A solution has [ H + ] = 0.001 M . What sis the value of [ OH − ], 1 0 − 2 M, 1 0 − 3 M, 1 M, 1 0 − 11 M

[ OH − ] = [ H + ] k w = 1 0 − 3 1 0 − 14 = 1 0 − 11 M

A solution has [ H + ] = 0.001 M . What sis the value of [ OH − ]

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A solution has $\left[\mathrm{H}^{+}\right]=0.001 \mathrm{M}$. What sis the value of $\left[\mathrm{OH}^{-}\right]$

ChemistryIonic EquilibriumMHT CETMHT CET 2022 (07 Aug Shift 2)

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2035 Upvotes Verified Answer

The correct answer is: $10^{-11} \mathrm{M}$

$\left[\mathrm{OH}^{-}\right]=\frac{\mathrm{k}_{\mathrm{w}}}{\left[\mathrm{H}^{+}\right]}=\frac{10^{-14}}{10^{-3}}=10^{-11} \mathrm{M}$

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