Dilution

How do chemists describe the "strength" or concentration of a solution?

• molarity

• concentrated

• diluted

• strong

How do chemists calculate molarity?

• grams/mole

• moles/Liter

• ounces/container

What is the molarity of 0.50 moles of NaCl in 0.25 L of solution?

• 1.0 M

• 0.5 M

• 2.0 M

• 1.5 M

Determine the molarity of 2.25 moles of sulfuric acid, H₂SO₄, dissolved in 725 mL of solution.

• 322 M

• 3.10 M

• 0.325 M

• 2.25 M

How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?

• 10.74 mol

• 0.0695 mol

• 1.07 mol

• 62.7 mol

How many moles are needed to make 2.5 L of a 3.8 M solution? 

• 9.5 mol

• 0.66 mol

• 1.5 mol

• 15 mol

Tags

NGSS.HS-PS1-7

If 20.0 mL of a 3.80 M solution is diluted to 50.0 mL, what is the ending molarity?

• 1.52

• 2.67

• 2.95

• 5.62

If 50.0 mL of a 0.78 M solution is diluted to 90.0 mL, what is the ending molarity?

• .14

• .43

• 14.2

• 43.3

Tags

NGSS.HS-PS1-7

If 30.0 mL of a solution that has a 1.82 M is diluted to 1.14 M, what is the VOLUME of my ending solution?

• .07mL

• 19mL

• 47.9mL

• 63.8mL

What is the volume (in liters) of a 0.20 M solution that contains 0.30 moles of Na₂SO₄ dissolved in it?

• 1.5 L

• 0.060 L

• 0.67 L

• 2.3 L