What would the concentration of hydroxide anions be in an aqueous solution that has $[H_{3} O^{+}] = 0.325 M$ $["H"_3"O"^(+)] = "0.325 M"$ ? Given: $K_{w} = 10^{- 14}$ $K_w = 10^(-14)$ ${mol}^{2} L^{2}$ $"mol"^2"L"^2$

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What would the concentration of hydroxide anions be in an aqueous solution that has $[H_{3} O^{+}] = 0.325 M$ $["H"_3"O"^(+)] = "0.325 M"$ ? Given: $K_{w} = 10^{- 14}$ $K_w = 10^(-14)$ ${mol}^{2} L^{2}$ $"mol"^2"L"^2$

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Answer 1 · 2016-04-21T11:41:27

$3.08 \times 10^{- 14} mol / l$ $3.08xx10^(-14)" ""mol""/""l"$

Explanation:

At $25^{\circ} C$ $25^@"C"$ the ionic product of water is given by:

$K_{w} = [H_{3} O_{(a q)}^{+}] [O H_{(a q)}^{-}] = 10^{- 14} {mol}^{2} . l^{- 2}$ $K_w=[H_3O_((aq))^(+)][OH_((aq))^(-)]=10^(-14)" ""mol"^(2)."l"^(-2)$

$:.[OH_((aq))^(-)]=K_w/[[H_3O_((aq))^(+)]]$

$[OH_((aq))^(-)]=10^(-14)/0.325=3.08xx10^(-14)" ""mol""/""l"$

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What would the concentration of hydroxide anions be in an aqueous solution that has $[H_{3} O^{+}] = 0.325 M$ $["H"_3"O"^(+)] = "0.325 M"$ ? Given: $K_{w} = 10^{- 14}$ $K_w = 10^(-14)$ ${mol}^{2} L^{2}$ $"mol"^2"L"^2$

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What would the concentration of hydroxide anions be in an aqueous solution that has ["H"_3"O"^(+)] = "0.325 M"[H3O+]=0.325 M["H"_3"O"^(+)] = "0.325 M" ? Given: K_w = 10^(-14)Kw=10−14K_w = 10^(-14) "mol"^2"L"^2mol2L2"mol"^2"L"^2

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What would the concentration of hydroxide anions be in an aqueous solution that has $[H_{3} O^{+}] = 0.325 M$ $["H"_3"O"^(+)] = "0.325 M"$ ? Given: $K_{w} = 10^{- 14}$ $K_w = 10^(-14)$ ${mol}^{2} L^{2}$ $"mol"^2"L"^2$