For u=0.1, the activity coefficient (gamma) of M2+ is 0.41 while gamma of X- is 0.75. Calculate how many micrograms of MX2 dissolve in 336 mL of 0.10 M NaX solution. The molar mass of MX2 is 205 g/mol, and its Ksp is 1.2 x 10-9. Note that NaX is a salt of X, an ion that participates in the equilibrium that applies to the solubility of MX2.

For u=0.1, the activity coefficient (gamma) of M2+ is 0.41 while gamma of X- is 0.75. Calculate how many micrograms of MX2 dissolve in 336 mL of 0.10 M NaX solution. The molar mass of MX2 is 205 g/mol, and its Ksp is 1.2 x 10-9. Note that NaX is a salt of X, an ion that participates in the equilibrium that applies to the solubility of MX2.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 71AP

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Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that it is not appropriate to neglect the changes in the initial concentrations of the common ions. (a) TICl(s) in 0.025 M TlNO3. (b) BaF2(s) in 0.0313 M KF. (c) MgC2O4 in 2.250 L of a solution containing 8.156 g of Mg(NO3)2. (d) Ca(OH)2(s) in an unbuffered solution initially with a pH of 12.700
Which of the following is the expression for the solubility product of Fe2(CrO4)3? Ksp 2[Fe2+13 +3[CrO4³-1² O O Ksp=3[Fe2+]2[CrO4³-] OKsp=[2x Fe2+13[3 x CrO4³-12 Ksp [Fe2+]³[CrO43-1² Ksp=[Fe3+12[CrO4²-1³
Calculate the molar solubility of CaF, at 25°C in a 0.010 M NaF solution. (Ksp CaF2 = 3.9 x 1011) %3D O 3.9 x 107 M O 3.9 x 10-9 M O 3.1 x 105 M O 6.2 x 105 M
Calculate the molar solubility of SrC₂O4 in a solution that has a fixed H3O+ concentration of (Ksp (SrC₂O4) = 5.0 x 10-8, K₁ (H₂C₂O4) = 5.60 x 10-2, K2 (H₂C₂O4) = 5.42 x 10-5) a. 5.1 x 10-6 M. Molar solubility= b. 5.1 x 10-7 M. Molar solubility = c. 5.1 x 10-9 M. Molar solubility = d. 5.1 x 10-11 M. Molar solubility = M M M M چار 4
Solid PbI2 (Ksp=9.8x10-9) is placed in a beaker of water. After a period of time the lead(II) concentration is measured and found to be 1.1x10-3 M. Has the system reached equilibrium? That is, is the solution saturated? If not, will more PbI2 dissolve?
If 20.0 mL of 0.50M NH3 is added to 80.0 mL of 0.0010M FESO4 and then enough NHẠC1 is added so that the NH4* present becomes 1.0M, a) What will be the [OH-] in the resulting solution? b) Will Fe(OH)2 precipitate? %3D K½ for ammonia = 1.8 x 10-5; Ksp for Fe(OH)2 = 1.6 x 10-14
If the Ksp of copper (II) iodate is 1.4 x 10 -7 M3 at 25 oC, what is the solubility of the salt at that temperature? What is the solubility of copper (II) iodate if it is dissolved in 0.050 M sodium iodate at that same temperature?
The solubility of Cr(OH)3 in 0.1 M solution of NaOH is (Ksp of Cr(OH)3 is 6.3 × 10-31) 1.26 x 10-32 mol/L 1.26 x 10-30 mol/L 6.3 x 10-31 mol/L 6.3 x 10-28 mol/L
The formation constant of [M(CN), is 5.30 x 1018, where M is a generic metal. A 0.130 mole quantity of M(NO3) is added to a liter of 0.490 M NaCN solution. What is the concentration of M+ ions at equilibrium? IM2+1- M
Calculate the solubility of Mercury (II) iodide (HgI2)(HgI2) when a 3.0 M solution of NaI is added, assuming (HgI4)2−(HgI4)2− is the only Hg-containing species present in significant amounts. Ksp=2.9x10−29Ksp=2.9x10−29 for HgI2HgI2 and Kf = 6.8x1029Kf = 6.8x1029 for (HgI4)2−(HgI4)2−. Kf = 6.8x1029
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Calculate the molar solubility of Ag2S in a solution maintained at pH 11.00 and where the concentration of free ammonia is 0.100 M. Ag2S: pKsp = 48.70H2S: Ka1 = 1.0 x 10-7 ; Ka2 = 1.2 x 10-15[Ag(NH3)2]+: Kf1 = 2.04 x 103 ; Kf2 = 8.13 x 103

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