Chemistry Chapter 15 and 17 Practice Test

If you have 2.5 moles of glucose in 0.5 L of solution, what is the concentration of the solution?

• 0.5 M

• 1.25 M

• 2.5 M

• 5 M

What is the molarity of a solution containing 45 g of NaCl in 300 mL of solution?

• 0.15 M

• 230 M

• 2.6 M

• 8.8 M

Which unit should be used for solution concentration?

• mol/L

• L/mol

• J/g

• mol²/L•s

How many moles of sodium nitrate are in 0.75 L of a 0.50 M NaNO₃ solution?

• 0.66 mol

• 0.37 mol

• 3.1 mol

• 24 mol

Tags

NGSS.HS-PS1-7

How can you decrease the concentration of a solution?

• You cannot decrease the concentration.

• Add solvent.

• Pour out some of the solution.

• Add solute.

Explain how you would prepare a solution of salt water, NaCl(aq), with a molarity of 2.5 M.

• Add water to 146 grams of salt to make 1.0 L of solution.

• Add water to 59 grams of salt to make 1.0 L of solution

• Add water to 30 grams of salt to make 1.0 L of solution

• Add water to 117 grams of salt to make 1.0 L of solution.

How can milliliters (mL) be converted into liters (L)?

• multiply mL by 100

• divide mL by 100

• multiply mL by 1000

• divide mL by 1000

Use the solubility table to answer the question. Suppose you mix lithium chloride and silver (I) nitrate solutions. What is the precipitate (solid) that forms ? (S: soluble, N: not soluble)

• ClNO₃

• AgCl

• LiAg

• LiNO₃

Use the solubility table to answer the question. Which pair of solutions will produce a clear solution of ions in water when they are mixed? (S: soluble, N: not soluble)

• silver (I) nitrate and lithium phosphate

• sodium sulfate and mercury (I) nitrate

• magnesium sulfate and potassium chloride

• sodium hydroxide and nickel (II) chloride

Which of the following is the correct net ionic equation for the reaction?

K₂CO₃(aq) + Ca(NO₃)₂(aq) → CaCO₃(s) + KNO₃(aq)

• 2K⁺(aq) + CO₃^2-(aq) → K₂CO₃(aq)

• K⁺(aq) + NO₃^-(aq) → KNO₃(aq)

• Ca²⁺(aq) + 2NO₃^-(aq) → Ca(NO₃)₂(aq)

• Ca²⁺(aq) + CO₃^2-(aq) → CaCO₃(s)

Tags

NGSS.HS-PS1-7