Concept explainers
(a)
Interpretation:
For the given concentration of
Concept Introduction:
The relation between protons and hydroxide ions in any aqueous solution is shown here:
From this expression, the concentration of both protons and hydroxide ions can be calculated as shown here:
Classification of acidic, neutral or basic solution:
A solution can be classified as acidic, basic or neutral based on the concentrations of both hydroxide ions and protons as discussed here:
- If the concentration of proton is larger than the concentration of hydroxide ion then the solution is acidic.
- If the concentration of hydroxide ion is larger than the concentration of proton then the solution is basic.
- If the concentrations of both proton and hydroxide ion are equal then the solution is neutral.
(b)
Interpretation:
For the given concentration of
Concept Introduction:
The relation between protons and hydroxide ions in any aqueous solution is shown here:
From this expression, the concentration of both protons and hydroxide ions can be calculated as shown here:
Classification of acidic, neutral or basic solution:
A solution can be classified as acidic, basic or neutral based on the concentrations of both hydroxide ions and protons as discussed here:
- If the concentration of proton is larger than the concentration of hydroxide ion then the solution is acidic.
- If the concentration of hydroxide ion is larger than the concentration of proton then the solution is basic.
- If the concentrations of both proton and hydroxide ion are equal then the solution is neutral.
(c)
Interpretation:
For the given concentration of
Concept Introduction:
The relation between protons and hydroxide ions in any aqueous solution is shown here:
From this expression, the concentration of both protons and hydroxide ions can be calculated as shown here:
Classification of acidic, neutral or basic solution:
A solution can be classified as acidic, basic or neutral based on the concentrations of both hydroxide ions and protons as discussed here:
- If the concentration of proton is larger than the concentration of hydroxide ion then the solution is acidic.
- If the concentration of hydroxide ion is larger than the concentration of proton then the solution is basic.
- If the concentrations of both proton and hydroxide ion are equal then the solution is neutral.
Want to see the full answer?
Check out a sample textbook solutionChapter 8 Solutions
Chemistry In Context
- s practice Identify Brensted-Lowery Acids and bases and their Conjugates (a) C,H;N (aq) + H,O (I) 2 CH,NH* (aq) + OH (aq) (b) HNO, (aq) + H,O () → NO, (aq) + H,O* (aq) Created with Darrow_forwardPractice Exercise What is the pH of a solution containing 0.30 M HCOOH and 0.52 M HCOOK? Compare your result with the pH of a 0.30 M HCOOH solution.arrow_forwardoxygen. Practice Exercise Nitric acid (HNO3) is used in the production of fertilizer, dyes, drugs, and explosives. Calculate the pH of a HNO; solution having a hydrogen ion concentration of 0.76 M.arrow_forward
- Which of the following ions could be classified as basic? (select all that apply) K+ co32- CH3CO- H+ (H30) Nat NO3 NH4* PO43- OH CI Which of the following ions could be classified as acidic? (select all that apply) Co2- NH4* CI H* (H30*) CH3COO" PO43- Na+ K+ NO3 OH Which of the following ions could be classified as pH neutral? (select all that apply) co32- H* (H30*) NO3arrow_forwardComplete the table below. Round each of your entrles to 2 signific nt digits. You may assume the temperature is 25 conjugate acid conjugate base K, formula formula HSO 0.012 10 H,BO, 5.8 x 10 C,H,ONH 2.1 X 10 Explanation Checkarrow_forwardComplete the table below. Round each of your entries to 2 significant digits. You may assume the temperature is 25 °C. conjugate acid conjugate base K. K, formula formula H,BO, 10 5.8 x 10 HF -4 6.8 x 10 NH, 1.8 x 10 Explanation Check O 2021 McGraw-Hill Education. All Rights Reserve APR 11arrow_forward
- Fill in the missing chemical formulae in the tables below. conjugate base base conjugate acid acid co, 2- H,CO, H,0 H,0 H,PO, NH, Explanation Checkarrow_forwardDeriving Kp trom Ka Complete the table below. Round each of your entries to 2 significan ligits. You may assume the temperature is 25 °C. conjugate acid conjugate base Ka K, formula formula Cio 3.3 x 10 -7 H,CO, 4.5 x 10 10 4.9 x 10 HCN Explanation Checkarrow_forwardKnowledge check. Based on the fact that NaOH is a strong base and C₆H₈O₇ is a weak acid, how would you describe the pH of the solution at the endpoint, where moles of base = 3 times the moles of acid? A) strongly basic pH B) weakly basic pH C) neutral pH D) weakly acidic pH E) strongly acidic pHarrow_forward
- Macmillan Learning Incorrect Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic pH = 1.09 Basic Neutral pH = 13.24 [OH-] = 9.4 × 10-4 POH = 4.76 POH = 12.91 [H+] = 3.5 x 10-5 [H+] = = 5.8 × 10-8 [OH-] = 5.7 × 10-9 [H+] = 1.0 × 10-7 POH = 7.00 Answer Bankarrow_forwardWhat is the pH of a 0.30 M solution of NH3? (Kb 1.8 x 10-5) a) 6.84 b) 8.32 c) 11.43 d) 7.09 e) 7.99 f) 2.57 g) 13.11arrow_forwardtion will be acidic. Simila Practice Exercise Predict whether the following solutions will be acidic, basic, or nearly neutral: (a) LiClO,, (b) Na,PO4, (c) Bi(NO3)3, (d) NH,CN. Finally we note that some anions can act either as an acid or as a base. For example, the bicarbonate ion (HCO;) can ionize or undergo hydrolvsis nn follarrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples 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 EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY