**Titration of Ammonia Solution with HIO₃ Solution***Problem Statement:*An analytical chemist is titrating 88.9 mL of a 0.2700 M solution of ammonia (NH₃) with a 0.4900 M solution of HIO₃. The pKᵦ of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 54.8 mL of the HIO₃ solution to it.*Note 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.*---In this problem, the analytical chemist is performing a titration of a basic solution, ammonia (NH₃), with an acidic solution, iodic acid (HIO₃). The goal is to calculate the pH of the solution after a certain amount of HIO₃ solution has been added.### Step-by-Step Solution:1. **Calculate the amount of $ \text{NH}_3 $ in moles**: \[ \text{Moles of } \text{NH}_3 = \text{Volume} \times \text{Concentration} = 0.0889 \, \text{L} \times 0.2700 \, \text{M} = 0.024003 \, \text{moles} \]2. **Calculate the amount of $ \text{HIO}_3 $ in moles**: \[ \text{Moles of } \text{HIO}_3 = \text{Volume} \times \text{Concentration} = 0.0548 \, \text{L} \times 0.4900 \, \text{M} = 0.026852 \, \text{moles} \]3. **Determine the limiting reactant**: Ammonia ($ \text{NH}_3 $) is the limiting reactant because it is present in a smaller amount.4. **Calculate the amount of $ \text{NH}_3 $ and $ \text{HIO}_3 $ left or reacted**: Since $ \text{NH}_3 $ is the limiting reactant,

Ammonia, NH3(aq) is a monoacidic weak base with pKb = 4.74 HIO3(aq) is a monoprotic strong acid.…

An analytical chemist is titrating 88.9 mL of a 0.2700M solution of ammonia (NH3) with a 0.4900M solution of HIO3. The pK, of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 54.8 mL of the HIO3 solution to it. Note 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 88.9 mL of a 0.2700M solution of ammonia (NH3) with a 0.4900M solution of HIO3. The pK, of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 54.8 mL of the HIO3 solution to it. Note 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 74.2 mL of a 0.3000 M solution of methylamine (CH3NH2) 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 10.4 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. PH = ☐
Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 2.668 g KH2PO4 and 2.095 g K2HPO4 in water to give 200. mL of solution. Stepwise acid dissociation constants for phosphoric acid may be found in your textbook. (b) a solution made by mixing 35.00 mL 0.33 M NH2OH with 15.00 mL 0.27 M NH3OHCl. The base dissociation constant Kb is 6.60 x 10-9 for NH2OH. Assume that the final volume is the sum of the volunes of the two solutions that are mixed.
An analytical chemist is titrating 238.1 mL of a 0.5500M solution of propionic acid (HC₂H₂CO₂) with a 0.8000M solution of KOH. The pK of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 119.8 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. pH = X S ?
A chemist titrates 250.0 mL of a 0.5571M hypochlorous acid (HC1O) solution with 0.1436M KOH 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 KOH solution added. pH = |
The p?a of hypochlorous acid is 7.530 . A 58.0 mL solution of 0.130 M sodium hypochlorite ( NaOCl ) is titrated with 0.299 M HCl . Calculate the pH of the solution after the addition of 9.78 mL of 0.299 M HCl . (please type answer not write by hend)
An analytical chemist is titrating 186.4 mL of a 0.3400M solution of methylamine (CH3NH₂) with a 0.6900M solution of HIO3. The pK² of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 98.0 mL of the HIO3 solution to it. Note 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. pH = 1 X Ś
Ascorbic acid C5H7O4CO2H (Ka =7.9x10^-5) also known as vitamin C is an essential nutrient for all mammals. In lab it can also be used to make buffers. Calculate the pH of a buffer solution which is made by mixing 0.250 moles of ascorbic acid and 0.200 moles of the conjugate base sodium ascorbate in a total volume of 0.750 liters.
A chemist titrates 130.0 mL of a 0.6533 M cyanic acid (HCNO) solution with 0.5467 M KOH solution at 25 °C. Calculate the pH at equivalence. The pK, of cyanic acid is 3.46. 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 KOH solution added. pH = U
An analytical chemist is titrating 143.6 mL of a 0.7000M solution of piperidine (C,H10NH) with a 0.4000M solution of HNO3. The p K, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 267.7 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
An analytical chemist is titrating 77.9 mL of a 1.000M solution of hydrazoic acid (HN₂) with a 0.9800M solution of NaOH. The pK, of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 34.3 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 $
An analytical chemist is titrating 79.6 mL of a 0.9000M solution of cyanic acid (HCNO) with a 1.200 M solution of NaOH. The pK of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 69.4 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 = ☐
Twenty millimeters of 0.50N HOAc is diluted with water to 100mL, and the resulting solution is titrated with 0.50N HOAc. Calculate the pH value (a) at the start, (b) when 0.8 ml of the NaOH has been added, (c) at the equivalence point (when 20mL of NaOH has been added, (d) when 30mL of the NaOH has been added. Ka=1.8x10^-5