Ch.3 - Chemical 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: A hydrate of copper (II) chloride has the following formula: CuCl2 • xH2 O. The water in a 3.41-g sample of the hydrate was driven off by heating. The remaining sample had a mass of 2.69 g .Find the n

Solution: A hydrate of copper (II) chloride has the following formula: CuCl2 • xH2 O. The water in a 3.41-g sample of the hydrate was driven off by heating. The remaining sample had a mass of 2.69 g .Find the n

Problem

A hydrate of copper (II) chloride has the following formula: CuCl2 • xH2 O. The water in a 3.41-g sample of the hydrate was driven off by heating. The remaining sample had a mass of 2.69 g .

Find the number of waters of hydration (x) in the hydrate.

Solution

Recall that for hydrates, water molecules can be evaporated by heating. 

We can solve for x = waters of hydration or the # of molecules of H2O in the hydrate by doing these steps:

  1. Determine mass of water removed
  2. Do mass to mole conversion for both H2O and CuCl2. 
  3. Determine x or the # of H2O molecules using the equation:
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