Answer:
Volume of NaOH required = 3.61 L
Explanation:
H2SO3 is a diprotic acid i.e. it will have two dissociation constants given as follows:
--------(1)
where, Ka1 = 1.5 x 10–2 or pKa1 = 1.824
--------(2)
where, Ka2 = 1.0 x 10–7 or pKa2 = 7.000
The required pH = 6.247 which is beyond the first equivalence point but within the second equivalence point.
Step 1:
Based on equation(1), at the first eq point:
moles of H2SO3 = moles of NaOH
Step 2:
For the second equivalence point setup an ICE table:
Initial 1.98 ? 0
Change -x -x x
Equil 1.98-x ?-x x
Here, ?-x =0 i.e. amount of OH- = x
Based on the Henderson buffer equation:
![pH = pKa2 + log\frac{[SO3]^{2-} }{[HSO3]^{-} } \\6.247 = 7.00 + log\frac{x}{(1.98-x)} \\x=0.634 moles](https://tex.z-dn.net/?f=pH%20%3D%20pKa2%20%2B%20log%5Cfrac%7B%5BSO3%5D%5E%7B2-%7D%20%7D%7B%5BHSO3%5D%5E%7B-%7D%20%7D%20%5C%5C6.247%20%3D%207.00%20%2B%20log%5Cfrac%7Bx%7D%7B%281.98-x%29%7D%20%5C%5Cx%3D0.634%20moles)
Volume of NaOH required is:
Step 3:
Total volume of NaOH required = 3.22+0.389 =3.61 L
The problem applies Charles' law since constant pressure with varying volume and temperature are given. Assuming ideal gas law, the equation to be used is
=
. We make sure the temperatures are expressed in Kelvin, hence the given added with 273. The volume 2 is equal to 25.2881 liters.
Answer:
using public transportation
Explanation:
With the use of public transport, there will be a reduction in the number of cars on the streets, this reduction will cause a reduction in the gases released by cars into the atmosphere, which will result in a reduction in air pollution.
Haber's process is used for the industrial production of ammonia. The process conditions at which maximum yield can be obtained, include 15-20mPa pressure, 400-500 degrees Celsius of the temperature, use of methane as a source of hydrogen, use of iron-based catalysts and combined with K2O, CaO, SiO2, and Al2O3<span>. Reuse of unreacted gases can lead to the achievement of 97% yield. </span>
4 hydrogen atoms must bond
