Chem 2222 Study Guide Study Guide for Chem 2222 Introductory Quantitative Analysis Part 3. Neutralization Titrations. Linked documents are in various formats, including HTML, Microsoft PowerPoint (ppt), Adobe Acrobat (pdf), Microsoft Excel (xls), and Mathsoft Mathcad (mcd).
Go to the page to download free software to view ppt and pdf files. Mathcad files can be accessed using some computers on campus (Engr 204 full access). Chapters 8, 9, 10, 12 (selected sections) In this unit we first take up titrations of monoprotic acids and bases (parts of Ch 10). The material in Ch 8 (covered earlier) provides useful reference to the equilibrium treatments involved.
Next we examine polyprotic acid-base equiilibria (Ch 9) and titrations (parts of Ch 10). All of this will be followed by examination of selected applications (Ch 10) and advanced topics in chemical equilibrium (Ch 12).
Study Guide Acid Base And Titrations Answers
Topic Lecture Notes and Reference Materials Reading/Study Assignment 3A Neutralization Titrations of Monoprotic Acids and Bases. General features of acid-base titration curves.
Acid-base indicators. Locating endpoints in potentiometric titrations. Review materials on monoprotic acid-base equilibria:.
Review Notes:. Worked Examples: Ch 8.
Acid Base Titration Method
Monoprotic acid-base equilibria (covered earlier, review as needed). Please see the following sections dealing with titrations of monoprotic systems and related topics. Strong acid + strong base. 10.2. Weak acid + strong base. 10.3.
Weak base + strong acid. 10.5.
Potentiometric endpoint. 10.6. Visual endpoint and indicators. 10.7. Practical notes. 10.10. Calculation of titration curves using spreadsheets Ch 10, exercises A-C, E-H, I(a), and J.
Suggested problems from Ch 10:. Set A (monoprotic acids and bases): #1, 3, 4, 7, 8, 12, 13, 18. Set B (potentiometric endpoints, indicators): #35, 36, 38, 40 Extras. (requires Mathcad) Goal Seek and Equilibrium Calculations. You can use Excel Goal Seek for solving equilibrium problems that when an algebraic solution is complicated.
See examples in Harris Ch 7.5 and 8.5, or view a that used Goal Seek to compute the pH of a dilute buffer solution. Titration of strong acids and weak acids. Effect of Ka on titration curves. Titration of weak bases, buffer systems.
Neutalization Titations III. 580 super l service manual. A Comparison of Computational Approaches (covered in Unit 2). 3B Titrations of Polyprotic Acids and Bases. Ch 9, 10 Titration of Polyfunctional Acids and Bases I.
Titration of phosphoric acid, sodium carbonate.Titration of Polyfunctional Acids and Bases II. Titration curves for mixtures. Polyprotic acid-base equilibria, all sections. Exercises A-H.
Suggested problems: #3, 4, 14, 19, 20, 24, 25, 28, 29. Ch 10, section 10.4, Titrations in diprotic systems Exercise D. Suggested problems: #21, 27. Problem Set 6, Part B.
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3C Applications and Advanced Topics Titration of sodium carbonate; Kjeldahl method for nitrogen. Ch 10, sections 10.4 (diprotic systems) and 10.8 (Kjeldahl method for ntirogen). Suggested problems: #45, 48, 52, 54, 58.
Effect of pH on Solubility Ch 12, section 12.3. (Not included on Exam 3).
Titration is the quantitative technique, where the concentration of the unknown is determined to form a known concentration. Titration is useful to determine the concentration of either unknown acid or base. Acid-base titration can be further classified into four types, Strong acid-strong base Weak acid-weak base Strong acid-weak base Strong base-weak acid Titration consists of an unknown acid or base. There are different methods used to measure the completion of acid-base reaction, such as pH indicator, conductance, potentiometer, color change, and precipitation. Strong acid vs Strong base titration Strong acid (inorganic acids) and Strong base react together to give salt in the form of a precipitate. This reaction occurs in stoichiometric, which means that each mole of strong acid reacts with each mole strong base by forming salt. The equivalent point of the reaction is the endpoint of the reaction.
Example: Here the strong acid is the hydrochloric acid and the strong base is the sodium hydroxide, which react together forming sodium chloride salt. Strong acid vs Weak base Titration between strong acid (inorganic acids) and weak bases like ammonium hydroxide. Since the titration involves strong acid and weak base, the titration curve is predominantly acidic (see fig). Example: Since, the titration involves ammonium hydroxide, a weak base, ammonium chloride is acidic in nature.
Weak acid vs Strong base Titration of weak acid and strong base forming salt and water. Here the salt formed is slightly basic due to the presence of strong base. Example: H 2CO 3 is a weak acid and NaOH is a strong base forming a basic salt sodium carbonate. Weak acid vs weak base Since, this titration involves acid as well as bases which are weak, resulting solution will be neutral. At the end point pH is neutral that is pH of the solution is 7 Example: Since, both acid and base are weak; the resultant salt ammonium hydroxide will be neutral in nature. Graphical representation of titration curves.
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Perhaps no two classes of compounds are more important in chemistry than acids and bases. All acids have several properties in common: They have a sour taste, and they all react with most metals to form hydrogen gas (H 2) and with baking soda to form carbon dioxide (CO 2). All acids turn blue litmus paper red, and their solutions conduct electricity because acids form ions when dissolved in water.
All bases also share several common properties: They have a bitter taste; their solutions feel slippery like soapy water; and they turn red litmus paper blue (the opposite of acids). Solutions of bases also conduct electricity because they, too, form ions in water. Acids are similar because they produce a hydronium ion, H 3O + ( aq), in water.
Bases, on the other hand, all form a hydroxide ion, OH –( aq), in water. These ions are responsible for the properties of acids and bases. The pH scale was developed to express, in a convenient way, the concentration of hydrogen ion in solutions and is widely used when discussing acids and bases. In the late 1800s, Svante Arrhenius defined an acid as a substance that increases the hydronium ion (H 3O +) concentration in water, and a base as any substance that increases the hydroxide ion (OH –) concentration in water. Acids and bases react with one another in a process called neutralization to form a salt and water.
Shimano nexus gear shifter user manual. Hydrochloric acid neutralizes potassium hydroxide forming potassium chloride (a salt) and water.