Molarity
What is the Molarity of a solution if 1.0 mole of KF is dissolved to make 0.10 L of solution?
(1.0 mol / 0.10 L) = 10 M
What is the formula for calculating dilutions?
M1V1 = M2V2
Define a solute.
The substance that is dissolved into a solvent.
What is the formula for calculating the percent concentration of a solution?
% = 100 x mass(volume) of solute / mass(volume) soln.
What is the formula for calculating the Molarity of a solution?
M=mol/L
What is the molarity of a 0.30 liter solution containing 0.50 moles of NaCl?
(0.50 mol / 0.30 L) = 1.7 M
If you take 100 mL of a 16.0 M stock solution of HCl and bring it up to a final volume of 500 mL, what is the Molarity of the working solution?
(100 mL x 16.0 M) / (500 mL) = 3.2 M
Which mixture has tiny particles suspended in a solvent, that do not settle?
colloid
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
(0.62 g / 45.0 g) x 100 = 1.4 %
How many moles of NaCl are present in 600 ml of a 1.55 M NaCl solution?
(1.55 M x 0.600 L) = 0.93 mol
Calculate the molarity of 46.9 grams of FeCl3 dissolved in 120 ml of solution?
(46.9 g / 162.2 g/mol) / 0.120 L = 2.41 M
You have to make 500 mL of a 0.50 M BaCl2 . How much of the 2.0 M stock do you need?
(500 mL x 0.50 M) / (2.0 M) = 125 mL
Milk is an example of a
colloid
What mass of solute is needed to make 100.0 g of a 3.4% solution?
(3.4% /100) x 100.0 g = 3.4 g
How many milliliters of solution are needed to make a 1.66 M solution containing 2.11 moles of KMnO4?
(2.11 mol / 1.66 M) = 1.27 L = 1,270 mL
What is the Molarity of a solution prepared by dissolved 42.31 g of NaCl into 500 mL?
(42.31 g / 58.44 g/mol) / 0.500 L = 1.45 M
You need to make 300 mL of a 0.40 M solution of sodium chloride. The only available solution is 1.0 M. How much of the stock solution do you need?
(300 mL x 0.40 M) / (1.0 M) = 120 mL
Concrete is an example of a
suspension
What is the percent by volume of a solution made by dissolving 20.0 mL of methanol into 180.0 mL of water?
(20.0 mL / (20.0 mL + 180.0 mL)) x 100 = 10.0%
How many grams of H2SO4 are present in 1.63 liters of a 0.954 M solution?
(0.954 M x 1.63 L) x 98.10 g/mol = 152.5 g
If you dissolve 425.2 g of Ca(OH)2 into 2.5 L of water, what is the Molarity?
(425.2 g / 74.10 g/mol) / 2.5L = 2.30 M
What is the molarity of a NaNO3 solution made by diluting 250.0 mL of a 1.60 M solution to a final volume of 400. mL?
(250. mL x 1.60 M) / (400. mL) = 1.00 M
The substance in which the solute is dissolved is called the
solvent
What is the percent by mass of a solution made by dissolving 150. g of KCl in 100. g of water?
(150. g / (150.g + 100. g)) x 100 = 60.0%
How many grams of Ca(OH)2 are needed to produce 500 ml of 1.66 M Ca(OH)2 solution?
(1.66 M x 0.500 L) x 74.10 g/mol = 61.5 g