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APPLY 15.22 Carbonated drinks are prepared by dissolving CO2 under high pressure. CO2 reacts with water to product carbonic acid according to the equation:
Assume all the dissolved CO2 is converted to H2CO3. Calculate the pH and the concentrations of all species present (H2CO3 HCO3-, CO32-, H3O+, and OH-) in a can of carbonated water with a partial pressure of CO2 of 4.5 atm. The solubility of a gas can be calculated from Henry’s Law, Solubility = k • P (Section 12.4). The Henry’s Law constant (k) for CO2, at 25°C is 3.2 × 10-2 mol/(L • atm) and Kavalues for H2CO3 are in Table 15.3.
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Chapter 15 Solutions
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- At 25 C, a 0.10% aqueous solution of adipic acid, C5H9O2COOH, has a pH of 3.2. A saturated solution of the acid, which contains 1.44 g acid per 100. mL of solution, has a pH = 2.7. Calculate the percent dissociation of adipic acid in each solution.arrow_forwardWrite the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HCN (hydrocyanic acid) b. HC6H7O6 (ascorbic acid)arrow_forwardWhat is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?arrow_forward
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