Question

What is the molarity of a solution that contains 1000.0 mg of AgNO3 that has been dissolved in 500 mL of water

Answer 1

0.012moldm⁻³

Explanation:

Given parameters:

Mass of AgNO₃  = 1000mg

Volume of water = 500mL

Unknown:

Molarity of solution  = ?

Solution:

The molarity of a solution is the number of moles of a solute dissolved in volume of solvent.

 Molarity = $\frac{xnumber of moles}{Volume}$

 

Number of moles of AgNO₃  = ?

   Number of moles = $\frac{mass}{molar mass}$

Molar mass of AgNO₃ = 108 + 14 + 3(16) = 170g/mol

   convert mass to g;

      1000mg = 1g

 Number of moles  = $\frac{1}{170}$  = 0.00588moles

   convert the given volume to dm³;

       1000mL  = 1dm³;

        500mL = 0.5dm³

Now solve;

  Molarity = $\frac{0.00588}{0.5}$  = 0.012moldm⁻³

learn more:

Molarity brainly.com/question/9324116

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