Question

In: Chemistry

Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. M(0H)2 yields M+2OH M(OH)2 +2OH...

Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. M(0H)2 yields M+2OH M(OH)2 +2OH yields (M(OH4)2- Ksp=3x10^-16 Kf= .05 Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, and 14.0.

Solutions

Expert Solution


Related Solutions

At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2 , is mixed with...
At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2 , is mixed with pure water. The resulting equilibrium solution has a pH of 10.34 . What is the ?sp of the salt at 22 °C? A solution contains 0.25 M Pb2+ and 0.44 M Al3+. Calculate the pH range that would allow Al(OH)3 to precipitate but not Pb(OH)2. The Ksp values for Al(OH)3 and Pb(OH)2 can be found in this table.
Consider the dissolution of calcium hydroxide: Ca(OH)2(s) --> Ca2+(aq) + 2OH‑(aq) K = 4.7 x 10‑6...
Consider the dissolution of calcium hydroxide: Ca(OH)2(s) --> Ca2+(aq) + 2OH‑(aq) K = 4.7 x 10‑6 Write the equilibrium expression for this reaction. 2. Identify whether the following actions would favor the formation of products, reactants, or have no affect upon the dissolution of calcium hydroxide. Explain each answer. a. Addition of CaCO3 to an equilibrium mixture of calcium hydroxide and water. b. Addition of Na2CO3 to an equilibrium mixture of calcium hydroxide and water. c. Addition of HCl to...
The formation constant* of [M(CN)2]– is 5.30 × 1018, where M is a generic metal. A...
The formation constant* of [M(CN)2]– is 5.30 × 1018, where M is a generic metal. A 0.170-mole quantity of M(NO3) is added to a liter of 0.570 M NaCN solution. What is the concentration of M ions at equilibrium?
The formation constant* of [M(CN)2]– is 5.30 × 1018, where M is a generic metal. A...
The formation constant* of [M(CN)2]– is 5.30 × 1018, where M is a generic metal. A 0.160-mole quantity of M(NO3) is added to a liter of 0.720 M NaCN solution. What is the concentration of M ions at equilibrium?
The formation constant* of [M(CN)4]2– is 7.70 × 1016, where M is a generic metal. A...
The formation constant* of [M(CN)4]2– is 7.70 × 1016, where M is a generic metal. A 0.140-mole quantity of M(NO3)2 is added to a liter of 0.890 M NaCN solution. What is the concentration of M2 ions at equilibrium?
The formation constant* of [M(CN)4]2– is 7.70 × 1016, where M is a generic metal. A...
The formation constant* of [M(CN)4]2– is 7.70 × 1016, where M is a generic metal. A 0.140-mole quantity of M(NO3)2 is added to a liter of 0.890 M NaCN solution. What is the concentration of M +2 ions at equilibrium?
Consider these reactions where M represents a generic metal: 2M(s) + 6HCl(aq) ---->2MCl3(aq) + 3H2(g) Delta...
Consider these reactions where M represents a generic metal: 2M(s) + 6HCl(aq) ---->2MCl3(aq) + 3H2(g) Delta H1 = -569kj HCl(g) ----> HCl(aq)   DeltaH2 = -74.8 H2(g) + Cl2(g) ----> 2HCl(g) Delta H3 = -1845kj MCl3(s) ----> MCl3(aq)   Delta H4 = -405kj Use the above information to determine the enthalpy of the following reaction: 2M(s) + 3Cl2(g) ----> 2MCl3(s)   What is Delta H for this reaction?
At 22 °C an excess amount of a generic metal hydroxide M(OH)2 is mixed with pure water. The resulting equilibrium solution has a pH of 10.26. What is the Ksp of the salt at 22 °C?
At 22 °C an excess amount of a generic metal hydroxide M(OH)2 is mixed with pure water. The resulting equilibrium solution has a pH of 10.26. What is the Ksp of the salt at 22 °C?  
Consider an ionic compound, MX2 , composed of generic metal M and generic, gaseous halogen X...
Consider an ionic compound, MX2 , composed of generic metal M and generic, gaseous halogen X . The enthalpy of formation of MX2 is Δ?∘f=−677 kJ/mol. The enthalpy of sublimation of M is Δ?sub=161 kJ/mol. The first and second ionization energies of M are IE1=647 kJ/mol and IE2=1377 kJ/mol. The electron affinity of X is Δ?EA=−339 kJ/mol. (Refer to the hint). The bond energy of X2 is BE=221 kJ/mol. Determine the lattice energy of MX2 . Δ?lattice= kJ/mol
The formation constant* of [M(CN)6]4– is 2.50 × 1017, where M is a generic metal. A...
The formation constant* of [M(CN)6]4– is 2.50 × 1017, where M is a generic metal. A 0.160-mole quantity of M(NO3)2 is added to a liter of 1.460 M NaCN solution. What is the concentration of M2 ions at equilibrium? Please post all of your work with it! I have tried 3 seperate times and have gotten the wrong answer each time. The first and third time I got 1.00 x 10^-20 and the second I got 4.00 x 10^-20.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT