A student prepares a solution for titration by adding a 10.00 mL aliquot of a solution saturated with Ca(OH)2 at 82.9°C to 25.0 mL of deionized water. This solution is titrated with a standardized 0.01252 M HCl solution. The equivalence point is observed after 17.94 mL of the HCl solution has been added. Use this data to answer the questions below. Calculate the moles of OH- in the 10.00ml sample. (Hint, moles of OH- at the equivalence point = moles HCl) Your answer should have 4 sig figs. Enter answers in scientific notation
A student prepares a solution for titration by adding a 10.00 mL aliquot of a solution saturated with Ca(OH)2 at 82.9°C to 25.0 mL of deionized water. This solution is titrated with a standardized 0.01252 M HCl solution. The equivalence point is observed after 17.94 mL of the HCl solution has been added. Use this data to answer the questions below. Calculate the moles of OH- in the 10.00ml sample. (Hint, moles of OH- at the equivalence point = moles HCl) Your answer should have 4 sig figs. Enter answers in scientific notation
Chapter9: Acids, Bases, And Salts
Section: Chapter Questions
Problem 9.102E
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A student prepares a solution for titration by adding a 10.00 mL aliquot of a solution saturated with Ca(OH)2 at 82.9°C to 25.0 mL of deionized water. This solution is titrated with a standardized 0.01252 M HCl solution. The equivalence point is observed after 17.94 mL of the HCl solution has been added.
Use this data to answer the questions below.
Calculate the moles of OH- in the 10.00ml sample.
(Hint, moles of OH- at the equivalence point = moles HCl)
Your answer should have 4 sig figs.
Enter answers in scientific notation
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