a) KHC4H4O6
This is potassium hydrogen titrate. It will dissociate as
KHC4H4O6 ---> K+ + HC4H4O6-
At equilibrium s s
where solubility is "s"
Ksp = 3.8 x 10-4 = [K+][HC4H4O6-] = s2
s = 1.95 X 10^-2 mole / L
b) PbI2
PbI2 ---> Pb+2 + 2I-
at equilibrium s 2s
Where "s" is molar solubility of PbI2
Ksp = 1.4 x 10-8 = [Pb+2][I-]2 = [s][2s]2
1.4 x 10-8= 4s3
s3 = 3.5 X 10-9
Therefore s= molar solubility of PbI2 = 1.518 X 10-3 moles / L
c) Ag4[Fe(CN)6] ---> 4Ag+ + [Fe(CN)4]-
Ksp = [Ag+]4 [[Fe(CN)4]-] = [4s]4[s]
1.6 x 10-41 = 256s^5
62.5 X 10^-45 = s^5
s = 2.286 X 10^-9 Moles / L
d) Hg2I2 ---> Hg2+2 + 2I-
Ksp = [Hg2+2 ] [I-]2
Ksp = 4.5 X 10-29 = [s][2s]^2
4s3 = 4.5 X 10-29
s3 =11.25 X 10-30
s = 2.25 x 10-30 moles / L
13. Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each...
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following salts from its solubility product. (a) Ca(OH)2 Ksp = 5.0 ✕ 10−6 M (b) AgBr Ksp = 5.4 ✕ 10−13 M
Assuming that no other equilibria other than dissolution is involved, calculate the molar solubility of PbI2 given that the Ksp = 1.4 x 10-8.
2. Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in the following solution of salts (in contact with a solution containing a common ion.) Ksp AgCl 1.6 x 10-10 AgClI(s) in 0.025 M NaCl
8. Write the ionic equation for dissolution and the solubility product (K ) expression for each of the following slightly soluble ionic compounds: (a) PbCl2 (b) Ag, S (C) Sr,(PO4)2 (d) SSO I 14. Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product: (a) Ag, SO4 (b) PbBr2 (C) Ag! (d) CaC0, H,0
Please explain Solubility Equilibria and the Solubility Product Constant. Below you will find key questions. 1. Know that the solubility product constant, Ksp, defines the equilibrium constant for the dissolution of an ionic compound into its constituent ions. 2. Calculate the molar solubility of an ionic compound in pure water using the Ksp expression and an ICE table. 3. Know that the solubility of an ionic compound is lower in a solution containing a common ion than in pure water....
1. For each of the following species, indicate whether the resulting solution would be acidic, basic, or neutral, if 1.00 mole of each were dissolved in 1.0 liter of water. Provide the predominant acid-base reaction that occurs to explain your choice. (a) NH4NO3 (b) K2CO3 (c) NaF (d) Al2(SO4)2 (e) KClO4 2. Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product: (a) Ag2SO4 (Ksp= 1.2 x 10-5) (b)...
7.Calculate the molar solubility for the binary salt MX3 with Ksp=0.0000071. Enter your answer as a decimal number with two significant figures. 8.Calculate the molar solubility of the binary salt MX2 with Ksp=0.000016. Enter your answer as a decimal with two significant figures. 9. Calculate the molar solubility of MX2 (Ksp=0.0000011) in 0.085 M NaX. Enter your answer as a decimal with two significant figures. 10.Determine the molar solubility of MX (Ksp=4.2x10-8) in 0.083 M NaCN. The metal ion M+...
17.99 The solubility of CaCO3 is pH dependent. (a) Calculate the molar solubility of Caco, (K,,-4.5 × 10-9) neglecting the acid-base character of the carbonate ion. (b) Use the K expression for the CO, ion to determine the equilibrium constant for the reaction CaCO3(s) + H2O(1) (c) If we assume that the only sources of Ca2, HCO3, and OH ions are from the dissolution of CaCO3, what is the mo- lar solubility of CaCO, using the equilibrium expression from part...
1. Calculate the molar solubility of LaF; in each of the following (Ksp. LaF3 = 2.0x10-19). a) pure water b) 0.50 M NaF c) 0.25 M La(NO3)3 The Kan of Cul is 1.1x10 and the Krfor the [Cu(CN), complex ion is 1.0x1024 Write the equilibrium reaction associated with the given K value b) Write the equilibrium reaction associated with the given Kr value. Find the final concentration of cyanide ion in a solution containing excess Cul and 0.60 M NaCN.
Calculate the molar solubility of La(IO)s in 0.050 M NalOs by taking into account the activity coefficients of the ions involved. Utilize for the activity coefficients: Where Iz is the ionic strength: CiZi With appropriate summation over all ions, ci being the molar concentration of the i'th ion and zi being its charge. Explain why you either ignore or take into account the additional ions from dissolution of La(I03)3. If you make any approximations, check whether they are justified.