Determine the pH of a 0.74 M aqueous solution of hydrocyanic acid (HCN) and the concentration of all species in solution. The K, of hydrocyanic acid is 4.9 x 1010. HCN (aq) + H20 (1) CN (aq) + H3o* (aq) The pH of the solution is (Select] The concentration of HCN at equilibrium is (Select ] The concentration of CN' at equilibrium is (Select] The concentration of H30O* at equilbrium is (Select] The concentration of OH` at equilbrium is (Select] The pOH of the solution is [Select ]

Determine the pH of a 0.74 M aqueous solution of hydrocyanic acid (HCN) and the concentration of all species in solution. The K, of hydrocyanic acid is 4.9 x 1010. HCN (aq) + H20 (1) CN (aq) + H3o* (aq) The pH of the solution is (Select] The concentration of HCN at equilibrium is (Select ] The concentration of CN' at equilibrium is (Select] The concentration of H30O* at equilbrium is (Select] The concentration of OH` at equilbrium is (Select] The pOH of the solution is [Select ]

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 7RQ: Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a...

See similar textbooks

Similar questions

Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.
What is the concentration of the hydroxide ion, OH-, in solution at equilibrium if the pH of the solution is 7.65? Nitrogen and oxygen react at high temperatures according to the following equation: N2(g) +O2(g) ⇄ 2NO(g) where ∆H=181kJ At equilibrium what will happen to the concentrations of N2, O2, and NO at equilibrium if N2 is removed? Calculate the pH of the following weak base: 0.5M NH3 with Kb =1.8x10−5
Calculate [H], [CIO], and [OH-] in an aqueous solution that is 0.175 M in HClO4 (aq) at 25 °C. [H+] = x10 [CIO] = [OH-] = TOOLS y M M M
The pH of an aqueous solution of 3.14×10-2 M ammonium chloride, NH4Cl (aq), is
1) Vinegar sold commercially is typically 0.8−1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00 M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures?
The antibiotic Penicillin G is obtained from a mold and is treated before being ready for human consumption. Penicillin G is a weak acid with Ka = 1.6 x 10-3. Using HP to represent this weak acid, in water the following reaction represents an equilibrium that could develop. HP (aq) ↔↔ H+(aq) + P- (aq) Use the quadratic equation to solve for the equilibrium concentrations (that result from a 1.0 x 10-4 M solution of Penicillin G, HP) of each component.
The pH of an aqueous solution of 0.522 M benzoic acid, C6H5COOH is
Palmitic Acid, CH3(CH2)14COOH, found in both bacon fat and many soaps. Palmitic acid partially ionizes in water. Write a balanced chemical reaction for the dissociation of palmitic acid into its conjugate base and hydrogen ion. Write an expression for the equilibrium constant for palmitic acid. The equilibrium concentrations are [CH3(CH2)14COOH] = 0.1 M and [H+] = [CH3COO-] = 0.0133352 M. Calculate the equilibrium constant of ionization KA. Calculate the pKA of palmitic acid. Draw (by hand) the titration curve for palmitic acid. Please label your axes appropriately.
The Ksp of aluminum hydroxide, Al(OH)3, is 2 × 10−31. What pH is required to limit the Al3+ concentration to less than or equal to 1 × 10−10 M?
Calculate the pH of a solution containing a salt B Cl derived from a strong acid (HCl) and a weak Base (B OH), like NH4Cl, CH3NH3I, Ph-NH3Br and so on. In this case two processes have to be considered: 1. Dissociation of the salt, within the assumption that the salt is a strong electrolyte: B Cl → B + + Cl-, for instance: NH4Cl → NH4+ + Cl- 2. the hydrolysis of the water B + + H2O ⇌ B OH + H+, for example: NH4+ + H2O ⇌ NH4OH + H+ (often shown as NH4+ ⇌ NH3 + H+ ) knowing that the initial concentration of the salt is 1.67 M, and the base dissociation constant, Kb , is 8.43e-7.
The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, –NH2, and a carboxylic acid group, –CO2H. An amino acid can function aseither an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid, CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3.(a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH.(b) Write the Lewis structure of glycine when this amino acid is dissolved in water.
Saccharin, a sugar substitute, is a weak acid with the formula, HC7H4NSO3. The pKa of saccharin is 2.320. d. What are the equilibrium concentrations of the reactants and products in a 0.100M solution of saccharin? e. What is the pH, pOH, and %ionization of this weak acid?