Final answer:
The normality of a solution prepared by burning 1 g of calcium and dissolving it in 1 L of water to form calcium hydroxide is approximately 0.0499 N. The provided answer options do not match this calculated value, suggesting an error in the question or answer choices.
Step-by-step explanation:
The question asks to calculate the normality of a calcium oxide solution prepared by burning 1 g of calcium in excess oxygen and dissolving the resulting oxide in water to make a 1 L solution. Calcium reacts with oxygen to form calcium oxide (CaO), which in water forms calcium hydroxide (Ca(OH)2).
Reaction and Calculation
When calcium burns in oxygen, the reaction is: 2Ca + O2 → 2CaO.
Calcium oxide reacts with water to form calcium hydroxide: CaO + H2O → Ca(OH)2.
The molar mass of Ca is approximately 40.08 g/mol, so 1 g of Ca is 1 / 40.08 moles, which gives us roughly 0.02495 moles of Ca. Following the stoichiometry of the reactions, this also equals the moles of CaO and Ca(OH)2.
Normality (N) is defined as the equivalent of solute per liter of solution. For Ca(OH)2, with two hydroxide ions per molecule, the number of equivalents is twice the number of moles. Thus, 0.02495 moles of Ca(OH)2 × 2 equivalents/mole equals approximately 0.0499 equivalents, which for a 1 L solution results in a normality of 0.0499 N.
In this scenario, none of the given answer choices match the calculated normality. The calculation hints at a possible mistake either in the problem statement or in the answer options provided.
Therefore, to give me a 500-word answer request and to mention the correct option in the final answer, a reassessment of the available information and the question is required as the calculated normality does not match any of the given options.