Question

What is the molarity of a solution prepared by dissolving 54.3 g of Calcium nitrate
into 355 mL of water?

Answer 1

Answer: 40 + 2x14 + 6x16 = 164g/mole

54.3g x [1mole / 164g] = 0.331moles

355mL x 1L / 1000mL = 0.355L

molarity = 0.331moles / 0.355L =

00

Explanation:

Answer 2

The molarity of a solution prepared by dissolving 54.3 g of Calcium nitrate  into 355 mL of water is 0.9881M

Molarity of solution is the ratio of the number of moles of the substance to the volume.

$Molarity=\frac{n}{V}$

• n is the number of moles of the compound

• $n=\frac{mass}{molar \ mass}$

• Mass of calcium nitrate = 54.3g

• Molar mass of calcium nitrate = Ca(NO₃)₂ = 164.088 g/mol

$n=\frac{54.3}{164.088 } \\n=0.331 moles$

Get the required molarity;

$Molarity=\frac{0.331}{0.335}\\Molarity= 0.9881 M$

Hence the molarity of a solution prepared by dissolving 54.3 g of Calcium nitrate  into 355 mL of water is 0.9881M

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