Question

Suppose you need to prepare 1.0 L of Stock solution which must have a concentration of...

Suppose you need to prepare 1.0 L of Stock solution which must have a concentration of 150 mg N/L. You start with solid Potassium Nitrate, KNO3 .

A. How many moles of Nitrogen should 1.0 L of Stock solution contain?

B. How many moles of KNO3 should 1.0 L of stock solution contain?

C. Please show working. How many grams of KNO3 will you have to weigh out to prepare 1.0 L of stock solution? (Show ALL work!) (Reminder: the concentration of stock must be known to 3 significant figures!)

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Homework Answers

Answer #1

A) We calculate the moles of Nitrogen.

- Calculating how much milligrams are present in 1.0 L of stock solution.

- Converting milligrams into grams.

- Calculating moles of Nitrogen present in the solution: with grams of Nitrogen (0.150 g) and the Molar Mass of Nitrogen (14.0067 g).

B) Calculate the moles of KNO3 present in 1.0 L of stock solution.

- Since 1 mol of Nitrogen is equivalent to 1 mol of KNO3, we say that the moles calculated in part A are equivalent to moles of KNO3.

C) Grams of KNO3 needed to make 1.0 L of stock solution.

- With the moles of KNO3 calculated in part B and the Molar Mass of KNO3 (101.1635 g), we calculate the grams of KNO3 needed to make the stock solution.

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