Round off your answers in four decimal places. Use whole numbers for the molecular weights. 1. Suppose you had 58.44 g of NaCl and you dissolved it in exactly 2.00 L of water. What would be the molality?

An aqueous solution of K2SO4 (174.27 g/mol) has a freezing point of –12.3°C and density of 1.05 g/mL. a. What is the concentration of the solution in molality? b. What is the concentration of the solution in molarity?

I mix 64.84 milliliters of isopropyl alcohol with water, creating an 71.94 percent-by-volume solution. What volume of solution did I prepare? a. 90.13 milliliters O b. 110.95 milliliters O c. 7.10 milliliters O d. 119.83 milliliters O e. 129.81 milliliters

The circle shown here represents 1.0 L of a solution with a solute concentration of 1 M: Part A Explain what you would add (the amount of solute or volume of solvent) to the solution to obtain a solution represented by each diagram: Match the items in the left column to the appropriate blanks in the sentences on the right. solvent adding 0.33 L more of the original solution to 1 L of that solute less greater adding 0.5 mol solute to each 1 L solution diluting 1 L of the original solution to 1.5 L diluting 1 L of the original solution to 1.3 L diluting 1 L of the original solution to 2 L adding 0.25 mol solute to each 1 L solution Concentration of solution (a) is Solution (a) is obtained by Concentration of solution (b) is Solution (b) is obtained by Concentration of solution (c) is Solution (c) is obtained by than the original, so than the original, so than the original, so a. & Reset Help needs to be added. needs to be added. needs to be added. b. C.