Question

calculate the volume in liters of a ( 8.61\times10^{-4} ) mm copper(ii) fluoride solution that contains 900. mg of copper(ii) fluoride ( (\text{cuf}_2) ). be sure your answer has the correct number of significant digits.

Explanation:

Step1: Calculate the molar mass of \(CuF_2\)

The molar mass of \(Cu\) is \(63.55\space g/mol\), and the molar mass of \(F\) is \(19.00\space g/mol\).
For \(CuF_2\), \(M = 63.55+(2\times19.00)=101.55\space g/mol\)

Step2: Convert the mass of \(CuF_2\) to moles

Given \(m = 900.\space mg=0.900\space g\)
Using \(n=\frac{m}{M}\), \(n=\frac{0.900\space g}{101.55\space g/mol}\approx8.86\times 10^{-3}\space mol\)

Step3: Convert the concentration from \(mM\) to \(M\)

Given \(C = 8.61\times 10^{-4}\space mM\)
Since \(1\space mM = 10^{- 3}\space M\), \(C=8.61\times 10^{-7}\space M\)

Step4: Calculate the volume using \(V=\frac{n}{C}\)

\(V=\frac{8.86\times 10^{-3}\space mol}{8.61\times 10^{-7}\space mol/L}\approx1.03\times 10^{4}\space L\)

Answer:

\(1.03\times 10^{4}\space L\)