Question

question 3 (1 point) what is the percent mass of water in the hydrated compound you investigated? a) 26.52% b) 20.96% c) 0.21% d) 4.7710%

Explanation:

To determine the percent mass of water in a hydrated compound, we typically use the formula: $\text{Percent mass of water} = \frac{\text{Mass of water lost}}{\text{Mass of hydrated compound}} \times 100\%$. Without the specific investigation data, but based on common hydrated compounds (e.g., some hydrates like copper sulfate pentahydrate or magnesium sulfate heptahydrate), the percent mass of water can vary, but among the options, if we assume a common hydrated compound (e.g., maybe a calcium hydrate or others), but often, for example, in some standard experiments, the percent mass of water can be calculated. However, since this is a multiple-choice question and likely based on a specific experiment (e.g., maybe a lab where the calculation gave around 26.52% for a particular hydrate like $\ce{CuSO4.5H2O}$: molar mass of $\ce{CuSO4.5H2O}$ is $63.55 + 32.07 + 4\times16.00 + 5\times(2\times1.01 + 16.00) = 249.69\space g/mol$, mass of water is $5\times18.02 = 90.10\space g/mol$, so percent water is $\frac{90.10}{249.69}\times100\% \approx 36.1\%$ – wait, maybe another compound. Wait, maybe the experiment in question had data leading to 26.52%. Alternatively, maybe a different hydrate. But among the options, if we consider typical results, option A (26.52%) is a plausible percent mass of water in a hydrated compound.

Answer:

A) 26.52%