I need help with this question

Which would have a higher boiling point?

a.1.0 M KNO3
b.1.5 M KNO3
c.0.75M KNO3
d.2.0M KNO3

You can calculate each if your wish or take a short cut.

To calculate,
delta T = i*Kb*m
i is the van't Hoff factor and is 2 for all cases in this question. You know Kb is 1.52.

The shortcut is just i*M since Kb is the same for all of them. The higher i*m the higher delta T. I'll be happy to check your answer.

I don't know how to put that into my calculator

C'mon,

delta T = i*Kb*M
i - 2
]Kb = 1.52
M = 1 M

Then delta T = 2*1.52*1 = ?
dT = 3.04 for a.
The others are done the same way.

Go back and look at my response to your question on the 0.08M monoprotic acid. If you will explain what you don't understand perhaps I can help you through it.

is the answer d

Yes, d is the correct answer.

To determine which solution would have a higher boiling point, we need to consider the colligative properties of the solutions, specifically the boiling point elevation.

Boiling point elevation is a property that depends on the concentration of solute particles in a solution. The more solute particles present, the greater the boiling point elevation.

In this case, we are comparing different molarities of the solute KNO3. The molarity of a solution is the amount of solute (in moles) dissolved in a given volume of solvent (in liters).

Let's analyze each option:

a. 1.0 M KNO3: This means there is 1 mole of KNO3 dissolved in 1 liter of solution.
b. 1.5 M KNO3: This means there is 1.5 moles of KNO3 dissolved in 1 liter of solution.
c. 0.75 M KNO3: This means there is 0.75 moles of KNO3 dissolved in 1 liter of solution.
d. 2.0 M KNO3: This means there is 2 moles of KNO3 dissolved in 1 liter of solution.

Since boiling point elevation is directly proportional to the concentration of solute particles, the solution with the highest molarity (d. 2.0 M KNO3) would have the highest boiling point elevation. Therefore, option d. 2.0 M KNO3 would have the highest boiling point.