HomeworkLib
Question

The Henry’s law constant for H2S is 0.1 mole/L-atm. H2S(aq) ↔ HS-(aq) + H+ , where...

The Henry’s law constant for H2S is 0.1 mole/L-atm. H2S(aq) ↔ HS-(aq) + H+ , where Ka = 0.86 x 10-7. If you bubble pure H2S gas into a beaker of water (meaning the partial pressure for H2S(g) is 1 atm), calculate [HS-(aq)] and [H2S(aq)] at a pH of 5 in moles/L, respectively. Ans: [H2S] = 0.1 M; [HS-] = 8.6 x 10-4 M at pH = 5

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Request Professional Answer

Request Answer!

We need at least 10 more requests to produce the answer.

0 / 10 have requested this problem solution

The more requests, the faster the answer.

Request! (Login Required)

All students who have requested the answer will be notified once they are available.
Know the answer?
Add Answer to:
The Henry’s law constant for H2S is 0.1 mole/L-atm. H2S(aq) ↔ HS-(aq) + H+ , where...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Similar Homework Help Questions

  • 1. The Henry’s Law constant for O2 is 770 L atm mol-1 at 25 °C. What...

    1. The Henry’s Law constant for O2 is 770 L atm mol-1 at 25 °C. What mass of oxygen would be dissolved in a 40-L aquarium at 25 °C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of O2 is 0.21 atm? 2.The carbon dioxide concentration in a bottle of club soda is 0.12 mol L-1 at 25 °C. What is the pressure of carbon dioxide in the headspace? The Henry’s Law constant for CO2 at...

  • The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq)&nb...

    The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq)          + H2O (l) <=> HS -(aq)     + H3O +(aq)                   Ka =    1.0 x 10 -7 HS -(aq)     + H2O (l) <=> S-2 (aq)    + H3O +(aq)                                     Ka =    1.3 x 10 -13    What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?

  • Henry’s law states that the solubility of a gas is directly proportional to the partial pressure...

    Henry’s law states that the solubility of a gas is directly proportional to the partial pressure of the gas if the temperature is constant. Hyperbaric chambers, which provide high pressures (up to 6 atm) of either air or pure oxygen, are used to treat a variety of conditions, ranging from decompression sickness in deep-sea divers to carbon monoxide poisoning. Look up the Henry’s Law Constant (kH) for N2, O2, and CO2 in the textbook. a) Calculate the solubility (concentration in...

  • 1- At 25 oC the Henry’s Law constant for carbon dioxide (CO2) dissolved in water is...

    1- At 25 oC the Henry’s Law constant for carbon dioxide (CO2) dissolved in water is 3.3 x 10-2 mol/L atm. Calculate the solubility of CO2 if the partial pressure of carbon dioxide gas inside a bottle of Fizzy Cola Drink is 6 atm at 25 C 2- Using Raoult’s Law, calculate vapor pressure lowering, DP = C · Po, when 14.0 mL of glycerol (C3H8O3) is added to 496.0 mL of water at 50.0 C. The density of glycerol...

  • In a closed system with 0.1 L water and 50 mg of solids, 3 x 10-5 moles of benzene are added. Hbenzene = 5.56 atm-L/mole...

    In a closed system with 0.1 L water and 50 mg of solids, 3 x 10-5 moles of benzene are added. Hbenzene = 5.56 atm-L/mole MW of benzene = 78 g/mole R = 0.082 atm-L/mole-K T=25C Kd for benzene = 50 L-water/kg-solids a. What is the concentration of dissolved benzene? b. What is the concentration of benzene sorbed to the solids in moles/L?, moles/kg-solids? c. What fraction of the benzene is in the solid?

  • The log Henry's law constant (units of L-atm/mole and measured at 25 C) for trichloroethylene is...

    The log Henry's law constant (units of L-atm/mole and measured at 25 C) for trichloroethylene is 1.03; for tetrachloroethylene, 1.44; for 1, 2-dimethylbenzene, 0.71; and for parathion, -3.42. (a) What is the dimensionless Henry's law constant for each of these chemicals? (b) Rank the chemicals in order of ease of stripping from water to air. If needed use ideal gas Law (pV= nRT). R = 0.08205 (atm times L)/(mole times K). The dimensionless Henry's law constant is equal to K_H(L_H_2...

  • a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated...

    a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated beverages are less acidic than pure water. B. carbonated beverages contain measurably less water than the same volume of pure water. C. rainwater is slightly acidic b) A 1.0 M solution of a weak monoprotic acid with Ka = 1.0 10-6 would have a pH of: A. 1 B. 2 C. 3 D. 6 c) Ascorbic acid is a diprotic acid with Ka1 =...

  • Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O...

    Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O (l) A 1.0 L buffer solution is 0.280 M in HC2H302 (acetic acid) and 0.320 M in NaC2H302 (sodium acetate). Calculate the pH of the budder and he Ka for HC2H3O2 IS 1.8 X 10-5 Calculate the pH of te solution above after the addition of 0.0400 moles of solid NaOH. Assume no volume change upon the addition of base.

  • a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated beverages are less acidic than pure water. B. carbonated beve...

    a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated beverages are less acidic than pure water. B. carbonated beverages contain measurably less water than the same volume of pure water. C. rainwater is slightly acidic b) A 1.0 M solution of a weak monoprotic acid with Ka = 1.0 10-6 would have a pH of: A. 1 B. 2 C. 3 D. 6 c) Ascorbic acid is a diprotic acid with Ka1 =...

  • (8 pts) Carbon dioxide in the atmosphere dissolves in water to establish an equilibrium that can...

    (8 pts) Carbon dioxide in the atmosphere dissolves in water to establish an equilibrium that can increase the acidity of aqueous solutions in the environment. This equilibrium is CO2 (g) ⇌ CO2 (aq), Kh = 3.1 * 10^2 at 25°C. Kh is called the Henry’s law constant, which relates the solubility of the gas CO2 in the aqueous solution, [CO2], to the partial pressure of CO2 over the solution, p(CO2): [CO2] (M) = Kh * p(CO2) (atm) During the preceding...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT