Certainly! Here's a transcription suitable for an educational website:---**Title: Analysis of H₂S Using Colorimetry and Iodine Generation**Hydrogen sulfide (H₂S) can be analyzed by titration with colorimetrically generated iodine (I₂). The I₂ is generated from potassium iodide (KI) via the following reaction:\[ 2I^- (aq) \rightarrow I_2 (aq) + 2e^- \]The generated I₂ then reacts in a 1:1 titration via:\[ H₂S (aq) + I₂ (aq) \rightarrow S (s) + 2H^+ (aq) + 2I^- (aq) \]**Example Calculation:**To determine the concentration of H₂S in a solution, consider the analysis of 50.00 mL of a solution containing H₂S. This solution was analyzed with dissolved KI using electrolysis requiring 812 seconds at a constant current of 526.0 mA. The task is to calculate the concentration of H₂S in the original solution.---This transcription provides a clear and concise explanation of the chemical reactions and procedure used for analyzing hydrogen sulfide via colorimetry, including relevant details for understanding the process.

The given reactions are 2I-(aq) →I2(aq)+2e-H2S(aq)+I2(aq)→S(s)+2H+(aq)+2I-(aq)

Coulometry - H₂S can be analyzed by titration with coulometrically generated 12 The 12 is generated from KI via 2 I- (aq)---> 1₂ (aq) + 2 e- The generated I2 then reacts in a 1:1 titration via: H₂S (aq) + 12 (aq) ------------>S (s) + 2 H+ (aq) + 2 I (aq) Analysis of 50.00 mL of a solution containing H₂S was analyzed with dissolved KI. Electrolysis required 812 seconds at 52.6 mA current. What is the [H₂S] in the original solution?

Coulometry - H₂S can be analyzed by titration with coulometrically generated 12 The 12 is generated from KI via 2 I- (aq)---> 1₂ (aq) + 2 e- The generated I2 then reacts in a 1:1 titration via: H₂S (aq) + 12 (aq) ------------>S (s) + 2 H+ (aq) + 2 I (aq) Analysis of 50.00 mL of a solution containing H₂S was analyzed with dissolved KI. Electrolysis required 812 seconds at 52.6 mA current. What is the [H₂S] in the original solution?

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

An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution? 2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution? 3. What is the concentration of Ag+ in solution?
Question Completion Status: QUESTION 3 3. A weak acid was titrated using 0.20 M KOH. The pH at several volumes added was recorded and plotted as shown below. If 175 mg of the weak acid was used, what was the molar mass of the weak acid solution? pH vs Volume of KOH(aq) 13 12 11 10 6. 7. 6. 4. 3 4 5 6 8 9 10 mL KOH(aq) QUESTION 4
Each graph below represents a titration involving solutions of two of the following substances: HC2H3O2, HNO3, CH3NH2 and NaOH. Which graph best represents HC2H3O2 being titrated using NaOH? Which graph best represents HC2H3O2 being titrated using CH3NH2? Which graph best represents HNO3 being titrated using NaOH? Which graph best represents HNO3 being titrated using CH3NH2? Which graph has the lowest pH at the equivalence point? Which graph has the equivalence point pH that is equal to 7?
7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. H3C6H5O7 (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?
What type(s) of reactions occurred in this titration?
An alkaline earth hydroxide, M(OH)2, was taken to lab for analysis. The unknown powder was poured into a flask and swirled in room temperature DI water until a saturated solution formed. This solution was then slowly filtered to remove the undissolved solid hydroxide. 11.9 mL of this saturated solution was titrated with 0.148 M HCI (ag). Endpoint required 15.6 mL of the HCl (ag) solution. Calculate the Kan for this alkaline earth hydroxide.
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
The following titration curve is expected from which acid-base pair? See the picture below.
If KI was not available to precipitate AgI from AgNO3 then what reagent can be used instead? HNO3 AgNO3 NH3 HI
You used the back-titration method to experimentally determine the amount of CaCO3 in an Ultra Strength Tums antacid tablet. You calculated that you used 21.5 mmol HCl to complete the titration of a 2.139 g Tums tablet. What is the mass (in mg) of the active ingredient in the Tums tablet? (CaCO3 = 100.1 g/mol)
What is the pH at the equivalence point when 56 mL of 0.270 M hydroxylamine is titrated with 0.130 M ? Kb = 1.1x10^-8
A student carries out the following titration by adding H2SO4.