Question 10.12: A typical concentration of Cl^- in blood is 106 mEq/L. At th......
A typical concentration of Cl^{-} in blood is 106 mEq/L. At this concentration, how many moles of Cl^{-} ion are present in 1.00 L of blood?
Step 1: The given quantity is 1.00 L of blood and the desired quantity is moles of Cl^{-} ion.
1.00 L blood = ? moles Cl^{-}ion
Step 2: The pathway for solving the problem is
\boxed{L \ blood}\longrightarrow \boxed{mEq \ Cl^{-}}\longrightarrow \boxed{Eq \ Cl^{-}}\longrightarrow \boxed{moles \ Cl^{-}}
The mathematical setup, using dimensional analysis and conversion factors (Chapter 2), is
1.00 \ \cancel{L \ blood}\times \frac{106 \ \cancel{mEq \ Cl^{-}}}{1 \ \cancel{L \ blood}} \times \frac{10^{-3} \cancel{ Eq \ Cl^{-}}}{1 \ \cancel{mEq \ Cl^{-}}}\times \frac{1 \ \ mole \ Cl^{-}}{1 \ \cancel{Eq \ Cl^{-}}}
= 0.106 mole Cl^{-} ion
The first conversion factor in the setup is the given concentration of Cl^{-}. The second conversion factor effects the change from mEq to Eq units and the final conversion factor effects the change from Eq to moles. This final factor comes from the definition for an