What is the concentration of [OH^-] in a mixt | vedclass

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(A) The reaction is: $2HCl + Ba(OH)_2 ightarrow BaCl_2 + 2H_2O$. Moles of $HCl = M 	imes V(L) = 0.050 	imes 0.020 = 0.001 \ mol$. Moles of $Ba(OH)

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$0.10$

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(A) The reaction is: $2HCl + Ba(OH)_2 ightarrow BaCl_2 + 2H_2O$. Moles of $HCl = M 	imes V(L) = 0.050 	imes 0.020 = 0.001 \ mol$. Moles of $Ba(OH)_2 = M 	imes V(L) = 0.10 	imes 0.030 = 0.003 \ mol$. Since $1 \ mol$ of $Ba(OH)_2$ reacts with $2 \ mol$ of $HCl$,$0.003 \ mol$ of $Ba(OH)_2$ would require $0.006 \ mol$ of $HCl$. Since we only have $0.001 \ mol$ of $HCl$,$HCl$ is the limiting reagent. Moles of $Ba(OH)_2$ remaining $= 0.003 - (0.001 / 2) = 0.003 - 0.0005 = 0.0025 \ mol$. Total volume $= 20 \ mL + 30 \ mL = 50 \ mL = 0.050 \ L$. Concentration of $Ba(OH)_2 = 0.0025 \ mol / 0.050 \ L = 0.05 \ M$. Since $Ba(OH)_2 ightarrow Ba^{2+} + 2OH^-$,$[OH^-] = 2 	imes [Ba(OH)_2] = 2 	imes 0.05 = 0.10 \ M$.

What is the concentration of $[OH^-]$ in a mixture of $20 \ mL$ of $0.050 \ M \ HCl$ and $30 \ mL$ of $0.10 \ M \ Ba(OH)_2$ (in $M$)?

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