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Chemical Equilibrium

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˚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

Calculate Eqiulibrium Constant

Calculate the value of the equilibrium constant for each of the following reactions ( we abbreviate citric acid as H3Cit) using the Ka values for citric acid and for carbonic acid: H3Cit + HCO3- <--> H2Cit- + H2O +CO2 H3Cit + 3HCO3- <--> Cit3- + 3H2O +3CO2 Given Ka1 of H3Cit =8.4x10-4; Ka2 of H3Cit = 1.8x10-5; Ka3 of H3Ci


I am enclosing a problem is causing me some doubt. As you will read from the problem wording, It seems that the value should be 0.3 mole as well. However, it is not within the options. (See attached file for full problem description) --- When 2.0 mol of carbon disulfide and 4.0 mol of chlorine are placed in a 1.0 Liter fl

Equilibrium Constant in Half-Reactions

What is the Ecell and the equilibrium constant, Kc, for the cell represented by the combination of the following half-reactions? 2 Hg2+(aq) + 2e- equilibrium Hg2 2+(aq) E= 0.92V Cr3+(aq) + 3e- equilibrium Cr(s) E= -0.74 V

The hemoglobin molecule carries oxygen in the blood

Please help answer the following problems. Include references in the solution. The hemoglobin molecule carries O2 in the blood from the lungs to the cells, where the O2 is released for metabolic processes. The molecule can be represented as Hb in its unoxygenated form and as Hb.O2 in its oxygented form. One reason CO is to

Equilibrium Concentration Functions

3. A complex ion forms between Ag+ and CN- to give [Ag(CN)2]- with a formation constant of 1.3 x 10 to the 21. To a 0.5 M aqueous solution of silver nitrate you and sufficient HCN to make it 2 M. The Ka for HCN is 6.03 x 10 negative 10. What are the equilibrium concentrations of Ag+, [Ag(CN)2]-2, H+, and HCN?

Pressure's Effect on Equilibrium

When hydrogen gas reacts with Iodine as a gas, Hydrogen Iodine is produced in its gaseous form. The equilibrium concetrations for both reactants were found to be 0.86 M and the product was found to be 0.27. Calculate the value of the equilibrium constant. How would pressure effect the equilibrium of this reaction?

Chemistry Calculations and Concepts

Determination of the Molar Mass and Ionization Constant of a Weak Monoprotic Acid Acetic Acid + Water yields Conjugate Base + Hydronium Ion Or HA + H20; H30+ + A- Calculation of the ionization constant for acetic acid from the measured pH of acetic acid samples: Acetic Acid titrated with Sodium Hydroxide and the followin

Gas Reaction Explanation

Step by Step Explanation Ethylene, C2H4, will react with hydrogen gas under appropriate conditions to form ethane, C2H6. A 10.0-liter vessel is charged with 1.5 atm of hydrogen and 1.0 atm of ethylene at 25°C. The reaction is allowed to proceed to completion. Determine the total pressure in the vessel at 25° at the completi

Calculating Values of Equilibrium Constants

Question states: In the reaction of ammonium chloride (as a solid) dissociating to produce ammonia and hydrogen chloride (both as gases), the equilibrium concentration of each product was found to be 3.71x10^-3 (they each have the same concentration, ammonia is 3.71x10^-3 and hydrogen chloride is 3.71x10^-3). Calculate the v

Chemistry Equilibria Example Problem

Of the following equilibria, only _______ will shift to the left in response to a decrease in volume. a. H2 (g) + CL 2 (g) <-> HCL (g) b. 2SO3 (g) <-> 2SO2 (g) + O2(g) c. Ns (g) = 3H2 (g) <-> 2NH3 (g) d. 4Fe (s) = 3O2 (g) <-> 2Fe2O3 (s) e. 2HI (g) <-> H3(g) + I3 (g)

Equilibrium & Buffers

1. You have a 0.087565 M solution of a weak acid, HA, pH=4.18177. How many grams of NaA (molar mass = 62.476 g/mol) would you have to add to this solution (assume that there is no change in volume) to have a solution with a pH of 7.40000. Would this new solution be a good buffer? Please explain. 2. You have a mixture of

Reaction Kinetics - Equilibrium

A.) Consider the reaction: 4HCl (aq) + MnO2 (s) <--> Cl2 (g) + 2 H2O (l) + MnCl2 (aq) Delta (H)degree The equilibrium is displaced to the left if: a. Catalyst is added b. pressure is lowered c. temp is lowered d. H2O is added e. none of these b.) Consider the following gas phase reaction at 25 oC. N2 (g) + C2H2

Some Chemistry Problems

A.) For the reaction: 2Cl2 (g) + 2H2O(g) <----> 4HCl(g) + O2 (g), Kp = 6.4 x 10-6 at 500 K. If a fixed volume is filled with initial concentrations of these gases at 227 oC such that [Cl2] = 0.5 M, [H2O] = 0.40 M, [HCl] = 0.5 M, and [O2] = 0.015 M, in which direction will the reaction proceed? b.) 4.00 mol chlotine and 2.00 m

General Chemistry

1. 4CuO(s) + CH4(g) CO2(g) + 4Cu(s) + 2H2O(g) The value of Kc for this reaction is 1.10 at 25.0°C. What is the value of Kp for this reaction? (R = 0.0821 L-atm/K-mol) a. 4.63 b. 26.9 c. 658 d. 37.2 e. 1.52 x 10-3 2. At a certa

Complex ion equilibria

Complex-Ion Equilibria. When sufficient ammonia is added to a 0.00500 M silver nitrate solution to initially give 0.100 M aqueous ammonia, what is the molarity of the silver ion (Ag+) after the complex ion Ag(NH3)2+ has been formed at equilibrium? Ag+(aq) + 2 NH3(aq) = Ag(NH3)2+(aq)

Solubility and common ion effect

Please help with the following problem. Provide a step by step solution. Solubility and the Common-Ion Effect. In problem 1 it was stated that the molar solubility of PbBr2 in pure water is 1.3 x 10-2 M. Calculate the molar solubility of PbBr2 in A) 0.20 M KBr and in B) 0.20 M Pb(NO3)2 Problem 1 in reference is: The Sol

The solubility product constant

The Solubility Product Constant. PbBr2 is a slightly soluble salt. Write A) the chemical equilibrium equation that describes the salt partially dissolving in water and B) the solubility product expression. C) Calculate the Ksp value for lead(II) bromide if the molar solubility in pure water is 1.3 x 10-2 M.

Chemistry Derivative

LnP = - (delta H vap/ T) (1/T)+C ln P2 = lnP1 + delta H vap / R (1/T - 1/T2) )Gvap=)Hvap - T) Svap G=0. See the attached file.

Calculating Equilibrium Concentrations

Calculating Equilibrium Concentrations. Consider the reaction SO2(g) + NO2(g) = NO(g) + SO3(g) at 460 C. What are the equilibrium concentrations of all reactants and products if the initial concentrations are [SO2]o = [NO2]o = 3.00 x 10-3 M and [NO]o = [SO3]o = 4.00 x 10-2 M? The value of the equilibrium constant for the