Aqueous Solutions: Concentration Dilution

The term molar concentration, which describes a solution's concentration, is written as?

• mol/L

• mol

• g

• g/L

You need to make 200 mL of a 0.20 mol/L aqueous solution of sodium chloride. The only available solution is 1.0 mol/L. Determine how to make the needed dilution.

• Add 160 mL to the initial volume

• Add 160 grams to the initial volume

• Evaporate 160 mL from the initial volume

• the experiment cannot be conducted with the materials provided

A dilution is when

• solute is added to the volume of stock solution

• water is added to the volume of stock solution

• solute is removed from the volume of stock solution

• water is removed from the volume of stock solution

Calculate the Molarity in a solution containing 40.0 g of NaCl dissolved in 500.0 ml of H2O.

• 0.08 mol/L

• 12.5 mol/L

• 1.37 mol/L

• 0.74 mol/L

Calculate the grams of NaOH present in 10.0 mL of a 2.0 mol/L NaOH solution.

• 0.8 grams

• 2000 grams

• 0.3 grams

• 5 grams

Molarity is ...

• grams of solute/deciliters of solvent.

• grams of solute/liters of solution.

• moles of solute/liters of solution.

• moles of solute/milliliters of solvent.

Tags

NGSS.HS-PS1-5

A solution is made by dissolving 0.50 mole of NaCl in enough water to give a final volume of 400.0 mL. What is the molar concentration of the solution?

• 0.10 mol/L

• 0.40 mol/L

• 1.25 mol/L

• 2.33 mol/L

Tags

NGSS.HS-PS1-7

The definition of a stock solution is ...

• a highly concentrated solution that is meant to be diluted to some lower concentration.

• moles of solute divided by liters of solvent

• a solution used to make soup and is usually either chicken or beef flavor

• a solution with less dissolved solute than a dilute solution.

A 0.500 mol/L solution of NaOH, which contains 0.750 mole of solute, would have a volume, in milliliters

• 0.667 mL

• 1200 mL

• 1500 mL

• 2100 mL

What volume, in milliliters, of 10.0 mol/L NaOH is needed to prepare 300 mL of 2.00 mol/L NaOH by dilution?

• 0.067 mL

• 60.0 mL

• 100 mL

• 125 mL