Recap - Acid for the Plant

Part of the Stoichiometry section of Coddy's Chemistry journey. Lesson 30 of 41.

Challenge

A fertilizer plant leads ammonia into sulfuric acid solution to make ammonium sulfate:

2NH₃(g) + H₂SO₄(aq) → (NH₄)₂SO₄(aq)

A container of ammonia gas labeled 6.8 g beside a beaker of sulfuric acid solution, 200 mL

Ammonia gas is led into 200 mL of sulfuric acid solution

In one test run, $6.8\ \mathrm{g}$ of ammonia (NH₃, 17 g/mol) reacts completely with all the acid in $200\ \mathrm{mL}$ of solution. Calculate the concentration of the sulfuric acid solution, $c$ .

Try it yourself

Solve for $c$

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 PlantRecap - Acid for the PlantRecap - 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