<u>Answer:</u> The hydroxide ion concentration and pOH of the solution is
and 2.88 respectively
<u>Explanation:</u>
We are given:
Concentration of barium hydroxide = 0.00066 M
The chemical equation for the dissociation of barium hydroxide follows:
![Ba(OH)_2\rightarrow Ba^{2+}+2OH^-](https://tex.z-dn.net/?f=Ba%28OH%29_2%5Crightarrow%20Ba%5E%7B2%2B%7D%2B2OH%5E-)
1 mole of barium hydroxide produces 1 mole of barium ions and 2 moles of hydroxide ions
pOH is defined as the negative logarithm of hydroxide ion concentration present in the solution
To calculate pOH of the solution, we use the equation:
![pOH=-\log[OH^-]](https://tex.z-dn.net/?f=pOH%3D-%5Clog%5BOH%5E-%5D)
We are given:
![[OH^-]=(2\times 0.00066)=1.32\times 10^{-3}M](https://tex.z-dn.net/?f=%5BOH%5E-%5D%3D%282%5Ctimes%200.00066%29%3D1.32%5Ctimes%2010%5E%7B-3%7DM)
Putting values in above equation, we get:
![pOH=-\log(1.32\times 10^{-3})\\\\pOH=2.88](https://tex.z-dn.net/?f=pOH%3D-%5Clog%281.32%5Ctimes%2010%5E%7B-3%7D%29%5C%5C%5C%5CpOH%3D2.88)
Hence, the hydroxide ion concentration and pOH of the solution is
and 2.88 respectively
Answer:
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