Various Types of Solutions

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Various Types of Solutions Copyright © Cengage Learning. All rights reserved

Solution Composition Copyright © Cengage Learning. All rights reserved

Molarity Copyright © Cengage Learning. All rights reserved

EXERCISE! You have 1.00 mol of sugar in 125.0 mL of solution. Calculate the concentration in units of molarity. 1.00 mol / (125.0 / 1000) = 8.00 M Copyright © Cengage Learning. All rights reserved

EXERCISE! You have a 10.0 M sugar solution. What volume of this solution do you need to have 2.00 mol of sugar? 2.00 mol / 10.0 M = 0.200 L Copyright © Cengage Learning. All rights reserved

EXERCISE! Consider separate solutions of NaOH and KCl made by dissolving 100.0 g of each solute in 250.0 mL of solution. Calculate the concentration of each solution in units of molarity. [100.0 g NaOH / 39.998 g/mol] / [250.0 / 1000] = 10.0 M NaOH [100.0 g KCl / 74.55 g/mol] / [250.0 / 1000] = 5.37 M KCl Copyright © Cengage Learning. All rights reserved

Mass Percent Copyright © Cengage Learning. All rights reserved

EXERCISE! What is the percent-by-mass concentration of glucose in a solution made my dissolving 5.5 g of glucose in 78.2 g of water? [5.5 g / (5.5 g + 78.2 g)] × 100 = 6.6% Copyright © Cengage Learning. All rights reserved

Mole Fraction Copyright © Cengage Learning. All rights reserved

EXERCISE! A solution of phosphoric acid was made by dissolving 8.00 g of H3PO4 in 100.0 mL of water. Calculate the mole fraction of H3PO4. (Assume water has a density of 1.00 g/mL.) 8.00 g H3PO4 × (1 mol / 97.994 g H3PO4) = 0.0816 mol H3PO4 100.0 mL H2O × (1.00 g H2O / mL) × (1 mol / 18.016 g H2O) = 5.55 mol H2O Mole Fraction (H3PO4) = 0.0816 mol H3PO4 / [0.0816 mol H3PO4 + 5.55 mol H2O] = 0.0145 Copyright © Cengage Learning. All rights reserved

Molality Copyright © Cengage Learning. All rights reserved

EXERCISE! A solution of phosphoric acid was made by dissolving 8.00 g of H3PO4 in 100.0 mL of water. Calculate the molality of the solution. (Assume water has a density of 1.00 g/mL.) 8.00 g H3PO4 × (1 mol / 97.994 g H3PO4) = 0.0816 mol H3PO4 100.0 mL H2O × (1.00 g H2O / mL) × (1 kg / 1000 g) = 0.1000 kg H2O Molality = 0.0816 mol H3PO4 / 0.1000 kg H2O] = 0.816 m Copyright © Cengage Learning. All rights reserved