6. Chemical Quantities & Aqueous Reactions

Which of the following correctly describes how to calculate the molarity (M) of a solution?

A solution has a molality of 0.959 mol/kg for KBr and contains 0.350 kg of solvent. What mass of KBr (in grams) is present in the solution?

A 0.20 M solution contains 6.4 g of SO_2. What is the volume of the solution in liters?

How many sodium ions are present in 30.0 mL of 0.600 M Na2CO3 solution?

What is the molarity of a solution that contains 0.180 moles of KOH in 0.350 L of solution?

Which of the following 1.0 molar (1.0 M) solutions contains the greatest total number of dissolved particles?

What is the concentration of nitrate ions in a 0.125 M Mg(NO3)2 solution?

A solution is prepared by dissolving 0.50 mol of NaCl in enough water to make 2.0 L of solution. What is the molarity of the NaCl solution?

A 0.425 m aqueous solution of methanol (molar mass = 32.04 g/mol) is prepared. What is the concentration of methanol in %w/v (grams of solute per 100 mL of solution), assuming the density of the solution is approximately 1.00 g/mL?

What is the molarity of a solution containing 0.50 moles of NaCl dissolved in 0.30 liters of solution?

How many grams of sodium chloride (NaCl) are required to prepare 500.0 mL of a 0.100 M solution?

What is the molarity of a solution prepared by dissolving 15.0 grams of KNO_3 in 75.0 mL of solution? (Molar mass of KNO_3 = 101.1 g/mol)

To prepare a 0.750 M solution, how many liters of water are required to dissolve 2.5 moles of MgSO_4?

Which of the following correctly describes how to calculate the molarity of a solution?

Which of the following best describes the molarity (M) of a solution?