What is the pH of a 0.1 M phosphate buffer (pKa = 6.86) that contains equal amounts of acid and conjugate base?
1 answer:
Answer : The pH of a 0.1 M phosphate buffer is, 6.86
Explanation : Given,
Concentration of acid = 0.1 M
Concentration of conjugate base (salt) = 0.1 M
Now we have to calculate the pH of buffer.
Using Henderson Hesselbach equation :
Now put all the given values in this expression, we get:
Therefore, the pH of a 0.1 M phosphate buffer is, 6.86
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The molecular formula of the given compound is also known as Carbonic acid.
The simplest whole-number ratio of the various atoms in a compound is represented by an empirical formula.
The precise number of various atom types present in a compound's molecule is indicated by the molecular formula.
Given that,
H = 3.3%
C = 19.3%
O = 77.4%
No. of moles of H = 3.3/1
No. of moles of H = 3.3
No. of moles of C = 19.3 / 12
No. of moles of C = 1.60
No. of moles of O = 77.4/16
No. of moles of O = 4.83
Therefore, the ratio of the atoms of C, H and O = 3.3 : 1.60 : 4.83
Divide by smallest value which you get =3.3 / 1.60 : 1.60 / 1.60 : 4.83 / 1.60
The ratio of the atoms of C, H and O = 2 : 1 : 3
So, the empirical formula is
Let the molecular formula is
Then, molar mass
Molar mass = 62n
As the question, 62 n = 60
n = 0.96 or n = 1 (rounded off to nearest ones)
So, the molecular formula is i.e., the compound is Carbonic acid.
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(a) Balanced equation
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(b). Calculation
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