(a)
Interpretation:
Whether the ionization of pure acid, common-ion effect, buffer solution or hydrolysis occurs during the reaction of [H3O+] and [CH3COOH] to be high, but [CH3COO-] to be low needs to be explained.
Concept introduction:
Ionization is a process by which any particle (an atom or a molecule) acquires either a positive or a negative charge.
Acids that contain small amounts of covalent molecules/do not contain water are known as pure acids. When this occurs they form ions. Pure acids are poor conductors of electricity.
Any
(b)
Interpretation:
Whether the ionization of pure acid, common-ion effect, buffer solution or hydrolysis occurs during the reaction of [CH3COO-] to be high, but [CH3COOH] and [H3O+] are very low needs to be explained.
Concept introduction:
Ionization is a process by which any particle (an atom or a molecule) acquires either a positive or a negative charge.
Any chemical reaction where a molecule of water ruptures a chemical bond is known as hydrolysis. Mainly used for fragmentation, substitution, and elimination.
Ionization is a process by which any particle (an atom or a molecule) acquires either a positive or a negative charge.
(c)
Interpretation:
Whether the ionization of pure acid, common-ion effect, buffer solution or hydrolysis occurs during the reaction of [CH3COOH] is high, but [H3O+] and [CH3COO-] are low needs to be determined.
Concept introduction:
Acids that contain small amounts of covalent molecules and do not contain water are known as pure acids.
Ionization is a process by which any particle (an atom or a molecule) acquires either a positive or a negative charge.
Any chemical reaction where a molecule of water ruptures a chemical bond is known as hydrolysis. It is mainly used for fragmentation, substitution, and elimination.
(d)
Interpretation:
Whether ionization of pure acid, common-ion effect, buffer solution or hydrolysis occurs during the reaction of [CH3COOH] and [CH3COO-] are high, but [H3O+] is low, needs to be determined.
Concept introduction:
Acids that contain small amounts of covalent molecules and do not contain water are known as pure acids.
Ionization is a process by which any particle (an atom or a molecule) acquires either a positive or a negative charge.
Any chemical reaction where a molecule of water ruptures a chemical bond is known as hydrolysis. It is mainly used for fragmentation, substitution, and elimination.
Want to see the full answer?
Check out a sample textbook solutionChapter 17 Solutions
GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
- A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?arrow_forwardIsocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)arrow_forwardSketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.arrow_forward
- How much solid NaCH3CO23H2O must be added to 0300 L of a 0.50-M acetic acid solution to give a buffer with a pH of 5.00? (Him: Assume a negligible change in volume as the solid is added.)arrow_forwardWhat mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)arrow_forwardIn dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C) is a strong acid. In liquid HF, HNO3 acts like a base and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that ale Lewis acids and accept F- ion (for example, BF3 or SbF5]. Write balanced chemical equations for the reaction of pure HNO3 with pure HF and of pure HF with BF3.arrow_forward
- Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?arrow_forwardYou have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.arrow_forwardA 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.arrow_forward
- Calculate the pH of a buffer solution prepared from 0.155 mol of phosphoric acid, 0.250 mole of KH2PO4, and enough water to make 0.500 L of solution.arrow_forwardDefine a buffer solution. What makes up a buffer solution? How do buffers absorb added H+ or OH with little pH change? Is it necessary that the concentrations of the weak acid and the weak base in a buffered solution be equal? Explain. What is the pH of a buffer when the weak acid and conjugate base concentrations are equal? A buffer generally contains a weak acid and its weak conjugate base, or a weak base and its weak conjugate acid, in water. You can solve for the pH by setting up the equilibrium problem using the K.a reaction of the weak acid or the Kb reaction of the conjugate base. Both reactions give the same answer for the pH of the solution. Explain. A third method that can be used to solve for the pH of a buffet solution is the HendersonHasselbalch equation. What is the HendersonHasselbalch equation? What assumptions are made when using this equation?arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning