Write the chemical equation for the solubility equilibrium and the Ksp expression for each compound please help and explain steps
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Write the chemical equation for the solubility equilibrium and the Ksp expression for each compound please...
Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the following slightly soluble ionic compounds. (For the ionic equations, include states-of-matter under the given conditions in your answer. Solubility equilibrium expressions take the general form: Ksp = [An+ ]a . [Bm− ]b. Subscripts and superscripts that include letters must be enclosed in braces {}. For example: Ksp=[A+]2.[B2-] must be typed using K_{sp}=[A^+]^2.[B^2-] (a) Ag2CrO4 Net ionic equation Solubility product expression (c) Sn(OH)2 Net ionic...
1. Write the correct solubility-product expression for the following equilibrium reactions. (a) Pb12 (8) + Pb2+(aq) + 21"(aq) (b) AgCl(s) + Ag (aq) + CI+ (aq) (c) La(IO3)3 (9) + La**(aq) + 3103"(aq)
What is the correct expression of the solubility product constant (Ksp) for the following equilibrium? PbC14 (s) = P64+ (aq) + 4Cl- (s) P64+ K 8p [c1"]" Кsp [Pb2+] [c1-14 [PbC14] [Ps+]4x [C] K sp = (PbC14) O Køp = [P64+] [C1-14
What is the correct expression of the solubility product constant (Ksp) for the following equilibrium? PbCl4 (s) = P64+ (aq) + 4C1- (s) K SP [P0++] [C1-]4 4 [PB+][c1] sp [PbCl4] [Pb++]ax [cr] Ksp = [PbC14] OK sp = [Pb1+] [C1-14
What is the correct expression of the solubility product constant (Ksp) for the following equilibrium? PbCl(s) = P64+ (aq) + 4C1- (s) [P+ K sp Кр [c1")" [P6++] [c1-] [РЬСА) [P8*+]4x[01] Ksp = [PbC14] • Ksp = [P64+] [C1-14
1 a) Write reactions for solubility and the equilibrium expression Ksp. b) Solve for Ksp from molar solubility or molar solubility from Ksp. c) Solve for solubility when a common ion is present. d) Evaluate solubility changes according to pH changes. e) Determine if a combination of solutions will produce a precipitate. f) Determine minimum amount of a substance required to precipitate a substance.
For AgC2H3O2 salt, write a balanced equation showing the solubility equilibrium, write the solubility product expression, and determine the mass that dissolves in 375 mL of water at 25 °C. (for AgC2H3O2, Ksp = 1.94*10-3 )
IULUIGUIGULILETTUVICIILTU. LUUN Write solubility product constant expressions. Write the Ksp expression for each of the following sparingly soluble compounds. If either the numerator or denominator is 1, please enter 1. (a) BaCro4 Ksp = — (b) Pb(OH)2 se
D Question 6 3 pts Write the expression for the equilibrium constant for the reaction represented by the equation Pb2+ (aq) + 2Cl(aq) =PbCl2(s) Is Kc>1.<1, or 1? Explain your answer. Solubility Rules: Soluble compounds contain • group 1 metal cations (LI". Na, K, Rb and Cs) and ammonium ion NHA • the halide ions (CI", Br", and I") • the acetate (C2H302 ), bicarbonate (HCO3), nitrate (NO3), and chlorate (CIO) ions • the sulfate (S04)ion Exceptions to these solubility...
1) Write the solubility product equilibrium and the solubility product constant expression for barium fluoride. al 2) A solution is made by placing solid barium fluoride into pure water. The barium ion concentration in this solution was found to be 1.1 x 10-8 M, what would the numerical value of Ksp be for calcium fluoride? 3) A solution is made by diluting 10.0 mL of 0.021 M potassium dichromate to 200 mL. What is the molarity of the diluted solution?