(a)
Interpretation:
A sample contains 20.0 mL volume of
Polyprotic acid:
Polyprotic acid is an acid, which can donate minimum two or more than two protons from per molecule to an aqueous solution. Diprotic and triprotic acids are commonly available polyprotic acids, it can able to donate or loss two and three protons, respectively. The polyprotic acid shows more than one equivalence points in their titratin curves; it depends on the number of protons they possess.
(b)
Interpretation:
A sample contains 20.0 mL volume of
Concept introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 6 Solutions
CHEMICAL PRINCIPLES (LL) W/ACCESS
- The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)arrow_forwardPhenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH. C6H5OH(aq) + OH(aq) C6H5O(aq) + H2O() (a) What is the pH of the original solution of phenol? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5O? (c) What is the pH of the solution at the equivalence point?arrow_forwardThe titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major species in solution at points AF. b. Calculate the pH at the halfway points to equivalence, B and D. (Hint: Refer to Exercise 113.)arrow_forward
- a.) A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH(aq). The results are given in the graph attached. (i) What is the approximate pKa of the acid? (ii) What specific value from the graph is needed, in addition to the information in part (a) above, to calculate the molar concentration of the NaOH(aq) ? (iii) Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated is less than the concentration of its conjugate base.arrow_forwardThe following 4 questions involve the titration of a 50.00 mL sample of 0.200 M chlorous acid, HClO2, with 0.200 M NaOH (aq., 25 oC). The Ka HClO2 = 1.11 x 10–2 1. Calculate the pH of the solution before any NaOH has been added.arrow_forward4. Complete neutralization of 10 mL of hydrochloric acid solution by NaOH 0.1 N in the presence of phenol phthalein until the appearance of purple color (pHf= 9) 15 mL of NaOH is consumed. (a) What is the concentration of hydrochloric acid? (b) Calculate the indicator error.arrow_forward
- 7. You are given a 500 ml solution of 0.1 M HNO3 and an indicator Hin (Ka = 3.2x10) which changes from yellow (Hin) to green (In'). If you add two drops of indicator to the solution: (a) What colour is the solution initially? (b) What pH would the colour change become visible if you were adding 0.10M NaOH?arrow_forwardA titration is carried out for 50.00 mL of 0.100 M HNO3 (strong acid) with 0.200 M of a strong base NaOH (the titration curve is shown to the right). Calculate the pH at these volumes of added base solution: A B C D 0.200 M NaOH added 00.0 mL 15.0 mL 25.0 mL 40.0 mL HNO3(aq) + NaOH(aq) H₂O(9) + NaNO3(aq) pH of solution - Equivale point Midpoint HAlaq). Volume carrow_forwardThe student titrated 50.0 mL of 0.100 M HC2H3O2 with 0.100 M NaOH (aq). Calculate the pH of the solution at the equivalence point.arrow_forward
- The base dissociation constant (kb) of RNH2(aq) is 4.6 x 10^-4, Sketch the titration curve that would result from a titration of 35 mL of 0.200 M RNH2 with 0.2 M HCl(aq).arrow_forwardThe base dissociation constant (kb) of RNH * 2(aq) is 4.6 * 10 ^ - 4 , Sketch the titration curve that would result from a titration of 35 mL of 0.200 M RNH2 with 0.2MHCl(aq).arrow_forward7. The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq) (Z) 25.0 mL of 1.0 M CH3COOH(aq) Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)Truearrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning