# Acid base reactions

## 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.

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

Related Biology and Chemistry Homework Help News on Phys.org
epenguin
Homework Helper
Gold Member
"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