Acid-Base Reactions: Did the Solutions Neutralize Each Other? | Homework Help

[brycenrg]

Homework Statement

Student mix four reagents together, thinking the solutions will neutralize each other. The solutions mixed together are 50.0mL of .1 M HCl, 100mL of .2 M of HNO3, 500mL of .01 M CaOH, 200mL of .1 M RbOH. Did the acids and bases exactly neutralize each other? If not, calculate the concentration of excess H or OH ions left in solution.

Homework Equations

M = mole/liter

The Attempt at a Solution

I looked at the solution and I understand it but I'm having trouble getting a net ionic equation.
Here is my attempt
HCl+HNO3+CaOH+RbOH>2H2O+Ca(NO3)2+RbCl
HCl+2HNO3+CaOH+RbOH>2H2O+Ca(NO3)2+RbCl
2HCl+2HNO3+CaOH+RbOH>2H2O+Ca(NO3)2+2RbCl
I can't figure out how to balance the equation to get to a net ionic equation.
Any suggestions

 

[epenguin]

"CaOH" is a big mistake. You have after all written Ca(NO₂)₂.

One way, after you have corrected that, if you know how these things dissociate into ions, calculate how many moles of H⁺ are produced by that from the acids, then how many moles of OH^- the bases, and decide whether these are equal, or whether one is more than the other,

 

[brycenrg]

"CaOH" is a big mistake. You have after all written Ca(NO₂)₂.

One way, after you have corrected that, if you know how these things dissociate into ions, calculate how many moles of H⁺ are produced by that from the acids, then how many moles of OH^- the bases, and decide whether these are equal, or whether one is more than the other,

Thank you :D