1. Calculate the molarity of a 5.72 m aqueous sucrose (C12H22O11)solution with a density of 1.50 g/mL.
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Calculate the number of moles of solute present in each of the following solutions: (a) 255 mL of 1.50 M HNO3(aq), (b) 50.0 mg of an aqueous solution that is 1.50 m NaCl, (c) 75.0 g of an aqueous solution that is 1.50% sucrose (C12H22O11) by mass.
(a) Starting with solid sucrose, C12H22O11, describe how you would prepare 250 mL of a 0.250 M sucrose solution. (b) Describe how you would prepare 350.0 mL of 0.100 M C12H22O11 starting with 3.00 L of 1.50 M C12H22O11.
11.35 g (about one tablespoon) of table sugar (sucrose, C12H22O11) is dissolved in 242.9 mL of water (density 0.997 g/mL). The final volume is 250.0 mL (about one cup). 1.Calculate the molarity of sucrose in this solution. 2.Calculate the molality of sucrose in this solution. 3.Calculate the mass percent of sucrose in this solution.