# What is the average atomic mass of Titanium? Titanium has 5 isotopes: Ti-46 (8.0%) Ti-47(7.8%) Ti-48(73.4%) Ti-49(5.5%) Ti-50(5.3%)

##### 1 Answer

#### Explanation:

When the problem doesn't provide you with the *actual* **atomic mass** of an isotope, **mass number**,

In this case, you will have

#""^46"Ti " -> " "m_a ~~ "46 u"#

#""^47"Ti " -> " " m_a ~~ "47 u"#

#""^48"Ti " -> " " m_a ~~ "48 u"#

#""^49"Ti " -> " " m_a ~~ "49 u"#

#""^50"Ti " -> " " m_a ~~ "50 u"#

Now, the *average atomic mass* of titanium is calculated by taking the **weighted average** of the atomic masses of its stable isotopes.

Simply put, each isotope **in proportion** to its *decimal abundance*, which is simply the *percent abundance* divided by

#color(blue)(|bar(ul(color(white)(a/a)"avg. atomic mass" = sum_i m_"a i" xx "abundance of i"color(white)(a/a)|)))#

The *decimal abundances* for these five isotopes will be

#""^46"Ti: " 8.0/100 = 0.080#

#""^47"Ti: " 7.8/100 = 0.078#

#""^48"Ti: " 73.4/100 = 0.734#

#""^49"Ti: " 5.5/100 = 0.055#

#""^50"Ti: " 5.3/100 = 0.053#

The average atomic mass of titanium will thus be

#"avg. atomic mass " =#

#"46 u" xx 0.080 + "47 u" xx 0.078 + "48 u" xx 0.734 + "49 u" xx 0.055 + "50 u" xx 0.053#

#"avg. atomic mass " = color(green)(|bar(ul(color(white)(a/a)color(black)("47.923 u")color(white)(a/a)|)))#