Please answer this question 8. In this case, the pH of the Flint River is well-characterized at 7.92. Based on yourchemical intuition (think LeChatlier's principle), would increasing the solution pH causethe [Pb2*] to increase or decrease? Why?9. Since we know the measured pH of the River is 7.92, this simplifies our approach(slightly). Through the magic (algebra) of systematic treatment of equilibrium, we canrelate Pb2+ concentrations to pH through the following relationship.Ка, х Каz х КазKa,KażKaz + Ka,Każ[H*]+ Ka,[H*]² + [H*]³2Ksp = [Pb2*]*Use the relationship above to solve for the Pb2* concentration at the pH of 7.92.10. Compare this answer to that from number lc. Were the early journalists correct in theirassertions that the higher pH of the Flint River was the sole cause of the Pb leachingissue? How do you know?

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8. In this case, the pH of the Flint River is well-characterized at 7.92. Based on your chemical intuition (think LeChatlier's principle), would increasing the solution pH cause the [Pb²*] to increase or decrease? Why? 9. Since we know the measured pH of the River is 7.92, this simplifies our approach (slightly). Through the magic (algebra) of systematic treatment of equilibrium, we can relate Pb²* concentrations to pH through the following relationship. Ка, х Ка, х Каз Ka,KażKaz + Ka, Kaz[H*] + Kaj[H*]² + [H*]³) 2 Ksp [Pb2+j* Use the relationship above to solve for the Pb²* concentration at the pH of 7.92. 10. Compare this answer to that from number lc. Were the early journalists correct in their assertions that the higher pH of the Flint River was the sole cause of the Pb leaching issue? How do you know?

8. In this case, the pH of the Flint River is well-characterized at 7.92. Based on your chemical intuition (think LeChatlier's principle), would increasing the solution pH cause the [Pb²] to increase or decrease? Why? 9. Since we know the measured pH of the River is 7.92, this simplifies our approach (slightly). Through the magic (algebra) of systematic treatment of equilibrium, we can relate Pb² concentrations to pH through the following relationship. Ка, х Ка, х Каз Ka,KażKaz + Ka, Kaz[H] + Kaj[H]² + [H]³) 2 Ksp [Pb2+j Use the relationship above to solve for the Pb²* concentration at the pH of 7.92. 10. Compare this answer to that from number lc. Were the early journalists correct in their assertions that the higher pH of the Flint River was the sole cause of the Pb leaching issue? How do you know?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 3RQ

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What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
Strong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid. a Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions? b One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak? c Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer? d What is the concentration of A(aq) in the HA solution described in part c? e If HB(aq) is a strong acid, what is the hydronium-ion concentration? f In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide? g In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A+(aq), HA(aq), or OH(aq)? How did you decide? h Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer. i You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA(aq)? Be sure to support your answer.
What 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?
You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
The pH of a solution of Ba(OH)2 is 10.66 at 25 . What is the hydroxide ion concentration in the solution? If the solution volume is 125 mL, what mass of Ba(OH)2 must have been dissolved?
Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.
. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
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.
Write two BrnstedLowry acid-base reactions and show how they represent proton-transfer reactions.
Calculate the maximum concentration of Mg2+ (molarity) that can exist in a solution of pH 12.00.
Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.

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