Question

Hno3, a strong acid, is added to shift the ag2co3 equilibrium (equation 7.6) to the right. explain why the shift occurs.

b. what would have been observed if hcl (also a strong acid) had been added instead of the hno3?

Answer 1

Answer 1) When a strong acid like
`HNO_(3)` reacts with
`Ag_(2) CO_(3)` usually the equilibrium shifts to the right because

As per the Le chatelier's principle "if in any reaction, a dynamic equilibrium is disturbed by changing the any of the conditions, the position of equilibrium moves to counteract the change." So, in the given reaction when
`HNO_(3)` reacts with
`Ag_(2) CO_(3)` it generates carbon dioxide and water as a by product, if we are adding
`HNO_(3)` it will remove some of the
`CO_(3)` molecule from the reaction mixture, which then tends to shift the equilibrium towards right.

Answer 2) The same would be observed in this case, if we replace
`HNO_(3)` with HCl it will shift the equilibrium to the right as their will be generation of AgCl as the precipitate.

As per the definition of Le Chatelier's principle if we add reactants in the reaction the equilibrium will tend to move towards right, also if we replace the products or remove it then too it will shift the equilibrium towards right. So, in this reaction you are removing
`Ag^(+)` and
`Cl^(-)` ions from the solution.