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Recap - Ions in the Sample

Part of the Stoichiometry section of Coddy's Chemistry journey. Lesson 32 of 41.

Challenge

After a test run, $200\ \mathrm{mL}$ of solution holds $26.4\ \mathrm{g}$ of dissolved ammonium sulfate, (NH₄)₂SO₄ (132 g/mol):

(NH₄)₂SO₄(s) → 2NH₄⁺(aq) + SO₄²⁻(aq)

A $50\ \mathrm{mL}$ sample is taken. Calculate the number of moles of NH₄⁺ ions, nᵢₒₙ, in the sample.

Try it yourself

Physics diagram: beaker

Solve for $n_{ion}$

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 Dilution Recap - Lab Prep

6Practice Problems

Recap - Fertilizer Plant Recap - Acid for the Plant Recap - Gases for AmmoniaRecap - Ions in the SampleRecap - 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