Final answer:
The unit of measure for ionic charges in a solution is called an equivalent (Eq), which helps calculate the electrochemical cell potentials. Cell potentials measure the solubility products and concentrations of solutions. The concentration is expressed as molarity, the number of moles of solute per liter of solution.
Step-by-step explanation:
The unit measuring the number of ionic charges or electrocovalent bonds in a solution is known as equivalent, officially abbreviated as Equiv, but commonly abbreviated as Eq. This unit provides a measure of reactivity of a particular electrolyte solution. One equivalent equals 1 mol of positive or negative charge. Thus, a 1 mol/L solution of Na+(aq) is also 1 Eq/L because sodium has a 1+ charge, whereas a 1 mol/L solution of Ca2+(aq) ions is 2 Eq/L.
Using cell potentials and electrochemistry is a sensitive method to determine the solubility products (Ksp) of sparingly soluble substances and concentrations of very dilute solutions. The standard cell potential (E°cell), measured under standard conditions, serves as a basis for comparing potentials, directing electrochemical reactions, and measuring solubility. A potential reflects the driving force for the charge transfer process in electrochemistry, such as the transfer of electrons between redox reactants.
The concentration is another important term and refers to the quantitative measure of the relative amounts of solute and solvent present in a solution. Concentrations are often expressed in molarity, which describes the number of moles of a substance per liter of solution and indicated as mol/L.