NCl₃ + H₂O → NH₃ + HOCl , the resulting solution is acidic, basic or neutral?

When $\ce{NCl3}$ is dissolved in water, $\ce{NH3}$ and $\ce{HOCl}$ is formed.

Can you please explain me whether formed solution is acid or basic or neutral? thank you!

• Try balancing the equation. What do you notice? – Nicolau Saker Neto Jun 14 '14 at 12:28
• You should specify initial concentrations. generally, your question has no simple 'qualitative' answer, as both acid and base produced are weak. However, analytical chemistry textbooks should have an entire section about calculation of pH of similar solutions. – permeakra Jun 14 '14 at 19:15

Here's our initial reaction, $$\ce{NCl3 + 3H2O -> NH3 + 3HOCl}$$ $\ce{NH3}$ is a weak base and $\ce{HOCl}$ is a weak acid, but there is more of the acid, so at this point the solution would be mildly acidic. However $\ce{NH3}$ and $\ce{HOCl}$ are known to react as follows $$\ce{NH3 + HOCl->NH2Cl + H2O}$$ and in aqueous solution the resultant chloramine can decompose as shown in the following equation $$\ce{3 NH2Cl ⟶ N2 + NH4Cl + 2 HCl}$$ Clearly, an acid is generated in this last reaction. So although the initial products are neutral, eventually the solution will be strongly acidic.