QUESTION 19 You add solid Cug(PO4)2 to a beaker containing 100.0mL of water at 298K. The solid does not appear to dissolve. You wait a long time and eventually measure the equilibrium concentration of PO4 in water to be 5.01x108 M. What is the Ksp of Cu3(PO4)2? Express your answer to the correct number of significant figures and in scientific notation.

QUESTION 19 You add solid Cug(PO4)2 to a beaker containing 100.0mL of water at 298K. The solid does not appear to dissolve. You wait a long time and eventually measure the equilibrium concentration of PO4 in water to be 5.01x108 M. What is the Ksp of Cu3(PO4)2? Express your answer to the correct number of significant figures and in scientific notation.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Predict the equilibrium concentration of NH in the reaction described below (for which Kc = 1.210 at the reaction temperature) by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. = NHSH(s) NH¸(g) + H₂S(g) Using the data from your ICE Table (Part 1), construct the expression for the equilibrium constant, Kc. Each reaction participant must be represented by one tile. Do not combine terms. KC = II = 1.2 × 10-4 RESET [x] [2x] [2x]² [1.2 × 104+x] [1.2 × 104-x] [1.2 × 104 + 2x] [1.2 × 104 -2x] [1.2 × 10+ + x]² [1.2 × 10+ - x]² [1.2 × 10+ + 2x]² [1.2 × 104 -2x]²
During an experiment, O.257 mol of H2 and 0.257 mol of I2 were placed into a 1.28 liter vessel where the reaction H2(g) + 12(g) 2 2HI(g) came to equilibrium. For this reaction, Kc = 49.5 at the temperature of the experiment. What were the equilibrium concentrations of H2, 12, and HI? [H2] = M %3D [12] = M [HI] = i M
At 460 °C, the reaction * NO(g) + SO3(g) SO2(g) + NO2(g) has Kc = 85.0. Suppose 0.109 mol of SO2, 0.0612 mol of NO2, 0.0755 mol of NO, and 0.118 mol SO3 are placed in a 10.0 L container at that temperature. What will the concentrations of all the gases be when the system reaches equilibrium? %3D [SO2) = M i [NO2] = M %3D [NO] = i M [SO3] = i M
Consider the given reaction. A(aq) + B(s) = C(aq) K = 9.40 Suppose 22.1 mol A reacts with excess B in 9.15 L of solution. Calculate the concentration of C at equilibrium. [C] = M
Suppose a 500. mL flask is filled with 0.20 mol of N2 and 1.6 mol of NO. The following reaction becomes possil N2(g) + O2(g) 2NO(g) The equilibrium constant K for this reaction is 0.205 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Шм ✗
Write the equilibrium-constant expression for the reaction A(s) + 3 B(1) ⇒ 2 C(aq) + D(aq) in terms of [A], [B], [C], and [D], as needed. Note that Kc, which is sometimes symbolized as Keq, denotes that the equilibrium constant is expressed using molar concentrations. For this question, Kc means the same thing as Keq. Kc =
Suppose a 250. mL flask is filled with 0.80 mol of I, and 1.7 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) The equilibrium constant K for this reaction is 0.600 at the temperature of the flask. Calculate the equilibrium molarity of I2. Round your answer to two decimal places. M X
Suppose a 500. mL flask is filled with 0.10 mol of O, and 1.6 mol of NO. The following reaction becomes possible: N2(g) + 0,(g) =2NO (g) The equilibrium constant K for this reaction is 0.679 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. | M
Five moles of an acid HA was dissolved in 5.0 L of solution. After the system had come to equilibrium, the concentration of HA was found to be 0.43 M. Calculate Ka for HA. (Write your answer in scientific notation) Ka = Submit Question 348 45,838 MAY tv L (9) S
For the reaction: 2 H2(g) + O2(g) = 2 H20(g) at a certain temperature the Keg is 1.8x105 If the concentrations in a reaction vessel at a given time are [H2] = 3.0 mol/L, [02] = 2.0 mol/L and [H,O] = 0.010 mol/L, which of the following statements is true? %3D %3D %3D The system is not at equilibrium, the reaction will proceed to the left O The system is at equilibrium since Q = K O The E, for the forward reaction is very large The system is not at equilibrium, the reaction will proceed to the right
0.1 gram of solid aluminum phosphate (Al(PO:) (s) is added to 500 L of pure water. Immediately the solid begins to dissolve according to the reactions below. Complete dissolution: Al(PO,) (s) → Al + PO, No K Solid present: Al(PO.) (s) + Al + PO, Ksp = 1012 %3D What is the concentration of dissolved phosphate (in M and mg/L) in the water once all reactions proceed to completion? Is the solid still present or has it completely dissolved? Why or why not? If the solid is present, calculate the solid concentration (in M and mg/L). Develop a plot showing the aqueous (dissolved) concentration of PO; (in M) on the Y-axis versus different AI(PO,)(5) additions (in M) on the X-axis. Include the critical point that separates whether the solid is completely dissolved or is still present and label your plot appropriately.
Consider the following reaction to form the anionic metal complex [CuCl2]- Cu+ (aq) + 2 Cl- (aq) ⇆ [CuCl2]- This reaction has an equilibrium constant value of Kc = 3.0 x 105 If the equilibrium concentration of reactants is [Cu+] = 0.014 M and [Cl-] = 0.012 M, calculate the concentration of the product, [CuCl2]- .