A solution is made by equilibrating the two solids silver iodide (Ksp = 1.5×10-16) and silver hydroxide (Ksp = 2.0×10-8) with water. What are the concentrations of the three ions at equilibrium, if some of each of the solids remain?
[Ag+] = M
[I-] = M
[OH-]
= M
A solution is made by equilibrating the two solids silver iodide (Ksp = 1.5×10-16) and silver...
A solution is made by equilibrating the two solids silver hydroxide (Ksp = 2.0x10-) and silver bromide (Ksp = 3.3x10-13) with water. What are the concentrations of the three ions at equilibrium, if some of each of the solids remain? [Agt]= [OH-] = [Br] = What is the equilibrium Mn2+ concentration when 2.59 L of a 0.110 M manganese(II) chloride solution are mixed with 2.44 L of a 0.211 M potassium sulfide solution? [Mn) = A HCIO/NaClO buffer system is...
A solution is made by equilibrating the two solids calcium sulfide (Ksp = 8.0×10-6) and calcium chromate (Ksp = 7.1×10-4) with water. What are the concentrations of the three ions at equilibrium, if some of each of the solids remain? [Ca2+] = M [S2-] = M [CrO42-] = M
A solution is made by equilibrating the two solids barium carbonate (Ksp = 8.1×10-9) and barium sulfite (Ksp = 8.0×10-7) with water. What are the concentrations of the three ions at equilibrium, if some of each of the solids remain? [Ba2+] = _________M [CO32-] = _________M [SO32-] = ____________ M
A solution is made by equilibrating the two solids calcium chromate (Ksp = 7.1x104) and calcium sulfide (Ksp = 8.0x106) with water. What are the concentrations of the three ions at equilibrium, if some of each of the solids remain? [Ca2+3=1 (CrO42-) = [92-) = M
A solution is made by equilibrating the two solids barium sulfite (Ksp = 8.0x10-7) and barium sulfate (Ksp = 1.1x10-10) with water. What are the concentrations of the three ions at equilibrium, if some of each of the solids remain? [Ba2+] = [S032-) = [SO42-) =
Hi, I was having difficulty solving this, any help would be useful A solution is made by equilibrating the two solids barium carbonate (Ksp = 8.1×10-9) and barium sulfite (Ksp = 8.0×10-7) with water. What are the concentrations of the three ions at equilibrium, if some of each of the solids remain? [Ba2+] = _________M [CO32-] = _________M [SO32-] = ____________ M
ksp for silver iodide is 1.5x10^-16 The maximum amount of silver iodide that will dissolve in a 0.291 M silver acetate solution is
Given the Ksp of Zn(OH)2 is 3.0x10-1, determine the Zn2 ion concentration when the pH of the solution is buffered to pH=12.00 (so that the hydroxide ion concentration is 0.010 M). 1. Zn(OH)2(s) A. [Zn2] 3.0x10-12 M B. [Zn2 3.7x10- M C. [Zn23.0x10-10 M D. [Zn2] 9.1x10-3 M E. [Zn2] 1.5x10-13 M Zn2 (aq) + 20H (aq) Ksp 3.0x10-16 2. When silver carbonate, Ag,COs, is mixed with water, it dissolves to some extent to form a saturated solution where the...
1. What is the molar solubility of Agl if the Ksp is 1.5 x 10-16? 2. Calculate the Ksp for silver sulfite if the solubility of silver sulfite in pure water is 4.6 x 103 M.
A basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation. The I– concentration, which is 9.60×10-5 M, is 10,000 times less than that of the PO43– ion at 0.960 M . A solution containing the silver(I) ion is slowly added. Answer the questions below. Ksp of AgI is 8.30×10-17 and of Ag3PO4, 8.90×10-17. Calculate the minimum Ag+ concentration required to cause precipitation of AgI. Calculate the minimum Ag+ concentration required to cause precipitation...