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- . How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?What is the pH at 25 °C of water saturated with CO2 at apartial pressure of 1.10 atm? The Henry’s law constant forCO2 at 25 °C is 3.1 x 10-2 mol/L-atm.The acid dissociation constants for sulfurous acid are: Ka = 1.2 x 10-2 and Kaz = 6.6 x 10-8. (i) Calculate the pH of a solution of 0.100 M H2SO3. (ii) Calculate the pH of a solution of 0.100M NazSO.. (iii) Calculate the pH of a solution resulting when equal volumes of the solutions described in parts (i) and (ii) are mixed.
- A diprotic acid, H, A, has acid dissociation constants of K,j = 1.45 x 10-4 and K2 = 5.12 x 10-". Calculate the pH and molar concentrations of H,A, HA, and A²- at equilibrium for each of the solutions. A 0.184 M solution of H,A. pH = 2.2865 [H,A] = 0.1788 [HA"] = 5.17 xI10-3 [A?-] = M 5.12 x10-11 M A 0.184 M solution of NaHA. pH= [H,A] = M. [HA-] = [A2-] = M Ma) Why can you not prepare a solution of pH = 8 by diluting sufficiently a 0.01 M solution of HCl with water? b) You could determine Ka for benzoic acid by measuring the pH of a 0.010 M solution of benzoic acid. Why is the graphical method used in this experiment a better way of determining Ka? c) List the measurements along with their uncertainties made in the determination of the molar mass of benzoic acid. Calculate the uncertainty in the mola r mass of benzoic acid determined by the titration.Calculate the pH of a 0.0607 M solution of trimethylamine. The Kp of trimethylamine, (CH3)3N, is 6.4x10-5 Write your answer to 2 significant figures.
- Calculate the pH at 25 °C of a 0.72M solution of lidocaine HC1 (C,4H21NONH,CI). Note that lidocaine (C14H2 NONH) is a weak base with ap K, of 7.94. Round your answer to 1 decimal place. pH = ||7. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid. 8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach? 9. Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 solution. (Ka = 5.4 x 10-2)Choose the acid below that would make the most effective buffer for a solution to maintain a pH of 5.00 (aq., 25 oC), given a 0.500 M concentration of it and its conjugate salt. a) propionic acid, Ka = 1.34 x 10–5 b) HN3, Ka = 1.90 x 10–5 c) butanoic acid, Ka = 1.52 x 10–5 d) NH4Cl, Ka = 5.56 x 10–10 e) benzoic acid, Ka = 6.30 x 10–5
- COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…Consider the dissociation of hydrocyanic acid in aqueous solution HCN - CN + H* for which K, is 4.9 x 101°. (i) Find the pH of a solution initially 102 M in HCN, and the degree of dissociation of the HCN, a. (ii) To this solution is added more CN' until [CN'] = (0.1 M. What is the new pH of the solution? (ii) Without making a new numerical cakculation, explain qualitatively how the degree of dissociation would change if the solution is diluted.In the laboratory, a general chemistry student measured the pH of a 0.433 M aqueous solution of phenol (a weak acid), CoH5OH to be 5.167. Use the information she obtained to determine the K, for this acid. K₂(experiment) =