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Titration Problem

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Consider two solutions. One solution is 0.1115 M Ca(OH)(2). The other is 0.1050 M HClO(4).

a) Write a balanced equation for the reaction between the two solutions.

b) How many mL of Ca(OH)(2) will be required to neutralize 25.00 mL of the HClO(4)?

c) If a student starts to titrate 31.39 mL of the Ca(OH)(2) solution with HClO(4) and stops the titration after only 23.81 mL of HClO(4) 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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Question 2: Consider two solutions. One solution is .1115 M Ca(OH)(2). The other is .1050 M HClO(4).
a) Write a balanced equation for the reaction between the two solutions.

b) How many mL of Ca(OH)(2) will be required to neutralize 25.00 mL of the HClO(4)?

C) If a student starts to titrate 31.39 mL of the Ca(OH)(2) solution with HClO(4) ...

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