chem concentration review

To help prevent tooth decay, many communities treat their water supply with a fluoride compound such as CaF2. How many kilograms of CaF2 would be necessary to treat 287 kL of water to a concentration of 1.00 mg/L if CaF2?

.287 kg

What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L solution?

0.0253 M

Dissolved in water to make 100 mL of solution, 1.00 g of NaCl would have a concentration of

0.171 M

How many moles of HCl are present in 0.70 L of a 0.33 M HCl solution?

0.23 mol

What is the number of kilograms of solvent in a 0.70 molal solution containing 5.0 grams of solute? (molar mass of solute = 30 g)

0.24 kg

What is the molarity of a solution that contains 125 g NaCl in 4.00 L solution

0.535 M

What is the molality of a solution containing 8.0 grams of solute in 0.50 kg of solvent? (molar mass of solute = 24 g)

0.67 m

Example of the most concentrated solution

1 mol of C12H22O11 in 1 L of solution

The molality of a solution containing 8.1 moles of solute in 4847 g of solvent is

1.7m

What expresses molality?

10 mol of solute/1 kg of solvent

What is an example of a solution concentration expressed in terms of molarity?

10 mol of solute/1L of solution

What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?

12M

What is the solubility of silver nitrate if only 11.1 g can dissolve in 5.0 g of water at 20 degrees C?

222g/100 g H2O at 20 degrees C

An NaOH solution contains 1.90 mol of NaOH, and its concentration is 0.555 M. What is its volume?

3.42 L

How many grams of Na2SO4 are needed to prepare 750 mL of a 0.375 M solution?

40 g

What is the maximum amount of KCl that can dissolve in 200 g of water? (The solubility of KCl is 34g/100 g H2O at 20 degrees C

68 g

What mass of Na2SO4 is needed to make 2.5 L of 2.0 M solution (Na = 23 g; S = 32 g; O =16 g)

710 g

Which of the following substances is less soluble in hot water than in cold water?

CO2

What expresses concentration?

molality, molarity, and parts per million

The solubility of a solute depends on

the nature of the solute and the temperature of the solvent

In a solution at equilibrium...

the rate of dissolution and the rate of crystallization are equal