CHE 106 Lecture Notes - Lecture 12: Barium Hydroxide, Sodium Hydroxide, Lithium Hydroxide

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Writing net ionic equations: write a balanced molecular equation, dissociate all strong electrolytes to write a complete ionic equation, write the net ionic equation with the species that remain by crossing out anything else. (cid:885)(cid:1840)(cid:2870)+(cid:884)(cid:1840)(cid:2871)(cid:1842)(cid:1841)(cid:2872) "(cid:1840)(cid:2871)(cid:1842)(cid:1841)(cid:2872)+6(cid:1840) Write strong electrolytes in forms of ions to obtain complete ionic equation, after you cancel spectator ions you will obtain your net equation. Acids: substances that produce hydrogen ions, h+ (protons), when dissolved in water: nitric acid ((cid:1840)(cid:1841)(cid:2871)) dissolves in water to give h+ and no3- Bases: substances that produce hydroxide ions, oh-, when dissolved in water. Acid serves as the species that donates a proton to another species in a proton-transfer. Involved the transfer of a proton from the acid to the base reaction. Base serves as the species that accepts the proton (h+) in a proton-transfer reaction. Water can be an acid or a base in certain reactions.

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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.

1. (10)What ions and/or molecules are present in relatively large proportions in a solution of a weak acid, HF (aq)? Select all appropriate answers. H+ HF F- HF+ F+ F2+ H2- F2- H F 2. (10)What ions and/or molecules are present in relatively large proportions in a solution of a strong base NaOH (aq)? Select all appropriate answers. NaOH Na2+ OH2- OH- NaO+ OH+ Na Na+ OH 3. (10)What ions and/or molecules are present in relatively large proportions in a solution of a strong acid HClO3 (aq)? Select all appropriate answers. HClO3 ClO3- HCl+ Cl+ H+ ClO3+ O3- O32- HCl None of these is present in relatively large proportions 4. (10)What ions and/or molecules are present in relatively large proportions in a solution of the soluble ionic compound NiCl2 (aq)? Select all appropriate answers. Ni2+ NiCl2 Cl22- Cl2- Ni+ Cl2- Ni Cl Cl2 Cl- 5. (5)Which of the following equations represents the proper net ionic equation for the precipitation of an insoluble sulfide compound from ZnBr2(aq) and Na2S(aq). Na2S(aq) + ZnBr2(aq) ----> 2 NaBr(aq) + ZnS(s) Zn2+(aq) + S2-(aq) ----> ZnS(s) Na2S(aq) + 2 Br-(aq) ----> 2 NaBr(s) + S2-(aq) Br-(aq) + Na+(aq) ----> NaBr(s) S2-(aq) + ZnBr2(aq) ----> ZnS(s) + 2 Br-(aq) 3 S2-(aq) + 2 Zn3+(aq) ----> Zn2S3(s) Na2+(aq) + Br2-(aq) ----> Na2Br2(s) Na2S(aq) + ZnBr2(aq) ----> Na2Br2(aq) + ZnS(s) Zn+(aq) + S-(aq) ----> ZnS(s) 6. (5)Which of the following equations represents the proper net ionic equation for the complete neutralization reaction between the strong acid HI(aq) and the weak base NH3(aq)? H+ (aq) + NH3(aq) ----> NH4+ (aq) HI (aq) + OH- (aq) ----> H2O (l) + I- (aq) HI (aq) + NH3(aq) ----> NH4I (aq) I- (aq) + NH4+ (aq) ----> NH4I (aq) H+ (aq) + OH- (aq) ----> H2O (l) HI (aq) + OH- (aq) ----> H2IO (aq) H+ (aq) + NH4+ (aq) ----> NH5+ (aq) I- (aq) + OH- (aq) ----> HIO (aq) mark 7. (5)What are the spectator ions in the solution after completely precipitating an insoluble carbonate compound when mixing Ca(ClO3)2 (aq) and Na2CO3 (aq)? Ca2+ , ClO3- , Na+ , and CO32- Na+ and CO32- CO32- and ClO3- CO32- and Ca2+ Ca2+ and ClO3- Ca2+ and Na+ Na+ ClO3- ClO3- and Na+ Ca2+ 8. (5)What are the spectator ions in the solution after the complete neutralization reaction occurs when mixing the weak acid H2S (aq) and the strong base KOH (aq)? H+ , S2- , K+ , and OH- OH- and K+ H+ and OH- OH- and S2- K+ and S2- K+ and H+ S2- and H+ K+ S2-

CHE 106 Lecture Notes - Lecture 12: Barium Hydroxide, Sodium Hydroxide, Lithium Hydroxide

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