Suppose you have 4.75 g of powdered magnesium metal, 1.10L of 2.00 M potassium n

Question

Suppose you have 4.75g of powdered magnesium metal, 1.10L of 2.00M potassium nitrate solution, and 1.10L of 2.00M silver nitrate solution.
(a) Which one of the solutions will react with the magnesium powder?
(b) What is the net ionic equation that describes this reaction? Express your answer as a chemical equation. Identify all of the phases in your answer.

(c) What volume of solution is needed to completely react with the magnesium?

(d) What is the molarity of the Mg 2+ ions in the resulting solution?

Explanation / Answer

(a)

magnesium reacts with silver nitrate

it does not react with sodium nitrate because sodium in more elctropositive than magnesium

(b)

mg +2agno3 - > 2ag + mg2+ + 2no3-

(c)

moles of mg = 4.75/24 = 0.198 which needs 0.396 moles of silver nitrate

volume = moles/molarity = 0.396/2 = 198 ml or 0.198 l

(d)

molarity of in resulting solution = half molarity of silver nitrate = 1.0

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