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CHE 106 Lecture Notes - Lecture 10: Molar Concentration, Acid Strength, Oxidizing Agent

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School
Syracuse University
Department
Chemistry
Course
CHE 106
Professor
J.French

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CHE 106 Full Course Notes
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CHE 106 Full Course Notes
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Document Summary

Acids : anything that can donate a proton (h+) when associated in a solution. Bases : anything that generates (oh-) in solution (accept protons) The h+ (aq) ions made by acids quickly associate with water molecules to form. Strong acid : an acid that dissociates completely in solution. Weak base : only partially dissociate in solution. When you write an ionic eq. , ions. Neutralization reactions : a reaction between an acid and a base, resulting in the equations formation of a salt (and sometimes water) Strong acid / strong base reaction (example) : : h + (aq) + cl - (aq) + k + (aq) + oh - (aq) k + (aq) + cl - (aq) + h 2 o(l) Hcn(aq) + k+ (aq) kcn (aq) + h2o(l) Ionic: hcn(aq)+ k + (aq) + oh - (aq) k + (aq) + cn - (aq) + h 2 o(l) Carbonates and bicarbonates don"t produce the expected metathesis products.

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Related Questions


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 (HP−), which is a weak acid that has only one acidic hydrogen. This ionization is depicted below. KHP(s) → K+(aq)+HP−(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, HP− 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)→K2P(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 HP− to represent the acidic hydrogen phthalate ion and P2− to represent the phthalate ion. Express your answer as a net ionic equation including phases.

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