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- At a certain temperature, 0.35 g of BaF2 (Molar mass = 175) dissolves in pure water to form 1L of saturated solution. The solubility product for BaF, at this %3D temperature is... Oa. 3.2 x 10-6 b. 4.0 x 10-9 c. 3.2 x 10-8 d. 1.7 x 10-2 e. 3.2 x 10-9 Next pageSolubility 1. Lead (II) Cromate PbCrO4 is a slightly soluble salt with a Ksp = 2.8 x 10-13. a. Write the dissociation reaction (solubility expression) of PbCrO4 in water. b. What is the solubility product, Ksp, expression for PbCrO4 ? c. Calculate the solubility of PbCrO4.For the reaction: PbCl2(s) Pb2+(aq) +2C11-(aq), what is Q* when 8.0 mL of 0.050 M lead nitrate is added to 14 mL of 0.031 M sodium chloride? Ksp of lead chloride is 1.6 x 10-5 M³. Hint given in general feedback *Recall: Q is compared to Ksp to determine whether a precipitate forms.
- 1. Why must the solution be saturated when it’s solubility is determined? 2. Is Ca(OH)2 more soluble in aqueous solution containing calcium ions or in pure water? Explain your observation in terms of shift in equilibrium and in terms of the ion product in relation to Ksp.I need solutions Q a, c,d5.a. Write the equation for the dissolution of a Metal(II) chloride in water as well as the expression for Ksp. b. Calculate the solubility(s) and the solubility product, Ksp, for a Metal(II) chloride, if 50.0 mL of a saturated solution of Metal(II) chloride was found to contain 0.2207 g of Metal(II) chloride dissolved in it (Molar mass of M(II)Cl2 = 278.1g/mol, T = 250C). c. Based on the given molar mass, calculate the atomic mass of the metal. d. Identify the metal. Write the formula of its chloride salt. e. Discuss the effect of addition of few drops of HCl to the previous system in equilibrium at the same temperature.A. Calculations to construct the standard curve 1. Molar concentration of Fe(NO3)3 (from the label). 2. Molar concentration of NaSCN (from the label) 0.200M 0.00100M Standard Solutions Blank 1 3. Volume of NaSCN (mL) 0.00 1.0 2 3 4 2.0 3.0 4.0 4. Moles of SCN 0.00 5. [SCN] (25.00 mL) 0.00 6. [FeNCS²+] 0.00 7. Absorbance, A 0.00 100 10.0 0.148 0.251 10.0 10.0 0.423 0.548
- 1. Write the Ksp reaction and Ksp expression of zinc hydroxide. 2. Calculate the solubility of zinc hydroxide in (a) pure water and (b) 0.0130M zinc sulfate. Report your final answer in units of grams/L. The Ksp of zinc hydroxide is 3.0x10-17 3. For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. Use Ksp data from the ALEKS Data tab if needed. Compound Does solubility change with pH? (yes or no) Highest Solubility? pH = 3, 4, or 5? PbF2 Cal2 BaCl2 NaNO3 Selected Answers 2. (a) = 1.9x104 g/L, (b) = 2.4x10-6 g/L,1. Write the dissociation reaction and solubility product constant expression for the following sparingly soluble salt. a. AgBr Ksp = 5.2 x 10-13 b. PbCl2 Ksp = 1.7 x 10-5 2. Determine the Molar Solubility of the following sparingly soluble salt in water. a. AgBr Ksp = 5.2 x 10-13 b. PbCl2 Ksp = 1.7 x 10-5 3. Express the solubility (S) in question #2 in g/L. 4. Calculate Ksp for the ff. substances, given the molar concentration of their saturated solution. a. Ag2C2O4 ( S= 2.06 x 10-4 ) b. Al(OH)3 ( S = 1.82 x 10-9 ) 5. Calculate the molar solubility of the salts in problem #2 for the solution in which the cation concentration is 0.050 M.Give the expression for the solubility product constant for Ca3(PO4)2- Select one: O a. B Ca2+PR PO43-P Ca3(PO4)2 O b. [ Ca2+P[ PO43-P Ca3(PO4)2 O c. R Ca2+P[3 PO43-3 Ca3(PO4)2 O d. [ Ca2+j?[ PO43-73 O e. [Ca2+j³[PO43-12
- 5.The solubility product, Ksp, of sparingly soluble salt with the formula M2X (where M ismonovalent) in pure water is 1.1 x 10-12 at 250C.a. Write the equation for the dissolution of M2X as well as the solubility product of it.b. Calculate the solubility(s)of this salt. c. The molar mass of the salt is 332 g/mol and X is the chromate ion. Calculate the atomic mass of the metal. d. Identify the metal. Write the formula of the salt. e. Discuss what will happen if the temperature of the previous system was increased up to50oC then decrease to 15oC.Sodium chloride is added slowly to a solution that is 0.010 M in Cu*, Ag*, and Au*. Because solubility "rules" are generalizations, we don't use solubility rules when we have the specific Ksp data available. Instead, here, we can just use the Ksp value for CuCl which is 1.9 x 10-7, for AgCl is 1.6 x 10-10, and for AuCl is 2.0 × 10-13. Based on these specific Ksp values, which compound will precipitate first?Aluminum hydroxide (Al(OH)3 is sparingly soluble in water. The Ksp value at 25°C is 2.0 x 10-33 1.1. Write an equation for this reaction 1.2. Calculate the solubility of aluminium hydroxide. Aluminum hydroxide reacts with an excess of hydroxide ions to form the complex ion Al(OH)4-. 2.1.Write an equation for this reaction. 2.2. Write an equation for the formation of the complex ion Al(OH)4-. The value of Kf for this reaction = 1.0 x 1033. 2.3. Show that Keq for the reaction between aluminum hydroxide and hydroxide is: Keq = Ksp x Kf 2.4. Calculate Keq for this reaction Determine the solubility of Al(OH)3 (in mol/L) in the following solutions When the pH = 12.0. A 0.010 M solution of HNO3 A 0.010 M solution of acetic acid. Ka = 1.8 x 10-5