A solution contains 0.020 M Mg2+ and 0.10 M Ca2+. Can 99.90% of Mg2+ be precipitated by addition of NaOH without precipitation of Ca2+? Note: use Ksp = 7.1 x 10-12 for Mg(OH)2 Ksp= 5.5 x 10^-6 CaOH2
A solution contains 0.020 M Mg2+ and 0.10 M Ca2+. Can 99.90% of Mg2+ be precipitated...
The magnesium and calcium ions present in seawater ([Mg2+] = 0.059 M and (Ca2+] = 0.011 M) can be separated by selective precipitation with KOH. Part A If the concentration of Mg2+ in the solution were 0.021 M. what minimum (OH-] triggers precipitation of the Mg2+ ion? (Ksp = 2.06 x 10-13.) Express your answer to two significant figures and include the appropriate units. | НА w ? Value Units Submit Previous Answers Request Answer
The magnesium and calcium ions present in seawater ([Mg2+] = 0.059 M and [Ca2+] = 0.011 MM) can be separated by selective precipitation with KOH. Part A If the concentration of Mg2+ in the solution were 0.036 M, what minimum [OH−] triggers precipitation of the Mg2+ ion? (Ksp=2.06×10^−13) Express your answer to two significant figures and include the appropriate units.
Purifying Mg2+ from sea water. Aqueous sodium hydroxide is added to an aqueous solution that contains 0.0099 M magnesium chloride and 0.021 M calcium chloride. What will be the concentration of the metal ion that precipitates first (as M(OH)2) at the time the second metal ion begins to precipitate? Ksp (Mg(OH)2) = 6.3 x 10-10 and Ksp (Ca(OH)2) = 6.5 x 10-6 Hint: Use Ksp values to determine the solubility of each product to determine the order of precipitation.
A solution contains 0.60 M NH4OH and 1.50 M NH4Cl. What is the maxiumum concentration of Mg2+ that can be present in such a solution without precipitating Mg(OH)2? (Ksp for Mg(OH)2 = 9.0 x 10^12; Kb fro NH4OH= 1.8 x 10^-5)
6-19. A solution contains 0.050 0 M Ca2+ and 0.030 0 M Ag+. Can 99% of Ca2+ be precipitated by sulfate without precipitating Ag+? What will be the concentration of Ca2+ when Ag,SO4 begins to precipitate? 6-19. A solution contains 0.050 0 M Ca2+ and 0.030 0 M Ag+. Can 99% of Ca2+ be precipitated by sulfate without precipitating Ag+? What will be the concentration of Ca2+ when Ag,SO4 begins to precipitate?
The magnesium and calcium ions present in seawater (Mg2+] = 0.059 M and (Ca2+] = 0.011 M) can be separated by selective precipitation with KOH. If the concentration of Mg2+ in the solution were 0.018 M, what minimum (OHtriggers precipitation of the Mg2+ ion? (Ksp = 2.06 x 10-13.) Express your answer to two significant figures and include the appropriate units. 03 O ? Value M
enodic Table The magnesium and calcium ions present in seawater ([Mg2+] = 0.059 M and (Ca2+] = 0.011 M) can be separated by selective precipitation with КОН. You may want to reference (Pages 775 - 778) Section 17.6 while completing this problem. Part A If the concentration of Mg2+ in the solution were 0.018 M, what minimum (OH) triggers precipitation of the Mg2+ ion?( Ksp = 2.06 x 10-13.) Express your answer to two significant figures and include the appropriate...
Using Ksp's from your textbook, calculate the solution concentration of Ca2+ and Mg2+ required to form a precipitate at pH 12. We would be forming the amorphous Mg(OH)2. Mg(OH)2 Ksp = 6x10-10
A solution contains 0.0100 M Ca2+ and 0.0500 M Sr2+. Can 99% of the first cation be precipitated before the second cation starts to precipitate as Na2CO3 is added to the solution? Find Ksp values in the table of solubility-product constants. For CaCO3, use the aragonite Ksp value. yes not enough information no What is the concentration of the first cation when the second cation starts to precipitate? concentration of the first cation:
A solution contains 0.10 M concentrations of Ba2+, Ca2+, and Sr2+. Na2CO3 is slowly added to the solution. In what order will the ions begin to precipitate? What is the concentration of the first ion when the 2nd begins to precipitate? Ksp for BaCO3 = 2.58 x 10-9, for CaCO3 = 3.36 x 10-9, and for SrCO3 = 5.60 x 10-10.