 |
| Strength of a Solution |
|
| Strength of a solution is defined as the amount of the solute in gms, present in one litre of the solution. It is expressed as gL-1. |
| |
| Mathematically, |
| |
 |
| |
| Molarity |
| |
| Molarity of a solution is defined as the number of moles of solute dissolved per litre of solution. |
| |
| Mathematically, |
| |
 |
| |
| For e.g., If 'a' is the weight of the solute (in gms) present in VCC volume of the solution. |
| |
| Then, |
| |
 |
| |
| Molarity is expressed by the symbol M. It can also be expressed as, |
| |
 |
| |
| Normality |
| |
| Normality of a solution is defined as the number of gram equivalents (gm.e) of a solute dissolved per litre of the given solution. |
| |
| Mathematically it is, |
| |
 |
| |
| For e.g., If a is the weight of the solute (in gms) present in VCC volume of the solution. Then, |
| |
 |
| |
| Normality is expressed by the symbol N. It can also be expressed as, |
| |
 |
| |
| Relationship between molarity and normality |
| |
| The molarity and normality of a solution is related to each other as follows: |
| |
 |
| |
| Molality |
| |
| Molality of a solution is defined as the number of moles of solute dissolved in 1000g of a solvent. Mathematically, it is expressed as |
| |
 |
| |
| Molality is expressed by the symbol m. |
| |
| Molality does not change with temperature. |
| |
| Formality |
| |
| In case of ionic compounds like KCl, CaCO3 etc. Formality is used in place of molarity. |
| |
| It is the number of gram formula masses of solute dissolved per liter of the solution. It is denoted by the symbol F. Mathematically it is given as, |
| |
 |
| |
| Mole Fraction |
| |
| It is the ratio of number of moles of one component (solute or solvent) to the total number of moles of all the components (solute and solvent) present in the solution. It is denoted by the symbol X. Let us suppose that a solution contains two components A and B and suppose that nA moles of A and nB moles of B are present in the solution then, |
| |
 |
| |
 |
| |
| Adding eq (i) and (ii) we get |
| |
| xA + xB = 1 |
| |
| Parts per million (ppm) |
| |
| When a solute is present in very small amounts, its concentration is expressed in parts per million. It is defined as the amount of the solute present in one million parts of the solution. |
| |
 |
| |
| It may be noted that the concentration units like molarity, mole fraction etc. are preferred as they involve the weight of the solute and solvent, which is independent of temperature. But units like, molarity, Normality etc., involve volume of the solution, hence changes with temperature. |
| |
