Question

100 ml of 0.2 M K2SO4 is diluted with 100ml of water . The concentration of K+ ions in the solution is

Answer 1

Answer:

What will be the molarity concentration of k + ion in the mixture obtained by mixing 100 ml, 2M KCl, 200 ml, and 3M K2SO4?

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4 Answers



Ashish Ranjan, IIT R Undergrad

Answered November 11, 2015

This is a simple problem of stoichiometry in which we have to consider the dissociation of ionic salts such as KCl and K2SO4.

Consider this...

KCl and K2SO4 being strong electrolytes, will undergo complete dissosciation and furnish ions as follows:

KCl-> K+ +Cl-

K2SO4-> 2K+ +SO42-

Dissosciation of 1 mole KCl solution produces 1 mol of K+ ions.

Whereas the dissosciation of 1 mol of K2SO4 solution produces 2 moles of K+ ions, considering the ionic equation mentioned above..

Number of moles=Molarity×Volume

Moles of K+ ions produced by Kcl solution(100 ml(0.1L) of 2M KCl)

=0.1×2=0.2 moles

Similarly moles of K2SO4=0.2×3=0.6 moles

Moles of K+ ions produced by K2SO4=2×0.6=1.2 moles

Total moles of K+=1.2+0.6=1.8 moles

Now the total volume of resulting mixture=300 ml

Molarity=moles of K+/Volume of solution

Molarity=1.8/0.3=6 M

Answer 2

Answer:

What will be the molarity concentration of k + ion in the mixture obtained by mixing 100 ml, 2M KCl, 200 ml, and 3M K2SO4?

This is a simple problem of stoichiometry in which we have to consider the dissociation of ionic salts such as KCl and K2SO4.

Consider this...

KCl and K2SO4 being strong electrolytes, will undergo complete dissosciation and furnish ions as follows:

KCl-> K+ +Cl-

K2SO4-> 2K+ +SO42-

Dissosciation of 1 mole KCl solution produces 1 mol of K+ ions.

Whereas the dissosciation of 1 mol of K2SO4 solution produces 2 moles of K+ ions, considering the ionic equation mentioned above..

Number of moles=Molarity×Volume

Moles of K+ ions produced by Kcl solution(100 ml(0.1L) of 2M KCl)

=0.1×2=0.2 moles

Similarly moles of K2SO4=0.2×3=0.6 moles

Moles of K+ ions produced by K2SO4=2×0.6=1.2 moles

Total moles of K+=1.2+0.6=1.8 moles

Now the total volume of resulting mixture=300 ml

Molarity=moles of K+/Volume of solution

Molarity=1.8/0.3=6 M

Explanation:

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