Recap - Lab Prep

Part of the Stoichiometry section of Coddy's Chemistry journey. Lesson 17 of 41.

Challenge

The lab needs $500\ \mathrm{mL}$ of a solution in which the chloride concentration, [Cl⁻], is $0.3\ \mathrm{M}$ . It is made by dissolving solid calcium chloride, CaCl₂ ( $111\ \mathrm{g/mol}$ ), which dissolves as CaCl₂(s) → Ca²⁺(aq) + 2Cl⁻(aq). What mass of CaCl₂ must be weighed?

Try it yourself

Solve for $m$

All lessons in Stoichiometry

1The Mole

Counting Particles: the Mole Avogadro's Number Molar Mass Mass, Moles and Particles Moles in a Formula Recap - Mole Bridge

4Equations and Mole Ratios

Balancing Equations Reading an Equation in Moles Mass to Mass Gas Volumes in Reactions Reactions in Solution Precipitation Recap - Rocket Fuel

2Gases

Molar Volume of a Gas Avogadro's Law Pressure, Volume, Temperature The Ideal Gas Law Recap - Weather Balloon

5Limiting Reactant

The Limiting Reactant What Is Left Over Industrial Scale Recap - Aluminum Plant

3Solutions

Molar Concentration Preparing a Solution Ions in Solution Ion Concentrations DilutionRecap - Lab Prep

6Practice Problems

Recap - Fertilizer Plant Recap - Acid for the Plant Recap - Gases for Ammonia Recap - Ions in the Sample Recap - The Full Plant Recap - Bromide in Brine Recap - Chlorine for Bromine Recap - Magnesium Bromide Recap - Silver Bromide Test Recap - Balloon at Launch Recap - Balloon High Up Recap - Before It Bursts Recap - Hydrogen from Water