Questions: Write the balanced equation for each reaction. Phases are optional. The carbonate ion (CO3^2-) acts as a Brønsted base with water. equation: The carbon-containing product from the first reaction acts as a Brønsted base with water. equation: The carbon-containing product from the second reaction decomposes into carbon dioxide gas and water. equation:

Write the balanced equation for each reaction. Phases are optional.

The carbonate ion (CO3^2-) acts as a Brønsted base with water. equation:

The carbon-containing product from the first reaction acts as a Brønsted base with water. equation:

The carbon-containing product from the second reaction decomposes into carbon dioxide gas and water. equation:

Transcript text: Write the balanced equation for each reaction. Phases are optional. The carbonate ion ($\mathrm{CO}_{3}^{2-}$) acts as a Brønsted base with water. equation: $\square$ The carbon-containing product from the first reaction acts as a Brønsted base with water. equation: $\square$ The carbon-containing product from the second reaction decomposes into carbon dioxide gas and water. equation: $\square$

Solution

Solution Steps

Step 1: Carbonate Ion Acting as a Bronsted Base with Water

The carbonate ion ($\mathrm{CO}_{3}^{2-}$) acts as a Bronsted base with water. The reaction can be written as: \[ \mathrm{CO}_{3}^{2-} + \mathrm{H_2O} \rightarrow \mathrm{HCO}_{3}^{-} + \mathrm{OH}^{-} \]

Step 2: Bicarbonate Ion Acting as a Bronsted Base with Water

The bicarbonate ion ($\mathrm{HCO}_{3}^{-}$) formed in the first reaction acts as a Bronsted base with water. The reaction can be written as: \[ \mathrm{HCO}_{3}^{-} + \mathrm{H_2O} \rightarrow \mathrm{H_2CO_3} + \mathrm{OH}^{-} \]

Step 3: Decomposition of Carbonic Acid

The carbonic acid ($\mathrm{H_2CO_3}$) formed in the second reaction decomposes into carbon dioxide gas and water. The reaction can be written as: \[ \mathrm{H_2CO_3} \rightarrow \mathrm{CO_2} + \mathrm{H_2O} \]

Final Answer

\[ \boxed{\mathrm{CO}_{3}^{2-} + \mathrm{H_2O} \rightarrow \mathrm{HCO}_{3}^{-} + \mathrm{OH}^{-}} \] \[ \boxed{\mathrm{HCO}_{3}^{-} + \mathrm{H_2O} \rightarrow \mathrm{H_2CO_3} + \mathrm{OH}^{-}} \] \[ \boxed{\mathrm{H_2CO_3} \rightarrow \mathrm{CO_2} + \mathrm{H_2O}} \]

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