Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Concept explainers
Question
Transcribed Image Text:**Question 12**
The following pictures represent solutions at various stages in the titration of a weak diprotic acid \( \text{H}_2\text{A} \) with aqueous KOH. Unshaded spheres represent H atoms, black spheres represent oxygen atoms, and shaded spheres represent \( \text{A}^{2-} \) ions. (\( \text{K}^+ \), \( \text{H}_3\text{O}^+ \) initially present, \( \text{OH}^- \) initially present and solvent water molecules have been omitted for clarity.)
**Diagram Explanation:**
1. **Picture (1):** Contains only molecules of the form \( \text{H}_2\text{A} \).
2. **Picture (2):** Contains a mix of \( \text{H}_2\text{A} \) and \( \text{HA}^- \) ions.
3. **Picture (3):** Contains a mix of \( \text{HA}^- \) and \( \text{A}^{2-} \) ions.
4. **Picture (4):** Contains only \( \text{A}^{2-} \) ions.
*Which picture represents the system halfway to the first equivalence point?*
- (1)
- (2)
- (3)
- (4)
*Instructions: Click Save and Submit to save and submit. Click Save All Answers to save all answers.*
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 2 steps with 1 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- We are looking for the molar mass and the pKa value of a weak monoprotonic acid. Two experimentswere carried out with the solid, anhydrous sodium salt of this acid:1st experiment: 10.00 g of the salt was dissolved in 1.000 L of water. Then 10.00 mL of hydrochloric acidwith a concentration of 3.000 mol/L was added. The resulting solution had a pH value of pH = 4.7903.2nd experiment: 10.00 g of the salt was dissolved in 1.000 L of water. Then 15.00 mL of hydrochloric acidwith a concentration of 3.000 mol/L was added. The resulting solution had a pH value of pH = 4.4246.arrow_forwardConsider the following: HClO2 + NaOH => H2O + NaClO2 50.0 mL of 0.250 M chlorous acid (HClO2, Ka=1.1x10-2) was titrated with 34.00 mL of 0.350 M sodium hydroxide (NaOH). Calculate the pH of the solution at this point. Group of answer choices 2.57 6.23 7.24 3.26arrow_forwardIf 25,0 cm3 of the NH3 (concentration 0,10 mol∙dm–3) is titrated with the HCl (concentration 0,050 mol∙dm–3), calculate the pH at the equivalence point of the titrationarrow_forward
- An analytical chemist is titrating 145.6mL of a 1.100M solution of hydrazoic acid HN3 with a 0.8100M solution of KOH . The pKa of hydrazoic acid is 4.72 . Calculate the pH of the acid solution after the chemist has added 236.7mL 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.arrow_forwardThe answer I got was 13.33 but that's not correctarrow_forward10 An analytical chemist is titrating 180.7 mL of a 0.5200M solution of piperidine (C5H₁0NH) with a 0.8300M solution of HIO3. The p K² of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 37.7 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. G 4 = 0 X 3arrow_forward
- The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.260 moles of a monoprotic weak acid (?a=1.4×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point?arrow_forwardAn unknown concentration of formic acid (HCOOH, Ka = 1.8 x 10^-4 M) is titrated with NaOH. If a 0.150 M solution of NaOH requires 35 mL of NaOH to neutralize 15.0 mL of the formic acid,calculate the concentration of the acid.Calculate the pH of the solution at the titration’s end point.arrow_forwardThe half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.260 moles of a monoprotic weak acid (Ka=7.6×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point?arrow_forward
- Determine the pH at the equivalence point in titration of 25.0 mL of 0.690 M HCOOH with 0.18 M NaOH. The Ka of HCOOH is 1.8 × 10−4.HCOOH (aq) + NaOH (aq) → NaHCOO (aq) + H2O (l)arrow_forwarda saturated solution of M(OH)2 is prepared. 15 ml of the saturated solution was titrated with a .055 M HCL solution. Examination of the pH titration curve indicated that it took 8.15 ml of the HCL solution to reach the equivalence point. What is the [OH-] in the saturated solutionarrow_forwardSuppose that 30.0 mL of a 0.150 M solution of ammonia ( NH 3 , K b = 1.8 × 10 –5 ) is titrated with a 0.200 M solution of HCl. Assume that less than 5% of NH 3 ionizes in solution. determine the pH at the equivalence point after 30 mL of KOH has been added.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY