All the equations where the reactants and products are shown as molecules with complete chemical formulas are called molecular equations. This, essentially, is what we use for most reactions. For example: 2K3PO4(aq) + 3BaCl2(aq) → Ba3(PO4)2(s) + 6KCl(aq) However, we … Read more
Before talking about electrolytes, let’s formulate the concept of solutions. A solution is a homogeneous mixture of two or more substances. The substance present in the greatest quantity is called the solvent, and the other substance(s) is called solute(s). The … Read more
The oxidation state (or oxidation number) is assigned to each atom in a compound as an indicator of whether the atom is neutral, electron-rich, or electron-poor. The general principle is that the more electronegative atom pulls the electron density of … Read more
In the previous post, we talked about the definition of acids and bases according to the Arrhenius, Brønsted–Lowry, and Lewis acid-base theories. Refresh these concepts if you need to, but most often, you are going to identify acids as compounds … Read more
In a precipitation reaction, an insoluble product is formed which is called a precipitate. Precipitation reactions usually involve ionic compounds. For example, when an aqueous solution of sodium chromate (Na2CrO4) is added to an aqueous solution of silver nitrate (AgNO3), a dark orange … Read more
In the previous post, we talked about molarity which is the ratio of the moles of solute over the volume of the solution. For example, if we dissolve 43.6 g K2SO4 in 1 L of water, the molarity of the … Read more
Water-soluble ionic compounds such as acids, bases, and salts dissociate in water forming ions. For example, sodium chloride (NaCl) dissociates into Na+ and Cl– ions when dissolved in water: NaCl(aq) → Na+(aq) + Cl–(aq) The “aq” notation indicates that the salt is water-soluble, … Read more
