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- The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem: MgF2(s)Mg2+(aq)+2F(aq) In a saturated solution of MgF2 at 18 C, the concentration of Mg2+ is 1.21103M . The equilibrium is represented by the preceding equation. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 18 C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible. (c) Predict whether a precipitate of MgF2 will form when 100.0 mL of a 3.00103 -M solution of Mg(NO3)2 is mixed with 200.0 mL of a .2.00103 -M solution of NaF at 18 C. Show the calculations to support your prediction.. (d) At 27 C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17103M . Is the dissolving of MgF2 in water all endothermic or an exothermic process? Give an explanation to support your conclusion.The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) 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 each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
- Write the expression for the equilibrium constant for each of the following reactions. Write the pressure of a gas, X, as PX.(a) 3Ag+(aq)+PO4(3-)(aq)-->Ag3PO4(s) (b) C6H6(l)+(15/2)O2(g)-->3H2O(l)+6CO2(g).com/course.html?courseld=17782388&OpenVellumHMAC=a4bc46ac4163ce8-The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20 so if a chemist added 1.19 x 10-2 M of Pb3(AsO4)2(aq) which is a common ion then what would be the concentration of the Arsenate ion AsO43-(aq) in Molarity at equilibrium? 1.97 x 10-2 2.78 x 10-2 2.38 x 10-2 1.74 x 10-2 3.24 x 10-2 2.99 x 10-2 2.57 x 10-2 2.11 x 10-2 1.55 x 10-2 1.35 x 10-2(a) Prepare the log C-pH diagram for Fe(OH);3 precipitation. Use the following equilibrium reactions. Fe(OH)3, + 3H Fe(OH);,3 + 2H" Fe(OH)3, + H Fe(OH):,s - Fe* + 3H:O - Fe(OH)* + 2H;O - Fe(OH)2* + H;O - Fe(OH); - Fe(OH); + H Ko = 1035 K1 = 1015 K2 = 10-25 K3 = 10120 K4 = 10*185 %3D %3D Fe(OH)3, + H;O %3D Start your answer by writing the equilibrium equation of each reaction and show the detailed mathematical manipulation steps on how you plot each of the equilibrium lines. Use the given grid paper and do not use spreadsheet software. Note that the given equilibrium constants are different from those used in the lecture.Consider the reaction IO4-(aq) + 2 H2O(l) = H4IO6-(aq) ; Kc = 3.5 * 10-2. If you start with 25.0 mL of a 0.905 M solution of NaIO4, and then dilute it withwater to 500.0 mL, what is the concentration of H4IO6- at equilibrium?For the reaction below, Kc = 1.10 x 10-8. What is the equilibrium %3D concentration of OH- if the reaction begins with 0.430 M HONH,? HONH, (aq) + H,O (I) = HONH;* (aq) + OH¯ (aq)Formic acid, HCOOH, ionizes in water according to the following equation. The equilibrium constant is K = 1.8 x 10-4. HCOOH(ag) - H,0(1) – HCOO (ag) + H,0*(aq) Calculate the equilibrium concentration of H3o* in a 0.985 Msolution. MThe thermodynamic solubility product of AGCN is 6.0x10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.7e-9 X mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.8e-15 X mol·L-1What is the ratio of SO42- to CO32- in a solution at equilibrium with both CaSO4 and CaCO3? (The solubility product of CaSO4 is 3.2 x 10-5).SEE MORE QUESTIONS