Final answer:
To maintain a concentration of 0.19 M of carbon dioxide in a bottle of club soda at 25 °C, a pressure of 5.59 atm of carbon dioxide is required.
Step-by-step explanation:
To determine the pressure of carbon dioxide required to maintain a concentration of 0.19 M at 25 °C, we can use Henry's Law. Henry's Law states that the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The equation is given by: C = kH * P, where C is the concentration, kH is the Henry's Law constant, and P is the partial pressure of the gas.
In this case, the concentration (C) is 0.19 M and the Henry's Law constant (kH) is 3.4 x 10^-2 M/atm. Plugging these values into the equation, we can solve for the partial pressure (P) of carbon dioxide: 0.19 M = (3.4 x 10^-2 M/atm) * P.
Dividing both sides by (3.4 x 10^-2 M/atm), we find that P = (0.19 M) / (3.4 x 10^-2 M/atm) = 5.59 atm.