Help ASAP How many moles of O2 are in 7.23 mol P
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The pH of the solution in which one normal adult dose aspirin is dissolved is : 2.7
Given data :
mass of aspirin = 640 mg = 0.640 g
volume of water = 10 ounces = 0.295735 L
molar mass of aspirin = 180.16 g/mol
moles of aspirin = mass / molar mass = 0.00355 mol
<h3>Determine the pH of the solution </h3>First step : <u>calculate the concentration of aspirin</u>
= moles of Aspirin / volume of water
= 0.00355 / 0.295735
= 0.012 M
Given that pKa of Aspirin = 3.5
pKa = -logKa
therefore ; Ka = =
From the Ice table
=
=
given that the value of Ka is small we will ignore -x
x² =
x =
Therefore
[ H⁺ ] =
given that
pH = - Log [ H⁺ ]
= - ( -3 + log 1.948 )
= 2.71 ≈ 2.7
Hence we can conclude that The pH of the solution in which one normal adult dose aspirin is dissolved is : 2.7
Learn more about Aspirin : brainly.com/question/2070753
Answer:
The vapor pressure at temperature 363 K is 0.6970 atm
The vapor pressure at 383 K is 1.410 atm
Explanation:
To calculate of the reaction, we use clausius claypron equation, which is:
where,
= vapor pressure at temperature
= vapor pressure at temperature
= Enthalpy of vaporization
R = Gas constant = 8.314 J/mol K
1)
= initial temperature =363 K
= final temperature =373 K
Putting values in above equation, we get:
The vapor pressure at temperature 363 K is 0.6970 atm
2)
= initial temperature =373 K
= final temperature =383 K
Putting values in above equation, we get:
The vapor pressure at 383 K is 1.410 atm