Calculating the molarity when mixing two different solutions

[AMan24]

Homework Statement

You mix 45-mL of 0.1174M K2SO4 and 35-mL of 0.2504M HNO3

Homework Equations

none.

The Attempt at a Solution

So I'm supposed to find the number of moles of the K2SO4 and add it to the number of moles of 0.2504, then add the two volumes, and divide the total number of moles by the total volume.

My question is, if i write a balanced equation, i get K2SO4 + 2HNO3 = 2KNO3 + H2SO4, does that mean for the number of moles of HNO3, before i add it to the number of moles of K2SO4 i have to multiply the number of moles of HNO3 by 2, because of the coefficient.

I could also be doing this problem entirely wrong by assuming a reaction is occurring and even needing to balance. There is nothing in my book talking about reactions when mixing two different solutions.

 

[Bystander]

That's the complete problem statement?

 

[AMan24]

That's the complete problem statement?

In this case the problem said to find the molarity of each ion present in the solution formed. But i can already do that, and on my test tomorrow there's going to be a question that has a part a) and b) (professor told us) and its going to ask for the ion concentration and the molarity of final solution.

Now you got me thinking that it isn't possible to do what I'm doing when given two different solutions, and that you can only find the ion concentration when mixing two different solutions, not the molarity. Is this true? If that's true then my professor might have meant mixing two same solutions of different molarity.

 

[Bystander]

might have meant mixing two same solutions of different molarity

That would be my take on it.

 

[AMan24]

That would be my take on it.

yeah you're definitely right, i just realized how it doesn't even make sense to have one molarity for a mixture of solutions