Which condition will decrease the rate of reaction between excess magnesium and hydrochloric acid?
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Hello!
First, we need to determine the pKa of the base. It can be found applying the following equation:
Now, we can apply the Henderson-Hasselbach's equation in the following way:
![pH=pKa+log( \frac{[CH_3NH_2]}{[CH_3NH_3Cl]} )=10,65+log( \frac{0,18M}{0,73M} )=10,04](https://tex.z-dn.net/?f=pH%3DpKa%2Blog%28%20%5Cfrac%7B%5BCH_3NH_2%5D%7D%7B%5BCH_3NH_3Cl%5D%7D%20%29%3D10%2C65%2Blog%28%20%5Cfrac%7B0%2C18M%7D%7B0%2C73M%7D%20%29%3D10%2C04)
So, the pH of this buffer solution is 10,04
Have a nice day!
First, we need to determine the pKa of the base. It can be found applying the following equation:
Now, we can apply the Henderson-Hasselbach's equation in the following way:
So, the pH of this buffer solution is 10,04
Have a nice day!
Total of 127.013 C of charge is passed
Given
weight of Ag solution before current has passed = 1.7854 g
weight of Ag solution after current has passed = 1.8016 g
Molecular mass of Ag = 107.86 g
Faraday's Constant = 96485
First of all we have to apply Faraday's First Law of Electrolysis i.e
m = ZQ
where
Z is propotionality constant (g/C)
Q is charge (C)
Hence,
Z = Atomic mass of substance/ Faraday's Constant
=
= 0.0011178 g/C
Now ,
change in mass before and after the passing of current (Δm)
Δm = 1.8016g-1.7854g
= 0.0162g
Now amount of coulombs passed =
amount of coulombs passed = 127.03524 C
Thus from the above conclusion we can say that amount of coulombs have passed is 127.03524 C
Learn more about Electrolysis here: brainly.com/question/16929894
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