Agricultural waste, municipal waste, plant material,
HCOOH + H2O <---> HCOO- + H3O+
<span>Ka = 1.8 X 10^-4 = [HCOO-][H3O+] / [HCOOH] </span>
<span>In the solution, [HCOO-] = [H3O+] = x </span>
<span>Quite properly, [HCOOH] = (2.30 X 10^-3 - x). </span>
<span>Since the formic acid solution is pretty dilute, and since Ka is sort of small, we can initially assume that x will be small compared to 2.3 X 10^-3, and so we can ignore it. If we do that, then, </span>
<span>Ka = x^2 / 2.30X10^-3 = 1.80 X 10^-4 </span>
<span>x = 6.4 X 10^-4 = [H3O+] </span>
<span>pH = 3.19 </span>
<span>Now, quite properly, our assumption that x would be small compared to 2.3 X 10^-3 is incorrect, and we really cannot ignore x in that expression. So, we should go back to the original expression for Ka: </span>
<span>Ka = x^2 / (2.30 X 10^-3 - x) = 1.80 X 10^-4 </span>
<span>Quite properly, you should rearrange this into a quadratic form and use the quadratic equation to solve for x. Once you've done that, x = [H3O+], and pH = - log (x).</span>
Answer :
Explanation : The ideal gas law, states that PV = nRT;
where, P is pressure;
V is volume;
n is number of moles
R is gas constant
T is temperature
If there are two entities to be compared then, it can be compared as,
;
as n and R can be considered as a constant.
Therefore, at constant pressure, the equation will get modified as;