### pH Calculation of a Titration of Methylamine with HIO3An analytical chemist is performing a titration using:- **169.0 mL** of a **0.8600 M** solution of methylamine (CH3NH2)- A **0.2200 M** solution of HIO3. The provided base dissociation constant (\( pK_b \)) of methylamine is **3.36**.#### Problem Statement:Calculate the pH of the base solution after the chemist has added **527.8 mL** of the HIO3 solution to it.**Note for advanced students:** You may assume that the final volume equals the initial volume of the solution plus the volume of the HIO3 solution added.**Instructions:**- Round your answer to two decimal places.### Input Section:The input fields include a space for the calculated pH value:- `pH = __`Below the input field, there are three buttons:1. A green check (✔︎) to submit the answer.2. A circular arrow (⟳) for resetting the input.3. A question mark (?) for providing help or guidance.### Explanation:This educational task guides the user through a titration problem involving the calculation of pH after mixing two solutions. The critical aspects are:1. **Initial Concentration and Volume of Methylamine:** - Volume: 169.0 mL - Concentration: 0.8600 M2. **Concentration and Volume of HIO3 Added:** - Volume: 527.8 mL - Concentration: 0.2200 M3. **pK_b of Methylamine:** - Value: 3.36### Steps for Calculation:1. Determine the moles of CH3NH2 and HIO3 initially present.2. Use the volumes added to find the new concentrations of CH3NH2 and the resulting species in the final solution.3. Compute the resulting pH after the titration using equilibrium expressions and the given \( pK_b \).By following these steps, students will practice key concepts in acid-base chemistry, equilibrium, and pH calculations during titrations.

The buffer is defined as the solution containing equal amount of a weak acid and its conjugate base…

An analytical chemist is titrating 169.0 mL of a 0.8600M solution of methylamine (CH3NH₂) with a 0.2200M solution of HIO3. The pK, of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 527.8 mL of the HIO3 solution to it. Nate for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 169.0 mL of a 0.8600M solution of methylamine (CH3NH₂) with a 0.2200M solution of HIO3. The pK, of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 527.8 mL of the HIO3 solution to it. Nate for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places.

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 analytical chemist is titrating 102.2 mL of a 0.1400 M solution of dimethylamine ((CH,) NH) with a 0.7900 M solution of HNO,. The pK, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 19.5 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = Explanation Check 2021 McGraw-Hil Terms of Use
The pH of a blood plasma is 7.36. Assuming the principle of buffer system is HCO3-/H2CO3, calculate the ratio HCO3-/H2CO3. Is this buffer solution more effective against an added acid or an added base? (Ka1= 4.2 x 10-7 and Ka2 = 4.8 x 10 -11) (Need to show your calculation.).
A chemist titrates 200.0 mL of a 0.7110M dimethylamine ((CH, NH) solution with 0.3310M HNO, solution at 25 °C. Calculate the pH at equivalence. The '2 pk, of dimethylamine is 3.27. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HNO, solution added. alo pH %3D Ar
You are asked to prepare a buffer solution with a pH of 3.50. The following solutions, all 0.100 M, are available to you: HCOOH, CH3COOH, H3PO4 , NaCHOO, NaCH3COO, and NaH2PO4. What ratio of [conjugate base]/[acid] would yield the best result for the required buffer solution created in the question above? ENTER YOUR ANSWER AS ONE NUMBER ROUNDED TO TWO DECIMAL PLACES.
A chemist titrates 150.0 mL of a 0.0676M dimethylamine ((CH,) NH) solution with 0.4402M HBr solution at 25 °C. Calculate the pH at equivalence. The pK, of dimethylamine is 3.27. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added. pH = Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibity MacBook Air
Calculating the pH at equivalence of a titration A chemist titrates 50.0 mL of a 0.1528M hypochlorous acid (HC10) solution with 0.7043 M NAOH solution at 25 °C. Calculate the pH at equivalence. The pK, of hypochlorous acid is 7.50. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added. pH = |
An analytical chemist is titrating 204.9 ml of a 0.2200M solution of cyanic acid (HCNO) with a 0.7300.M solution of KOH. The pK, of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 50.06 ml, of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. DH-0
An analytical chemist is titrating 204.7 mL of a 0.7700M solution of methylamine (CH₂NH₂) with a 0.2500M solution of HNO3. The pK, of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 99.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = 0 X S
An analytical chemist is titrating 109.3 ml. of a 0.8700 M solution of butanoic acid (HC,H,CO,) with a 0.9500 M solution of NaOH. The pK, of butanoic add is 4.82. Calculate the pH of the and solution after the chemist has added 36.93 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = 0 X
A chemist titrates 90.0 mL of a 0.7050M methylamine (CH3NH₂) solution with 0.5016M HBr solution at 25 °C. Calculate the pH at equivalence. The pK, of methylamine is 3.36. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added. pH = x 5 ?
A 25.000 mL aliquot of weak base that has a concentration of 0.30 M will be titrated with 0.80 M HCl. Calculate the pH of of the solution upon the addition of 9.375 mL of HCl. The Kb of the base is 4.6×10-6. Report your answer to the hundredths place.
2 An analytical chemist is titrating 220.6 mL of a 0.3500M solution of dimethylamine ((CH3) NH) with a 0.5200M solution of HNO3. The p Kof dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 83.5 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.