Sulfur dioxide (SO₂) is a gas pollutant that is released during combustion of coal. If the partial pressure of sulfur dioxide in the air above a smoke stack is 0.05 atm and the reactions below dictate how sulfur dioxide equilibrates with water, find the equilibrium pH of a rain drop falling over the smokestack. This may be considered an OPEN system. Solve this problem using the following methods: (i) approximation with the graphical method and simple solutions; and (ii) mathematically by solving the ENE. SO2(g) → SO2 (aq) SO2 (aq) +H₂O H₂SO3 H₂SO3 H+HSO) KH = 1.23 M/atm Note, H₂SO, is the aqueous form of sulfur dioxide KA-1.26 x 10-²

Sulfur dioxide (SO₂) is a gas pollutant that is released during combustion of coal. If the partial pressure of sulfur dioxide in the air above a smoke stack is 0.05 atm and the reactions below dictate how sulfur dioxide equilibrates with water, find the equilibrium pH of a rain drop falling over the smokestack. This may be considered an OPEN system. Solve this problem using the following methods: (i) approximation with the graphical method and simple solutions; and (ii) mathematically by solving the ENE. SO2(g) → SO2 (aq) SO2 (aq) +H₂O H₂SO3 H₂SO3 H+HSO) KH = 1.23 M/atm Note, H₂SO, is the aqueous form of sulfur dioxide KA-1.26 x 10-²

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

For the reaction aA(aq) + bB(1) cC(g) + dD(aq) the equilibrium constant, K, can be written as Pc- [D]d [A]a K= The equilibrium constant is unitless because the units always mathematically cancel when the pressure is expressed in torr and concentration is expressed in molality. each quantity is a dimensionless ratio of the actual concentration or pressure divided by standard state concentration or pressure. pressure and concentration are unitless quantities. taking each pressure or concentration to its coefficient power cancels out the units.
Initial (M) Change (M) Equilibrium (M) Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka for HC,H,O₂ is 6.3 x 105 Complete Parts 1-3 before submitting your answer. NEXT The buffer was prepared by dissolving 21.5 g HC,H,O₂ and 37.7 g of NaC,H,O₂ in 200.0 mL of solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. HC,H,Oz(aq) 0.178 0.880 x 0 0.888 1.31 + x Question 3 of 10 21.5 0.178 + x 37.7 H₂O(l) 0.888 + x 0.176 21.5 - x 0.261 37.7 + x HO*(aq) 0.880 0.176-x RESET 1.31 0.261+x + CH,Or(aa)
The osmotic pressure of a saturated solution of strontium sulfate at 25 °C is 21 torr. What is the solubility product of this salt at 25 °C?
Using the procedure in Determination of an Equilibrium Constant, a student combines equimolar amounts of acetic acid and ethanol to react as shown by the following equation. acetic acid + ethanol e ethyl acetate + water To determine the initial concentration of acetic acid, 1.00 mL of the resulting mixture was titrated with 0.2950 M NaOH, requiring 31.25 mL. What is the molarity of the acetic acid? Type answer:
In the laboratory, a general chemistry student measured the pH of a 0.470 M aqueous solution of diethylamine, (C2H5)½NH to be 12.272. Use the information she obtained to determine the Kp for this base. K„(experiment) :
(a) If the molar solubility of Sc(OH)3 at 25 °C is 9.52e-09 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 5.73e-05 g of Zn3(ASO4)2 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility-product constant for Zn3(ASO4)2. Ksp (c) The Ksp of Nd₂(CO3)3 at 25 °C is 1.08e-33. What is the molar solubility of Nd₂(CO3)3? solubility = mol/L
Write the expression for the solubility-product constant of the ionic compound: AgI
At 2257 K and 1.00 bar total pressure, water is 1.77 per cent dissociated at equilibrium by way of the reaction 2 H₂O(g) 2 H₂(g) + O₂(9) Calculate K. K = 40
Calculate the molar silver ion concentration in a saturated solution of silver sulfate, Ag2SO4, The Ksp of silver sulfate is 1.4 ´10–5).
3.) A 15.00 mL sample of 0.250 M formic acid (HCOOH, Ka = 1.8 x 104) is titrated with 0.300 M sodium hydroxide (NAOH), The following neutralization reaction is observed, Calculate the pH of the solution at the following intervals of NaOH added. HCOOH(ag) + NaOH(aq) → NaCOOH(aq) + H2O(1) a.) 4.50 mL NAOH b.) Half-equivalence point c.) 12.5 mL NaOH
(a) In the determination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in mg/L., on the basis of the solubility product principle, when the chloride concentration has been reduced to 0.2 mg/L? (b) If the concentration of chromate indicator used is 5 x 10 M, how much excess silver ion in mg/L. must be present before the formation of a red precipitate will begin?
Copper(I) ions in aqueous solution react with NH, (aq) according to Cu* (aq) + 2 NH, (aq) → Cu(NH, ) (aq) K = 6.3 x 1010 Calculate the solubility (in g-L-!) of CuBr(s) (Ksp = 6.3 × 10-9) in 0.73 M NH, (aq). solubility of CUB1(s): g/L