The given solution contains 4.0g of mixture of lodine and potassium lodide dissolved per 10 cm. What is the percentage composition of the sample?

To find the percentage composition of the sample, we need to determine the mass of iodine and potassium iodide separately, and then calculate the percentage of each component in the mixture.

Given:

• Mass of mixture = 4.0 g
• Volume of solution = 10 cm^3

First, we need to determine the concentration of the mixture in g/cm^3:

Concentration (g/cm^3) = Mass / Volume Concentration = 4.0 g / 10 cm^3 Concentration = 0.4 g/cm^3

Since the mixture contains both iodine (I2) and potassium iodide (KI), we need to use their molar masses to calculate their respective masses in the mixture:

• Molar mass of iodine (I2) = 2 * atomic mass of iodine = 2 * 126.9 g/mol = 253.8 g/mol
• Molar mass of potassium iodide (KI) = atomic mass of potassium + atomic mass of iodine = 39.1 g/mol + 126.9 g/mol = 166.0 g/mol

Let's denote:

• Mass of iodine in the mixture as ${�}_{{\text{I}}_2}$
• Mass of potassium iodide in the mixture as ${�}_{\text{KI}}$

We can set up the following equations:

1. Total mass of the mixture: ${�}_{\text{total}}={�}_{{\text{I}}_2}+{�}_{\text{KI}}$

2. Concentration of the mixture: $\text{Concentration}=\frac{{�}_{\text{total}}}{\text{Volume}}$

We know the concentration is $0.4{\text{g/cm}}^3$ and $\text{Volume}=10{\text{cm}}^3$, so we can rearrange equation (2) to find ${�}_{\text{total}}$: ${�}_{\text{total}}=\text{Concentration}\times \text{Volume}$

Substituting the known values: ${�}_{\text{total}}=0.4{\text{g/cm}}^3\times 10{\text{cm}}^3=4\text{g}$

Now, let's solve the system of equations:

${�}_{{\text{I}}_2}+{�}_{\text{KI}}=4\text{g}$

We have one equation with two unknowns, which means we cannot solve for the individual masses without further information. If you have additional data or assumptions about the composition of the mixture (such as the ratio of iodine to potassium iodide), please provide it so we can proceed with the calculation.