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8. Write the ionic equation for dissolution and the solubility product (K ) expression for each...
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...
Chapter 15 Classroom Assignment Write the one equation for dissolution and the solubility product of the following slightly soluble ionic compounds pression for each PCI PCI,() Pb(aq) + 2Cl(a). K - P C AS A S) 2Ag (aq) + (aq). K - Ag Tis 0:2 gives solubilities of the following compounds in grams per 100 ml of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for...
13. Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product: (a) KHC4H4O6 (b) PbI2 (C) Ag4[Fe(CN)6], a salt containing the Fe(CN)4- ion (d) Hg2I2
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
#3. - Determine the pH, [H3O+], pOH and [OH‾] for each of the following. Be sure to write balanced chemical equation and the set-up for solving the problem. a. 1.5 M HNO3 b. 0.25 M Sr(OH)2 c. 0.035 M HNO2 d. 0.0048 M Mn(OH)2 #1 - What are the [H3O+] and the pH of a solution that consists of 0.33 M C6H5COOH (benzoic acid) and 0.28 M C6H5COONa (sodium benzoate)? The Ka of benzoic acid is 6.3 x 10-5. #8-...
#5 Write the solubility product expression for PbCl2.
Using the concentration for the Pb+2 and Cl- ions, solve for your
experimental Ksp.
#6 Using your book, find the theoretical Ksp for PbCl2
to determine your percent error
A Solubility Product Constant Introduction: Many substances are very soluble in water. However, in this experiment you will be concerned with substances that are insoluble or only slightly soluble. Dynamic equilibrium is established when an excess of a slightly soluble substance is placed...
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)...
Module 26 Questions for Group Work 1) Write the expression for the solubility-product constant expression for each of the following compounds. (a) MnCO3 (b) Fe(OH)2 (c) Cu3(PO4)2
8/Write the dissociation equation of the following ionic compounds. (thromivm IT a. Cr3(PO4)2 C b. Bi2S5 c. Sr(OH)2
8/Write the dissociation equation of the following ionic compounds. (thromivm IT a. Cr3(PO4)2 C b. Bi2S5 c. Sr(OH)2