What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.3567 MNaOH? Ka = 1.8×10−4 for formic acid.
Answers
Explanation:
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Answer:
pH= 0.369
Explanation:
The formic acid reacts with NaOH as
HCOOH + NaOH= HCOONa + H2O
Apply CaVa/ CbVb = Na/Nb
Ca×25/(29.8×0.3587) = 1/1
Ca= (29.8×0.3587)/25= 0.428M
pH = - log(H+)
Since only 0ne H+ is in the stoichiometric equation, it means H+ = 0.428M
pH = -log(0.428) =0.369
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Answer:
call an vet ASAP 10 pounds of chocolate is very bad for a dog.
Explanation:
Chocolate is one of the worst things a dog can eat, and 10 pounds of it is worst! Take your dog to the vet IMMEDIATELY! I hope that that the dog will survive.
-------------------------------------------------------------------------------------------------------------Brainiest would make my day, but you don’t have to give it! You’re welcome.
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Answer:
To hit someone on the head
Explanation:
self protection
(2) CaH2 (4) NH3
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but it really depends on the amount of carbon
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Answers
Answer:
56.4 mmHg
Explanation:
Given:
Vapor pressure of the solution, P solution = 55 mmHg
The mass of sucrose (C₆H₁₂O₆) = 10 g
Also, Molar mass of sucrose (C₆H₁₂O₆) = 180 g/mol
So, moles = Given mass/ molar mass
Hence, moles of sucrose in the solution = 10 g / 180 g/mol = 0.05556 mol
Given that: Mass of ethanol = 100 g
Molar mass of ethanol = 46 g/mol
Hence, moles of ethanol = 100 g / 46 g/mol = 2.174 mol
Mole fraction of solvent, ethanol is:
X ethanol = 2.174 mol / (2.174 + 0.05556) mol = 0.975
Applying Raoult's Law
P solution = X ethanol*P° ethanol
=> P° ethanol = P solution / X ethanol = 55 mmHg / 0.975 = 56.4 mm Hg
Explanation:
The given data is as follows.
Vapor pressure of the solution = 55 mm Hg
Mass of sucrose = 10 g
Molar mass of sucrose = 180 g/mol
Therefore, moles of sucrose present into the solution will be calculated as follows.
No. of moles =
=
= 0.055 mol
Mass of ethanol is given as 100 g and its molar mass is 46 g/mol.
Hence, number of moles of ethanol will be calculated as follows.
No. of moles =
=
= 2.174 mol
As mole fraction =
Hence, mole fraction of etahnol will be calculated as follows.
=
=
= 0.975
Now, using Raoult's Law as follows.
=
=
= 56.4 mm Hg
Thus, we can conclude that the vapor pressure of the pure solvent is 56.4 mm Hg.