Answer:
The unknown compound is a weak acid.
Explanation:
Given that :
a 25 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution.
A buffer region was found around a pH of 3.5. We know that a pH of 3.5 is a weak acid. So, it is likely to be an organic acid
Let assume the solution of the unknown sample to be CH₃COOH
Now :
25 mL of CH₃COOH reacted with 0.115 M of NaOH
The equation for the reaction will be :
CH₃COOH + NaOH -----> CH₃COONa + H₂O
at x mole of 0.115y M of
CH₃COOH NaOH is present
If NaOH was added in excess;
CH₃COOH + NaOH -----> CH₃COONa , NaOH will be lost then CH₃COOH and CH₃COONa will be present
Therefore;
At equilibrium : Only CH₃COONa will be present but if it is above equilibrium NaOH will be present because the pH will increase due to the presence of the strong base
I believe the answer to this is A.
Answer:
Explanation:
PV / RT = n , n is number of moles
Total pressure = 96400 Pa
vapour pressure = 23.8 mm of Hg
= .0238 x 13.6 x 10³ x 10 Pa = 3236.8 Pa
Pressure of hydrogen gas P = 96400 - 3236.8
= 93163.2 Pa
n = 93163.2 x .0251 / 8.31 x 298
= .944 moles of hydrogen gas is produced
moles of magnesium reacted = .944
grams of magnesium reacted = .944 x 24 = 22.66 grams .
Answer:
They have no charge
Explanation:
Basically, They are just there to balance out the number of atoms. But, they don't really do anything else.
Pls give Brainliest! trying to get a challenge done! TYSM >w<
