CHM 111 Lecture Notes - Lecture 11: Hydrochloric Acid, Oxyanion, Potassium Hydroxide

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CHM 111 Full Course Notes

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Recall that the strength of an electrolyte is determined by the extent of its dissociation into component ions in solution. A strong electrolyte completely dissociates into ions in solution whereas a weak electrolyte only partially dissociates, strong and weak acids are defined accordingly. A strong acid completely ionizes in solution whereas a weak acid only partially ionizes. In any case, here are some of the strongest acids: Nitric acid (hno3) sulfuric acid (h2so4) chloric acid (hclo3) perchloric acid (hclo4) Hydrochloric acid (hcl) hydrobromic acid (hbr) hydroiodic acid (hi) By analogy, a strong base is a base that completely dissociates in solution. The extent then, of the ionization of a base can be quantified with the base ionization constant, kb. Some of the strongest bases worth noting are: Sodium hydroxide (naoh) -> lye potassium hydroxide (koh) barium hydroxide [ba(oh)2] Binary acids are composed of hydrogen and a nonmetal and, in nomenclature, take the form:

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Part A A fuel cell differs from a battery because the current is being generated from a reduction-oxidation (redox) reaction in which the reactant is consumed. A classic example of a fuel cell is the phosphoric acid fuel cell (PAFC), which have been used in stationary power generators, buses, and even submarines. Fuel cells require an electrolyte (similar to batteries) to carry electrically charged species between the electrodes, and a PAFC utilizes phosphoric acid (H3PO4) as its electrolyte. Phosphoric acid has three acidic protons that can dissociate in water, as highlighted in red here: H3PO4. However, it is considered a weak acid because some of the acid will remain in molecular form when dissolved in water. Write the complete ionic equation that depicts the dissociation of the first proton for the weak acid phosphoric acid (H3PO4). Make certain you include all charges for any ions produced. Express you answer as a chemical equation including phases. Titrations as analytical neutralization reactions Neutralization reactions can occur between any combination of weak/strong acids and bases. When we want to determine the concentration of a base in solution, we can apply the concept of neutralization by reacting the base with a known amount of an acid in the presence of an indicator (a compound that changes color depending on the pH). This method of determining the concentration of a base is called acid-base titration, and it can also be used to determine the concentration of an acid by titrating it with a known amount of base. A common acid to use for titrations is potassium hydrogen phthalate (written as KHP or KHPh; do not confuse the P for phosphorus). The reason KHP is common is because it is solid at room temperature, and we can accurately mass the amount that is added to solution. As a soluble salt, KHP completely dissociates to form a potassium ion (K+) and an acidic hydrogen phthalate ion (HPâ), which is a weak acid that has only one acidic hydrogen. This ionization is depicted below. KHP(s) â K+(aq)+HPâ(aq) Although ionization (the formation of ions) occurs as a result of acid dissociation for most weak acids, KHP ionizes before acid dissociation occurs. In other words, HPâ is a weak acid ion. Part C If you wanted to determine how much KOH (potassium hydroxide; a strong base) was dissolved in water, you could titrate it with a known amount of KHP (potassium hydrogen phthalate; a weak acid) until a color change indicates that the base is completely neutralized. The molecular equation below depicts this neutralization reaction. KHP(aq)+KOH(aq)âK2P(aq)+H2O(l) Write the net ionic equation that depicts the neutralization of the base by potassium hydrogen phthalate. Instead of using the entire chemical formula of phthalate, use HPâ to represent the acidic hydrogen phthalate ion and P2â to represent the phthalate ion. Express your answer as a net ionic equation including phases.

CHM 111 Lecture Notes - Lecture 11: Hydrochloric Acid, Oxyanion, Potassium Hydroxide

CHM 111 Full Course Notes

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