Question
In: Chemistry
A chemist adds 370.0mL of a 1.41/molL potassium iodide KI solution to a reaction flask. Calculate...
A chemist adds 370.0mL of a 1.41/molL potassium iodide KI solution to a reaction flask. Calculate the millimoles of potassium iodide the chemist has added to the flask. Be sure your answer has the correct number of significant digits.
Solutions
Expert Solution
As we know moalrity of a solution is given by,
Molarity = No. of moles of substance / Volume of solution
Also, we are given
Volume of KI (Potassium Iodide) solution = 370 ml = 0.370 L (3 significant figures)
Molarity of KI solution = 1.41 mol / L (3 significant figures)
On substituting given values we get,
No. of moles of KI (Potassium Iodide) in solution = Volume * Molarity of Solution
No. of moles of KI (Potassium Iodide) in solution = (0.370 L) * (1.41 mol/L) = 0.5217 mol
No. of moles of KI = 0.5217 moles = 521.7 millimoles = 522 millimoles (rounded off to 3 significant figures)
NOTE : ( 1 mole = 1000 millimole)
queen_honey_blossom answered 2 years agoRelated Solutions
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