Question

What is the required molarity of a ba(oh)₂ solution to prepare a 1.0 m oh⁻ solution?

Answer 1

  The   molarity   of  a  Ba(OH)2  solution  required to prepare   a1.0 OH-  solution  is  calculated  as  follows


write   the  equation  for  dissociation of  Ba(Oh)2


that  is,

Ba(Oh)2  -----> Ba^2+   +  2Oh-

by  use  of  reacting   ratio  between  Ba(Oh)2  to  Oh  which  is   1:2  the  molarity of  Ba(oh)2  =    1.0/2 =  0.5 M

Answer 2

Answer: The molarity of the solution of barium hydroxide is 0.5 mol/L.

Explanation:

$Ba(OH)_2\rightarrow Ba^{2+}+2OH^-$

Given , concentration of hydroxide ion = $[OH^-]=1.0 M$

1.0 M of hydroxide ion means that 1 mole of hydroxide ion is present in 1 L solution.

According to reaction 1 mole of barium hydroxide gives 2 moles of hydroxide ions.

Then, 1 mole of hydroxide ion  will be given by:

$\frac{1}{2}\times 1 moles=0.5 moles$ of barium hydroxide

Since, there are 1 mole of hydroxide ions present 1 L of water and 0.5 moles of barium hydroxide in 1 L.

So, the molarity of the solution of barium hydroxide is 0.5 mol/L.