Final answer:
To calculate the amount of 3.0 M HBr solution required to react completely with 8.10 g of Be(OH)2, we need to use the balanced chemical equation and mole ratios. The balanced equation for the reaction is: Be(OH)2 + 2HBr -> BeBr2 + 2H2O. completely react with 8.10 g of Be(OH)2, you would need 31.42 mL of a 3.0 M HBr solution.
Step-by-step explanation:
To calculate the amount of 3.0 M HBr solution required to react completely with 8.10 g of Be(OH)2, we need to use the balanced chemical equation and mole ratios. The balanced equation for the reaction is: Be(OH)2 + 2HBr -> BeBr2 + 2H2O First, we need to calculate the number of moles of Be(OH)2: Molar mass of Be(OH)2 = 9.01 g/mol (Be) + 2 * (16.00 g/mol (O) + 1.01 g/mol (H)) = 43.03 g/mol Moles of Be(OH)2 = 8.10 g / 43.03 g/mol = 0.1885 mol.
According to the balanced equation, 2 moles of HBr react with 1 mole of Be(OH)2. So, the number of moles of HBr required is: Moles of HBr = 0.1885 mol / 2 = 0.09425 mol Now we can calculate the volume of 3.0 M HBr solution needed: Volume of HBr solution = Moles of HBr / Molarity of HBr = 0.09425 mol / 3.0 mol/L = 0.03142 L = 31.42 mL Therefore, the volume of 3.0 M HBr solution required to react completely with 8.10 g of Be(OH)2 is 31.42 mL.