Question

Express the result, taking into account the following:

A three significant figures

With the right unit

1) 50.0 mL of a solution contains 0.0285 moles of AgNO3. Calculate Molarity for a solution

2) A sample of 0.00116 moles of NaCl is placed in a volumetric flask and water is added to dissolve it up to 25.0 mL. Calculate the Molarity of the solution.

3) Determine the molarity for a NaCl solution, whose volume is 0.01006 L and the amount of moles is 0.00164 moles.

4) 0.018 moles of H2SO4 is dissolved in enough water to have 0.100 L of solution. What is the Molarity of H2SO4 in solution?

Answer 1

1)

We know that, Molarity = No. of moles of solute / volume of solution in L

[ AgNO₃ ] = No. of moles of AgNO₃ / volume of solution in L

[ AgNO₃ ] = 0.0285 mol / 0.0500 L

[ AgNO₃ ] = 0.570 M

ANSWER :  [ AgNO₃ ] = 0.570 M

2)

We have, [ NaCl ] = No. of moles of NaCl / volume of solution in L

[ NaCl ] = 0.00116 mol / 0.0250 L

[ NaCl ] = 0.0464 M

ANSWER :  [ NaCl ] = 0.0464 M

3)

We have, [ NaCl ] = No. of moles of NaCl / volume of solution in L

[ NaCl ] = 0.00164 mol / 0.01006 L

[ NaCl ] = 0.163 M

ANSWER :  [ NaCl ] = 0.163 M

4)

We know that, Molarity = No. of moles of solute / volume of solution in L

[ H₂SO₄  ] = No. of moles of H₂SO₄ / volume of solution in L

[ H₂SO₄  ] = 0.018 mol / 0.100 L

[ H₂SO₄  ] = 0.180 M

ANSWER : [ H₂SO₄  ] = 0.180 M