-33 For the equilibrium; = (1.3×10 a. What is the minimum pH at which Al(OH)3() will precipitate 3+ 3+ from a solution that is 0.75M in Al ? b. A solution has [41²+] = 0.075M and [CHOH] = = 1.00M. 3 What is the maximum quantity of NaCHo that can be added to 250.0mL of this solution before 30 precipitation of Al(OH). begins? 3(s)

-33 For the equilibrium; = (1.3×10 a. What is the minimum pH at which Al(OH)3() will precipitate 3+ 3+ from a solution that is 0.75M in Al ? b. A solution has [41²+] = 0.075M and [CHOH] = = 1.00M. 3 What is the maximum quantity of NaCHo that can be added to 250.0mL of this solution before 30 precipitation of Al(OH). begins? 3(s)

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

If a solution contained Ni2+ ions at a concentration of 0.1 M, what pH would have to be reached toprecipitate 99% of the Ni2+ as Ni(OH)2?
The initial in the unknown analysis is the addition of 6. M HCl. This results in the formation of a precipitate. The solid precipitate is separate from the liquid solution. The solution could potentially contain K+, Ca2+, and Al3+. Next, 3M NH3 is added to the solution to separate the Al3+. This is a result of the fact that the Al3+ forms the hydroxide, Al(OH)3. But Ca2+ also forms the hydroxide, Ca(OH)2. Why does the Ca(OH)2 not separate out with the Al(OH)3?
K₂CrO₂(aq) is slowly added to a solution that has [Ba²+] = [Sr²+] = 0.10 M. Calculate the [CrO²-] needed to start the precipitation of: (a) BaCrO4(s) (b) SrCrO₂ (s) Ksp = 1.2 x 10-10 Ksp = 2.2 x 10-5 What is the concentration of the first ion to precipitate when the second ion begins to precipitate? Is complete separation of Ba²+(aq) and Sr²+(aq) by fractional precipitation feasible? Justify your answer. 1. 2. 3.
4. A solution is 0.0350 M in Na2SO4 and 0.0350 M Na2CO3. Solid Pb(NO3)2 is added without changing the volume of the solution. Which salt will precipitate first, PbSO4 or PbCO3? Explain clearly.
What would happen to the color of the solution in part (b) as shown if a small amount of NaOH were added and Fe(OH)3 precipitated? Explain your answer.
2- Will a precipitate be observed if 0.10 mol Ag+ and 0.001 mol SO4²- are added to make 1.0 L of solution? (Ksp = 1.4 x 10-5) yes, because Q Ksp Ono, because Q< Ksp
Cdf2 (s) = Cd²+ (aq) + 2 F- (aq) 1. A saturated solution of CdF2 is prepared. The equilibrium in the solution is represented above. In the solution [Cd2+] eq = 0.0585 M and [F-] eq = 0.117 M. a. Determine the solubility of CdF2. b. Some 0.90 M NaF is added to the saturated solution. Does the solubility of CdF2 increase, decrease, or remain the same? Justify your answer based on Q. 2. Is the solubility of AgCI(s) greater in distilled water or in tap water where the [CI-] = 0.010 your answer based on Q. M? Justify
1) A 1.0L solution of 1.0 M NaF is titrated with 1.0 M HCI, What is the pH of the solution after the addition of 0.00, 0.50, 1.0, and 1.5 L of 1.0 M HCI? The pk, of HF is 3.17. 2) A15L solution of 1.0x10 M HCIO, is titrated with 2.0x10 MCa(OH),. What is the pH of the solution after the addition of 0.00, 0.25, and 0.50 L of 2.0x10 M Ca(OH);? The pk, of HCIO, is 1.96.
Which of the following 1.0 L solutions would produce a buffer with a pH of approximately 3.2? O A solution of 6.3 x 104 moles of HNO3. O A solution of 0.100 moles of NH3 (Kp 1.8 x 10-5) and 0.100 moles of NH,CI. O A solution of 0.100 moles of HBr and 0.099 moles of NaOH. O A solution of 0.100 moles of HF (K, = 6.4 x 10 4) and 0.100 moles of KF. O A solution of 0.100 moles of CH;CO,H (K, 1.8 x 10-) and 0.100 moles of NACH,CO2.
a. Determine the pH change when 0.100 mol KOH is added to 1.00 L of a buffer solution that is 0.452 M in HClO and 0.357 M in ClO-.pH after addition − pH before addition = pH change= ? b. A buffer solution contains 0.387 M CH3NH3Br and 0.409 M CH3NH2 (methylamine). Determine the pH change when 0.084 mol HI is added to 1.00 L of the buffer.pH after addition − pH before addition = pH change = ? c. Determine the pH change when 0.057 mol HI is added to 1.00 L of a buffer solution that is 0.414 M in HF and 0.229 M in F-.pH after addition − pH before addition = pH change =?
17. In which of the following solutions, Mn(OH)2 has the greatest solubility? (by assuming sufficient Mn(OH)2 (s) present in solution). Ksp (Mn(OH)2) 2.0 × 10-13. a) 0.20 M HNO3 b) 0.20 M NaNO3 c) b) 0.20 M Mn(NO3)2 e) same solubility for all
When potassium iodide is added to soluble lead iodide at 25 oC, what will happen? PbI2 <=> Pb2+ (aq) + 2 I- (aq) a. the reaction will become more soluble b. the equillibrium will shift to the left and precipitate c. the equilibrium will shift to the right d. lead iodide will become supersaturated