Please answer this question step by step. Previous expert response was incorrect. Thank you in advance....
Please answer this question step by step. Previous expert response was incorrect. Thank you in advance. Part A. Calculate the pH in 0.025 M H2SO3 (Ka1 =1.5 x 10^-2, Ka2 = 6.3 x 10 ^-8). Part B. Calculate the concentration of H2SO3, HSO3^- , SO3^2-, H3O^+, OH^- in 0.025 M H2SO3
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Thanks and please ask if u have any further doubts on this answer. Basically these kind of problems are solved using ICE table only.
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Please answer this question step by step. Previous expert
response was incorrect. Thank you in advance....
Calculate the concentrations of all species present in 0.14 M H2SO3. (Ka1=1.5×10−2, Ka2=6.3×10−8). Calculate the concentration...
Calculate the concentrations of all species present in 0.14 M H2SO3. (Ka1=1.5×10−2, Ka2=6.3×10−8). Calculate the concentration of H2SO3, HSO3- , H3O+, SO32- in solution.
A large volume of 0.150M Sulfurious Acid (H2SO3) is treated with a strong base to adjust...
A large volume of 0.150M Sulfurious Acid (H2SO3) is treated with a strong base to adjust the pH to 5.50. Assume that the additions of the base, a solid, does not significantly affect the volume of the solution. Estimate the molar concentration of H2SO3, HSO3(-), SO3 (2-) present in the final solution. Ka1 = 1.5 x 10^-2 Ka2 = 1.2 x 10^-7 Answers are H2SO3 = .000032 M HSO3(-)=.14 M SO3 (2-) = .0054 M
Part 3 – Put it all together. Calculate the concentrations of all species in a 0.330...
Part 3 – Put it all together. Calculate the concentrations of all species in a 0.330 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8. Na+ H+ OH- H2SO3 SO3 2- HSO3 -
Calculate the concentrations of all species in a 0.340 M Na2SO3 (sodium sulfite) solution. The ionization...
Calculate the concentrations of all species in a 0.340 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8. (NA+) (SO3^2-) HSO3^-1 H2SO3 OH^-1 H^+
Worksheet 19 Titration of Polyprotic Acids Name: 1. Calculate the sulfite ion [SO3'] concentration in a...
Worksheet 19 Titration of Polyprotic Acids Name: 1. Calculate the sulfite ion [SO3'] concentration in a 0.123 M solution of the weak acid, sulfurous acid (H2SO3). The stepwise dissociation constants of carbonic acid are: Ka1 1.41 x 102 Ka2-6.31 x 108 3. Consider the following dissociation of the triprotic acid, phosphoric acid (HsPOs): Step 1 H3POa + H2O <=> H30+ + H2PO4, Step 2 HP0i + H2O <=> H30+ + HP042- Step 3 HPO42-+ H2O <-> H3O+ + PO43- Kal=7.1...
Calculate the concentrations of all species in a 0.610 M Na2SO3 (sodium sulfite) solution. The ionization...
Calculate the concentrations of all species in a 0.610 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8. A. [HSO3-] B. [H2SO3] C. [OH-] D. [H+]
180Q1 Part A Calculate the pH and the concentrations of all species present in 0.14 M...
180Q1 Part A Calculate the pH and the concentrations of all species present in 0.14 M H2SO3. (Ka1 = 1.5×10−2, Ka2 = 6.3×10−8) Express your answer to three significant figures and include the appropriate units. Part B Calculate the concentration of H2SO3 in solution. Express your answer to two significant figures and include the appropriate units. Part C Calculate the concentration of HSO−3 in solution. Express your answer to two significant figures and include the appropriate units. Part D Calculate...
Polyprotic acids contain more than one dissociable proton. Each dissociation step has its own acid-dissociation constant,...
Polyprotic acids contain more than one dissociable proton. Each dissociation step has its own acid-dissociation constant, Ka1, Ka2, etc. For example, a diprotic acid H2A reacts as follows: H2A(aq)+H2O(l)⇌H3O+(aq)+HA−(aq) Ka1=[H3O+][HA−][H2A] HA−(aq)+H2O(l)⇌H3O+(aq)+A2−(aq) Ka2=[H3O+][A2−][HA−] In general, Ka2 = [A2−] for a solution of a weak diprotic acid because [H3O+]≈[HA−]. Many household cleaning products contain oxalic acid, H2C2O4, a diprotic acid with the following dissociation constants: Ka1=5.9×10−2, Ka2=6.4×10−5 Part A) Calculate the equilibrium concentration of H3O+ in a 0.20 M solution of oxalic...
I solved it myself and i got 1.06 but for some reason thats not correct. 1.02...
I
solved it myself and i got 1.06 but for some reason thats not
correct. 1.02 is and i dont know how to get that
Part A Calculate the pH of a 0.60 M H2SO3, solution that has the stepwise dissociation constants Ka1 = 1.5 x 10-2 and K 2 6.3 x 108 1.02 1.06 2.04 1.82 Submit Previous Answers Correct
Calculate the pH of each of the following aqueous solutions at 25 °C. (Please help me...
Calculate the pH of each of the following aqueous solutions at 25 °C. (Please help me solve #4 with your work, and check my answers for #1-3, if incorrect please show me why, Thank you) 1) 0.65 M boric acid (B(OH)3, Ka = 7.3 x 10-10) (pH=4.66) 2) 3.15 M ammonia (NH3, Kb = 1.76 x 10-5) (pH= 4.37) 3) 0.82 M benzoic acid (C6H5COOH, Ka = 6.3 x 10-5) (pH=2.14) 4) 0.100 M H3AsO4 (Ka1 = 2.5 x 10-4,...
Worksheet 19 Titration of Polyprotic Acids Name: 1. Calculate the sulfite ion [SO3'] concentration in a 0.123 M solution of the weak acid, sulfurous acid (H2SO3). The stepwise dissociation constants of carbonic acid are: Ka1 1.41 x 102 Ka2-6.31 x 108 3. Consider the following dissociation of the triprotic acid, phosphoric acid (HsPOs): Step 1 H3POa + H2O <=> H30+ + H2PO4, Step 2 HP0i + H2O <=> H30+ + HP042- Step 3 HPO42-+ H2O <-> H3O+ + PO43- Kal=7.1...
I
solved it myself and i got 1.06 but for some reason thats not
correct. 1.02 is and i dont know how to get that
Part A Calculate the pH of a 0.60 M H2SO3, solution that has the stepwise dissociation constants Ka1 = 1.5 x 10-2 and K 2 6.3 x 108 1.02 1.06 2.04 1.82 Submit Previous Answers Correct
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