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Butoxors [25]
3 years ago
6

A chemist adds of a M mercury(II) iodide solution to a reaction flask. Calculate the mass in milligrams of mercury(II) iodide th

e chemist has added to the flask. Round your answer to significant digits.
Chemistry
1 answer:
Oksi-84 [34.3K]3 years ago
7 0

Answer:

0.42 mg

Explanation:

It seems the question is incomplete, however I'll use values that have been found in a web search:

"A chemist adds 55.0 mL of a 1.7x10⁻⁵ M mercury(II) iodide solution to a reaction flask. Calculate the mass in milligrams of mercury(II) iodide the chemist has added to the flask. Round your answer to 2 significant digits."

<u>Keep in mind that while the process of solving the problem remains the same, if the values in your question are different, your answer will differ as well</u>.

First we <u>calculate the moles of mercury (II) iodide</u> (HgI₂):

  • 1.7x10⁻⁵M * 55.0 mL = 9.35x10⁻⁴ mmol HgI₂

Then we<u> convert mmol to mg, using the molar mass</u> (454.4 g/mol):

  • 9.35x10⁻⁴ mmol HgI₂* 454.4 mg/mmol = 0.42 mg
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Mass defect for oxygen-16 = 0. 13261 amu, in the kilograms the mass defect equals to 2.20 × 10⁻²⁸ kg.

<h3>What is mass defect?</h3>

Mass defect is the difference between the mass of of an whole atom and the combined mass of its individual particles present in that atom.

We know that, 1 amu = 1.6 × 10⁻²⁷ kg

Given that, mass defect for oxygen-16 = 0.13261 amu

To calculate this defect in terms of kilograms, we have to convert into kg unit as:

0.13261 amu = 0.13261 amu × 1.6 × 10⁻²⁷ kg/amu

0.13261 amu = 2.20 × 10⁻²⁸ kg

Hence option (2) is correct.

To know more about Mass defect, visit the below link:

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