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What is the concentration of 10.00 mLof HBr if it takes 5 mL of a 0.253 M LiOH solution to neutralize it?

1 Answer

Dec 12, 2016

$Concentration$ $"Concentration"$ $≅$ $~=$ $0.1 \cdot m o l \cdot L^{- 1}$ $0.1*mol*L^-1$

Explanation:

AS with all these problems, we need a stoichiometrically balanced equation:

$H B r (a q) + L i O H (a q) \to L i B r (a q) + H_{2} O (l)$ $HBr(aq) + LiOH(aq) rarr LiBr(aq) + H_2O(l)$

So, there is $1:1 molar equivalence$ $"1:1 molar equivalence"$

$[H B r]$ $[HBr]$ $=$ $=$ $(5xx10^-3*cancelLxx0.253*mol*L^-1)/(10.00xx10^-3*cancelL)$ $=??mol*L^-1$

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