6. Chemical Quantities & Aqueous Reactions

A solution has a molarity of 8.59 M NaCl and a volume of 125 mL. How many moles of NaCl are present in the solution?

What is the molarity of a solution prepared by dissolving 4.2 grams of NaF (molar mass = 42 grams/mol) in 200 mL of water?

What is the molarity of a solution that contains 0.50 mole of NaOH in 0.50 liter of solution?

How many millimoles (mmol) of HBr are present in 17.6 mL of a 0.0200 M HBr solution?

Which of the following preparations would give a glucose solution with a concentration of 0.5 M? Select the correct option.

Which term describes the number of moles of solute dissolved per liter of solution?

What are the concentrations of Al^{3+} and Cl^- ions in a 0.12 M solution of AlCl_3, assuming complete dissociation?

What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?

What is the concentration of nitrate ions in a 1.5 M aqueous solution of aluminum nitrate, Al(NO_3)_3?

Which of the following solutions contains the greatest total ion concentration in 1.0 L of solution?

Four beakers contain aqueous solutions: Beaker A has 0.5 mol NaCl in 1.0 L, Beaker B has 1.0 mol NaCl in 2.0 L, Beaker C has 0.25 mol NaCl in 0.5 L, and Beaker D has 2.0 mol NaCl in 4.0 L. Which beaker contains the solution with the highest concentration?

Which of the following units can be used to express the concentration of a solution in terms of molarity?

What is the concentration of Cl⁻ ions in a 0.1 M solution of calcium chloride (CaCl₂)?

How many liters of solution are required to prepare a 1.66 M solution containing 2.11 moles of KMnO4?

What is the molarity of a 0.30 L solution containing 43 g of H_2SO_4? (Molar mass of H_2SO_4 = 98 g/mol)