Concentration

Chemical Reaction And Equation of Class 10

Solution is a homogenous mixture of two or more components. A solution consists of a dissolved substance known as solute and a substance in which the solute is dissolved is known as solvent. The concentration of a solution reflects the relative proportion of solute and solvent present in the solution. The various concentration terms are

1. % w/W (Weight percent or mass percent)

% w/ W = Concentration

10% H2SO4 w/w means 10 grams of pure H2SO4 is present in 100 gram of H2SO4 solution.

2. % w/V (Weight/volume)

concentration

10% w/V H2SO4 solution means 10 gram of pure H2SO4 is present in 100 ml of H2SO4 solution.

3. % v/V (volume/volume)

This concentration term is defined for a solution of liquid into liquid

concentration

42.8% v/V ethanol solution means that 42.8 ml pure ethanol is present in 100 ml of ethanol solution.

4.Molality (m): It is defined as no. of moles of solute present in 1 kilogram of solvent.

concentration

5.Mole Fraction (X): Suppose a solution of A and B contains nA moles of A and nB moles of B then mole fraction of A(XA) = Concentration

Similarly mole fraction of B(XB) = Concentration

It is clear that

XA + XB = 1.

Out of all the concentration terms we will discuss molarity and normality in detail because these two concentration terms are related with two important methods of stoichiometry i.e.

(i) Method of Moles

(ii) Method of Gram equivalents

6.Molarity (M): It is defined as the number of moles of solute dissolved in one litre of solution

M = No. of Moles of solute/Volume of solution in litre

Suppose w gram solute is dissolved in Vml solution and molecular weight of solute
is m.

concentration

So if a substance is in solid form then it’s moles or millimoles can be calculated by using w/m or w/m x 100 and when the same substance is in solution then M x Vl or M x Vml will give the mole or mill moles respectively.

7. Parts per million (ppm) : It is defined as the quantity of the solute in grams present in 106 grams of the solution

Concentration

Atmospheric pollution in cities is also expressed in ppm by volume. It refers to the volume of the pollutant in 106 units of volume. 10 ppm of SO2 in air means 10 mL of SO2 in present in 106 mL of air.

Illustration 5 : Calculate the total number of oxalic acid molecules present in a 100 ml of 0.01 M oxalic acid solution.

Solution : No. of millimoles of solute (oxalic acid) present = M x Vml= 0.01 x 100 = 1.

Since 1 mole of any substance contains 6.023 x 1023 molecules so 1 millimole will contain 6.023 x 1020  molecules.

Illustration 6 : A 2 M aqueous solution of Potash Alum [K2SO4. Al2 (SO4)3 24H2O], an ionic solid is prepared. Calculate moles of SO²4¯ present in 800 ml of solution.

Solution : Moles of solute (Potash Alum) present in 800 ml of solution

= concentration.

Since potash alum is an ionic solid. So it will split into ions in solution.

concentration

it is apparent from balanced equation than 4 moles of SO²4¯are produced from 1 mole of potash alum.

So moles of SO²4¯present = 1.6 x 4 = 6.4.


Concentration

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