What is common to solving all mola mass problems?
1 answer:
You might be interested in
Answer:
Total pressure at equilibrium is 0.2798atm.
Explanation:
For the reaction:
H₂S(g) ⇄ H₂(g) + S(g)
Kp is defined as:
If initial pressure of H₂S is 0.150 atm, equilibrium pressures are:
H₂S(g): 0.150atm - x
H₂(g): x
S(g): x
Replacing in Kp:
X² = 0.1251 - 0.834X
X² + 0.834X - 0.1251 = 0
Solving for X:
X = -0.964 → False solution: There is no negative pressures
X = 0.1298
Thus, pressures are:
H₂S(g): 0.150atm - 0.1298atm = <em>0.0202atm</em>
H₂(g): <em>0.1298atm</em>
S(g): <em>0.1298atm</em>
Thus, total pressure in the container at equilibrium is:
0.0202atm + 0.1298atm + 0.1298atm = <em>0.2798atm</em>
This is an incomplete question, here is a complete question.
Calculate the pH of a solution made by adding 59 g of sodium acetate, NaCH₃COO, to 23 g of acetic acid, CH₃COOH, and dissolving in water to make 400. mL of solution. Hint given in feedback. The Ka for CH₃COOH is 1.8 x 10⁻⁵ M. As usual, report pH to 2 decimal places.
Answer : The pH of the solution is, 4.97
Explanation :
First we have to calculate the moles of CH₃COOH and NaCH₃COO
and,
Now we have to calculate the value of .
The expression used for the calculation of is,
Now put the value of in this expression, we get:
Now we have to calculate the pH of the solution.
Using Henderson Hesselbach equation :
Now put all the given values in this expression, we get:
(As the volume is same. So, we can write concentration in terms of moles.)
Therefore, the pH of the solution is, 4.97