Pka and solubility

[accarter15]

The pKa of p-nitrophenol is 7.15. Would you expect it to dissolve in sodium bicarbonate solution? The pKa of 2,5-dinitrophenol is 5.15. Will it dissolve in bicarbonate solution. Pka of bicarbonate solution is 6.34. Any help will be greatly appreciated, thanks.

[Borek]

Pka of bicarbonate solution is 6.34.

That was pH I suppose?

Both substances will dissolve if converted to ions. Use Henderson-Hasselbalch equation (http://www.chembuddy.com/?left=pH-calculation&right=pH-buffers-henderson-hasselbalch) to calculate how much of the substance will be in the ionic form.

Best,
Borek
--
Chemical calculator (http://www.chembuddy.com/?left=chemical_calculators)s at www.chembuddy.com (http://www.chembuddy.com)
pH calculator (http://www.chembuddy.com/?left=BATE&right=right=basic_acid_titration_equilibria)
concentration conversion (http://www.chembuddy.com/?left=CASC&right=concentration_conversion)

[GCT]

at equal concentrations of p-nitrophenol and its conjugate base, the solution will be basic, since pKa=pH at equal concentrations. This means that the molecule has basic characteristics (the alcohol motif), assuming that p-nitrophenol is insoluble in pure water, than in an acidic solution of bicarbonate.......think about the common ion effect. You should apply the same reasoning with your other compound.

[GCT]

ok, I went off on a tangent there, you simply need to compare the pKas, in a mixture of bicarbonate and either of the two compounds, which would be the weaker acid, thus the stronger base?

For instance, p-nitrophenol has a higher pKa, thus would it be more acidic than bicarbonate? If not, than bicarbonate would dissolve the compound in an aqueous solution.