Final answer:
Using Henry's law, the solubility of carbon dioxide in water at 25 °C and 1690 Torr is approximately 0.0757 M, which is calculated using the ratio of new pressure to known pressure multiplied by the known solubility.
Step-by-step explanation:
The solubility of carbon dioxide (CO2) in water at a given temperature changes directly with the pressure of the gas above the liquid. This relationship is described by Henry's law, which states that at a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.
According to the information given, at 25 °C and 795 Torr, the solubility of CO2 is 0.0356 M. To find the solubility at a higher pressure, we can use the ratio of pressures, since temperature remains constant. The relationship that we will use is:
Solubility at new pressure = Solubility at known pressure × (New pressure / Known pressure)
In this case, the new pressure is 1690 Torr, and the known pressure is 795 Torr. Thus, we calculate the solubility at the new pressure:
Solubility at 1690 Torr = 0.0356 M × (1690 Torr / 795 Torr)
First, find the pressure ratio:
1690 Torr / 795 Torr = 2.1264
Now, calculate the new solubility:
0.0356 M × 2.1264 = 0.0757 M
Therefore, the solubility of carbon dioxide in water at 25 °C and 1690 Torr is 0.0757 M.