How to calculate Normality of a barium hydroxide solution?

Question

What is the normality of a barium hydroxide solution if 33.6 mL require 71.2 mL of 4.72 M hydrochloric acid solution?

Answer 1

N1V1=N2V2

let us take as N1= Normality of barium hydroxide
V1= Volume of barium hydroxide
N2= Normality of HCl
V2= Volume of HCl
HCl is a mono basic acid therefore its molarity= normality
Now substitute the values in the formula
N1V1=N2V2
N1X33.6=4.72X71.2
N1= 4.72 X 71.2/33.6
THATS IT.

Answer 2

1) The reaction first:

Ba(OH)2 + 2HCl ------> BaCl2 + H2O

We can use the simple formula:

C2 = C1*V1/V2=(71.2 mL)(4.72M) / 33.6 mL = 10.01 M

but due to the availability of two OH(-) in Barium Hydroxide, we have to divide the molarity by two in order to get the normality (N):

N (Ba(OH)2) = 10.01 / 2 = 5.005 N

Good luck!

Answer 3

i think that if you calculate the moles of barium hydroxid that you have, then calculate the molarity of the Ba(OH)2 solution, and multiply by two, you get the normality. The multiplication step is because there are two hydroxides for each molecule of Ba(OH)2.
hope this helps!

Answer 4

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