126k views
0 votes
An empty weighing dish has a mass of 1.0041 ± 0.0002 g. After you add dried sodium chloride to the dish, the mass is 3.2933 ± 0.0002 g. You quantitatively transfer the sodium chloride into a 500.00 ± 0.05 mL volumetric flask and dilute to the mark with deionized water. The molar mass of sodium chloride is 58.440 g/mol. What is the absolute error in the concentration of the resulting solution? Report your answer normally to the correct number of significant figures with the correct unit.

User Mouhamed
by
8.0k points

1 Answer

3 votes

Answer:

The correct answer to the following question will be "0.0013%".

Step-by-step explanation:

The given values are:

Weight of an empty dish = 1.0041 ± 0.0002 g

Weight of dish + sodium chloride (NaCl) = 3.2933 ± 0.0002 g

Weight of NaCl = 2.2892 ± 0.0002 g

Now,

Volume of the solution = 500.00 ± 0.05 ± 0.0002

= 500.00 ± 0.0502 ml

So,

Molarity =
(W \ NaCl)/(M \ NaCl) * (1000)/(Volumes \ of \ solution)

On putting the values in the above formula, we get

=
((2.2892\addeq +0.0002))/(58.440)* (1050)/((500.00+0.0502))

= (
3.917 ±
0.0002) × (
2 ±
0.0502)

= (
0.7834 ±
.00001004)

Now,

Absolute error =
(0.00001004)/(0.7834)* 100

=
0.0013%

User Rfrittelli
by
7.6k points

Related questions

asked Sep 15, 2024 107k views
Chayan Ghosh asked Sep 15, 2024
by Chayan Ghosh
8.1k points
1 answer
2 votes
107k views
asked Jun 8, 2022 181k views
Chip Hogg asked Jun 8, 2022
by Chip Hogg
8.5k points
1 answer
1 vote
181k views