What is the average atomic mass of titanium if we have an isotopic distribution of #78.5%# of #""^46Ti#, #45.95263*"amu"#, #12.3%# of #""^48Ti#, #47.94795*"amu"#, and #""^50Ti#, #49.94479*"amu"#?

Question

Caleb Adams · Accepted Answer

This is simply the WEIGHTED AVERAGE of the individual isotopes.....I gets approx. #46.6*"amu"#.

#"Atomic mass of titanium"={0.785xx45.95263+0.123xx47.94795+0.092xx49.94479}*"amu"=??# Does this compare to what's on this planet?

Wyatt Adkins · Answer

undefined The formula to determine the average atomic mass of titanium is: Average atomic mass = (% abundance of isotope 1 × atomic mass of isotope 1) + (% abundance of isotope 2 × atomic mass of isotope 2) + (% abundance of isotope 3 × atomic mass of isotope 3) +...
 Entering the values: Average atomic mass = (78.5% × 45.95263) + (12.3% × 47.94795) + (9.2% × 49.94479)
 Average atomic mass = (0.785 × 45.95263) + (0.123 × 47.94795) + (0.092 × 49.94479)
 Average atomic mass = 36.10197655 + 5.89643785 + 4.59505748
 Average atomic mass = 46.59347188 amu