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
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A large volume of 0.150M Sulfurious Acid (H2SO3) is treated with
a strong base to adjust...
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.
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
Sulfurous acid (H2SO3) is a diprotic acid, (Ka1 - 17 10-2 and Ka2 - 6,0 x...
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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...
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10. Which of these species is probably the weakest acid? (a) HCI (b) H3PO4 (c) H2SO3 (d) HOBI (e) HNO3 11. What volume of 0.50 M KOH would be required to neutralize completely 500.0 mL of 0.25 M H3PO4 solution? KOH is sufficiently strong as a base to remove all three protons from H3PO (a) 2.5 x 10 mL (6) 1.4 x 10mL (c) 83 mL (d) 7.5 x 10 mL (e) 5.2 x 10 mL
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10. A 25.0-mL sample of 0.150M hypochlorous acid is titrated with a 0.150 M NaOH solution. What is the pH after 13.3 mL of base is added? The Ka of hypochlorous acid is 3.0 x 10-8 A) 7.25 B) 1.34 C) 4.43 D) 7.58 E) 7.46 11. Calculate the pH and pOH of a solution that is 0.075 M HCN and 0.06 M NaCN. 12. The solubility of silver bromide is greater in 0.10 M...
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Titration of a Weak Monoprotic Acid with a Strong Base Volume of Base (mL) 1. Using the graph, determine the K, of the weak acid. 2. Suppose 100mL of the monoprotic acid referred to in the graph was titrated with 1M NaOH, determine the molarity of the weak acid. The corresponding balanced chemical equation is shown below. HA + NaOH + H2O + A + Nat 3. If the weak acid above was prepared by using 5g of the weak...
1 of 1 Name Date CHM 1032 Acid/Base Focus Concepts Period Directions: read each section and...
1 of 1 Name Date CHM 1032 Acid/Base Focus Concepts Period Directions: read each section and answer the questions accordingly. Show all mathematical work. (1) Which species is the conjugate base of H2SO3? a. H,SO b. HSO3 C. SO (2) Write a molecular equation for the neutralization reaction between aqueous HCl and aqueous Ca(OH)2? (3) The titration of 20.0-ml of a sulfuric acid solution of unknown concentration requires 22.87-mL of a 0.158M KOH solution to reach the equivalence point. What...
Sulfurous acid (H2SO3) is a diprotic acid, (Ka1 - 17 10-2 and Ka2 - 6,0 x 10-8 what is the equilibrium concentration of SO3? if the initial concentration of H2SO3 is 1.2 M? O 6.0 x 10-8 M O2.0 x 10-2 M O 1.7 x 10-8 M O 17 x 10-2M 7.2 x 10-8 Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH4l(s) = NH3(g) + HI(g) At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at...
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help with all these please
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