Carbonic anhydrase is an important enzyme that allows CO₂ and H₂O to be converted into H₂CO₃. In addition to allowing CO₂ to be dissolved into the blood and transported to the lungs for exhalation, the products of the carbonic anhydrase reaction, H₂CO₃ and a related compound HCO₃^-, also serve to control the pH of the blood to prevent acidosis or alkalosis. The carbonic anhydrase reaction and acid-base reaction are presented below.

CO₂ + H₂O  H₂CO₃

 H₂CO₃  HCO₃^- + H⁺

Assuming that reacting CO₂ is in the gas phase, increasing the pressure would shift the carbonic anhydrase reaction to the __________.

Carbonic anhydrase is an important enzyme that allows CO₂ and H₂O to be converted into H₂CO₃. In addition to allowing CO₂ to be dissolved into the blood and transported to the lungs for exhalation, the products of the carbonic anhydrase reaction, H₂CO₃ and a related compound HCO₃^-, also serve to control the pH of the blood to prevent acidosis or alkalosis. The carbonic anhydrase reaction and acid-base reaction are presented below.

CO₂ + H₂O  H₂CO₃

 H₂CO₃  HCO₃^- + H⁺

While the kidney is able to compensate for many acid/base changes in our bodies, vomiting is a temporary cause of acid/base imbalance. While vomiting may allow our bodies to get rid of toxic substances, it also causes us to lose gastric acid, which influences blood pH. How would the loss of gastric acid change the pH of our blood?

Carbonic anhydrase is an important enzyme that allows CO₂ and H₂O to be converted into H₂CO₃. In addition to allowing CO₂ to be dissolved into the blood and transported to the lungs for exhalation, the products of the carbonic anhydrase reaction, H₂CO₃ and a related compound HCO₃^-, also serve to control the pH of the blood to prevent acidosis or alkalosis. The carbonic anhydrase reaction and acid-base reaction are presented below.

CO₂ + H₂O  H₂CO₃

 H₂CO₃  HCO₃^- + H⁺

What happens to the pH of our blood if we hyperventilate?

Le Chatlier's principle states that when a stressor is introduced to a system, the system will shift its equilibrium state as a way of countering the stress. What are the factors (stressors) that apply to Le Chatlier's principle?

The Haber process for creating ammonia is written below.

This reaction takes place in a glass container, and is allowed to progress to equilibrium. Which of the following manipulations to the system will NOT shift the equilibrium to the left?

A scientist is studying a reaction, and places the reactants in a beaker at room temperature. The reaction progresses, and she analyzes the products via NMR. Based on the NMR readout, she determines the reaction proceeds as follows:

In an attempt to better understand the reaction process, she varies the concentrations of the reactants and studies how the rate of the reaction changes. The table below shows the reaction concentrations as she makes modifications in three experimental trials.

The scientist in the passage attempts to modify the conditions for the reactions by placing the reactants in a sealed, variable-volume vessel at 1atm, and allowing it to reach equilibrium. She then decreases the volume of the vessel, increasing the pressure to 5atm. Which of the following is most likely to occur?

A scientist is studying a reaction, and places the reactants in a beaker at room temperature. The reaction progresses, and she analyzes the products via NMR. Based on the NMR readout, she determines the reaction proceeds as follows:

In an attempt to better understand the reaction process, she varies the concentrations of the reactants and studies how the rate of the reaction changes. The table below shows the reaction concentrations as she makes modifications in three experimental trials.

The scientist in the passage attempts to modify the conditions for the reaction by placing the reactants in a sealed vessel at 1atm, and allowing it to reach equilibrium. She then adds helium gas to the vessel, increasing the pressure to 5atm. Which of the following is most likely to occur?

Acids and bases can be described in three principal ways. The Arrhenius definition is the most restrictive. It limits acids and bases to species that donate protons and hydroxide ions in solution, respectively. Examples of such acids include HCl and HBr, while KOH and NaOH are examples of bases. When in aqueous solution, these acids proceed to an equilibrium state through a dissociation reaction.

All of the bases proceed in a similar fashion.

The Brønsted-Lowry definition of an acid is a more inclusive approach. All Arrhenius acids and bases are also Brønsted-Lowry acids and bases, but the converse is not true. Brønsted-Lowry acids still reach equilibrium through the same dissociation reaction as Arrhenius acids, but the acid character is defined by different parameters. The Brønsted-Lowry definition considers bases to be hydroxide donors, like the Arrhenius definition, but also includes conjugate bases such as the A^- in the above reaction. In the reverse reaction, A^- accepts the proton to regenerate HA. The Brønsted-Lowry definition thus defines bases as proton acceptors, and acids as proton donors.

In studying the acid , a scientist finds that heat is released when the acid dissociates in solution. If this scientist raises the temperature in the vessel after the reaction has reached equilibrium, which of the following is most likely true?

In the given reaction, which of the following changes takes place if the temperature of the system is increased?

This reaction is allowed to proceed to equilibrium in a  container. Which of the following results will occur if the volume is suddenly decreased to ?