Please find below answer
maximum solubility is 4.493*10-10mol/L
QUESTION 6 What is the maximum solubility of Fe(OH)3 (Ksp = 1.1 x 10-36?
Question 10 1 Point What is the Ksp expression for the dissociation of Fe(OH)3 ? Select the correct answer Ksp = [Fe3+] x [OH-]3 Ksp = [Fe3+] x [OH-]3 / [Fe(OH)3] Ksp = [Fe3+] x 3 [OH-] / [Fe(OH)3] Ksp = [Fe3+] x [OH-] / [Fe(OH)3]
Calculate the solubility (in moles per liter) of Fe(OH)3 ( Ksp = 4 x 10-38) in each of the following. a. water Solubility = mol/L b. a solution buffered at pH = 6.0 Solubility = mol/L c. a solution buffered at pH = 11.0 Solubility = mol/L Approximately 0.15 g cadmium(II) hydroxide, Ca(OH),(s), dissolves per liter of water at 20°C. Calculate Ksp for Ca(OH)2(s) at this temperature. Kp =
What is the molar solubility of Fe(OH)2 when buffered at pH of 9.00? [Fe(OH)2 : Ksp = 7.9 x 10^-16]
15a) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4? a. 1.0 x 10-5 b.2.0 x 10-5 c. 4.0 x 10-5 d. 8.0 x 10-5 o o 15b) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4 in 0.10 M Na2SO4? a. 2.8 x 10-10 b.5.5 x 10-10 c. 1.1 x 10-9 d. 2.2 x 10-9
QUESTION 1 If the solubility of iron(III) hydroxide Fe(OH)3 is s, what is the value of Ksp equal to? Ksp = 353 Ksp=9s3 Ksp = 954 Ksp = 354 Ksp = 2754 QUESTION 2 At a certain temperature the Ksp of Ni(OH)2 is 5.68 x 10-16. What is the molar soliubility of nickel(l) hydroxide in water in units of M (mol/liter)? Express your answer in scientific notation.
The solubility product constant of Ag4[Fe(CN)6] is Ksp = 1.55 x 10–41. Select the expression for the solubility product constant. Let x be the molar solubility. A. Ksp = [Ag+]4[Fe(CN)6-4] = 256x5 B. Ksp = [Ag+]4[Fe(CN)6-4] = x4 C. Ksp = [Ag+]4[Fe(CN)6-4] = x5 D. Ksp = [Ag+][Fe(CN)6-4] = x2
If the solubility of iron(III) hydroxide Fe(OH)3 is s, what is the value of Ksp equal to? Ksp = 3s4 Ksp = 27s4 Ksp = 3s3 Ksp = 9s3 Ksp = 9s4
1 Ferrous hydroxide Fe(OH)2 has a Ksp = 4.87 x 10-17. What is its molar solubility? AO 1.22 x 10-17 BO 2.30×100 CO 3.49 × 109 DO 1.40 × 10 -10 Competencies Assessed • Calculate solubility products and solute concentrations usinn an
calculate the molar solubility of Fe(OH)2 at pH of 8.56. Ksp=1.8*10^-15 for Fe(OH)2
Fe(OH)2 has a value of Ksp = 1.8 x 10-17 in water at 25oC What is the molar solubility of Fe(OH)2 in a basic solution of pH = 11