Following a standardization reaction, the concentration of an aqueous solution of NaOH is determined to be 0.4510 M. a. What is the mass of NaOH in 50.0 mL of this solution? Show your work. b. What mass of KHP would be needed to completely react with 50.0 mL of this NAOH solution? Show your work.
Following a standardization reaction, the concentration of an aqueous solution of NaOH is determined to be 0.4510 M. a. What is the mass of NaOH in 50.0 mL of this solution? Show your work. b. What mass of KHP would be needed to completely react with 50.0 mL of this NAOH solution? Show your work.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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I need help with questions 3a and 3b
Transcribed Image Text:Experiment # 11: Acid-Base Titration: Standardization of NaOH
Data and results
Data table *Remember to include units
Trial 1
Trial 2
Trial 3
Trial 4
Mass of KHC&H4O4 (KHP)
1.0210g
1.0284g
1.0476g
Initial buret reading (NaOH)
0.00ml
0.00ml
0.00ml
Final buret reading (NAOH)
15.78ml
15.00ml
15.27ml
Volume of NAOH used
15.78ml
15.00ml
15.27ml
Results table
Trial 1
Trial 2
Trial 3
Trial 4
1.0284g/204.22MW-0.50357 n
Moles of KHP
n=g/MW
Moles of NaOH
n(NaOH)=n(KHP)
n(NaOH)=n(KHP)=0.50357 n
Volume of NaOH (L)
15/1000=0.015 L
Molarity of NaOH
M= n/V
0.0050357n/0.015L=0.34 M
Average molarity of NaOH
0.34+0.3359+0.3168=0.99/3=0.3 average Molarity
Sample calculation:
Transcribed Image Text:3. Following a standardization reaction, the concentration of an aqueous solution of NaOH is
determined to be 0.4510 M.
a. What is the mass of NaOH in 50.0 mL of this solution? Show your work.
b. What mass of KHP would be needed to completely react with 50.0 mL of this NAOH
solution? Show your work.
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