Question

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

m?

Answer 1

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

Step-by-step 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:

`(1)/(2)* 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.

Answer 2

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