Acids → proton (H+) donor
Bases → proton (H+) acceptor
• weak triprotic acid
• 3 H+ to donate
H3PO4(aq) ⇌ 3 H+(aq) + PO43-(aq)
• strong base → will completely dissociate in the solution
Sr(OH)2(aq) → Sr2+(aq) + 2 OH-(aq)
Consider the acid/base neutralization reaction of strontium hydroxide and phosphoric acid:
a. Write a balanced molecular equation for this reaction. Include all phases for both reactants and products.
b. If a titration of 61.00 mL of an unknown H3PO4 solution requires the addition of 82.50 mL of 0.300 M Sr(OH)2, what was the original concentration of the phosphoric acid solution?
c. At the end of the titration, what is the final concentration of Sr2+ ions?
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Titrations of Diprotic and Polyprotic Acids concept. You can view video lessons to learn Titrations of Diprotic and Polyprotic Acids. Or if you need more Titrations of Diprotic and Polyprotic Acids practice, you can also practice Titrations of Diprotic and Polyprotic Acids practice problems.