The molarity of a solute in solution is defined to be the number of moles of solute per

Chapter 2, Problem 7

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The molarity of a solute in solution is defined to be the number of moles of solute per liter of solution \((\left(1 \text { mole }=6.02 \times 10^{23} \text { molecules }\right)\). If X is the molarity of a solution of magnesium chloride \(\left(\mathrm{MgCl}_{2}\right)\), and Y is the molarity of a solution of ferric chloride \(\left(\mathrm{FeCl}_{3}\right)\), the molarity of chloride ion \(\left(\mathrm{Cl}^{-}\right)\) in a solution made of equal parts of the solutions of

\(\mathrm{MgCl}_{2} \text { and } \mathrm{FeCl}_{3}\) is given by \(M=X+1.5 \mathrm{Y}\) . Assume that X has mean 0.125 and standard deviation 0.05, and that Y has mean 0.350 and standard deviation 0.10.

a. Find \(\mu_{M}\).

b. Assuming \(X \text { and } Y\) to be independent, find \(\sigma_{M}\)

Equation Transcription:

 

   

 

   

 

Text Transcription:

(1 mole=6.02 x 1023 molecules)  

(MgCl2)    

(FeCl3)  

(Cl -)  

MgCl2 and FeCl3

M=X+1.5Y

\mu_M  

X and Y

\sigma_M