Video About Chemistry English
The Colligative Nature of Solution
Colligative nature of solution is a complementary property
that depends on the amount of solute particles, and not on the type of solute. In
everyday life we encounter many changes in the nature of the solution, whether
caused by the type and concentration of the solute, the amount of solute
particles or their conductivity. Included in the colligative nature of the
solution is the decrease in vapor pressure, boiling point rise, decrease in
freezing point, and osmotic pressure. In order to learn and understand the
nature of a good solution kologative, it is necessary to review the concepts of
solution.
Various ways can be used to express the composition of the
solution such as:
1. Molarity
The definition of molar or polarity denotes the number of
moles of solute in each liter of solution. Therefore the unit of kemolaran (M)
is mole L-1 or Molaritas. For example: 0.4 M solution CuSO4 means that in 1
liter of solution there is 0.4 mol of CuSO4. From the above definition, then
the formula of molarity is:
2. Mol Fraction
The mole fraction expresses the number of concentrations of
a solution which expresses the ratio of the number of moles of a substance
determined by its mole fraction compared to the total mole. Thus there are two
types of mole fractions namely, the mole fraction of the solute and the solvent
fraction. If the solvent mole is nA, then the solute mol is nB, then the
solvent mole fraction (XA) and the solute mole fraction (XB) are:
The following will be discussed further on the nature of
colligative, lets watching my video on YOUTUBE
please give me example problem of decrease in freezing point.
BalasHapusA 0.05 mol solution of a binary electrolyte in 100 grams of water (Kf = 1.86) freezes at a temperature of - 1,55 ºC. Calculate the degree of electrolyte ionization!
Hapusanswer :
∆f = i.kf.m
1,55 = 1,86 x 1000/100 x 0,05 ( 1 + ∝ )
∝ = 2/3
BalasHapusCould you explain about relation of mol fraction and stoichiometry?
In stoichiometry need a consentration, Concentration is a general term for expressing the number of parts of solute and solvent present in the solution. Concentration can be expressed either quantitatively or qualitatively. For qualitative size, the concentration of the solution is expressed as concentrated and dilute. These two terms represent the relative portion of solute and solvent in solution. Concentrated solutions mean relatively large amounts of solutes, while aqueous solutions mean relatively fewer total solutes. Typically, the term concentrated and dilute is used to compare the concentrations of two or more solutions.
HapusIn quantitative measure, the concentration of the solution is expressed in g / mL (same as the unit for density). However, in the stoichiometric calculation the gram unit is replaced by the unit of mole so that the unit of mol / L is obtained. The concentration in mol / L or mmol / mL is known as molarity or molar concentration.
Below are various ways to express the concentration of the solution, The mole fraction is the ratio between the number of moles of a component and the number of moles of all components present in the solution
What about osmotic pressure of complex compound .. is it using van hoff factor or not?
BalasHapusSince the non-ionizing electrolyte is non-ionized, the value of a non-electrolyte-based compound is 0, hence the van't hoff factor for all non-electrolyte solutions is 1, and since in the formula we multiply by i the non-electrolyte compound of factor i has no effect on the colligative nature solution
HapusOsmosis is the movement of water molecules from a solution wit a lower solute concentration (hypotonic solution) to a solution with high solute concentration (hypertonic solution) through a permeable selective membrane.
BalasHapusCan you give examples of osmotoc pressure in daily life?
The solution inserted into the patient's body through a blood vessel must have the same pressure as the pressure of the blood cells. If the infusion fluid pressure is higher then the infusion fluid will come out of the blood cells. The working principle of this infusion is essentially osmotic pressure. The pressure here is the pressure that must be applied to a solution to prevent the entry of solute molecules through a semipermeable membrane from pure solvent to solution. The pure liquid or aqueous solution will move through the membrane or obstacle to achieve a more concentrated solution. This is called osmosis. These membranes or obstructions are called semipermiabel membranes
HapusWhy osmotic pressure includes a colligative nature ?
BalasHapusBecause osmotic pressure Does not depend on the type of solute and Osmotic pressure is included in the colligative properties because the magnitude depends only on the amount of solute particles of the volume solvent volume. Osmotic pressure does not depend on the type of solute. The equations written below (known as Van't Hoff equations) are suitable for calculating the osmotic pressure of aqueous solutions. Pressure denoted by π, R is a gas constant (0.0821 L atm / mol K) and T in Kelvin temperature. The sign n says the mol of solute and V is the volume (in liters) of the solution, so the n / V ratio is the solution molalitas (M)
HapusWhat is the formula if the numbers in the calculations are in liter?
BalasHapus