Van't Hoff Equation for Elevation in Boiling Point of Electrolyte Calculator

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Elevation in Boiling Point

Clausius-Clapeyron Equation

Depression in Freezing Point

Gibb's Phase Rule

Immiscible Liquids

Important Formulas of Clausius-Clapeyron Equation

Important Formulas of Colligative Properties

Osmotic Pressure

Relative Lowering of Vapour Pressure

Van't Hoff Factor

✖A Van't Hoff Factor is the ratio of observed colligative property to theoretical colligative property.ⓘ Van't Hoff Factor [i]			+10% -10%
✖The Ebullioscopic Constant of Solvent relates molality to boiling point elevation.ⓘ Ebullioscopic Constant of Solvent [k_b]			+10% -10%
✖Molality is defined as the total number of moles of solute per kilograms of solvent present in the solution.ⓘ Molality [m]			+10% -10%

✖Boiling point elevation refers to the increase in the boiling point of a solvent upon the addition of a solute.ⓘ Van't Hoff Equation for Elevation in Boiling Point of Electrolyte [ΔT_b]

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Formula

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Van't Hoff Equation for Elevation in Boiling Point of Electrolyte

Formula

`"ΔT"_{"b"} = "i"*"k"_{"b"}*"m"`

Example

`"0.923812K"="1.008"*"0.512K*kg/mol"*"1.79mol/kg"`

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Van't Hoff Equation for Elevation in Boiling Point of Electrolyte Solution

STEP 0: Pre-Calculation Summary

Formula Used

Boiling Point Elevation = Van't Hoff Factor*Ebullioscopic Constant of Solvent*Molality
ΔT_b = i*k_b*m
This formula uses 4 Variables

Variables Used

Boiling Point Elevation - (Measured in Kelvin) - Boiling point elevation refers to the increase in the boiling point of a solvent upon the addition of a solute.
Van't Hoff Factor - A Van't Hoff Factor is the ratio of observed colligative property to theoretical colligative property.
Ebullioscopic Constant of Solvent - (Measured in Kelvin Kilogram per Mole) - The Ebullioscopic Constant of Solvent relates molality to boiling point elevation.
Molality - (Measured in Mole per Kilogram) - Molality is defined as the total number of moles of solute per kilograms of solvent present in the solution.

STEP 1: Convert Input(s) to Base Unit

Van't Hoff Factor: 1.008 --> No Conversion Required
Ebullioscopic Constant of Solvent: 0.512 Kelvin Kilogram per Mole --> 0.512 Kelvin Kilogram per Mole No Conversion Required
Molality: 1.79 Mole per Kilogram --> 1.79 Mole per Kilogram No Conversion Required

STEP 2: Evaluate Formula

Substituting Input Values in Formula

ΔT_b = i*k_b*m --> 1.008*0.512*1.79

Evaluating ... ...

ΔT_b = 0.92381184

STEP 3: Convert Result to Output's Unit

0.92381184 Kelvin --> No Conversion Required

FINAL ANSWER

0.92381184 ≈ 0.923812 Kelvin <-- Boiling Point Elevation

(Calculation completed in 00.004 seconds)

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< 24 Elevation in Boiling Point Calculators

Elevation in Boiling Point given Vapour Pressure

Go Boiling Point Elevation = ((Vapour Pressure of Pure Solvent-Vapour Pressure of Solvent in Solution)*[R]*(Solvent Boiling Point^2))/(Molar Enthalpy of Vaporization*Vapour Pressure of Pure Solvent)

Elevation in Boiling Point given Depression in Freezing Point

Go Boiling Point Elevation = (Molar Enthalpy of Fusion*Depression in Freezing Point*(Solvent Boiling Point^2))/(Molar Enthalpy of Vaporization*(Solvent Freezing Point^2))

Relative Lowering of Vapour Pressure given Elevation in Boiling Point

Go Relative Lowering of Vapour Pressure = (Molar Enthalpy of Vaporization*Boiling Point Elevation)/([R]*Solvent Boiling Point*Solvent Boiling Point)

Ebullioscopic Constant using Molar Enthalpy of Vaporization

Go Ebullioscopic Constant of Solvent = ([R]*Solvent Boiling Point*Solvent Boiling Point*Molar Mass of Solvent)/(1000*Molar Enthalpy of Vaporization)

