# If #"14 g"# of calcium nitrate is dissolved in #"200 g"# of water, and it experiences a #70%# dissociation, what is the solution's vapor pressure if the solvent began at the normal boiling point of water? Hint: the normal boiling point occurs at 760 torr.

Vapor pressure of the solution relative to the solvent is given by Raoult's law for ideal solutions:

where:

Again, three times the mols of ions result from 100% dissociation, so:

With 70% dissociation, we simply have 70% of the mols, or

This gives us a mol fraction of:

Therefore, the solution vapor pressure is:

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To solve this problem, first, calculate the number of moles of calcium nitrate. Then determine the number of moles of ions produced due to dissociation. Next, find the total number of moles of solute particles. Use the formula for Raoult's law to calculate the vapor pressure of the solution. Finally, apply the given percentage of dissociation to adjust the calculation accordingly. Using Raoult's law:

P_solution = X_solvent * P°_solvent

Where: P_solution = vapor pressure of the solution X_solvent = mole fraction of the solvent P°_solvent = vapor pressure of the pure solvent

Now, calculate the mole fraction of the solvent:

X_solvent = moles of solvent / total moles of solute and solvent

Substitute the values into the equation and solve for the vapor pressure of the solution. Adjust the calculation for the percentage of dissociation.

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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