Several brands of antacids use Al1OH23 to react with stomach acid, which contains primarily HCl: Al(OH)₃(s) + HCl(aq) → AlCl₃(aq) + H₂O(l) (b) Calculate the number of grams of HCl that can react with 0.500 g of Al(OH)₃. (c) Calculate the number of grams of AlCl₃ and the number of grams of H₂O formed when 0.500 g of Al(OH)₃ reacts.

Verified step by step guidance

1. Identify the balanced chemical equation for the reaction: \[ \text{Al(OH)}_3 (s) + 3\text{HCl} (aq) \rightarrow \text{AlCl}_3 (aq) + 3\text{H}_2\text{O} (l) \]
2. Determine the molar mass of \( \text{Al(OH)}_3 \) by adding the atomic masses of Al, O, and H.
3. Calculate the number of moles of \( \text{Al(OH)}_3 \) in 0.500 g using the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).
4. Use the stoichiometry of the balanced equation to find the moles of \( \text{HCl} \) that react with the moles of \( \text{Al(OH)}_3 \). According to the equation, 1 mole of \( \text{Al(OH)}_3 \) reacts with 3 moles of \( \text{HCl} \).
5. Calculate the mass of \( \text{HCl} \) using its molar mass and the moles of \( \text{HCl} \) determined in the previous step.

Key Concepts

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the proportions of substances involved in a reaction, which is essential for converting between grams and moles. In this case, stoichiometry will help us find out how much HCl can react with a given mass of Al(OH)3.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles. To solve the problem, we need to calculate the molar mass of Al(OH)3 to determine how many moles correspond to 0.500 g.

Limiting Reactant

The limiting reactant is the substance that is completely consumed in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is important in stoichiometric calculations, as it affects how much HCl can react with the available Al(OH)3. In this scenario, understanding which reactant limits the reaction will be key to finding the grams of HCl that can react.