Question

Choose the best possible answer for Q.No. A, B, and C.

The following is an acid-base reaction between sulfuric acid and aluminum hydroxide. Use the provided molar masses to answer the questions below:

molar

mass

3 H2SO4

+

2 Al(OH)3

⟶

Al2(SO4)3

+

6 H2O

g/mol

98.08



78.00



342.15



18.02

Note: You need to upload the documents for A, B, and C to show your work.



A. How many moles of sulfuric acid would be required to form 65.21g of Water?

moles of H2SO4 = ________
[ Select ]



B. How many grams of Aluminum Sulfate could be formed if 197.0g aluminum hydroxide reacts with sulfuric acid?

mass of Al2(SO4)3 = ________
[ Select ]



C. To determine the concentration of a sulfuric acid sample, a titration is performed with the above reaction. What is the concentration of the sulfuric acid if a 15.00mL sample reached its titration endpoint with 29.26mL of 0.2855M Al(OH)3?

Molarity of H2SO4 = ________
[ Select ]

Answer 1

The student's stoichiometry problems involving an acid-base reaction between sulfuric acid and aluminum hydroxide are solved using molar mass calculations and titration data to find the required moles and mass of reactants and products, as well as the concentration of sulfuric acid.

Step-by-step explanation:

Stoichiometry Calculations for a Chemical Reaction

To solve the stoichiometry problems presented by the student, it is first essential to understand the balanced chemical equation and use the provided molar masses. The reactions can be broken down into a series of steps to find the correct answers for each part.

A. Moles of Sulphuric Acid to Form Water

First, the number of moles of water produced needs to be calculated using its molar mass. Then, using the stoichiometry from the balanced equation, we can find the moles of sulfuric acid required.

B. Mass of Aluminum Sulfate from Aluminum Hydroxide Reaction

Here, we begin by finding the moles of aluminum hydroxide using its molar mass. Then, using the balanced equation, we can calculate the mass of aluminum sulfate that could be formed.

C. Concentration of Sulfuric Acid via Titration

For titration, we use the provided volumes and molarity of Al(OH)3 to find moles of Al(OH)3, which we then convert to moles of sulfuric acid. Finally, we calculate the molarity of H2SO4 using the initial sample volume.