The concentration of hydroxide ions and the pH value that are required to separate the magnesium ions without altering the calcium ion concentration in the given solution are to be calculated. Concept Introduction: Metal sulfides have the ability to dissolve and dissociate themselves into their respective ions in the presence of an acid or hydrogen ions. The solubility of these sulfides in acids is called acid solubility product and is denoted as K spa . Not all metal sulfides are soluble in acids; therefore, they are divided into two categories depending upon their solubility, namely acid-soluble sulfides (that are soluble in nature) and acid-insoluble sulfides (that are insoluble in nature).
The concentration of hydroxide ions and the pH value that are required to separate the magnesium ions without altering the calcium ion concentration in the given solution are to be calculated. Concept Introduction: Metal sulfides have the ability to dissolve and dissociate themselves into their respective ions in the presence of an acid or hydrogen ions. The solubility of these sulfides in acids is called acid solubility product and is denoted as K spa . Not all metal sulfides are soluble in acids; therefore, they are divided into two categories depending upon their solubility, namely acid-soluble sulfides (that are soluble in nature) and acid-insoluble sulfides (that are insoluble in nature).
Solution Summary: The author explains that the concentration of hydroxide ions and the pH value that are required to separate the magnesium ion in the given solution are to be calculated.
The concentration of hydroxide ions and the pH value that are required to separate the magnesium ions without altering the calcium ion concentration in the given solution are to be calculated.
Concept Introduction:
Metal sulfides have the ability to dissolve and dissociate themselves into their respective ions in the presence of an acid or hydrogen ions. The solubility of these sulfides in acids is called acid solubility product and is denoted as Kspa. Not all metal sulfides are soluble in acids; therefore, they are divided into two categories depending upon their solubility, namely acid-soluble sulfides (that are soluble in nature) and acid-insoluble sulfides (that are insoluble in nature).
(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?
As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na+B(C6H5)4−. Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non‑negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K2CO3 and all ammonium is present as NH4Cl.
A 5.095 g soil sample was dissolved to give 0.500 L of solution. A 150.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K+ and NH4+ ions completely.
B(C6H5)4-+K+⟶KB(C6H5)4(s)
B(C6H5)4-+NH4+⟶NH4B(C6H5)4(s)
The resulting precipitate amounted to 0.269 g. A new 300.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH4+ as NH3. The resulting solution was then acidified, and excess sodium tetraphenylborate was added to give 0.129 g of precipitate.
Find the mass percentages of NH4Cl and…
A solution contains 0.04900 M Ca²+ and 0.09100 M Agt. If solid Na3PO4 is added to this mixture, which of the phosphate
species would precipitate out of solution first?
When the second cation just starts to precipitate, what percentage of the first cation remains in solution?
A solution contains 0.0490 M Ca²+ and 0.0910 M Agt. If solid Na3PO4 is added to this mixture, which of the phosphate
species would precipitate out of solution first?
O Ca3(PO4)2
Ag3PO4
O Na3PO4
When the second cation just starts to precipitate, what percentage of the first cation remains in solution?
percentage:
%
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell