To determine the amount of a hypothetical compound KHA. H2A 2H2O in a pure sample, Senku asked his friend Chrome to titrate it with 0.100M NaOH. Unfortunately, an accident occurred while he was away and all of the 50.0 mL NaOH solution was mixed into the sample. To remedy the situation, Senku decided to perform back titration with a 2.375 mL of 0.0800M H2SO4 solution. a) How many excess moles of NaOH were added to the solution? b) How many moles of the compound KHA.H2A.2H2O are present in the sample? c) When the reaction between the same sample of KHA.H2A.2H2O and NaOH was carried out in a coffee cup calorimeter, the measured total temperature rise from 25.0°C was 54.0°C. Determine the magnitude of the heat of the neutralization of KHA.H2A.2H2O and NaOH in Joules. Assume that the Cp of the solution is 18.0 cal/mol-K.

To determine the amount of a hypothetical compound KHA. H2A 2H2O in a pure sample, Senku asked his friend Chrome to titrate it with 0.100M NaOH. Unfortunately, an accident occurred while he was away and all of the 50.0 mL NaOH solution was mixed into the sample. To remedy the situation, Senku decided to perform back titration with a 2.375 mL of 0.0800M H2SO4 solution. a) How many excess moles of NaOH were added to the solution? b) How many moles of the compound KHA.H2A.2H2O are present in the sample? c) When the reaction between the same sample of KHA.H2A.2H2O and NaOH was carried out in a coffee cup calorimeter, the measured total temperature rise from 25.0°C was 54.0°C. Determine the magnitude of the heat of the neutralization of KHA.H2A.2H2O and NaOH in Joules. Assume that the Cp of the solution is 18.0 cal/mol-K.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 128CP: Consider the titration curve in Exercise 115 for the titration of Na2Cr3 with HCl. a. If a mixture...

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A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
Consider the titration curve in Exercise 115 for the titration of Na2Cr3 with HCl. a. If a mixture of NaHCO3 and Na2CO3 was titrated, what would be the relative sizes of V1, and V2? b. If a mixture of NaOH and Na2CO3 was titrated, what would be the relative sizes of V1 and V2? c. A sample contains a mixture of NaHCO3 and Na2CO3. When this sample was titrated with 0.100 M HCl, it took 18.9 mL to reach the first stoichiometric point and an additional 36.7 mL to reach the second stoichiometric point. What is the composition in mass percent of the sample?
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