Answer:
Explanation:
Consider that, as the system is adiabatic, where U1 and U2 are the internal energies before the process and after that respectively.
Consider that: , and that the internal energy of the first state is the sum of the internal energy of each tank.
So,
Where A y B are the tanks. The enthalpy for an ideal gas is only function of the temperature, as the internal energy is too; so it is possible to assume:
So,
Isolating ,
So,
The relationship between pH and pKa of buffer solution in given atomic view:
In figure I pH= pKa ( since [HA] =[A-] )
In figure II pH > pKa ( since [A-] > [HA] )
In figure III pH < pKa ( since [A-] < [HA] )
The pH and pKa are related by the Henderson-Hasselbalch equation. It should not be used for concentrated solutions, extremely low pH acids, or extremely high pH bases because it is simply an approximation.
pH = pKa + log(conjugate base/weak acid).
pH equals pKa plus log ([A-] / [HA]).
pH is determined by dividing the weak acid concentration by the log of the conjugate base concentration and the pKa value.
About halfway to the equivalence point:
pH = pKa
It's important to note that this equation is familiar with the connection because it is sometimes written for the Ka value rather than the pKa value.
pKa = – log Ka
Hence, value of pH depend on relative concentration of [A-] and HA]
To know more about Ka.
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