Boiling point of Solvent given Ebullioscopic Constant and Molar Enthalpy of Vaporization

Go Solvent Boiling Point = sqrt((Ebullioscopic Constant of Solvent*1000*Molar Enthalpy of Vaporization)/([R]*Molar Mass of Solvent))

Elevation in Boiling Point given Osmotic Pressure

Go Boiling Point Elevation = (Osmotic Pressure*Molar Volume*(Solvent Boiling Point^2))/(Temperature*Molar Enthalpy of Vaporization)

Osmotic Pressure given Elevation in Boiling Point

Go Osmotic Pressure = (Molar Enthalpy of Vaporization*Boiling Point Elevation*Temperature)/((Solvent Boiling Point^2)*Molar Volume)

Solvent Boiling Point in Boiling Point Elevation

Go Solvent Boiling Point = sqrt((Molal Boiling Point Elevation Constant*Molal Heat of Vaporization*1000)/([R]*Molecular Weight))

Molar Enthalpy of Vaporization given Boiling Point of Solvent

Go Molar Enthalpy of Vaporization = ([R]*(Solvent Boiling Point^2)*Molar Mass of Solvent)/(1000*Ebullioscopic Constant of Solvent)

Molar Mass of Solvent given Ebullioscopic Constant

Go Molar Mass of Solvent = (1000*Ebullioscopic Constant of Solvent*Molar Enthalpy of Vaporization)/([R]*(Solvent Boiling Point^2))

Elevation in Boiling Point given Relative Lowering of Vapour Pressure

Go Boiling Point Elevation = (Relative Lowering of Vapour Pressure*[R]*(Solvent Boiling Point^2))/Molar Enthalpy of Vaporization

Solvent Molecular Weight in Boiling Point Elevation

Go Molecular Weight = (Molal Boiling Point Elevation Constant*Molal Heat of Vaporization*1000)/([R]*(Solvent Boiling Point^2))

Latent Heat of Vaporization given Boiling point of solvent

Go Latent Heat of Vaporization = ([R]*Solvent Boiling Point*Solvent Boiling Point)/(1000*Ebullioscopic Constant of Solvent)

Boiling point of Solvent given Ebullioscopic Constant and Latent Heat of Vaporization

Go Solvent Boiling Point = sqrt((Ebullioscopic Constant of Solvent*1000*Latent Heat of Vaporization)/[R])

Ebullioscopic Constant using Latent Heat of Vaporization

Go Ebullioscopic Constant of Solvent = ([R]*Solvent BP given Latent Heat of Vaporization^2)/(1000*Latent Heat of Vaporization)

Molal Boiling Point Elevation Constant given Ideal Gas Constant

Go Molal Boiling Point Elevation Constant = (Universal Gas Constant*(Boiling Point of Solvent)^2*Molecular Weight)/(1000)

Van't Hoff Factor of Electrolyte given Elevation in Boiling Point

Go Van't Hoff Factor = Boiling Point Elevation/(Ebullioscopic Constant of Solvent*Molality)

Ebullioscopic Constant given Elevation in Boiling Point

Go Ebullioscopic Constant of Solvent = Boiling Point Elevation/(Van't Hoff Factor*Molality)

Molality given Elevation in Boiling Point

Go Molality = Boiling Point Elevation/(Van't Hoff Factor*Ebullioscopic Constant of Solvent)

Van't Hoff Equation for Elevation in Boiling Point of Electrolyte

Go Boiling Point Elevation = Van't Hoff Factor*Ebullioscopic Constant of Solvent*Molality

Molal Boiling Point Elevation Constant given Boiling Point Elevation

Go Molal Boiling Point Elevation Constant = Boiling Point Elevation/Molality

Molality given Boiling Point Elevation and Constant

Go Molality = Boiling Point Elevation/Molal Boiling Point Elevation Constant

Boiling Point Elevation

Go Boiling Point Elevation = Molal Boiling Point Elevation Constant*Molality

Elevation in Boiling Point of Solvent

Go Boiling Point Elevation = Ebullioscopic Constant of Solvent*Molality

< 22 Important Formulas of Colligative Properties Calculators

Van't Hoff Osmotic Pressure for Mixture of Two Solutions

Go Osmotic Pressure = ((Van't Hoff Factor of Particle 1*Concentration of Particle 1)+(Van't Hoff Factor of Particle 2*Concentration of Particle 2))*[R]*Temperature

