A 44.00 mL mixture containing 0.0748 M Mn²+ and 0.0748 M Pb²+ is titrated with 0.0881 M K₂S resulting in the formation of the precipitates MnS and PbS. Calculate pS² at the given points in the titration. The Ksp values for MnS and PbS are 4.6 x 10-14 and 8.9 x 10-29, respectively. 20.6 mL ps²- 53.0 mL PS²- = 81.4 mL ps²- = second equivalence point ps²-

A 44.00 mL mixture containing 0.0748 M Mn²+ and 0.0748 M Pb²+ is titrated with 0.0881 M K₂S resulting in the formation of the precipitates MnS and PbS. Calculate pS² at the given points in the titration. The Ksp values for MnS and PbS are 4.6 x 10-14 and 8.9 x 10-29, respectively. 20.6 mL ps²- 53.0 mL PS²- = 81.4 mL ps²- = second equivalence point ps²-

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section: Chapter Questions

Problem 32PS: Without doing detailed calculations, sketch the curve for the titration of 50 mL of 0.050 M...

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Without doing detailed calculations, sketch the curve for the titration of 50 mL of 0.050 M pyridine, C6H5N (a weak base), with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence point. What is the total solution volume at the equivalence point?
2.1 Calculate the pH of the pre-equivalence solution for the titration of 25mL of a 0.025 M H2SO4 solution with 0.050 M NaOH, after the addition of 25.9 mL NaOH. 2.2 Name 5 requirements of a compound that will be used as a primary standard in titrimetry
In which case will a precipitate form? (i) a 0.050 M MnCl2 solution with pH = 8.00 (Does Mn(OH)2 precipitate?) Ksp = 1.9 x 10-13. (ii) 100. mL of 0.010 M AgNO3 is added to 20. mL of .050 M Na2SO4 (Does Ag2SO4 precipitate?) Ksp = 1.4 x 10-5.
If you mix 50.0 mL of 0.50 M AgNO3 (aq) with 25.0 mL of 0.010 M NaI (aq) at 25°C, does AgI (s) precipitate? The Ksp for AgI is 8.52 x 10^-17.
Calculate the molar solubility of lead(II) iodide in water at 25° given that Ksp = 7.1 x 10-9 and Calculate the molar solubility of Mg(OH)2 (Ksp = 1.8 * 10-11) in 0.0862 M MgCl2
1.Given that the solubility products (Ksp) of silver chloride(AgCl),silver iodide(AgI) and silver bromide (AgBr) are 1.82×10^-10,1×10-16,5.2×10^-13 and 1.82×10^-10 respectively.Plot an arbitrary titration curve of pAg versus volume of AgNO3 for each of the above on the same set of axis.You may assume that the concentration and volume of starting materials the same. 2.Using the information above,predict the order in which each species would precipitate from first to last
Unlike propanoic acid, magnesium hydroxide, Mg(OH)2 does not dissolve well in water. The Ksp of Mg(OH)2 is only about 2 × 10–11. Yet, what will be the result if 75 mL of 0.0050 M Mg2+ are mixed together with 55 mL of 0.00010 M OH–? Write an appropriate expression (equation) for the Ksp of Mg(OH)2(s). Then, calculate Qsp and state accordingly whether a precipitate will form or not
5.The solubility product, Ksp, of sparingly soluble salt with the formula M2X (where M ismonovalent) in pure water is 1.1 x 10-12 at 250C.a. Write the equation for the dissolution of M2X as well as the solubility product of it.b. Calculate the solubility(s)of this salt. c. The molar mass of the salt is 332 g/mol and X is the chromate ion. Calculate the atomic mass of the metal. d. Identify the metal. Write the formula of the salt. e. Discuss what will happen if the temperature of the previous system was increased up to50oC then decrease to 15oC.
(a) Will Mn(OH)2 precipitate from solution if the pH of a 0.050 M solution of MnCl2 is adjusted to 8.0? (b) Will Ag2SO4 precipitate when 100 mL of 0.010 M AgNO3 is mixed with 20 mL of 5.0 x 10-2 M Na2SO4 solution?
The solubility products of Fe(OH)2 and Fe(OH)3 are 10-17 and 10-38 respectively. If the concentrationsof Fe2+ and Fe3+ are each 10-5, at what pH will each hydroxide just begin to precipitate? A compound containing chlorine is titrated with a solution of 0.075 M Ag2SO4. If 0.250 g of thesample requires 22.07 ml of Ag2SO4 to reach the endpoint, what is the mass percent of chlorine in thesample?
A 1 L solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. A. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3. Ksp of CuCO3 = 1.4 x10-10Ksp of NiCO3 = 1.42X 10-7B. What would be the Molarity of Na2CO3 you will use in A , so that assumption of no volume change on addition of Na2CO3 will be valid ? please answer only B.
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