CHem Lecture 6

CHem Lecture 6 - C) How many grams of NaCl are required to...

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Sheet1 Page 1 Solution composition Expressed as concentraion: HOw much substance in solution? A) % Composition by mass B) Molarity Several other ways of expressing concentration such as molality, mole fraction will be discussed later A) 10% NaCl solution contains 10g of NaCl in 100g NaCl solution Calculate the concentration by mass of the following -10.5g of solid sodium hydroxide dissolved in 80.5g sodium hydroxide solution Solution: 10.5g/ total mass of solution (80.5) x 100% = 13.0% B) 25.0g of KNO3 dissolved in 100.0g water Calculate the concentration by mass of the following Solution: 25.0/125.0 = 20%
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Unformatted text preview: C) How many grams of NaCl are required to make 650.0g of a 15.6% NaCl Solution: 650.0g NaCl x 15.6g NaCl/ 100 NaCl(soln)---Molarity: Molarity = # of Mol / Vol of solution (L) Units: Mol/L or M D) 5.623g sample of NaHCO3 in 250.0mL solution Solution: 5.623g NaHCO3 / Atomic mass of NaHCO3 (84.008g) = 6.693 x 10^-2mol NaHCO3---1. How many mol of Al3+ and Cl- are present in 100.0mL of 0.30M AlCl3 solution? 2. For a .201M NaOH solution, calculate the number of mol of NaOH present in 825mL NaOH solution 3. Calculate the mass of KMnO4 required to make 2.0L of a 0.12M KMNo4 solution....
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This note was uploaded on 05/06/2008 for the course CHEM 151 taught by Professor Campbell during the Spring '08 term at Lansing.

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