Calculate the mass of KI in grams required to prepare 5.00 X10^2 mL of a 2.80 M solution

2 answers:

3 0

Volume in liters:

5.00x10² mL / 1000 => 0.5 L

Molar mass of KI => 166.0028 g/mol

Calculating mass of KI = volume x molar mass x molarity

Mass of KI = 0.5 x 166.0028 x 2.80

= 232.40392 g of KI

I hope this is helpful!

Alekssandra [3K]3 months ago

3 0

Explanation:

Molarity refers to moles per liter of solution, while the number of moles is defined as mass divided by molar mass.

Consequently, Molarity = $\frac{mass}{molar mass \times volume of solution}$

Given that the molarity is 2.80 M, the volume is 500 mL or 0.5 L, and the molar mass of KI is 166 g/mol.

Thus, mass = $Molarity \times molar mass \times volume of solution}$

= $2.80 mol/L \times 166 g/mol \times 0.5 L$

= 232.4 g

Therefore, the mass of KI required to prepare 5.00 X10^2 mL of a 2.80 M solution is 232.4 g.

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The production of NOx gases is an unwanted side reaction of the main engine combustion process that turns octane, C8H18, into CO

lorasvet [2795]

Answer:

710.33 g NO2

Explanation:

2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

(800 g octane) / (114.2293 g C8H18/mol x (25/2)) = 87.54 mol O2 utilized for combusting octane

$87.54 mol O2 x \frac{15}{85}$ = 15.44 mol O2 used for generating NO2

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4 0

3 months ago

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