Addition of 50.00 mL of 2.238 m H2SO4 1solution density = 1.1243 g>mL2 to 50.00 mL of 2.238 M BaCl2 gives a white precipitate. (b) If you filter the mixture and add more H2SO4 solution to the filtrate, would you obtain more precipitate? Explain.

Verified step by step guidance

1. Identify the chemical reaction: The reaction between H2SO4 and BaCl2 forms BaSO4 as a precipitate and HCl as a byproduct.
2. Write the balanced chemical equation: \( \text{BaCl}_2 (aq) + \text{H}_2\text{SO}_4 (aq) \rightarrow \text{BaSO}_4 (s) + 2\text{HCl} (aq) \).
3. Determine the limiting reactant: Calculate the moles of H2SO4 and BaCl2 using their concentrations and volumes to find which reactant is limiting.
4. Consider the effect of adding more H2SO4: If BaCl2 is the limiting reactant, adding more H2SO4 will not produce more BaSO4 precipitate because there is no additional BaCl2 to react.
5. Conclude based on the limiting reactant: If H2SO4 is in excess, adding more will not change the amount of precipitate formed, as all BaCl2 has already reacted.

Key Concepts

Precipitation Reactions

Precipitation reactions occur when two soluble salts react in solution to form an insoluble product, known as a precipitate. In this case, the reaction between H2SO4 and BaCl2 produces barium sulfate (BaSO4), which is insoluble in water and appears as a white precipitate. Understanding the solubility rules helps predict whether a precipitate will form when two solutions are mixed.

Concentration and Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. In this scenario, both H2SO4 and BaCl2 are provided in molarity, which is crucial for calculating the amounts of reactants and products in the reaction. The concentration of the reactants influences the extent of the reaction and the amount of precipitate formed.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will shift in a direction that counteracts the disturbance. When more H2SO4 is added to the filtrate, the increased concentration of sulfate ions can drive the formation of more barium sulfate precipitate, as the system attempts to re-establish equilibrium by consuming the additional reactant.