The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations...

The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A] = 0.100 M, [C] = 0.0340 M, and [AC5] = 0.100 M. Determine the formation constant, Kf, of AC5. The solubility of AB(s) in a 1.000-M solution of C(aq) is found to be 0.163 M. What is the Ksp of AB?

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

± Common-Ion Effect on Solubility for a Metal Hydroxide Consider the dissolution of AB(s): AB(s)⇌A+(aq)+B−(aq) Le...

± Common-Ion Effect on Solubility for a Metal Hydroxide Consider the dissolution of AB(s): AB(s)⇌A+(aq)+B−(aq) Le Châtelier's principle tells us that an increase in either [A+] or [B−] will shift this equilibrium to the left, reducing the solubility of AB. In other words, AB is more soluble in pure water than in a solution that already contains A+ or B− ions. This is an example of the common-ion effect. The generic metal hydroxide M(OH)2 has Ksp = 4.85×10−12. (NOTE: In...

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 25 °C only 0.0500 mol of the generic salt AB is soluble in 1.00 L...

At 25 °C only 0.0500 mol of the generic salt AB is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C?

At 25 °C only 0.0500 mol of the generic salt AB is soluble in 1.00 L...

At 25 °C only 0.0500 mol of the generic salt AB is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C?

13. a) A generic salt, AB, has a molar mass of 321 g/mol and a solubility...

13. a) A generic salt, AB, has a molar mass of 321 g/mol and a solubility of 8.80 g/L at 25 °C. What is the Ksp of this salt at 25 °C? b) The Ksp of manganese(II) hydroxide, Mn(OH)2, is 2.00 × 10-13. Calculate the molar solubility of this compound. c) Above what Fe2 concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 9.73? The Ksp of Fe(OH)2 is 4.87×10-17. d) What concentration of SO32– is...

Consider the equilibrium shown. PbBr2(s)−⇀↽− Pb2+(aq)+2Br−(aq)Ksp=2.10×10−6 Determine the concentrations of Pb2+ and Br− in a saturated...

Consider the equilibrium shown. PbBr2(s)−⇀↽− Pb2+(aq)+2Br−(aq)Ksp=2.10×10−6 Determine the concentrations of Pb2+ and Br− in a saturated solution of PbBr2 in pure water (assume μ=0 M). [Pb2+]= M [Br−]= M Determine the concentrations of Pb2+ and Br− in a saturated solution of PbBr2 in a solution with an ionic strength of 0.010 M. [Pb2+]= M [Br−]= M Determine the concentrations of Pb2+ and Br− in a saturated solution of PbBr2 in a solution with an ionic strength of 0.10 M. [Pb2+]=...

Pyridine is a weak organic base, and readily forms a salt with hydrochloric acid. C5H5N(aq) +...

Pyridine is a weak organic base, and readily forms a salt with hydrochloric acid. C5H5N(aq) + HCl(aq) → C5H5NH+(aq) + Cl–(aq) What is the pH of a 0.075 M solution of pyridinium hydrochloride, [C5H5NH]+Cl–, if Kb for pyridine is 1.5 × 10–9? pH =_____

1) Consider the insoluble compound cobalt(II) carbonate , CoCO3. The cobalt(II) ion also forms a complex...

1) Consider the insoluble compound cobalt(II) carbonate , CoCO3. The cobalt(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of CoCO3(s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Co(NH3)62+, Kf = 1.3×105. Use the pull-down boxes to specify states such as (aq) or (s). Knet = 2) Consider the insoluble compound nickel(II) carbonate, NiCO3. The nickel ion also forms a complex...

Will a precipiate of BaSO4(s) form when various concentrations and volumes of BaCl2(aq) and Na2SO4(aq) are...

Will a precipiate of BaSO4(s) form when various concentrations and volumes of BaCl2(aq) and Na2SO4(aq) are mixed? BaSO4 Ksp = 1.1 x 10−10 Μ Remember to account for the total volume in determinting the new concentration of each ion when the solutions are mixed. - A. B. 100 mL of 4.0 x 10−3 Μ of BaCl2 and 300 mL of 6.0 x 10−4 Μ Na2SO4 - A. ...

Insoluble PbBr2(s) precipitates when solutions of Pb(NO3)2(aq) and NaBr(aq) are mixed. Pb(NO3)2(aq) + 2 NaBr(aq) →...

Insoluble PbBr2(s) precipitates when solutions of Pb(NO3)2(aq) and NaBr(aq) are mixed. Pb(NO3)2(aq) + 2 NaBr(aq) → PbBr2(s) + 2 NaNO3(aq) ΔrH° = ? To measure the enthalpy change, 200. mL of 0.75 M Pb(NO3)2(aq) and 200. mL of 1.5 M NaBr(aq) are mixed in a coffee-cup calorimeter. The temperature of the mixture rises by 2.44 °C. Calculate the enthalpy change for the precipitation of PbBr2(s), in kJ/mol. (Assume the density of the solution is 1.0 g/mL, and its specific heat...

Subjects