Multiple Choice 1 point Determine the empirical formula:for the compounds with the following percent composition: 80.38% bismuth, 18.46% oxygen, and d 1.16% hydrogen 1.16% BiO_(3)H_(2) BiO_(3)H_(3) BiO_(2)H_(3) Bi_(2)O_(3)H_(3)

To determine the empirical formula, we need to convert the given percentages to moles and then find the simplest whole number ratio.<br /><br />Given:<br />- Bismuth (Bi): 80.38%<br />- Oxygen (O): 18.46%<br />- Hydrogen (H): 1.16%<br /><br />Step 1: Convert the percentages to grams.<br />- Bi: 80.38 g<br />- O: 18.46 g<br />- H: 1.16 g<br /><br />Step 2: Convert the grams to moles using the molar masses of each element.<br />- Bi: 80.38 g / 208.98 g/mol = 0.386 mol<br />- O: 18.46 g / 16.00 g/mol = 1.148 mol<br />- H: 1.16 g / 1.01 g/mol = 1.146 mol<br /><br />Step 3: Find the simplest whole number ratio by dividing each mole value by the smallest mole value.<br />- Bi: 0.386 mol / 0.386 mol = 1<br />- O: 1.148 mol / 0.386 mol = 2.97 ≈ 3<br />- H: 1.146 mol / 0.386 mol = 2.97 ≈ 3<br /><br />Therefore, the empirical formula for the compound is BiO3H3.<br /><br />Answer: BiO3H3