Molarity Calculation for a PbNO3 Solution

What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL?

The molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL is:

a) 3.13 mol/L

b) 6.26 mol/L

c) 0.783 mol/L

Answer:

The correct molarity of the solution is 3.13 mol/L.

Molarity is a crucial concept in chemistry that refers to the concentration of a solution. It is defined as the number of moles of solute dissolved in one liter of solution. In this case, the molarity of a solution containing 1.565 moles of PbNO3 in 500 mL is calculated to be 3.13 mol/L.

The formula to calculate molarity is:

Molarity = Number of moles / Volume of solution in liters

In this scenario, the volume of the solution is 0.5 L (500 mL = 0.5 L) and the number of moles of PbNO3 is 1.565. By substituting these values into the formula, we get:

Molarity = 1.565 moles / 0.5 L = 3.13 mol/L

Therefore, the molarity of the solution made by adding 1.565 moles of PbNO3 to 500 mL is 3.13 mol/L. This calculation is important in various fields like biochemistry, where accurate concentrations of solutions are needed for experiments and research.