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Homework Help: Acid base reactions

  1. Mar 4, 2016 #1
    1. The problem statement, all variables and given/known data
    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.

    2. Relevant equations
    M = mole/liter

    3. 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
    I can't figure out how to balance the equation to get to a net ionic equation.
    Any suggestions
  2. jcsd
  3. Mar 4, 2016 #2


    User Avatar
    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,
  4. Mar 4, 2016 #3
    Thank you :D
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