Solubility - Zinc hydroxide, Zn(OH)2, has a low solubility and also forms several complex ions.The four stepwise equilibria constants are given (K1, K2, K3, K4). In a solution that is saturated (withZn(OH)2 solid present), the [OH-] was measured to be 3.2 x 10-7 MCalculate the [Zn²+], [Zn(OH)*], [Zn(OH)2], [Zn(OH)3¯], [Zn(OH)4²¯]Zn(OH)2 (s) <=====> Zn²+ (aq) + 2 OH- (aq)Ksp = 3.0 x 10-16Zn2+(aq)+ OH(aq) <=====>Zn(OH)+ (aq)K₁ = 1.0 x 105Zn(OH) (aq) +OH(aq)<=====>Zn(OH)2(aq)K₂ = 1.6 x 105Zn(OH)2(aq) +OH(aq) <=====>Zn(OH)3 (aq)K3 = 4.9 x 103Zn(OH)3 (aq) +OH(aq)<=====>Zn(OH)2(aq)K4 = 4.1 x 101

Approach to solving the question: Detailed explanation:Step 1: Calculate the [Zn2+] using the Ksp…

Answered: Solubility - Zinc hydroxide, Zn(OH)2,…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section15.5: Factors Affecting Solubility

Problem 15.10CE: Consider 0.0010-M solutions of these sparingly soluble solutes in equilibrium with their ions....

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A 3.20-L solution of 1.25 103 M Pb(NO3)2 is mixed with a 0.80-L solution of 5.0 101 M NaCl. Calculate Q for the dissolution of PbCl2. No precipitate has formed. Is the solution supersaturated, saturated, or unsaturated?
Solubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.
The Ksp value for radium sulfate, RaSO4, is 4.2 1011. If 25 mg of radium sulfate is placed in 1.00 102 mL of water, does all of it dissolve? If not, how much dissolves?
When 1.55 g of solid thallium(I) bromide is added to 1.00 L of water, the salt dissolves to a small extent. TlBr(s)Tl+(aq)+Br(aq) The thallium(I) and bromide ions in equilibrium with TlBr each have a concentration of 1.9 103 M. What is the value of Ksp for TlBr?
A saturated solution of silver oxalate. Ag2C2O4. contains 6.9 105-M C2O42 at 25 C. Calculate the Ksp of silver oxalate at that temperature, assuming that the ions do not react with water and the dissociation is complete.
To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
Consider 0.0010-M solutions of these sparingly soluble solutes in equilibrium with their ions. Predict the effect on each equilibrium if a saturated solution of sodium iodide were added. Explain your prediction in each case. AgI(s) ⇌ Ag+(aq) + I−(aq) PbI2(s) ⇌ Pb2+(aq) + 2 I−(aq)
Sufficient sodium cyanide, NaCN, was added to 0.015 M silver nitrate, AgNO3, to give a solution that was initially 0.108 M in cyanide ion, CN. What is the concentration of silver ion, Ag+, in this solution after Ag(CN)2 forms? The formation constant Kf for the complex ion Ag(CN)2 is 5.6 1018.
At 20 C, a saturated aqueous solution of silver acetate, AgCH3CO2, contains 1.0 g of the silver compound dissolved in 100.0 mL of solution. Calculate Ksp for silver acetate. AgCH3CO2(s)Ag+(aq)+CH3CO2(aq)
1. Iron(II) chloride (0.025 mol) is added to 1.00 L of 0.500 M NaCN. What is the concentration of Fe2+ ions at equilibrium? Kr for [Fe(CN)6]4− is 1.0 × 1035. 1.0 × 1035M 1.0 × 10−36 M 5.2 × 10−38M
The Ksp of AgBr at 100 C is 5 1010. Calculate the solubility of AgBr at that temperature in moles per liter.
An analytical chemist has a solution containing chloride ion, Cl. She decides to determine the amount of chloride ion in the solution by titrating 50.0 mL of this solution by 0.100 M AgNO3. As a way to indicate the endpoint of the titration, she added 1.00 g of potassium chromate, K2CrO4 (see Figure 17.5). As she slowly added the silver nitrate to the solution, a white precipitate formed. She continued the titration, with more white precipitate forming. Finally, the solution turned red, from another precipitate. The volume of the solution at this point was 60.3 mL. How many moles of chloride ion were there in the original solution? How many moles of chloride ion were there in the final solution? You may make any reasonable approximations.

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