## What is the mole fraction of solute?

What is Mole fraction? Mole fraction represents the number of molecules of a particular component in a mixture divided by the total number of moles in the given mixture. It’s a way of expressing the concentration of a solution. Therefore, the sum of mole fraction of all the components is always equal to one.

## What is the mole fraction of the solute in a 1.00 aqueous solution?

It may be noted that a mole fraction is a dimensionless quantity. So the question says 1.00 molal aqueous solution, which means 1.00 moles of the solute is present in 1000 g of the solvent. Hence the answer is 0.017683. This can be rounded off to 0.0177.

## What is the mole fraction of the solute in a 1m?

It refers to the ratio of the number of moles of solute to the mass of the solvent in kilogram. The SI unit of molality is molal (m). Therefore the correct answer is (d) 0.018.

## Do mole fractions add up to 1?

Mole fractions are dimensionless, and the sum of all mole fractions in a given mixture is always equal to 1.

## What is the formula for calculating mole fraction?

The mole fraction formula for a solution with containing one or more solutes is: Mole fraction of each solute = Number of moles of that solute divided by the total number of moles of all solutes and the solvent.

## What is the mole fraction of solvent in 1.5 molal aqueous solution?

Answer: The mole fraction of solvent in 0.1 molal aqueous solution is 0.9982. Explanation: 1 molal aqueous solution means that 1 mol/kg that is 1 mol of solute is present in the 1000 g of the water(here the aqueous means that solvent is water). The mole fraction of solvent in 0.1 molal aqueous solution is 0.9982.

## Which equimolar concentrated solution has highest freezing point?

The freezing point of equimolal aqueous solutions will be highest for : Aniline hydrochloride. Calcium Nitrate. Lanthanium Nitrate.

## Which concentration term depends on temperature?

The volume changes as the temperature is varied. Thus, such concentration terms are temperature dependent. On the other hand, terms like molality and mole fraction do not depend on volume, thus being temperature independent.

## What is the molality of pure water?

Just like there’s a real molar concentration for water by itself ( 55.348 M ), there is a real molality for water by itself ( 55.510 m ).

## What is the molarity of pure water?

Molarity of pure water is 55.55 M at 298 K.

## Is Molality of the dilute solution is doubled the value of molal depression constant will be?

If molality of the dilute solution is doubled, the value of molal depression constant (Kf) will be. Doubled. Halved.

## How do you calculate total pressure?

The total pressure of the gas mixture is the sum of the partial pressure of the component gases: Ptot = ∑Pi = P1 + P2 + P3 … ntot = the total number of moles in the gas mixture, which is the sum of all ni.

## How do you find the mole fraction from weight percent?

For that, all you need is the molar mass of the solute.

- Multiply w/v % by 10 to get grams per liter (e.g. 1% = 10 g/L).
- Divide g/L by the molar mass to get moles per liter.