
Henry's law constant is 3.2×10−2mol/(L⋅atm). Find the concentration of CO2 in: A can of soda under a CO2 pressure of 2.1 atm at 25 ∘C
6.7×10−2 M
7.7×10−2 M
5.7×10−2 M
8.7×10−2 M
Henry's law constant is 3.2×10−2mol/(L⋅atm). Find the concentration of CO2 in: A can of soda open to the atmosphere at 25 ∘C (CO2 is approximately 0.04% by volume in the atmosphere.) Express your answer to two significant figures and include the appropriate units. The answer is = M
Colligative properties are properties that changed when a solute is added. It depends on the number of solute particles not on what the solute is.