Osmotic Pressure given Vapour Pressure

Go Osmotic Pressure = ((Vapour Pressure of Pure Solvent-Vapour Pressure of Solvent in Solution)*[R]*Temperature)/(Molar Volume*Vapour Pressure of Pure Solvent)

Osmotic Pressure given Depression in Freezing Point

Go Osmotic Pressure = (Molar Enthalpy of Fusion*Depression in Freezing Point*Temperature)/(Molar Volume*(Solvent Freezing Point^2))

Relative Lowering of Vapour Pressure

Go Relative Lowering of Vapour Pressure = (Vapour Pressure of Pure Solvent-Vapour Pressure of Solvent in Solution)/Vapour Pressure of Pure Solvent

Van't Hoff Osmotic Pressure for Electrolyte

Go Osmotic Pressure = Van't Hoff Factor*Molar Concentration of Solute*Universal Gas Constant*Temperature

Ebullioscopic Constant using Latent Heat of Vaporization

Go Ebullioscopic Constant of Solvent = ([R]*Solvent BP given Latent Heat of Vaporization^2)/(1000*Latent Heat of Vaporization)

Osmotic Pressure given Concentration of Two Substances

Go Osmotic Pressure = (Concentration of Particle 1+Concentration of Particle 2)*[R]*Temperature

Ostwald-Walker Dynamic Method for Relative Lowering of Vapour Pressure

Go Relative Lowering of Vapour Pressure = Loss of Mass in Bulb Set B/(Loss of Mass in bulb set A+Loss of Mass in Bulb Set B)

Relative Lowering of Vapour Pressure given Number of Moles for Concentrated Solution

Go Relative Lowering of Vapour Pressure = Number of Moles of Solute/(Number of Moles of Solute+Number of Moles of Solvent)

Osmotic Pressure given Relative Lowering of Vapour Pressure

Go Osmotic Pressure = (Relative Lowering of Vapour Pressure*[R]*Temperature)/Molar Volume

Cryoscopic Constant given Latent Heat of Fusion

Go Cryoscopic Constant = ([R]*Solvent Freezing Point for Cryoscopic Constant^2)/(1000*Latent Heat of Fusion)

Van't Hoff Relative Lowering of Vapour Pressure given Molecular Mass and Molality

Go Colligative Pressure given Van't Hoff factor = (Van't Hoff Factor*Molality*Molecular Mass Solvent)/1000

Ebullioscopic Constant given Elevation in Boiling Point

Go Ebullioscopic Constant of Solvent = Boiling Point Elevation/(Van't Hoff Factor*Molality)

Van't Hoff Equation for Elevation in Boiling Point of Electrolyte

Go Boiling Point Elevation = Van't Hoff Factor*Ebullioscopic Constant of Solvent*Molality

Cryoscopic Constant given Depression in Freezing Point

Go Cryoscopic Constant = Depression in Freezing Point/(Van't Hoff Factor*Molality)

Van't Hoff equation for Depression in Freezing Point of electrolyte

Go Depression in Freezing Point = Van't Hoff Factor*Cryoscopic Constant*Molality

Total Concentration of Particles using Osmotic Pressure

Go Molar Concentration of Solute = Osmotic Pressure/([R]*Temperature)

Osmotic Pressure for Non Electrolyte

Go Osmotic Pressure = Molar Concentration of Solute*[R]*Temperature

Osmotic Pressure given Density of Solution

Go Osmotic Pressure = Density of Solution*[g]*Equilibrium Height

Relative Lowering of Vapour Pressure given Number of Moles for Dilute Solution

Go Relative Lowering of Vapour Pressure = Number of Moles of Solute/Number of Moles of Solvent

Boiling Point Elevation

Go Boiling Point Elevation = Molal Boiling Point Elevation Constant*Molality

Freezing Point Depression

Go Depression in Freezing Point = Cryoscopic Constant*Molality

Van't Hoff Equation for Elevation in Boiling Point of Electrolyte Formula

Boiling Point Elevation = Van't Hoff Factor*Ebullioscopic Constant of Solvent*Molality
ΔT_b = i*k_b*m

What is Ebullioscopic constant?

