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## 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