had taken place. What is 3) What is the effect on the determination of the sodium hydroxide concentration (high, low, no effect) a) If the KHP that was weighed was not completely transferred to the volumetric flask? b) If the KHP sample in this experiment was dissolved in 50 mL of water instead of 30 mL of water. of oralic acid (diprotic acid) required 17.5 mL of sodium

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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Solve 3 and 4
Experim
D. Post Laboratory Questions:
1) A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated
with NaOH and the concentration of the NaOH determined to be 0.110 M. For
the second titration, the student correctly diluted 6 M HCI from the reagent shelf
using a graduated cylinder to obtain approximately 0.6 M HCI. This solution
was titrated with the original NaOH solution. The student calculated the
concentration of NaOH from the experiment to be 0.099 M. In which experiment
should the student be more confident of the concentration of the NaOH solution?
Why?
2) A student needed to standardize a solution of NaOH which was approximately
0.04 M. The student weighed out 0.237 g of KHP. The student carefully prepared
the titration setup, but after 25 mL of NaOH was added, no observable change
had taken place. What is the procedural error in this experiment?
3) What is the effect on the determination of the sodium hydroxide concentration
(high, low, no effect)
a) If the KHP that was weighed was not completely transferred to the volumetric
flask?
b) If the KHP sample in this experiment was dissolved in 50 mL of water instead
of 30 mL of water.
4) A 0.261 g sample of oxalic acid (diprotic acid) required 17.5 mL of sodium
hydroxide solution for complete reaction. Write the equation for this reaction
and determine the molar concentration of the sodium hydroxide solution?
Transcribed Image Text:Experim D. Post Laboratory Questions: 1) A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCI from the reagent shelf using a graduated cylinder to obtain approximately 0.6 M HCI. This solution was titrated with the original NaOH solution. The student calculated the concentration of NaOH from the experiment to be 0.099 M. In which experiment should the student be more confident of the concentration of the NaOH solution? Why? 2) A student needed to standardize a solution of NaOH which was approximately 0.04 M. The student weighed out 0.237 g of KHP. The student carefully prepared the titration setup, but after 25 mL of NaOH was added, no observable change had taken place. What is the procedural error in this experiment? 3) What is the effect on the determination of the sodium hydroxide concentration (high, low, no effect) a) If the KHP that was weighed was not completely transferred to the volumetric flask? b) If the KHP sample in this experiment was dissolved in 50 mL of water instead of 30 mL of water. 4) A 0.261 g sample of oxalic acid (diprotic acid) required 17.5 mL of sodium hydroxide solution for complete reaction. Write the equation for this reaction and determine the molar concentration of the sodium hydroxide solution?
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