Given the equations and constants below, calculate the concentration of Zn(OH)* and of Zn(OH)2(aq) in a solution saturated with Zn(OH)2(s) and a fixed pH of 8.00. Zn(OH)2(s) Zn(OH)* Zn(OH)2(aq) Zn(OH)3 Zn(OH)42- Ksp = 3 x 10-16 B1 = 1 x 104 B2 = 2 x 1010 B3 = 8 x 1013 B4 = 3 x 1015 %3D [Zn(OH)*] = 6 x 106 and [Zn(OH)z] = 3 x 106

Given the equations and constants below, calculate the concentration of Zn(OH)* and of Zn(OH)2(aq) in a solution saturated with Zn(OH)2(s) and a fixed pH of 8.00. Zn(OH)2(s) Zn(OH)* Zn(OH)2(aq) Zn(OH)3 Zn(OH)42- Ksp = 3 x 10-16 B1 = 1 x 104 B2 = 2 x 1010 B3 = 8 x 1013 B4 = 3 x 1015 %3D [Zn(OH)*] = 6 x 106 and [Zn(OH)z] = 3 x 106

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

Chapter21: Transition Metals And Coordination Chemistry

Section: Chapter Questions

Problem 105CP

See similar textbooks

Similar questions

2. Calculate molar solubility of AgCl in pure water. The Ksp for Silver Chloride is: 1.83 x 10-10. Group of answer choices 2.34e-5 1.35e-5 1.35e5 2.34e5
Consider a saturated ferrous hydroxide solution. Ksp for Fe(OH)2= 4.47 × 10-17 Calculate the molar solubility of Fe(OH)2 in pure water. Calculate the molar solubility of Fe(OH)2 in 0.90M Fe(NO3)2. Compare the molar solubility of Fe(OH)2 in pure water and in the buffer solution with pH 6. Justify your answer.
A student prepared a saturated solution of magnesium hydroxide for analysis of the equilibrium of dissolution of this sparingly soluble solid. Titration was used to determine the concentration of hydroxide in solution after filtering the excess solid that persisted in the solution. If 30.0 mL of Mg(OH)2 solution were titrated using 4.83 mL 0.0020 M HCI, what is the value of Ksp for magnesium hydroxide?
8. Calculate the Molar solubility AgI in a 1.0M NH3 solution. (Ksp of AgI = 8.3 x 10 -17); Kf for Ag (NH3)+2 is 1.5 x 107. By what factor the solubility AgI has increased due to the presence of 1.0 M ammonia? You need to show your works.
calculate the molar solubility of AgBr in 3.1×10−2 M AgNO3 solution. Ksp = 5.0x10-13 for AgBr
Sodium sulfate is slowly added to a solution containing (aq)0.0500 M Ca^2+(aq) and 0.0310 M Ag+(aq). What will be the concentration of Ca^2+(aq) when Ag2SO4(s) begins to precipitate? Solubility-product constants, ?sp, can be found in the chempendix. [Ca^2+]= M What percentage of the Ca2+(aq) can be precipitated from the Ag+(aq) by selective precipitation? percentage: %
Calculate the solubility of AgBr in a 1.00 M aqueous solution of ammonia, given: AgBr(s) ⇌ Ag+(aq) + Br-(aq) Ksp = 7.7 x 10-13 Ag+(aq) + 2 NH3(aq) ⇌ Ag(NH3)2+(aq) Kf = 1.7 x 107 [Hint: combine these reactions into a single reaction].
2. Copper(II) hydroxide is only very slightly soluble in water. The reaction by which it goes into solution is: Cu(OH)2(s) (reaversable) Cu+2 (aq) +2OH-(aq) A) It is possible to dissolve siginificant amounts of Cu(OH)2 in solutions i which the concentrations of either Cu+2 or OH- is very small. Explain why this is true using Ksp. B) Explain why Cu(OH)2 might have very appreciable solubility in 1 M HCl. (Consider the effect of Reaction 3 on the Cu(OH)2 solution reactioin) -reaction 3 =H2O (reverse) H+(aq)+OH-(aq), Kc= [H+][OH-]=1*10-14 AT 25 C
When carrying out a precipitation volume, the concentrations of the reactive species must be calculated in the pre-equivalence region, equivalence point, and post-equivalence region. In this context, calculate the concentration of SCN- in the titrated solution during the titration of 50.00 mL of AgNO3 0.100 mol / L with KSCN 0.100 mol / L after adding 41.12 mL of the titrant solution Given: Kps (AgSCN) = 1.10.10-12 pSCN = ??
Calculate the molar solubility of Ag2S in a solution maintained at pH 11.00 and where the concentration of free ammonia is 0.100 M. Ag2S: pKsp = 48.70H2S: Ka1 = 1.0 x 10-7 ; Ka2 = 1.2 x 10-15[Ag(NH3)2]+: Kf1 = 2.04 x 103 ; Kf2 = 8.13 x 103
The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant.
The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant. Determiner the ff. volume of NaOH used moles of OH- used