SOLUBILITY PRODUCT PRINCIPLE At 25 °C, the molar solubility of the sparingly soluble salt M3X is 5.44 x 10² M. 1. Write the equilibrium reaction for the dissolution of M3X. 2. Construct an ICE table and calculate the Ksp of M3X at 25 °C. 3. If 1.04 g of M₂X was added to 1.00 L of a saturated M3X solution at 25 °C and produced a saturated solution at 60 what is the molar mass of M3X? Ksp of M3X at 60 °C: 4.36 x 10-4

SOLUBILITY PRODUCT PRINCIPLE At 25 °C, the molar solubility of the sparingly soluble salt M3X is 5.44 x 10² M. 1. Write the equilibrium reaction for the dissolution of M3X. 2. Construct an ICE table and calculate the Ksp of M3X at 25 °C. 3. If 1.04 g of M₂X was added to 1.00 L of a saturated M3X solution at 25 °C and produced a saturated solution at 60 what is the molar mass of M3X? Ksp of M3X at 60 °C: 4.36 x 10-4

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

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 500. ml. flask with 1.4 atm of sulfur dioxide gas and 1.8 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.84 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K Р 0 X ola
Express the equilibrium constant (K) for the chemical equations. (Note the physical states) A. CH3OH (g) ↔ CO (g) + 2 H2 (g) B. C3H8 (g) + 5 O2 (g) ↔ 3 CO 2 (g) + 4 H2O (g) C. SbCl5 (g) ↔ SbCl3 (g) + Cl2 (g)
A student ran the following reaction in the laboratory at 637 K: 2HI(g) H2(g) + I2(g) When she introduced 0.390 moles of HI(g) into a 1.00 liter container, she found the equilibrium concentration of HI(g) to be 0.313 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. K. =
produces N20 and oxygen. Calculate the value of the equilibrium constant K. for the reaction 2 N,O4(g) –2 N,0(g) + 3 O2(g) from the following information: N2(g) + ¿O2(g) =N‚O(g) K¸ = 2.7 × 10-18 N,O4(g) =2 NO;(g) K. = 4.6 × 10-3 N2(g) + 2 O2(g) =2 NO2(g) K. = 1.7× 10-17
A student ran the following reaction in the laboratory at 286 K:2CH2Cl2(g) CH4(g) + CCl4(g)When she introduced 6.64×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.09×10-2 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.Kc =
I had 1.0 mL of 1.0M CoCl2 in a test tube. I put it into boiling water. [Co(H2O)6]2+, [CoCl4]2- Equilibrium temperature effect. Effect of heat What happens to the equilibrium? Use this equation in your explanation... 4Cl_ (aq) + [Co(H20)6]2+(aq)---[CoCl4]2-(aq)+ 6 H20 (l) I did this in class. The color change was very slow but it changed from a burgandy to fushia.
A student ran the following reaction in the laboratory at 544 K: COC12(g) → CO(g) + Cl₂ (9) When she introduced 0.930 moles of COCl2 (g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂ (g) to be 0.0369 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
G.193.
Calculating equilibrium concentrations using the raction quotient
2. A mixture of 0.500 mol Nz and 0.500 mol H2 was placed in a 1.00-L stainless-steel flask at 430 degrees Celsius. Determine the value of the equilibrium constant, Kc, when the equilibrium concentration of nitrogen [N2] (g) = 0.43 M. N2 (g) + 3H2 (g) -> 2NH3 (g)
The following reaction is known as the water- gas shift reaction: H2(g) + CO2(g) – – CO(g) + H20(g) for which Kc = 1.53 at a temperature of 686 •C. a. Write an equation for Kc for this reaction in terms of the reactant and product concentrations. b. If you start with only 1.50 M of H20 and 1.50 M of CO, what will the equilibrium concentrations of all four substances be? Construct an ICE table and use the value for Кс above. c. What is the value of Kp for this reaction at 686 •C? d. If the reaction were at equilibrium and then CO2 was removed, in what direction would the reaction shift to recover equilibrium?
At a particular temperature, the equilibrium amounts of hydrogen, iodine and hydrogen iodide present in a 4.00 L flask are found to be: 0.25 moles of hydrogen gas, 0.15 moles of iodine gas and 1.37 moles of hydrogen iodide gas. H2(g) + I2(g) ↔ 2 HI(g) Calculate the equilibrium constant, Kc, value for the reaction.