[PDF] Formulas for Colligative Properties





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Formulas for Colligative Properties

The boiling point and freezing point change according to the number of particles that go into the solution. The boiling point elevates and the freezing point 



Class XII Chemistry Ch. 2: Solutions Important formulae & Concepts

?. 13. Normal molar mass i. Abnormal molar mass. Observedcolligative property. Calculatedcolligative property. Totalnumber of moles of particles after 



Solutions and Colligative Properties

Molecular masses of nonvolatile nonelectrolyte solutes from dilute solutions can be determined by using the value of colligative property. From these equations 



SOLUTIONS & COLLIGATIVE PROPERTIES

we will consider mostly liquid solutions and their properties. 1. SOLUTIONS. 1.1 Definition Substituting the value of molality in equation we get.



(968)-chemistry-gyan-sutra-jee-main.pdf

Solution & Colligative Properties Formula : Oxidation Number = number of electrons in the valence shell ... Such sharing forms two dimension sheet.



Solutions

studying the properties of the solutions like vapour pressure and colligative properties. It is obvious from equation (2.11) that higher the value of K.



Solutions

studying the properties of the solutions like vapour pressure and colligative properties. It is obvious from equation (2.11) that higher the value of K.



Solution And Colligative Properties

06-Apr-2020 Determination of molecular mass of solute from osmotic pressure: By van't Hoff solution equation. 2. 2. 2 n. W RT.



?Tb = m × Kb ?Tf = m × Kf

Use the Equations given in your notes to solve the Colligative Property Questions. A solution of 58.5 grams of NaCl in 1000 grams of water is made.



SOLUTIONS AND COLLIGATIVE PROPERTIES

Calculate its molarity. (JEE MAIN). Sol: We are provided with strength of solution and density hence for this numerical following formula can be applied.

Formulas for Colligative Properties

Lowering

of

Vapor Pressure

Elevating

the

BOILING Point

Depression

of the

FREEZING Point

Osmotic

Pressure

Vapor Pressure

P = X Po

P = vapor pressure of the

solvent

X = the mole fraction of the

solvent

Po = vapor pressure of the

pure solvent (a book value, CRC reference) T = i kb m

T = change in temperature

kb = the boiling point elevation constant (a book value, CRC reference tables) for the solvent. For calculating changes in colligative properties the is used. Example: LiCl dissociates into Li+ and Cl- so i = 2 BaCl2 dissociates into Ba+ and 2Cl- so i = 3 This allows the researchers to account for the number of solute particles without being concerned about the type of particle being used. The boiling point and freezing point change according to the number of particles that go into the solution. The boiling point elevates and the freezing point becomes depressed. Note: ions so they are given a factor of 1. Ionic substances will dissociate into ions and so each ion must be counted.

T = i kf m

T = change in temperature

kf = the freezing point depression constant (a book value, CRC reference tables) for the solvent.

Example:

What is the boiling point of a 2 m solution of NaCl in water if the boiling point elevation constant is 0.5o C / m?

Solution:

i = 2 Na+ and CL-

T = i kb m = (2) (0.5o C m) (2m) = 2oC

Note: The boiling point of water is 100o C so ADD the value to obtain the elevated boiling point.

Example:

What is the freezing point of a 2 m solution of NaCl in water if the freezing point elevation constant is -1.858 o C /m?

Solution:

i = 2 Na+ and CL-

T = i kf m = (2) (0.5o Cl m) (2m) = 2oC

Note: The freezing point of water is 0o C so SUBTRACT the value to obtain the elevated boiling point.

Molality Formula

Molality moles of solute

kilograms of solvent = m = moles kg Notes/ J. Haugh Visual Notes/ X Drive/Chemistry/2012

Op = M R T

Op = Osmotic

Pressure atm

M = molarity of

the solution

R = gas constant

T = temperature

in Kelvin (K) Units

Reference Only Reference Only

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