What is the molarity of 5.0 L of a solution containing 200. g of dissolved CaCO3?

2 Answers

justaguide's profile pic

justaguide | College Teacher | (Level 2) Distinguished Educator

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The molarity of a solution in which a particular compound is dissolved is defined as the number of moles of the compound dissolved per liter of the solution.

Here we have 5.0 L of solution which has 200 g of CaCO3 dissolved in it. The molar mass of CaCO3 is 100.0869 g/mol. This can be taken as 100 g/mol. approximately.

200 g of CaCO3 is 200/100 = 2 moles of CaCO3.

As the 2 moles of CaCO3 is dissolved in 5 L of the solution, the resulting molarity is given by 2/5 = 0.4 mol/liter.

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lochana2500 | Student, Undergraduate | (Level 1) Valedictorian

Posted on

caco₃100g → 1mol

caco₃200g → 2mol

the amount of moles = volume(ml)*molarity*10⁻³

(get Molarity as x)

2 = 5000*x*10⁻³

2 = 5x

x = 2/5

x = 0.4M

Molarity = 0.4M