Question

What is the molar concentration of potassium ions in a 0.250 m k2so4 solution?

Answer 1

Answer : The molar concentration of $K^+$ ion is, 0.5 M

Explanation :

The dissociation reaction of $K_2SO_4$ is,

$K_2SO_4(aq)\rightarrow 2K^+(aq)+SO_4^{2-}(aq)$

By the stoichiometry we can say that, 1 mole of $K_2SO_4$ dissociates into 2 mole of $K^+$ ions and 1 mole of $SO_4^{2-}$ ions.

As we  are given the concentration of $K_2SO_4$ is, 0.250 M.

So, the molar concentration of $K^+$ ion = $2\times 0.250=0.5M$

The molar concentration of $SO_4^{2-}$ ion = 0.250 M

Therefore, the molar concentration of $K^+$ ion is, 0.5 M

Answer 2

When a compound is hydrated, it may or may not ionize. It means that a compound may or may not dissociate into its cation and anion form when solvated with water. The rule is that only electrolytes can dissociate in water. The electrolytes are composed of ionic compounds, as well as the 7 strong acids and bases: HBr, HCl, HI, HClO4, HNO3, H2SO4, LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2 and Ba(OH)2. But since K2SO4 is an ionic salt, it is also an electrolyte. So, when it dissociates into K⁺ and SO₄²⁻, both of those concentrations will be equal to 0.250 M.