Module 26 Questions for Group Work 1) Write the expression for the solubility-product constant expression for...
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
Write the ionic equation expression for the dissolution and the solubility product expression for each of the following slightly soluble ionic compounds. A) Mg(NH4)PO4 B)Ca5(PO4)3OH
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...
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
Pre-lab Study Questions 1. Write the solubility product Ksp for the following compounds. a. FeS b. AgNO3 c. Mg(OH)2 d. Ca3(PO4)2 2. Consider a saturated solution of magnesium hydroxide Mg(OH)2. Answer the following questions. a. What would happen to the solubility of Mg(OH)2 if the solution were made up in 0.01 M Mg(NO3)2 instead of pure water? Explain. b. What would happen to the solubility of Mg(OH)2 if the solution were made up in 0.01 M NaOH instead of...
Write the solubility product constant expression for the solubility of Chromium (III) Hydroxide, Cr(OH)3. What would the solubility in g/100 mL of this salt be in water given the solubility product is 6.1 x 10 ^-31
Question 24 1 pts Write the solubility product constant expression for calcium phosphate, Ca3(PO4)2 O [Ca2+][PO43-M[Ca3(PO4)2] O Ca2+1*[PO43-12 O [Ca2+][PO43-1 O [Ca2+12[PO43-13
Write the solubility product constant expression and solve it in terms of s (solubility) for the dissociation of calcium fluoride (CaF2).
40. (a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 0.000165 g of Mg3(PO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Mg3(PO4)2. Ksp = (c) The Ksp of Ga(OH)3 at 25 oC is 7.28e-36. What is the molar solubility of Ga(OH)3? solubility = _______mol/L
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?