Calculate the %(m/v) of hydrochloric acid using the molar concentration you found. Shows calculations. Records final answer to correct significant digits. Records the concentration with the appropriate units. The molar concentration I found was 0.1M.
Calculate the %(m/v) of hydrochloric acid using the molar concentration you found. Shows calculations. Records final answer to correct significant digits. Records the concentration with the appropriate units. The molar concentration I found was 0.1M.
Chemical Principles in the Laboratory
11th Edition
ISBN:9781305264434
Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Chapter24: The Standardization Of A Basic Solution And The Determination Of The Molar Mass Of An Acid
Section: Chapter Questions
Problem 2ASA: In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a...
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Calculate the %(m/v) of hydrochloric acid using the molar concentration you found.
Shows calculations. Records final answer to correct significant digits. Records the concentration with the appropriate units.
The molar concentration I found was 0.1M.
Transcribed Image Text:Calculate the average volume of NaOH used in your trials.
Correctly calculates the average amount of NaOH used.
Records the answer with proper units and significant digits.
Average of NAOH used:
(27.001+26.004+26.004)/3
= 26. 336
=30 mL
Transcribed Image Text:Table 1 - the concentration of NaOH and the volume of HCI
It is being shown, because it is to be used to calculate the concentration of HCI
Concentration of NaOH Used (M)
0.1M
Volume of Unknown Acid Used in Each Trial (mL)
25.00mL
Table 2 - the recorded volume of NaOH used in the beginning and remained
after the titration
It is being shown, because it is to be used to calculate the concentration of HCI
Trial 1
Trial 2
Trial 3
Initial Burette Reading (mL)
50.00mL
50.00mL
50.00mL
Final Burette Reading (mL)
22.999mL
23.996mL
23.998mL
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