Answer:
pH = 1.32
Explanation:
H₂M + KOH ------------------------ HM⁻ + H₂O + K⁺
This problem involves a weak diprotic acid which we can solve by realizing they amount to buffer solutions. In the first deprotonation if all the acid is not consumed we will have an equilibrium of a wak acid and its weak conjugate base. Lets see:
So first calculate the moles reacted and produced:
n H₂M = 0.864 g/mol x 1 mol/ 116.072 g = 0.074 mol H₂M
54 mL x 1L / 1000 mL x 0. 0.276 moles/L = 0.015 mol KOH
it is clear that the maleic acid will not be completely consumed, hence treat it as an equilibrium problem of a buffer solution.
moles H₂M left = 0.074 - 0.015 = 0.059
moles HM⁻ produced = 0.015
Using the Henderson - Hasselbach equation to solve for pH:
ph = pKₐ + log ( HM⁻/ HA) = 1.92 + log ( 0.015 / 0.059) = 1.325
Notes: In the HH equation we used the moles of the species since the volume is the same and they will cancel out in the quotient.
For polyprotic acids the second or third deprotonation contribution to the pH when there is still unreacted acid ( Maleic in this case) unreacted.
Answer:
The new volume of the balloon is 600cm³
Explanation:
Given parameters:
Initial Volume, which is V₁ = 200cm³
Initial temperature, T₁ = 60°C
Final temperature T₂ = 180°C
Final Volume V₂ =?
To solve this kind of problem, we apply one of the gas laws that shows the relationship between volume and temperature.
This law is the Charles law, it states that " the volume of a fixed mass of a gas is directly proportional to its absolute temperature if pressure is constant".
It is simply expressed as:
V₁/T₁ = V₂/T₂
Since our unknown is V₂, we make it the subject of the expression given above:
V₂ = V₁T₂/T₁
Now input the corresponding values and solve:
V₂ = 200 x 180 / 60
V₂ = 36000/60
V₂ = 600cm³
The new volume of the balloon is 600cm³
The number of mole of oxygen needed is of 0.080 mole.
To solve this question, we'll begin by writing the balanced equation for the reaction. This is illustrated below:
<h3>CH₃COOH + 2O₂ —> CO₂ + 2H₂O</h3>
From the balanced equation above,
2 moles of O₂ reacted to produce 2 moles of H₂O.
Finally, we shall determine the number of mole of O₂ needed to produce 0.080 mole of H₂O. This can be obtained as follow:
From the balanced equation above,
2 moles of O₂ reacted to produce 2 moles of H₂O.
Therefore,
0.080 mole of O₂ will also react to produce 0.080 mole of H₂O.
Thus, 0.080 mole of oxygen, O₂, is needed for the reaction.
Learn more: brainly.com/question/1563415
