Question

What is the molar concentration of Pb+ in a solution that contains 6.73 ppm of Pb(NO3)2?

Answer 1

The molar concentration of Pb+ in a solution that contains 6.73 ppm of Pb(NO3)2 is 2.031 × 10⁻⁵

The molar concentration refers to the molarity of a solution which can be defined as the number of moles of a compound that is present in the solution (usually a 1-liter solution)

Mathematically,

the number of moles = $\mathbf{\dfrac{mass}{molar \ volume }}$

From the information given:

• 6.73 ppm (part per million) = 6.3 mg     (since 1 ppm = 1 mg)
• the mass of 6.73 mg = 0.00673 g

Under standard conditions;

• the molar mass of Pb(NO3)2 = 331.22 g/mol

∴

The number of moles of Pb(NO3)2 = $\mathbf{\dfrac{0.00673 \ g}{331.22 \ g/mol}}$

The number of moles of Pb(NO3)2 = 2.031 × 10⁻⁵ mole

Now, the molarity(molar concentration) of the Pb+ in Pb(NO3)2 is:

$\mathbf{=\dfrac{2.305\times 10^{-5}}{1} }$

= 2.031 × 10⁻⁵

Therefore, we can conclude that the molar concentration of Pb+ in a solution that contains 6.73 ppm of Pb(NO3)2 is 2.031 × 10⁻⁵

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