Which of rhe following changes occurs when cxcess of C O1...

Which of rhe following changes occurs when cxcess of $C O_{1}$ gas is passca into a clear solution of lime warcr? (a) A whirc prccipirare conraining both $\mathrm{CaCO}_{3}$ and $\mathrm{Ca}\left(11 \mathrm{CO}_{3}\right)$, is formcd. (b) Initially, a white precipitate of $\mathrm{CaCO}_{3}$ is formed which charlges into soluble $\mathrm{Ca}\left(\mathrm{HCO}_{3}\right)_{2}$ on passing excess $\mathrm{CO}_{2}$ gas. (c) $\Lambda$ white precipitate of $\mathrm{Ca}\left(\mathrm{HCO}_{3}\right)$ is formed. (d) $\Lambda$ white precipitate of $\mathrm{CaCO}_{3}$ is formed.

Which of rhe following changes occurs when cxcess of $C O_{1}$ gas is passca into a clear solution of lime warcr?
(a) A whirc prccipirare conraining both $\mathrm{CaCO}_{3}$ and $\mathrm{Ca}\left(11 \mathrm{CO}_{3}\right)$, is formcd.
(b) Initially, a white precipitate of $\mathrm{CaCO}_{3}$ is formed which charlges into soluble $\mathrm{Ca}\left(\mathrm{HCO}_{3}\right)_{2}$ on passing excess $\mathrm{CO}_{2}$ gas.
(c) $\Lambda$ white precipitate of $\mathrm{Ca}\left(\mathrm{HCO}_{3}\right)$ is formed.
(d) $\Lambda$ white precipitate of $\mathrm{CaCO}_{3}$ is formed.

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Key Concepts

Solubility and Equilibrium Shifts

This key idea explains how the solubility of compounds can change based on the concentrations of reactants or products in a solution. An initially formed insoluble product can dissolve upon the addition of an excess reagent if the equilibrium shifts to favor the formation of a more soluble species. This dynamic equilibrium concept is essential in understanding how reactions evolve under varying conditions.

Precipitation Reactions

This concept involves the formation of an insoluble solid (a precipitate) when two soluble reactants in an aqueous solution combine. It is a key aspect of many qualitative chemical tests where the appearance of a precipitate indicates the presence of a specific ion or compound in solution.

Acid-Base Reactions and Carbonate Equilibria

Acid-base reactions in aqueous systems often lead to the formation of different species depending on the pH of the solution. In the context of carbonate chemistry, carbon dioxide dissolved in water produces carbonic acid, which reacts with bases to form either carbonate or bicarbonate ions. The shift between these forms is a classic example of how equilibrium can be influenced by the relative amounts of reactants and the pH of the medium.

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