158 mL of a 0.148M NaCl solution is added to 228 mL of a 0.369M NH4NO3 solution. What's the concentration of ammonium ions?
What is the concentration of ammonium ions in the resulting mixture and how would one go about solving this?
What is the concentration of ammonium ions in the resulting mixture and how would one go about solving this?
1 Answer
Mar 27, 2018
Explanation:
This is the formula for finding molarity:
First, let's find the number of moles of ammonium ions in the resulting solution:
- In
#"158 mL"# , or#"0.158 L"# of#"0.148 M"# #NaCl# solution, there are no ammonium ions. - In
#"228 mL"# , or#"0.228 L"# of#"0.369 M"# #NH_4NO_3# solution, there are#"0.369 mol/L" xx "0.228 L" = 0.0819# moles of ammonium ions.
That means that the total number of ammonium ions in the final solution is
Then, we just need to add up the volumes of the two mixed solutions to find the volume of our final product.
Finally, we can just plug in these values to find molarity! :)
