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 HCI 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 HCI) Your answer should have 4 sig figs. Enter answers in scientific notation using E, as 1.234 E-2 for example. Answer: 8.984e-3 Calculate the moles of Ca2* in the 10.00ml sample. (See equation 1 in the procedure) Your answer should have 4 sig figs. Answer: 0.000032
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 HCI 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 HCI) Your answer should have 4 sig figs. Enter answers in scientific notation using E, as 1.234 E-2 for example. Answer: 8.984e-3 Calculate the moles of Ca2* in the 10.00ml sample. (See equation 1 in the procedure) Your answer should have 4 sig figs. Answer: 0.000032
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter14: Acid- Base Equilibria
Section: Chapter Questions
Problem 97AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...
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