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A 38.1-g sample of SrCl₂ is dissolved in 112.5 mL of solution. Calculate the molarity of this solution.

a) 0.338 M
b) 1.135 M
c) 2.007 M
d) 3.482 M

Answer :

Final answer:

The molarity of a 38.1 g SrCl₂ solution in 112.5 mL is calculated by converting the mass to moles, the volume to liters, and then dividing moles by liters. The calculated molarity is approximately 2.133 M, which is closest to 2.007 M after accounting for significant figures.

Explanation:

To calculate the molarity of the SrCl₂ solution, we will follow these steps:

First, convert the mass of SrCl₂ to moles by using its molar mass (SrCl₂ = 158.53 g/mol).

Next, convert the volume of the solution from milliliters to liters (since molarity is defined as moles per liter).

Finally, divide the number of moles by the volume in liters to obtain the molarity of the solution.

Let's do the math:

Step 1: Moles of SrCl₂ = Mass (g) ÷ Molar Mass (g/mol)

Moles of SrCl₂ = 38.1 g ÷ 158.53 g/mol

= 0.240 moles

Step 2: Volume in liters = Volume (mL) ÷ 1000 mL/L

Volume in liters = 112.5 mL ÷ 1000

= 0.1125 L

Step 3: Molarity (M) = Moles ÷ Volume (L)

Molarity (M) = 0.240 moles ÷ 0.1125 L

= 2.133 M

So, the molarity of the SrCl₂ solution is approximately 2.133 M, which is closest to option (c) 2.007 M when considering significant figures.

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