Math

QuestionVilken är al [Cu2+]\left[\mathrm{Cu}^{2+}\right], b) [NO3]\left[\mathrm{NO}_{3}^{-}\right]i en lösning med koncentrationen 0,15 mol/dm3Cu(NO3)20,15 \mathrm{~mol} / \mathrm{dm}^{3} \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2} ?

Studdy Solution
From the dissociation equation, we see that one mole of Cu(NO3)2\mathrm{Cu(NO}_3\mathrm{)}_2 produces two moles of NO3\mathrm{NO}_3^{-}.
Therefore, the concentration of NO3\mathrm{NO}_3^{-} is twice the concentration of Cu(NO3)2\mathrm{Cu(NO}_3\mathrm{)}_2:
[NO3]=2×0.15mol/dm3=0.30mol/dm3[\mathrm{NO}_3^{-}] = 2 \times 0.15 \, \mathrm{mol/dm}^3 = 0.30 \, \mathrm{mol/dm}^3
The concentrations are:
a) [Cu2+]=0.15mol/dm3[\mathrm{Cu}^{2+}] = 0.15 \, \mathrm{mol/dm}^3
b) [NO3]=0.30mol/dm3[\mathrm{NO}_3^{-}] = 0.30 \, \mathrm{mol/dm}^3

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