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4 5 points - The compound PbSOhas a Ksp value of 1.82x10-6. What is the predicted...
Return Submit 5 points What is the molality of a solution of 20.% of a compound with a molar mass of molar mass=208.46 g/mol by mass? The density of the solution is 1.18 g/ml BIVAAI EE XX, e 12p . Paragraph - EAD 5 points A solution is 0.125 Min HNO, and 0.225 M in NaNO2. The K, for HNO2 is 4.5' 104. What is the pH of 100.0 mL of this solution after 1.00 mL of 3.00 M NaOH...
Determine the molar solubility and value of Ksp for each compound in water at 25°C. Include the chemical equation for each equilibrium, the expression for Ksp (in terms of molarities and x), and show all work in calculations Compound 1: SrSO4 Compound 2: Ag2SO4 Chemical equation: Molar solubility (x) = Ksp =
Mg(OH)2 is a sparingly soluble compound, in this case, a base,
with a solubility product, Ksp, of 5.61×10−11. It is used to
control the pH and provide nutrients in the biological (microbial)
treatment of municipal wastewater streams.
Based on the given value of the Ksp, what is the molar
solubility of Mg(OH)2 in pure H2O?
Mg(OH), is a sparingly soluble compound, in this case a base, with a solubility product, K sp, of 5.61 x 10-11. It is used to...
5 points) A substance MX has a Ksp of 1.27 x 10-36. a. What is it's molar solubility in pure water? (hint: ICE Table-reminder: MX(s) will fall out of your equilibrium expression) b. What is it's molar solubility in 0.25 MBrz? (hint: ICE Table-but what is M2+ initial?)
28. -70.1 points 0/4 Submissions Used (a) If the molar solubility of YF3 at 25 °C is 4.23e-06 mol/L, what is the Ksp at this temperature? Ksp =D (b) It is found that 0.0628 g of BaF2 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility-product constant for BaF2. Ksp = (c) The Ksp of Ca3(PO4)2 at 25 °C is 2.05e-35. What is the molar solubility of Ca3(PO4)2? solubility = mol/L
The molar solubility and the pH of Ce(OH)3 with a Ksp value of 1.5x10-20 is: a) 4.86x10-6, 9.16 b) 1.5x10-10, 4.16 c) 1.46x10-5, 5.8 d) 6.31x10-4, 6.5 e)4x10-6, 12
Which compound listed below has the highest molar solubility in water? Calcium hydroxide Ca(OH)2 Ksp= 5.5x10-6 Calcium oxalate CaC204 Ksp= 2.7x10-9 Calcium phosphate Ca3(PO4)2 Ksp=2.0x10-29 Calcium sulfate CaSO4 Ksp= 9.1x10-6 A. CaC204 B. They are all equally insoluble C. Ca(OH)2 D. Ca3(PO4)2 E. CaSO4
Question 6 Provide a name for the product of the reaction shown below. + Br2 B I VAAI E 1 1 XX, SE De V 12pt Paragraph - Provide a name for the product of the reaction shown below. O + Hz Pd , ? E BI UAA - I E - 2 N VX c 1 XX, 12pt V Paragraph Question 8 Which best describes a polymer? O a) compound containing multiple double bonds. b) compound containing multiple aromatic...
1. Mg(OH)2 is a sparingly soluble compound, in this case a base, with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in pure H2O? Answer = Mol Solubility = 2.41 x 10^-4 2. Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2...
I found that the molar solubility of Calcium Sulfate is
0.00490 if its Ksp is 2.40x10^-5.
But I do not really know how to find the solubility of CaSO4
(136.2 g/mol) in g/mL.
Could someone also explain the different parts of this problem
as well please? (solubility, molar solubility, and Ksp)
Much thanks :)
-5.9x107 Find the molar solubility (mol/L) of calcium sulfate if its Ksp = 2:40 Casoy, 7 Cacaq) + soucans K[x][y] 8 52.40xions =x² chong x= .00490...