When 60.0 milliliter of 3.0-molar K2CO3 is added to 40.0 milliliters of 1.0-molar KHCO3, see details?

Question

When 60.0 milliliters of 3.0-molar K2CO3 are added to 40.0 milliliters of 1.0 molar KHCO3, what is the resulting concentration of K+?

I got 4M by adding .36 mols [in 60 mL of 3.0 M solution K2CO3] with .04 [in 40 mL 1 M KHCO3], which is .4 and dividing it by the amount of liters that would come out of it, [.04+.06=].1, which equals .4=.1=4. Please explain this to me even if I got it right. Thanks a lot!

Answer 1

First, I believe you have the correct answer.

60 mL + 40 mL = 100 mL of the solution.

3.0 M K2CO3 will have a concentration of 6 M K+ ions since there are two K+ for each molecule of K2CO3.

1.0 M KHCO3 will have a concentration of 1.0 M K+ ions since there is one K+ for each molecule of KHCO3.

M1 V1 + M2 V2 = Mt Vt
(6.0 M) (60 mL) + (1.0 M) (40 mL) = Mt (100 mL)
360 + 40 = Mt (100)
400 = (Mt) 100
4.0 M = molarity

Answer 2

you are right