Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: What is the molarity of a solution that contains 17g of NH 3 in 0.50 L of solution.

Solution: What is the molarity of a solution that contains 17g of NH 3 in 0.50 L of solution.

Problem

What is the molarity of a solution that contains 17g of NH 3 in 0.50 L of solution.

Solution

We’re being asked to calculate the molarity (M) of a solution of NH3. Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters). In other words:



We first need to determine the number of moles of NH3 since this is the only information missing for us to find molarity. Notice that the volume of the solution in liters is already given.


We’re given the mass of NH3, 17 g. We can use the molar mass of NH3 to find the moles. The molar mass of NH3 is:

NH3     1 N × 14 g/mol N = 14 g/mol          

            3 H × 1 g/mol H = g/mol     

  Sum = 17 g/mol

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