The sequence of reactions to be driven to the left or the right of the given equation, if an underwater volcano bubbled additional CO 2 into the ocean and its effect on the pH of the ocean. Introduction: According to the Le Chatelier's principle, the equilibrium law is mainly used for predicting the effect of a change in the conditions on a chemical equilibrium . This principle states that the chemical equilibrium will shift toward the direction opposite to the other side, in which concentration of species is increased. The increase in the concentration of the carbon dioxide shifts the chemical equilibrium to the right side, which leads to the production of the carbonic acid. Consider the reaction between carbon dioxide and water to form carbonic acid: CO 2 (g) + H 2 O(l)⇌CH 2 O 3 (aq) In the ocean, carbonic acid immediately dissociates to form a proton and bicarbonate ion, as follows: CH 2 O 3 (aq)⇌H + (aq) + CHO 3 − (aq)

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Chapter 2, Problem 12TYU

Summary Introduction

To analyze:

The sequence of reactions to be driven to the left or the right of the given equation, if an underwater volcano bubbled additional CO₂ into the ocean and its effect on the pH of the ocean.

Introduction:

According to the Le Chatelier's principle, the equilibrium law is mainly used for predicting the effect of a change in the conditions on a chemical equilibrium. This principle states that the chemical equilibrium will shift toward the direction opposite to the other side, in which concentration of species is increased. The increase in the concentration of the carbon dioxide shifts the chemical equilibrium to the right side, which leads to the production of the carbonic acid.

Consider the reaction between carbon dioxide and water to form carbonic acid:

CO₂(g) + H₂O(l)⇌CH₂O₃(aq)

In the ocean, carbonic acid immediately dissociates to form a proton and bicarbonate ion, as follows:

CH₂O₃(aq)⇌H⁺(aq) + CHO₃⁻(aq)

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