At Westonci.ca, we make it easy to get the answers you need from a community of informed and experienced contributors. Connect with a community of experts ready to provide precise solutions to your questions quickly and accurately. Connect with a community of professionals ready to provide precise solutions to your questions quickly and accurately.
Sagot :
The question is incomplete as the measured value isn't given. However, an hypothesized measured value will be used to explain how to calculate the percentage error.
Answer:
2.5%
Explanation:
Percentage error :
[(measured value - True value)/ True value] * 100%
The measured value is the value obtained during an while using a measuring device.
If the measured value is = 0.123
Then, the percent error will be :
[(0.123 - 0.120) / 0.120] * 100%
(0.003 / 0.120) * 100%
0.025 * 100%
= 2.5%
Answer:
For each trial, compute the mol of titrant; (molarity x L) and keep the number of significant figures to 4.
Trial 1: 12.49 mL =
0.0025
mol NaOH
Trial 2: 12.32 mL =
0.0025
mol NaOH
Trial 3: 11.87 mL =
0.0024
mol NaOH
Because the moles of titrant should equal the moles of analyte at the equilibrium point, copy these values into the row of the data table marked “mol of analyte.”
Compute the concentration of HCl for all three trials using the formula molarity = mol / L.
Trial 1 (20.61 mL HCl):
0.121
M
Trial 2 (20.06 mL HCl):
0.125
M
Trial 3 (19.67 mL HCl):
0.122
M
Compute the average concentration (molarity) of HCl for all three trials:
0.123
M.
The true value was 0.120. What was your percent error?
2.5
%
Explanation:
We appreciate your time. Please come back anytime for the latest information and answers to your questions. Thank you for your visit. We're committed to providing you with the best information available. Return anytime for more. We're dedicated to helping you find the answers you need at Westonci.ca. Don't hesitate to return for more.