The (mathrm{pH}) of a (1.00 times 10^{-2} mathrm{M}) solution of cyanic acid ((mathrm{HOCN})) is 2.77 at (25^{circ}
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The \(\mathrm{pH}\) of a \(1.00 \times 10^{-2} \mathrm{M}\) solution of cyanic acid \((\mathrm{HOCN})\) is 2.77 at \(25^{\circ} \mathrm{C}\). Calculate \(K_{\mathrm{a}}\) for \(\mathrm{HOCN}\) from this result.
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This problem involves the calculation of the acid dissociation constant Ka for an acid given its con...View the full answer
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