Fe3+ ions are to be separated from Hg2+ ions from an aqueous solution in which their concentrations are both 0.05500 M . The criterion for "complete" separation is that the Fe3+ ion concentration must be 10,000 times larger or 10,000 times smaller that the Hg2+ ion concentration. Answer the questions below.
At what pH will Fe(OH)3 precipitate from a 0.05500
M Fe3+ solution?
Ksp = 2.800×10-39
At what pH will Hg(OH)2 precipitate from a Hg
M Hg2+ solution?
Ksp = 3.100×10-26
At what pH will Hg(OH)2 precipitate from a Hg
M Hg2+ solution?
Ksp = 3.100×10-26
Fe3+ ions are to be separated from Hg2+ ions from an aqueous solution in which their...
A solution contains 0.100 mM of Ni2+ and Zn2+. Hydroxyl ions are slowly added to this solution to precipitate either Ni(OH)2 or Zn(OH)2. Determine which ion precipitates first at the pH range from 0-14 and the range of OH- concentrations that will allow a clean separation of the two ions. Ksp for Ni(OH)2=6x10^-16 and for Zn(OH)2 Ksp=3x10^-16
Problem 4 (30 pts) Ignore activity corrections. Fe3+ + OH = Fe(OH)2+ Fe3+ + 2OH = Fe(OH)2+ Fe3+ + 3OH = Fe(OH)3(aq) Fe3+ + 40H = Fe(OH)4 Fe(OH)3°(s) = Fe3+ + 3OH log K10H = log B20H = log B3OH = log B4OH = log Ksp = 11.81 22.4 30.2 34.4 -38.8 a. (10 pts) Will Fe(OH)3'(s) precipitate in a solution prepared in water and with Fer = 1.00 mM and buffered to pH 7.0? Hint: There are several ways...
The Hg2+ ion forms complex ions with I- as
follows:
Hg2+ + I-
HgI+
K1 = 1.0 × 108
HgI+ + I-
HgI2
K2 = 1.0 × 105
HgI2 + I-
HgI3-
K3 = 1.0 × 109
HgI3- + I-
HgI42-
K4 = 1.0 × 108
A solution is prepared by dissolving 0.053 mol
Hg(NO3)2 and 5.00 mol NaI in enough water to
make 1.0 L of solution.
Calculate the equilibrium concentration of
[HgI42- ].
[HgI42- ] = M
Calculate...
The Hg2+ ion forms complex ions with I- as follows:
Hg2+ + I-
HgI+
K1 = 1.0 × 108
HgI+ + I-
HgI2
K2 = 1.0 × 105
HgI2 + I-
HgI3-
K3 = 1.0 × 109
HgI3- + I-
HgI42-
K4 = 1.0 × 108
A solution is prepared by dissolving 0.045 mol
Hg(NO3)2 and 5.00 mol NaI in enough water to
make 1.0 L of solution.
Calculate the equilibrium concentration of
[HgI42- ].
[HgI42- ] = ? M...
Typically the concentration of hydronium, H3O+, or hydroxide, OH−, ions in an aqueous solution is less than 1 M. It is not uncommon to have hydronium ion concentrations that are much smaller, such as 2.60×10−5. pH, therefore, is a convenient way to restate the hydronium concentration. pH is equal to the negative log of a hydronium ion concentration in solution: pH=−log[H3O+] Access the pH calculation simulation, which will open in a new window. Edit the concentration by typing a value...
Lunes CHEMWORK The Hg2+ ion forms complex ions with I as follows: Hg2+ + HgT+ HgI + 1 =Hg2 K1 = 1.0 108 K2=1.0 x 105 K3 -1.0 x 10° K4 = 1.0 * 108 Hgl2 + 1 + HgI3 HgI3 + 1 = Hg142 A solution is prepared by dissolving 0.057 mol Hg(NO3)2 and 5.00 mol Nal in enough water to make 1.0 L of solution. Calculate the equilibrium concentration of [Hg142]. (Hg142) = M Calculate the equilibrium concentration...
A basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation. The I– concentration, which is 9.60×10-5 M, is 10,000 times less than that of the PO43– ion at 0.960 M . A solution containing the silver(I) ion is slowly added. Answer the questions below. Ksp of AgI is 8.30×10-17 and of Ag3PO4, 8.90×10-17. Calculate the minimum Ag+ concentration required to cause precipitation of AgI. Calculate the minimum Ag+ concentration required to cause precipitation...
Determine whether a precipitate form in the following reaction conditions: a. A solution containing lead (II) nitrate is mixed with one containing sodium bromide to form a solution that is 0.0150 M in Pb(NO3)2 and 0.00350 M in NaBr. Does a precipitate form in the newly mixed solution? Ksp PbBr2 = 4.67 x 10-6 . b. A solution containing iron (II) nitrate is mixed with one containing sodium phosphate to form a solution that is 0.0365 M in Fe(NO3)2 and...
Question: A basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation. The I– concentration, which is 9.10×10-5 M, is 10,000 times less than that of the PO43– ion at 0.910 M . A solution containing the silver(I) ion is slowly added. Answer the questions below. Ksp of AgI is 8.30×10-17 and of Ag3PO4, 8.90×10-17. Part 1. Calculate the minimum Ag+ concentration required to cause precipitation of AgI. Part 2. Calculate the minimum Ag+...
. The concentration of magnesium, calcium, and nickel(II) ions in an aqueous solution are 0.0010 M. (a) In what order to they precipitate when potassium hydroxide is added?; (b) determine the pH at which each salt will precipitate. The molarity of CrO42– in a saturated Tl2CrO4 solution is 6.3×10–5 mol·L–1, what is the Ksp of Tl2CrO4?