Molar Concentration

What is the molarity of a 0.5 L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)? The molar mass of NaOH is 40.00 g = 1 mol.

• 0.8 M

• 1.5 M

• 3.0 M

• 6.0 M

What is the formula to calculate the number of moles of a solute in solution?

• Moles = mass/Molarity

• Moles = milliliters of solution x Molarity

• Moles = Molarity x Liters of Solution

• Moles = Molarity/Liters of Solution

What is the molarity of 4.0 grams of sodium chloride in 3,800 mL of solution? The molar mass of sodium chloride is 58.44 g = 1 mol.

• 0.018 M

• 0.068 M

• 260 M

• 1.1 M

What is the molarity of 122.5 g of AlCl₃ in 1.0 L of solution? The molar mass of AlCl₃ is 133.33 g = 1 mol.

• 1.225 M

• 0.92 M

• 0.1225 M

What is the molarity of 2.5 mol of NaOH in 12.0 L of solution?

• 0.21 M

• 30 M

• 4.8 M

• 20.8 M

You are given 200 mL of a 0.400 M solution of KMnO₄.

If you add water until the total volume is 800 mL, what will be the final concentration of the solution?

• 0.080 M

• 0.10 M

• 0.20 M

• 0.40 M

• 1.6 M

How many moles of solute are in the beaker? (.5 mol/ Liter, beaker 1/2 L full)

• 0.05 moles

• 0.50 moles

• 1.00 moles

• 1.5 moles

• None of these

How many Liters of solution are required to make 3.5 M hydrochloric acid using 1.1 moles?

• 3.2 L

• 0.31 L

• 3.9 L

• 4.6 L

How many grams of AgNO₃ are needed to prepare 0.125M solution in 250. mL of water? (the molar mass of AgNO₃ is 169.87g=1 mole)

• .0313 g

• 31.3 g

• 5.31 g

• 84.9 g

What is the molar concentration of each ion present in 0.75 M K₃PO₄

• 0.75 M K⁺ and 0.75 M PO₄^3-

• 0.75 M K⁺ and 2.3 M PO₄^3-

• 2.3 M K⁺ and 0.75 M PO₄^3-

• 2.3 M K⁺ and 3.0 M PO₄^3-