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A vapor composed of 0.20 mole fraction ethanol and 0.80 mole fraction acetic acid at 120.0 mmHg (absolute), is in equilibrium with a liquid phase also composed of ethanol and acetic acid. Assume that the liquid is an ideal solution and apply Raoult's law to find the following.
1-What is the temperature of the liquid? (in Celsius)
2 What are the mole fractions of the liquid phase?
3. X_E (mol ethanol / mol)?
4. X_A (mol acetic asid / mol)?
How much will the pH change? The pKa of acetic acid is 4.760.
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You dissolve 1.00 gram of an unknown diprotic (two titratable protons) acid in 200.0 mL of H2O. This solution is just neutralized by 5.00 mL of a 1.00 M NaOH solution. What is the molar mass of the unknown acid?
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