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Find the equilibrium concentrations for HA, H+, and A - HA<-->H^++A^-
Kc=0.20
Initial concentrations HA=.30 H+=0 A-=0
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- For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Kc1,1, or 1 for a titration reaction?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.For the reaction 4 PH; (g) = 6 H,(g) + P¿(g) the equilibrium concentrations were found to be [PH,] = 0.250 M, [H,] = 0.370 M, and [P] = 0.750 M. What is the equilibrium constant for this reaction? K.
- Question 15 of 25 Submit For the reaction below, Kc = 1.10 x 10-8. What is the equilibrium concentration of OH- if the reaction begins with 0.610 M HONH,? HONH, (aq) + H,O (1) = HONH;* (aq) + OH¯ (aq) | M 1 2 3 C 7 9. +/- x 10 0 LO 00For 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)For the reaction 4 PH, (g) = 6 H, (g) + P,(g) the equilibrium concentrations were found to be [PH,1-0.250 M, [H,]-0.540 M, and [P,] = 0.750 M. %3D What is the equilibrium constant for this reaction? K, - + TOOLS x10
- Consider the reaction: HC,H;O-(aq) + H2O(1) = H;0*(aq) + C,H;O, (aq) K = 1.8 x 10-5 at 25 °C If a solution initially contains 0.210 M HC,H;O, what is the equilibrium concentration of H30* at 25 °C?For 0.10 M aqueous solutions of each of the following acids, which one will have the fewest number of product ions at equilibrium? O CH3COOH (K = 1.8 x 10-5) %3D O HF (Ka = 3.5 x 10-4) O HCIO2 (K, = 1.0 x 10 2) O HCIO (K, = 3.0 x 10 8) « Previous t (9).docx BluebeardBrothers.pdf Discussion week.docx upd wnkep ype here to searchConstruct an "I-C-E" table that describes the equilibrium system of HCOOH with a nominal concentration of 0.50 M. Define clearly what is meant by "x" in the table. Use a squiggly li (~) to indicate approximate values. I - C E
- The acid-dissociation constant for benzoic acid 1C6H5COOH2 is 6.3 * 10-5. Calculate the equilibrium concentrations of H3O+, C6H5COO-, and C6H5COOH in the solution if the initial concentration of C6H5COOH is 0.050 M.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?Calenlate the ptl of I15 M tydrofluoric acíd (HP) it the K, =7.2x10*?
