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The of a solution is a measure of the amount of that is dissolved in a given amount of A is one that contains a small amount of solute. A contains large amount of solute. • Molarity: Molarity = - 1. If you had 1 Liter of an aqueous solution containing 0.085 moles of dissolved potassium chloride (KCI), what is the molarity? 2. 12 grams of sodium chloride is added to 0.5 L beaker. What is the molarity of the solution?

The of a solution is a measure of the amount of that is dissolved in a given amount of A is one that contains a small amount of solute. A contains large amount of solute. • Molarity: Molarity = - 1. If you had 1 Liter of an aqueous solution containing 0.085 moles of dissolved potassium chloride (KCI), what is the molarity? 2. 12 grams of sodium chloride is added to 0.5 L beaker. What is the molarity of the solution?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Back molarity ws.pdf Q Name Date Period Molarity CALIFORNIA STATE STANDARD Solutions 6. Solutions are homogeneous mixtures of two or more substances. As a basis for understanding this concept: d. Students know how to calculate the concentration of a solute in terms of grams per liter, molarity, parts per million, and percent composition. Sections 16.2 The of a solution is a measure of the amount of that is dissolved in a given amount of A is one that contains a small amount of solute. contains large amount of solute. Molarity: Molarity = Examples: 1. If you had 1 Liter of an aqueous solution containing 0.085 moles of dissolved potassium chloride (KCI), what is the molarity? 2. 12 grams of sodium chloride is added to 0.5 L beaker. What is the molarity of the solution?
Transcribed Image Text:Back molarity ws.pdf Q Name Date Period Molarity CALIFORNIA STATE STANDARD Solutions 6. Solutions are homogeneous mixtures of two or more substances. As a basis for understanding this concept: d. Students know how to calculate the concentration of a solute in terms of grams per liter, molarity, parts per million, and percent composition. Sections 16.2 The of a solution is a measure of the amount of that is dissolved in a given amount of A is one that contains a small amount of solute. contains large amount of solute. Molarity: Molarity = Examples: 1. If you had 1 Liter of an aqueous solution containing 0.085 moles of dissolved potassium chloride (KCI), what is the molarity? 2. 12 grams of sodium chloride is added to 0.5 L beaker. What is the molarity of the solution?
3. A 100 mL intravenous (IV) solution contains 5.10 grams of glucose (CeH12O6). What is the molarity of this solution? 4. How many moles is needed to make a 0.1 molar solution of HCI in a 2.0 liter solution? 5. What volume is needed to make a 2.0 molar solution with 5.25 grams of KNO3? Dilutions M,V, = M,V, 1. How many millimeters of a solution of 4.00 M KI is needed to prepare 250.0 mL of 0.760 KI? 2. How could you prepare 250 mL of 0.20 M NaCl using only a solution of 1.0 M NaCl solution? Summary
Transcribed Image Text:3. A 100 mL intravenous (IV) solution contains 5.10 grams of glucose (CeH12O6). What is the molarity of this solution? 4. How many moles is needed to make a 0.1 molar solution of HCI in a 2.0 liter solution? 5. What volume is needed to make a 2.0 molar solution with 5.25 grams of KNO3? Dilutions M,V, = M,V, 1. How many millimeters of a solution of 4.00 M KI is needed to prepare 250.0 mL of 0.760 KI? 2. How could you prepare 250 mL of 0.20 M NaCl using only a solution of 1.0 M NaCl solution? Summary
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