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: Describe how you would prepare 2.00 L of 0.100 M K2CrO4 from solid K2CrO4.

Solution: Describe how you would prepare 2.00 L of 0.100 M K2CrO4 from solid K2CrO4.

Problem

Describe how you would prepare 2.00 L of 0.100 M K2CrO4 from solid K2CrO4.

Solution

Recall that molarity is the ratio of the moles of solute and volume of solution in liters.

Solutions are usually prepared in volumetric flasks, which is calibrated at a certain volume.

First, we need to determine the mass of K2CrO4 needed to be dissolved. The molar mass of K2CrO4 is 2(39.10 g/mol K) + 52.00 g/mol Cr + 4(16.00 g/mol O) = 194.20 g/mol.

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