(a) Given the following equilibria, calculate what % of the total dissolved Zn species is present in the form of Zn(OH);". Zn(OH),(s) Zn(OH)* Zn(OH),(aq) Zn(OH), Zn(OH),² Kp =3x10-16 B, =1x10* B, = 2×1010 B3 =8x1013 B, =3x1015 (b) When the pH increases, would [Zn?*] increase, decrease, or remain the same? Explain your answer. (This question does not require any calculations to answer.) (c) When the pH increases, would [Zn(OH),] increase, decrease, or remain the same? Explain your answer. (This question does not require any calculations to answer.) (d) When the pH increases, would [Zn(OH),(aq)] increase, decrease, or remain the same? Explain your answer. (This question does not require any calculations to answer.)

(a) Given the following equilibria, calculate what % of the total dissolved Zn species is present in the form of Zn(OH);". Zn(OH),(s) Zn(OH)* Zn(OH),(aq) Zn(OH), Zn(OH),² Kp =3x10-16 B, =1x10* B, = 2×1010 B3 =8x1013 B, =3x1015 (b) When the pH increases, would [Zn?*] increase, decrease, or remain the same? Explain your answer. (This question does not require any calculations to answer.) (c) When the pH increases, would [Zn(OH),] increase, decrease, or remain the same? Explain your answer. (This question does not require any calculations to answer.) (d) When the pH increases, would [Zn(OH),(aq)] increase, decrease, or remain the same? Explain your answer. (This question does not require any calculations to answer.)

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter17: Solubility And Complex-ion Equilibria

Section: Chapter Questions

Problem 17.117QP

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A scientist was interested in how soluble rust is in acidic soils, so she set up an idealized problem to get an initial feel for the situation. A fairly acidic soil has a pH of 4.50. Also, rust is essentially Fe(OH)3. Therefore, she considered the following problem: Suppose a 1.00-g sample of iron(III) hydroxide is exposed to 1.00 L of a buffer with a pH of 4.50. She then calculated the nanograms of Fe3+ that dissolve in a liter of this buffer. Show how you would do this problem. Explain your work.
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