Titration calculation 2 - calculating volume

Summary

In this educational video, Chris Harris from Adobe teachers.com guides viewers through a titration calculation involving a solid sample, calcium carbonate, and sulfuric acid. He meticulously explains the process of determining the volume of acid required for neutralization. Key steps include calculating moles of calcium carbonate from its mass and molecular weight, using the molar ratio to find moles of sulfuric acid, and then calculating the volume of acid needed. The video also touches on unit conversion from decimeters cubed to centimeters cubed, emphasizing the importance of understanding mole equations and molar ratios in chemistry.

Takeaways

• 🔍 Chris Harris introduces a video on titration calculations, focusing on a specific example involving a solid sample.
• 🧪 The example involves titrating solid calcium carbonate with sulfuric acid to determine the volume of acid required.
• 📚 A previous video, 'Titration Calculation One', covers calculating the concentration of a known volume of solution.
• 📉 The reaction between calcium carbonate and sulfuric acid produces calcium sulfate, water, and carbon dioxide.
• 🔬 The practical setup includes a burette with sulfuric acid and a conical flask containing calcium carbonate.
• 🧮 The first step in the calculation is to determine the moles of calcium carbonate from its mass and molecular weight.
• 📐 The molar ratio between calcium carbonate and sulfuric acid is 1:1, simplifying the calculation of moles of sulfuric acid needed.
• 📘 The volume of sulfuric acid is calculated using the formula: volume = moles / concentration.
• 🔄 Conversion from decimeters cubed to centimeters cubed is necessary to match the units requested in the problem.
• 📝 The final calculation results in a volume of 30 centimeters cubed of sulfuric acid needed to neutralize the calcium carbonate.

Q & A

What is the main topic of the video?

The main topic of the video is titration calculation, specifically focusing on calculating the volume of acid required to neutralize a solid amount of calcium carbonate.

Who is the presenter of the video?

The presenter of the video is Chris Harris from Adobe teachers.com.

What is the chemical reaction between calcium carbonate and sulfuric acid?

Calcium carbonate reacts with sulfuric acid to form calcium sulfate, water, and carbon dioxide.

What is the molar mass of calcium carbonate used in the calculation?

The molar mass of calcium carbonate (CaCO3) is 100 grams per mole.

How many moles of calcium carbonate are present in 0.75 grams?

The number of moles of calcium carbonate in 0.75 grams is 7.5 times by 10 to the minus 3 moles.

What is the molar ratio of calcium carbonate to sulfuric acid in this reaction?

The molar ratio of calcium carbonate to sulfuric acid in this reaction is 1:1.

What is the concentration of sulfuric acid used in the titration?

The concentration of sulfuric acid used in the titration is 0.25 moles per decimeter cubed.

How is the volume of sulfuric acid calculated?

The volume of sulfuric acid is calculated by dividing the number of moles by the concentration of the acid.

What is the volume of sulfuric acid needed to neutralize 0.75 grams of calcium carbonate?

The volume of sulfuric acid needed to neutralize 0.75 grams of calcium carbonate is 0.03 decimeters cubed.

How is the volume converted from decimeters cubed to centimeters cubed?

To convert the volume from decimeters cubed to centimeters cubed, multiply by 1000 or shift the decimal point three places to the right.

What is the final volume of sulfuric acid required in centimeters cubed?

The final volume of sulfuric acid required to neutralize the calcium carbonate is 30 centimeters cubed.

What is the importance of knowing mole equations in titration calculations?

Knowing mole equations is crucial in titration calculations as it allows you to determine the number of moles of reactants and products, which is essential for calculating volumes and concentrations.