I have 1ml of 0.1M potassium iodide, what is the mole fraction of iodide ion?
To calculate the mole fraction of iodide ion in the potassium iodide solution, we first need to determine the number of moles of potassium iodide and the number of moles of iodide ion present in the solution.
To find the number of moles of potassium iodide, we use the formula:
moles = concentration (M) x volume (L)
Given:
Concentration of potassium iodide = 0.1 M
Volume of the solution = 1 mL = 1/1000 L (since 1 mL = 1/1000 L)
Therefore, the number of moles of potassium iodide can be calculated as follows:
moles of potassium iodide = 0.1 M x 1/1000 L
= 0.0001 moles
Since potassium iodide dissociates into one potassium ion (K+) and one iodide ion (I-), the number of moles of iodide ion is equal to the number of moles of potassium iodide, which is 0.0001 moles.
Now, to calculate the mole fraction of iodide ion, we use the equation:
mole fraction = moles of iodide ion / total moles of all components
The total moles of all components in this case is also 0.0001 moles (due to the 1:1 ratio of potassium iodide and iodide ion).
Therefore, the mole fraction of iodide ion is:
mole fraction of iodide ion = 0.0001 moles of iodide ion / 0.0001 total moles of all components
= 1
So, the mole fraction of iodide ion in the solution is 1, which means that the entire solution consists of iodide ions.