Problem: A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.What is the concentration of K+ that remains in solution?

FREE Expert Solution

A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.

What is the concentration of K+ that remains in solution?

Balanced reaction: 2 KOH(aq) + NiSO4(aq) → K2SO4(aq) + Ni(OH)2(s)

Total ionic equation: 2 K+(aq) + 2 OH-(aq) + Ni2+(aq) + SO42-(aq) → 2 K+(aq) + SO42-(aq) + Ni(OH)2(s)


K+ will remain unreacted and remain in the solution. Calculate the concentration of K+:

KOH(aq) → K+(aq) + OH-(aq) 

[KOH] = [K+]

View Complete Written Solution
Problem Details

A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.

What is the concentration of K+ that remains in solution?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.