There are approximately of formula units in that of (the solute of this solution.)
Explanation:
A solution includes two substances: the solute and the solvent. Note the solution here contains significantly more water than . Hence, assume that water is the solvent (as it is in many other solutions.)
The (molar) formula mass of is necessary for finding the number of moles of
One atom,
One atom, and
One atom.
The formula mass of will thus be the sum of:
The mass of one mole of atoms,
The mass of one mole of atoms, and
The mass of one mole of atoms.
On the other hand, the mass (in grams) of one mole of atoms of an element is (numerically) the same as its relative atomic mass. The relative atomic mass data can be found on most modern periodic tables.
Relative atomic mass data from a modern periodic table:
: .
: .
: .
For example, the relative atomic mass of (potassium, atomic number ) is (3 sig. fig.) Hence, the mass of one mole of
The formula mass of is the sum of these three masses:
.
The number of moles of formula units in this sample would be:
In solution, before the reaction, the ions are Cu²⁺ and Cl⁻. The addition of NaOH (Na⁺ + OH⁻) produce the precipitation of Cu²⁺ forming Cu(OH)₂(s). When you reach the equivalence point, there is no Cu²⁺ because precipitates completely. All OH⁻ ions reacts when are added but when Cu²⁺ is finished, excess OH⁻ ions still in solution helping to detect the equivalence point.
Thus, ions present after the equivalence point are:<em> Cl⁻, Na⁺</em> (Don't react, spectator ions), and <em>OH⁻</em>.