Different intermolecular attractions accessible to solvent molecules cause various solvent effects, in part.
Certain solvents form hydrogen bonds. A fairly typical example is water, as well as alcohols like methanol. Others don't donate hydrogen bonds; they can only accept them.
Some solvents may more effectively stabilize the anions that result from the deprotonation of Bronsted acids. As a result, when measured in various solvents, pKa values may vary.
<h3>What is pKa value?</h3>
In layman's terms, pKa is a measurement of an acid's strength. A strong acid will have a pKa value that is lower than 0.
To be more specific, pKa is the Ka value's negative log base ten value (acid dissociation constant).
How tightly a proton is retained by a Bronsted acid is how the strength of an acid is measured.
<span>Van der waal or ideal eqn is given by PV = NRT; P = NRT/ V.
Where N = 1.335 is the number of moles. T = 272K is temperature. V = 4.920L is the volume. And R = 0.08205L. Substiting the values into the eqn; we have,
P = (1.331* 0.08205 * 272)/ 4.920 = 29.7047/ 4.920 = 6.03atm.</span>
The statement that best describes the composition of potassium chlorate, KCIO3 is "<span> The proportion by mass of elements combined in potassium chlorate is fixed."</span>
