What is N(normal) and how is it different from M(molar) in the concentration of a solution?
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Answer:
Molarity (M) is moles solute divided by Liters of solution
Normality (N) is used for acids and bases, I use it to simplify titration calculations. You take the Molarity of the acid/base and multiply it by the number of ionizable hydrogens/hydroxides.
For example, H2SO4 that is 2.0 M would be 4.0 N because it has 2 Hs
Ca(OH)2 that is 3.0 M would be 6.0 N because it has 2 OHs
They are the same when it is a monoprotic acid.
1.2 M HCl = 1.2 N HCl
Molarity (M) is equal to the number of Moles of solute divided by the total liters of solution.
Normality is calculated using equivalent weights (not molecular weights). In a chemical reaction there is always a clearly defined and predictable ratio in which reactants combine. For example, H+ + OH- --> H2O; 1 equivalent of H+ always reacts exactly with 1 equivalent of OH-. Consider the equation H2SO4 + 2NaOH ---> Na2SO4 + 2 H2O. Here 1 mole of H2SO4 reacts with 2 moles of NaOH. Since H2SO4 contains 2 replaceable H+, we say that its equivalent weight is 1/2 of its molecular weight. For acids and bases the equivalent weight is the molecular weight divided by the number of replaceable H+ or OH- groups. 0.5 M H2SO4 equals 1 N H2SO4 and 1 M NaOH equals 1 N NaOH. 1 liter of 1 N H2SO4 will react completely with 1 liter of 1 N NaOH (a 1:1 relation) whereas if you use molarities 1 liter of 0.5 M H2SO4 requires 1 liter of 1.0 M NaOH to react completely.
Normality is also sometimes used in oxidation/reduction titrations. In this case the equivalent weight is the molecular weight divided by the number of electrons lost by the solute that is oxidized (or gained by the solute that is reduced).
Normality = equivalent weight / liters
equivalent weight = MW / replaceable H+ or OH- ions
equivalent weight = MW / total electrons gained (or lost)
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Answer:
Molarity (M) is moles solute divided by Liters of solution
Normality (N) is used for acids and bases, I use it to simplify titration calculations. You take the Molarity of the acid/base and multiply it by the number of ionizable hydrogens/hydroxides.
For example, H2SO4 that is 2.0 M would be 4.0 N because it has 2 Hs
Ca(OH)2 that is 3.0 M would be 6.0 N because it has 2 OHs
They are the same when it is a monoprotic acid.
1.2 M HCl = 1.2 N HCl
Molarity (M) is equal to the number of Moles of solute divided by the total liters of solution.
Normality is calculated using equivalent weights (not molecular weights). In a chemical reaction there is always a clearly defined and predictable ratio in which reactants combine. For example, H+ + OH- --> H2O; 1 equivalent of H+ always reacts exactly with 1 equivalent of OH-. Consider the equation H2SO4 + 2NaOH ---> Na2SO4 + 2 H2O. Here 1 mole of H2SO4 reacts with 2 moles of NaOH. Since H2SO4 contains 2 replaceable H+, we say that its equivalent weight is 1/2 of its molecular weight. For acids and bases the equivalent weight is the molecular weight divided by the number of replaceable H+ or OH- groups. 0.5 M H2SO4 equals 1 N H2SO4 and 1 M NaOH equals 1 N NaOH. 1 liter of 1 N H2SO4 will react completely with 1 liter of 1 N NaOH (a 1:1 relation) whereas if you use molarities 1 liter of 0.5 M H2SO4 requires 1 liter of 1.0 M NaOH to react completely.
Normality is also sometimes used in oxidation/reduction titrations. In this case the equivalent weight is the molecular weight divided by the number of electrons lost by the solute that is oxidized (or gained by the solute that is reduced).
Normality = equivalent weight / liters
equivalent weight = MW / replaceable H+ or OH- ions
equivalent weight = MW / total electrons gained (or lost)
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