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Chemical Equilibrium

equilibrium constant and pH during titration

HOBr(aq) ----> H+(aq) + OBr-(aq) Ka = 2.3 x 10-9 1. Hydrobromous acid, HOBr, is a weak acid that disassociates in water, as represented by the equation above. (a) Calculate the value of [H+] in a HOBr solution that has pH of 4.95. (b) Write the equilibrium constant expression for the ionization of the HOBr in water,

solubility of MgF2

5. In a saturated solution of MgF2 at 18C , the concentration of Mg2+ is 1.21 x 10-3 molar. The equilibrium is represented by the equation below MgF2(s) ---> Mg2+ (aq) + 2F- (aq) A) write the expression for the solubility product , Ksp , and calculate its value at 18C B) predict whether a precipitate of MgF2 will fo

Silver Chromate Solubility and Precipitation

Answer the Questions based on Ag2CrO4 (Silver Chromate) and Ag3PO4 . Silver Chromate dissociates in water according to the equation. Ag2CrO(s)<->2Ag+ CrO4 Ksp= 2.6x10^-12 at 25 deg C. a) Write the equilibrium constant expression for Ag2CrO4 (Silver Chromate) b) Calculate the concentration, in mol L-1 of Ag in a saturated so

Relating to the solubilities of two silver compounds

Answer the following questions relating to the solubilities of two silver compounds. Ag2CrO4 and Ag3PO4 Silver chronate dissociates in water according to the equation shown below Ag2CrO4 (s). = 2 Ag+ (aq) + CrO4 2- (aq) Ksp = 2.6 x 10^-12 at 25C A) write the equilibrium constant expression for the dissolving of Ag

Equilibrium: solubility

Answer the following questions that relate to solubility of salts of lead and barium: A) A saturated solution is prepared by adding excess PbI2(s) to distilled water to form 1.0 L of solution at 25C. The concentrations of Pb2+ (aq) in the saturated solution is found to be 1.3 x 10^-3 M. The chemical equation for the dissoluti

Chemical Equilibrium: Constants, Temperature, Concentrations

1. Describe the equilibrium constant in terms of the law of mass action and write equilibrium constant expression for multiple equilibria. 2. Relate the constants and equilibrium constants and describe how equilibrium varies with temperature. 3. Use equilibrium constants to predict the direction of a reaction towards equil

Mass of o-xylene

Im confused on how to set this problem up while incorporating the water, octanol, and air in one equation so I can solve for the mass. Help is much appreciated! thank you A stoppered flask at 25 C contains 250 mL water, 200 mL octanol, and 50 mL of air. An unknown mass of o-xylene is added to the flask and allowed to partit

Chemical Reaction - Find unknown mass

A stoppered flask at 25 C contains 250 mL water, 200 mL octanol, and 50 mL of air. An unknown mass of o-xylene is added to the flask and allowed to partition among the phases. After equilibrium has been established, 5.0 mg of o-xylene are measured in the water. What is the total mass (g) of o-xylene present in the flask?

partition of o-xylene among phases..

Could you please explain what formula and step are invovled and please provide (example) if possible A stoppered flask at 25 C contains 250 mL water, 200 mL octanol, and 50 mL of air. An unknown mass of o-xylene is added to the flask and allowed to partition among the phases. After equilibrium has been established, 5.0 mg of

HETP Calculations from Distillations

I am trying to figure out a few questions/problems. -You want a column to have 6 theoretical plates. Your packing material has a HETP value of 1.5. What is the length of the column that you would need? I thought I would multiply the 6 TP by the HETP value. (This was a past quiz question) How do I solve this type of question?

Equilibrium Temperature Calculation

1.) Calculate Ke for the following (equilibrium concentrations given below substances). See attached file for full problem description. 2.) For all three of the equilibria in problem #1 predict (1) how Ke is affected by an increase in temperature, (2) predict how the equilibrium will sh

Haber Process and Solving for Kc

The Haber process for ammonia synthesis is exothermic: N2(g) + 3H2(g) <--(double arrow for equilibrium) --> 2NH3(g) Change in H (degrees) = -92KJ If the equilibrium is constant Kc for this process at 500 Degrees Celsius is 6.0 X 10^-2, what is its value at 300 Degrees Celsius. I am not sure which equation I shou

Equilibrium Concentrations: Example Problem

Problem: Consider the following gas-phase equilibrium reaction: N2(g) + 02(g) <-- (double arrow for equilibrium) --> 2NO(g) Kc = 4.10 X 10 ^-4 at 2000 Degrees Celsius. If 1.0 mol of NO is introduced into a 1.0 L container at 2000 Degrees Celsius, what is the concentration of NO when equilibrium is reached.

