IMAT 2015 Q51 [Acidic Solutions]

Which two of the following oxides would NOT give acidic solutions in water?

CO, CO_2, SO_2, NO

A. NO and SO_2
B. NO and CO_2
C. CO and SO_2
D. CO and CO_2
E. CO and NO

1 Like
  1. CO (g) + H_2O (l) ā†’ CO_2 (g) + H_2 (g)
    This is not an acidic solution in water.

  2. CO_2 + H_2O ā†’ H_2CO_3
    This produces carbonic acid and is so obviously an acidic solution in water.

  3. SO_2 (aq) + H_2O (l) ā†’ H_2SO_4 (aq)
    This produces sulphuric acid, which is also an acidic solution in water.

  4. 4 NO (g) + 6 H_2O (l) ā†’ 5 O_2 (g) + 4 NH_3 (aq)
    This is not an acidic solution in water.

Therefore the answer is NO and CO, option E.


Are we not allowed to produce ions like

2NO + 4H2O ā†’ 3O2 + 2NH4+

If not, why?

Iā€™m not sure but in this case i believe if we put an ion version, the equation is not balanced charge vise

another good explanation, or at least that is how I solved it, is that the acidic strength of an oxyacid increases with the increase in the number of oxygen atoms


Can you please tell me how to predict the product of the equation like this and how to know if it acidic or not . Or can you please tell me what to write on the YouTube to get an explanation