pkal pK₂2 Phosphoric acid, H, PO, (aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.300 M phosphoric acid solution. 2.16 7.21 [H₂PO₂] = M [H*] = [H₂PO¡] = M [OH-] = [HPO ] = M pH = [PO] = M PK₂3 12.32 M M

pkal pK₂2 Phosphoric acid, H, PO, (aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.300 M phosphoric acid solution. 2.16 7.21 [H₂PO₂] = M [H*] = [H₂PO¡] = M [OH-] = [HPO ] = M pH = [PO] = M PK₂3 12.32 M M

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 106GQ: The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106....

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The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.
8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M solution of A−(aq)? The temperature is 25 ◦C. (b) For the reaction A(g) =A(l), the equilibrium constant is 0.666 at 25.0 ◦C and 0.222 at 75.0 ◦C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?
The pH of human blood is steady at a value of approximately 7.4 owing to the following equilibrium reactions: Acids formed during normal cellular respiration react with the HCO3- to form carbonic acid, which is in equilibrium with CO2(aq) and H2O(l). During vigorous exercise, a person’s H2CO3 blood levels were 26.3 mM, whereas his CO2 levels were 1.63 mM. On resting, the H2CO3 levels declined to 24.9 mM. What was the CO2 blood level at rest?
Calculate the pH of a solution prepared by dissolving 1.75 g of sodium acetate, CH3COON,, in 53.5 mL of 0.15 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5.
Calculate the pH of a solution prepared by dissolving 1.15g of sodium acetate, CH3COONa, in 95.5 mL of 0.10 M acetic acid, CH3 COOH(aq). Assume the volume change upon dissolving the sodium is negligible. Ka of CH3COOH is 1.75 x 10-5.
calculate the pH of a solution prepared by dissolving 1.15g of sodium acetate, CH3COONa, in a 71.0mL of 0.10M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75x10^-5.
Calculate the pH of the following acid solutions at 25 °C: (a) 1.0 x 10-4 M H3BO3(aq) (boric acid acts as a monoprotic acid), (b) 0.015 M H3PO4 (aq), (c) 0.10 M H2SO3(aq). Values for the successive acidity constants for each of these acids are given in the below table.
A student does a titration of 86.0 mL of a 0.37 M solution of methylamine (CH3NH2(aq) (pKb =3.36) with HCl(aq). When 100 mL of HCl had been added to the mixture, the pH was measured and found to be 9.54. What was the molarity of the HCl solution?
Rainwater is acidic because CO2(g) dissolves in the water, creating carbonic acid, H2CO3. If the rainwater is too acidic, it will react with limestone and seashells (which are principally made of calcium carbonate, CaCO3). Calculate the concentrations of carbonic acid, bicarbonate ion (HCO3-) and carbonate ion (CO32-) that are in a raindrop that has a pH of 5.60, assuming that the sum of all three species in the raindrop is 1.0 * 10-5 M.
For CO2 in the atmosphere at 25 degrees C, kH = 3.4 x 10-2 mol L-1 atm-1 and the partial pressure of CO2 is .000405 atm: Calculate the concentration of dissolved H2CO3 (aq) air-saturated rainwater. Determine the pH expected for rainwater on the basis of the first dissociation constant of the carbonic acid, H2CO3 (aq), from the dissolved CO2. The pKa values of carbonic acid are pKa1 = 6.35 and pKa2 = 10.33 at 25 C.
An organic acid(HA) has a molecular weight of 100. g mol^-1, a Kow=5.6 and a Ka=2.7x10^-2. If originally 2.0g of the acid is dissolved in 100mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100mL of water, what will be the pH of the water? (consider the equilibrium processes to be sequential and unrelated chemically)
Calculate the pH, pOH, and fraction of solute protonated or deprotonated in the following aqueous solutions: (a) 0.150 M CH3CH(OH)COOH(aq) (lactic acid), (b) 2.4 x 10-4 M CH3CH(OH)COOH(aq), (c) 0.25 M C6H5SO3H(aq) (benzenesulfonic acid). The appropriate values for pKa or pKb are given inthe table.