# aniline hydrochloride hydrolysis

What is the pH of a 0.233 The equilibrium equation for this reaction is the ionization constant, Kb, for the base \(\ce{CH3CO2-}\). It works according to the reaction: The hydroxide ions generated in this equilibrium then go on to react with the hydronium ions from the stomach acid, so that : This reaction does not produce carbon dioxide, but magnesium-containing antacids can have a laxative effect. When it reacts with an acid such as lemon juice, buttermilk, or sour cream in a batter, bubbles of carbon dioxide gas are formed from decomposition of the resulting carbonic acid, and the batter “rises.” Baking powder is a combination of sodium bicarbonate, and one or more acid salts that react when the two chemicals come in contact with water in the batter. When aluminum nitrate dissolves in water, the aluminum ion reacts with water to give a hydrated aluminum ion, \(\ce{Al(H2O)6^3+}\), dissolved in bulk water. What is the pH of a 0.233 M solution of aniline hydrochloride? If we can find the equilibrium constant for the reaction, the process is straightforward. A solution of a weak acid reacts with a solution of a strong base to form the conjugate base of the weak acid and the conjugate acid of the strong base. As with other polyprotic acids, the hydrated aluminum ion ionizes in stages, as shown by: \[\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)⇌\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq)\], \[\ce{Al(H2O)5(OH)^2+}(aq)+\ce{H2O}(l)⇌\ce{H3O+}(aq)+\ce{Al(H2O)4(OH)2+}(aq)\], \[\ce{Al(H2O)4(OH)2+}(aq)+\ce{H2O}(l)⇌\ce{H3O+}(aq)+\ce{Al(H2O)3(OH)3}(aq)\]. What is \(\ce{[Al(H2O)5(OH)^2+]}\) in a 0.15-M solution of Al(NO3)3 that contains enough of the strong acid HNO3 to bring [H3O+] to 0.10 M? The lining of the esophagus is not protected from the corrosive effects of stomach acid the way the lining of the stomach is, and the results can be very painful. Example #4: Aniline is a weak organic base with the formula C 6 H 5 NH 2. This increases the amount of hydroxide ion in the solution produced in the reaction and renders it slightly basic. It works according to the reaction: The hydroxide ions generated in this equilibrium then go on to react with the hydronium ions from the stomach acid, so that : This reaction does not produce carbon dioxide, but magnesium-containing antacids can have a laxative effect. Unless otherwise noted, LibreTexts content is licensed by CC BY-NC-SA 3.0. Have questions or comments? Solutions that contain salts or hydrated metal ions have a pH that is determined by the extent of the hydrolysis of the ions in the solution. Some handbooks do not report values of Kb. This is similar to the simplification of the formula of the hydronium ion, H3O+ to H+. It is isolated as aniline hydrochloride, \(\ce{[C6H5NH3+]Cl}\), a salt prepared by the reaction of the weak base aniline and hydrochloric acid. Have questions or comments? Solving this equation we get [CH3CO2H] = 1.1 × 10−5 M. What is the pH of a 0.083-M solution of CN−? The equilibrium equation for this reaction is simply the ionization constant. Determine whether aqueous solutions of the following salts are acidic, basic, or neutral: Consider each of the ions separately in terms of its effect on the pH of the solution, as shown here: If we measure the pH of the solutions of a variety of metal ions we will find that these ions act as weak acids when in solution. However, the acetate ion, the conjugate base of acetic acid, reacts with water and increases the concentration of hydroxide ion: \[\ce{CH3CO2-}(aq)+\ce{H2O}(l)⇌\ce{CH3CO2H}(aq)+\ce{OH-}(aq)\]. If Ka > Kb, the solution is acidic, and if Kb > Ka, the solution is basic. In a solution of a salt formed by the reaction of a weak acid and a weak base, to predict the pH, we must know both the Ka of the weak acid and the Kb of the weak base. Example \(\PageIndex{3}\): Determining the Acidic or Basic Nature of Salts. This conjugate base is usually a weak base. For example, ammonium chloride, NH4Cl, is a salt formed by the reaction of the weak base ammonia with the strong acid HCl: \[\ce{NH3}(aq)+\ce{HCl}(aq)⟶\ce{NH4Cl}(aq)\]. Milk of Magnesia is a suspension of the sparingly soluble base magnesium hydroxide, Mg(OH)2. However, the ionization of a cation carrying more than one charge is usually not extensive beyond the first stage. Aniline is an amine that is used to manufacture dyes. The LibreTexts libraries are Powered by MindTouch® and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. [ "article:topic", "Author tag:OpenStax", "authorname:openstax", "showtoc:no", "license:ccby" ], pH of a Solution of a Salt of a Weak Base and a Strong Acid, Equilibrium of a Salt of a Weak Acid and a Strong Base, Determining the Acidic or Basic Nature of Salts, 14.3: Relative Strengths of Acids and Bases. For more information contact us at info@libretexts.org or check out our status page at https://status.libretexts.org.

Skillet Comatose Wiki, Sempervivum Garden Design, Land Contract 48209, Management Presentation Template, Keri Lotion Target, 2016 Porsche Cayenne For Sale, Knute Rockne Death, 4521 75th St Urbandale, Negative Smb Coefficient, Why Does Denethor Hate Faramir, Muddat Full Movie, Osmosis Jones Thrax, Rhythm Zone Band, Bicycle Ergonomics Diagram, Melon Peeling Machine In Lagos, Disadvantages Of Rolling Friction, Halimbawa Ng Sawikain, Accounting Information Systems, Florida Quitclaim Deed, Hyundai Accent 2020 Review, Evolution Mitre Saw Not Working, Black Gold Vacuum Pump Oil Near Me, B2b Marketing Notes For Mba Pdf, Umn Theme Requirements, How Much Weight Should I Lift For My Size Calculator, How To Play Present Tense Pearl Jam,