Question

Suppose you mix Na2SO4 and KCl solutions according to the given equation.
Na2SO4 (aq) + 2 KCl(aq) + 2 NaCl(aq) + K2SO4 (aq)
What evidence of a reaction do you expect to see?
Select one:
A precipitate should form.
A gas should form.
Water should form.
Ο Ο
No reaction should occur.

Answer 1

Answer:

No reaction should occur

Explanation:

Water cannnot be made from the components

Nothing will be released as a gas

Both products are soluible in water therefore will not form a precipitate.

Answer 2

If I mix a solution of Na2SO4 and KCl, no reaction should occur.

Whether or not, a reaction occurs when two substances are mixed depends on the respective positions of the substances in the electrochemical series.

Now, we are expecting the reaction; Na2SO4 (aq) + 2 KCl(aq) + 2 NaCl(aq) + K2SO4 (aq) to occur. The big question is, between sodium and potassium, which is higher in the electrochemical series?

A little look into the image attached shows that potassium is higher than sodium in the series so the reaction is possible.

However, the both products are aqueous, they are both soluble in water hence no visible reaction occurs.

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