In an acid-base titration, 27.21 mL of a 0.01730 M Ca(OH)2 solution is required to neutralize a volume of 26.45 mL of a phosphoric acid solution having an unknown concentration to a phenolphthalein end point. Determine the concentration, in molarity, of the phosphoric acid solution. Start with a balanced equation.

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Beverley SmithLv2

13 Dec 2019

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A group of students performed a titration experiment. They took25.00mL of solution of phosphoric acid of unknown concentration,and then added dropwise the 0.125 M solution of sodium hydroxide.When 17.37 mL of sodium hydroxide solution was dispensed, thestudents observed that the base has completely neutralized theacid.

a) Write the balanced equation of a chemical reaction betweensodium hydroxide ("base") and phosphoric acid ("acid"). Assumecomplete neutralization.

b) Calculate the molarity of phosphoric acid solution from givendata.

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?

A 27.03 mL sample of an unknown phosphoric acid solution is titrated with a 0.112 M sodium hydroxide solution. The equivalence point is reached when 25.57 mL of sodium hydroxide solution is added. What is the concentration of the unknown phosphoric acid solution? Enter a numerical answer only, in terms of M to 4 decimal places.