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  • Equal volumes of Hydrochloric acid of PH=2 is mixed with barium hydroxide solution of PH=12. The concentration of barium chloride in mixed solution is p×10−3M (

Equal volumes of Hydrochloric acid of PH=2 is mixed with barium hydroxide solution of PH=12. The concentration of barium chloride in the mixed solution is p×10−3M (in scientific notation). What is the value of 2p?

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We are given equal volumes of HCl with $\text{pH} = 2$ and Ba(OH)2 with $\text{pH} = 12$. From pH, we get $\left[ \text{H}^+ \right] = 10^{-2}  \text{M}$ and $\left[ \text{OH}^- \right] = 10^{-2}  \text{M}$.

Since Ba(OH)2 gives 2 OH- ions per molecule, its concentration is $\left[ \text{Ba(OH)}_2 \right] = \frac{10^{-2}}{2} = 5 \times 10^{-3} , \text{M}$.

Let the volume of each solution be $V$ L. Then:

Moles of H+ = $10^{-2} \times V$

Moles of OH- = $10^{-2} \times V$

Moles of Ba(OH)2 = $5 \times 10^{-3} \times V$

From the reaction: $\text{Ba(OH)}_2 + 2\text{HCl} \rightarrow \text{BaCl}_2 + 2\text{H}_2\text{O}$

Since moles of H+ and OH- are equal, complete neutralization occurs.

Moles of BaCl2 formed = moles of Ba(OH)2 = $5 \times 10^{-3} \times V$

Total volume after mixing = $2V$

So, final concentration of BaCl2 is:

$\left[ \text{BaCl}_2 \right] = \frac{5 \times 10^{-3} \times V}{2V} = 2.5 \times 10^{-3} , \text{M}$

Hence, $p = 2.5 \Rightarrow 2p ={5}$

Posted by

Saniya Khatri

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