[ss4adam]

i basically have a final tonight and dont understand how equvelents work. i missed a true/false problem on a test that went like this


normality is always greater than or equal to molarity

since normality is equiv/liter it seems like the answer is TRUE because equivelents is less than or equal to normality


Please help

[M:B]

1 eq/L neutralises 1 eq/L (eq = equivalent)
A 3N solution of Mg²⁺ (3eq/L) will neutralise a 3N solution of OH^-.
The ratio of charge is 2:1 thus 2 OH^- ions neutralised by 1 Mg²⁺ ion.
So the molar concentraions would be [OH^-] = 3M and [Mg²⁺]  = 1.5M per unit volume.
Here the molarity of Mg2+ is 0.5(Normality).
Using this principle, the normality will always be greater than or equal to the molarity value since half a charge does not exist.

Another perspective: In a xM solution of an ion with charge = y, normality = xy.

Eg. 0.15M of Al(OH)₃ = 0.15mol/L. Since charge of Al ion = 3+.Normality = 3(0.15) = 0.45 eq/L = 0.45N