If a stronger solution of sodium bicarbonate was used in beaker B, would it require more or less acetic acid to neutralize and w
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The question is incomplete, here is the complete question:
At 25°C Henry's Law constant for carbon dioxide gas in water is 0.031 M/atm . Calculate the mass in grams of gas that can be dissolved in 425. mL of water at 25°C and at a partial pressure of 2.92 atm. Round your answer to 2 significant digits.
<u>Answer:</u> The mass of carbon dioxide that can be dissolved is 1.7 grams
<u>Explanation:</u>
To calculate the molar solubility, we use the equation given by Henry's law, which is:
where,
= Henry's constant =
= molar solubility of carbon dioxide gas
= partial pressure of carbon dioxide gas = 2.92 atm
Putting values in above equation, we get:
To calculate the mass of solute, we use the equation used to calculate the molarity of solution:
Given mass of carbon dioxide = ? g
Molar mass of carbon dioxide = 44 g/mol
Molarity of solution =
Volume of solution = 425 mL
Putting values in above equation, we get:
Hence, the mass of carbon dioxide that can be dissolved is 1.7 grams