Question

Write a balanced net ionic equation to show why the solubility of Ag2CO3 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Consider only the FIRST STEP in the reaction with strong acid. Use the pull-down boxes to specify states such as (aq) or (s).

Answer 1

The silver carbonate would be or would act as a base, while the strong acid that we would choose is hydrochloric acid (HCl), these two will suffer a chemical reaction when they interact ...

As for the tables, none are visualized, so the question is considered incomplete.

Ag2CO₃ + 2HCl (diluted) → AgCl + CO₂ ↑ + H₂O

Step-by-step explanation:

Silver carbonate is considered a tertiary salt. Which these salts have three components, one is a metal, another is a carbon and the other an oxygen ...

When related to an acid, they act as a base forming an acid-base conjugation.