Ok, heres is the question.
Consider two solutions. One solution is 0.1115 M CA(OH)2. The other is 0.1050 M HClO4.
A. Write a balanced, net ionic equation for the reaction between the two solutions.
B. How many mL of Ca(OH)2 willbe required to neutralize 25.00 mL of the HCLO4?
C. If a student starts to titrate 31.39 mL of the Ca(OH)2 solution with HClO4 and stops the titration after only 23.81 mL of HClO4 have been added, then
1. How many moles of H+ have been added?
2. How many moles of OH- are left unreacted?
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Now, im a bit confused, I think im supposed to do the equation doing a redox equation right? Where I split it into half equations and then put them back together to cancel out electrons. But I must be putting the half equations together wrong because I get all the electrons on one side. Im supposed to use 2HClO4 and Ca(OH)2 for the half equations right...? And im not quite sure what titration means... :/