Molal elevation constant or ebullioscopic constant is defined as the elevation in boiling point when one mole of non-volatile solute is added to one kilogram of solvent. Ebullioscopic constant is the constant that expresses the amount by which the boiling point of a solvent is raised by a non-dissociating solute. Its units are K Kg mol-1.

How to Calculate Van't Hoff Equation for Elevation in Boiling Point of Electrolyte?

Van't Hoff Equation for Elevation in Boiling Point of Electrolyte calculator uses Boiling Point Elevation = Van't Hoff Factor*Ebullioscopic Constant of Solvent*Molality to calculate the Boiling Point Elevation, The Van't Hoff Equation for Elevation in Boiling Point of Electrolyte describes the phenomenon that the boiling point of a liquid (a solvent) will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent. Boiling Point Elevation is denoted by ΔT_b symbol.

How to calculate Van't Hoff Equation for Elevation in Boiling Point of Electrolyte using this online calculator? To use this online calculator for Van't Hoff Equation for Elevation in Boiling Point of Electrolyte, enter Van't Hoff Factor (i), Ebullioscopic Constant of Solvent (k_b) & Molality (m) and hit the calculate button. Here is how the Van't Hoff Equation for Elevation in Boiling Point of Electrolyte calculation can be explained with given input values -> 2.74944 = 1.008*0.512*1.79.

FAQ

What is Van't Hoff Equation for Elevation in Boiling Point of Electrolyte?

The Van't Hoff Equation for Elevation in Boiling Point of Electrolyte describes the phenomenon that the boiling point of a liquid (a solvent) will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent and is represented as ΔT_b = i*k_b*m or Boiling Point Elevation = Van't Hoff Factor*Ebullioscopic Constant of Solvent*Molality. A Van't Hoff Factor is the ratio of observed colligative property to theoretical colligative property, The Ebullioscopic Constant of Solvent relates molality to boiling point elevation & Molality is defined as the total number of moles of solute per kilograms of solvent present in the solution.

How to calculate Van't Hoff Equation for Elevation in Boiling Point of Electrolyte?

The Van't Hoff Equation for Elevation in Boiling Point of Electrolyte describes the phenomenon that the boiling point of a liquid (a solvent) will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent is calculated using Boiling Point Elevation = Van't Hoff Factor*Ebullioscopic Constant of Solvent*Molality. To calculate Van't Hoff Equation for Elevation in Boiling Point of Electrolyte, you need Van't Hoff Factor (i), Ebullioscopic Constant of Solvent (k_b) & Molality (m). With our tool, you need to enter the respective value for Van't Hoff Factor, Ebullioscopic Constant of Solvent & Molality and hit the calculate button. You can also select the units (if any) for Input(s) and the Output as well.

How many ways are there to calculate Boiling Point Elevation?

In this formula, Boiling Point Elevation uses Van't Hoff Factor, Ebullioscopic Constant of Solvent & Molality. We can use 7 other way(s) to calculate the same, which is/are as follows -

Boiling Point Elevation = Ebullioscopic Constant of Solvent*Molality
Boiling Point Elevation = ((Vapour Pressure of Pure Solvent-Vapour Pressure of Solvent in Solution)*[R]*(Solvent Boiling Point^2))/(Molar Enthalpy of Vaporization*Vapour Pressure of Pure Solvent)
Boiling Point Elevation = (Molar Enthalpy of Fusion*Depression in Freezing Point*(Solvent Boiling Point^2))/(Molar Enthalpy of Vaporization*(Solvent Freezing Point^2))
Boiling Point Elevation = (Osmotic Pressure*Molar Volume*(Solvent Boiling Point^2))/(Temperature*Molar Enthalpy of Vaporization)
Boiling Point Elevation = (Relative Lowering of Vapour Pressure*[R]*(Solvent Boiling Point^2))/Molar Enthalpy of Vaporization
Boiling Point Elevation = Molal Boiling Point Elevation Constant*Molality
Boiling Point Elevation = Molal Boiling Point Elevation Constant*Molality

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