It runs from 0 to 14. (A)
It is based off the -log [H+] where [H+] is the concentration of the Hydrogen ions.
The molar mass should be 14.898g/mol.
I used the equation 100gx(1/xg/mol)x(1mol/2mol)x(16g/mol+x)/1)=103.7 and solve for x.
I found that equation using stoichiometry and the equation 2m+1/2O2-->m2O
The molar mass of the metal I set to x and the molar mass of the metal oxide is 16+x.
The photos for the reaction arent here so ill insert them below