Which of the following elements could form a diatomic molecule?
1 answer:
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Answer: Partial pressure of at a depth of 132 ft below sea level is 2964 mm Hg.
Explanation:
It is known that 1 atm = 760 mm Hg.
Also,
where, = partial pressure of
P = atmospheric pressure
= mole fraction of
Putting the given values into the above formula as follows.
= 0.780
Now, at a depth of 132 ft below the surface of the water where pressure is 5.0 atm. So, partial pressure of is as follows.
=
= 2964 mm Hg
Therefore, we can conclude that partial pressure of at a depth of 132 ft below sea level is 2964 mm Hg.
Answer:
7.3
Explanation:
By Henderson Hasselbalch equation we can calculate the pH or the pOH of a solution by its pKa. Remember that , and pKa = -logKa. Ka is the equilibrium constant of the acid.
Henderson Hasselbalch equation :
Where [HA] is the concentration of the acid, and is the concentration of the anion which forms the acid.
So, acid X, has two ionic forms, the carboxyl group and the other one. First, we have 0.1 mol/L of the acid, in 100 mL, so the number of moles of X
n1 = (0.1 mol/L)x(0.1 L) = 0.01 mol
When it dissociates, it forms 0.005 mol of the carboxyl group and 0.005 mol of the other group. Assuming same stoichiometry.
Adding NaOH, with 0.1 mol/L and 75 mL, the number of moles of will be
n2 = (0.1 mol/L)x(0.075 L) = 0.0075 mol
So, the 0.0075 mol of reacts with 0.005 mol of carboxyl, remaining 0.0025 mol of
, which will react with the 0.005 mol of the other group. So, it will remain 0.0025 mol of the other group.
The final volume of the solution will be 175 mL, but both concentrations (the acid form and ionic form) have the same volume, so we can use the number of mol in the equation.
Note that, the number of moles of the acid form is still 0.01 mol because it doesn't react!
So,
6.72 = pKa - log 4
pKa - log4 = 6.72
pKa = 6.72 + log4
pKa = 6.72 + 0.6
pKa = 7.3