IMAT 2015 Q51 [Acidic Solutions]

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1

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

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  1. CO (g) + H_2O (l) → CO_2 (g) + H_2 (g)
    This is not an acidic solution in water.

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

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

  4. 4 NO (g) + 6 H_2O (l) → 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.

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3

Are we not allowed to produce ions like

2NO + 4H2O → 3O2 + 2NH4+

If not, why?

4

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

5

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

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6

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

9

How can SO2 become H2SO4?
That doesn’t match mole calculation.
It should be H2SO3