Molarity and Dilutions

If I have 340.0 mL of a 0.500 M NaBr solution, what will the concentration be if I add 560.0 mL more water to it? (Remember to use the total new volume)

• .188 M

• 3.78 M

• .389 M

• 1.76 M

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO₃ to a volume of 250. mL?

• 15.9 M

• 0.636 M

• 0.642 M

• 1.59 M

125.0 mL of 2.00 M calcium hydroxide solution is diluted to a concentration of 1.50 M. How many mL of water was added to the original volume?

• 167 mL

• 42.0 mL

• 93.8 mL

• 0.0240 mL

How do we make a dilution?

• Add more solute

• Remove solute

• Remove solvent

• Add more solvent

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.

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

• M

• mol

• g

• g/L

You can make a solution more concentrated by adding __________.

• solute

• solvent

• water

Tags

NGSS.HS-PS1-5

50 ml of a 1 M solution is diluted until the final volume is 80ml. How much water was added?

• 50 ml

• 1.3 ml

• 30 ml

• 130 ml

Calculate the molarity of the following solution:  1.0 mole of KCl in 750.0 mL of solution.

• 0.750 M

• 99 M

• 1.3 M

• 2.0 M

What is the molarity of 4 g of NaCl (MM=58.45g/mol) in 3,800 mL of solution?

• 0.018 M

• 0.0011 M

• 1.052 M

• 0.062 M