Question

While working in a pharmaceutical laboratory, you need to prepare 1.50 L of a 2.20-M NaCl solution. What mass of NaCl would be required to prepare this solution

Answer 1

193 grams of NaCl are needed to make 1.50 L of a 2.20-M NaCl solution.

Calculation of the mass of NaCl required:

The only thing we need to know is that a solution's molarity informs us of the exact amount of moles of solute that are contained in 1 L of a solution.

In this situation, a NaCl (sodium chloride) solution with a 2.20-M concentration will have 2.20 moles of the solute (sodium chloride) in every 1 L of the solution.

The solution's molarity of 2.20 M requires that every 1 L of this solution include 2.20 moles of sodium chloride, which implies that every 1.50 L of this solution needs to contain

$1.5 L solution .\frac{2.20 moles NaCl}{1L solution} = 3.30 moles NaCl$

Utilize the compound's molar mass to translate the amount of NaCl (sodium chloride) in moles to grams.

$3.30 moles NaCl . \frac{58.4 gm}{1 mole NaCl} = 192.7 gm$ ≈ 193 gm

Therefore it is concluded that the final answer is 193 gm.

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