Equilibrium constant expressions: Example problems

1. Write the equilibrium constant expression (K) for the following reaction CS2 (g) + 4H2 (g) --> CH4 (g) + 2H2S (g) 2. Write the equilibrium constant expression (K) for the following reaction CuO (s) + H2 (g) --> Cu (s) + H2O (g) 3. Ammonium chloride is sometimes used as a flux in soldering because it decomposes upon he

Equilibrium Concentration of Gas: Example Problem

The equilibrium constant for Kc for the reaction shown is 54.3 at 430 degrees C. H2(g) + I2(g) --> 2 HI(g) At the start if the reaction there are 0.714 moles of H2, 0.984 mole of I2 and 0.886 mole of HI in a 2.00 liter reaction chamber. At equilibrium, what are the concentrations of the gases-

Nitric oxide air polution

The equilibrium constant (Kp) for the formation of the air pollutant nitric oxide (NO) in an automobile engine at 530 degree C is 2.9 x 10 to the minus eleventh N2(g) + O2 (g) = 2 NO (g) What is the partial pressure of NO under these conditions if the partial pressures of nitrogen and oxygen are 3

Equilibrium Constant for the Decomposition of Compounds

1. What is the equilibrium constant for the decomposition of NO: 2NO ---> N2 + O2 at room temperature? For NO: DHf° = 90.25kJ/mol and DGf° = 86.57kJ/mol 2. Using the data in problem 1, find the temperature, if any, at which the equilibrium constant for the decomposition of NO would be 1.

Equilibrium Concentration for BaSO4

The Ksp for BaCO3 is 5.1 x 10-9, while that for BaSO4 is 1.1 x 10-10. What would be the equilibrium concentrations of CO3-2 and SO4-2, if solid BaSO4 were placed in a 0.01M CO3-2 solution?

Calculating PH Concentration

The formation constant for zinc tetraammine ion [ Zn(NH3)4+2] is 4.1 x 108. What is the concentration of free Zn+2 in a solution of 3M NH3 (total ammonia) buffered to a pH of 9.0 if the total zinc concentration is 0.1M? The Kb for NH3 is 1.8 x 10-5

Calculating the concentration of ion at equilibrium

Please help with the following problem. Provide step by step calculations. Consider a solution that is 0.10 M in a weak triprotic acid that is represented by the general formula H3A with the following ionization constants: For H3A: Ka1= 1.0 x 10 ^-3 Ka2= 1.0 x 10 ^-8 Ka3= 1.0 x 10 ^-12 What is the concentration of

For the water-gas reaction (Problem 43 attached) Kc = 0.111

For the water-gas reaction (Problem 43 attached) Kc = 0.111 at about 1100 K. If 0.100 mol H2) (g) and .100 mol H2 (g) are mixed with excess C(s) at this temperature and equilibrium is established, how many moles of CO (g) will be present? No CO (g) is present initially.

Isomers of D-glucose

4. Start with an open-chain model of glucose then form the hemi-acetal using the carbon #5 -OH and the carbonyl at carbon 1 then reverse the process and remake the open-chain form. 5. Reclose the ring making sure that you come up with a different product. a. Did you build the alpha or beta anomer? b. Based on your models,

Chemical Equilibrium

1. Define dynamic equilibrium state in terms of a) reaction rates b) change in observable properties c) energy and entropy state 2. In which of these closed containers is the vapour pressure the greatest? Explain the choice. a) a 1 L container with 5 mL of water held at 20&#730;C b) a 1 L container with 15 mL of water

Tautomerism and non-bonding electrons

The following tautomerism has been observed. Add any non-bonding electrons. Use arrows to push electrons and show how the structure on the left can be transformed to the structure on the right. Which side of the equilibrium is favored? Why? (see diagram in attached file) ---

Titration of Borax with HCl

1. Would the experimental values of Ksp, (see attachment for formatting); be affected if the samples titrated contained large amounts of solid borax? If so, would the experimental values be falsely high or falsely low? Explain 2. Does the equilibrium constant change as the temperature changes? If so, explain why the equi