Concept explainers
(a)
Interpretation:
A sample contains 25.0 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 25.0 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: The Quest for Insight
- What must the ratio of H2PO4 to HPO42 be to have a buffer with a pH value of 7.00?arrow_forwardThe 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_forwardCalculate the pH during the titration of 20.0 mL of 0.30 M HNO3(aq) with 0.30 M KOH after 19.24 mL of the base have been added.arrow_forward
- Sketch the pH curve of a solution containing 0.10 M NaCH3CO2(aq) and a variable amount of acetic acid .arrow_forwardnuse the relevant solubility data from tables and calculate the molar solubility ofcopper(II) sulfide in 1.2 M NH 3 (aq)arrow_forwardDetermine the pH at the equivalence (stoichiometric) point in the titration of 48.38 mL of 0.171 M HCN (aq) with 0.135 M NaOH(aq). The Ka of HCN is 4.9 * 10^-10.arrow_forward
- 1) Calculate the pH of a solution prepared by dissolving 2.35 g of sodium acetate, CH,COONA, in 81.5 ml of 0.10 Macetic acid, CH,COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. K, of CH,COOH is 1.75 x 10. pH=arrow_forwardWhat is the molar solubility (in mols/L)of silver chloride in 2.00 M NH3(aq) given that Kgp of AGCI = 1.77x10-10 and Kf of Ag(NH3)2* is 1.70×107? Express your answer in decimal notation rounded to three significant figures.arrow_forwardA sample of 0.10 M CH3COOH(aq) of volume 25.0 cm3 is titrated with 0.10 M NaOH(aq). The Ka for CH3COOH is 1.8 x 10-5. (a) What is the pH of 0.10 M CH3COOH(aq)? (b) What is the pH after the addition of 10.0 cm3 of 0.10 MNaOH(aq)? (c) What volume of 0.10 M NaOH(aq) is required to reach halfway to the stoichiometric point? (d) Calculate the pH at that halfway point. (e) What volume of 0.10 M NaOH(aq) is required to reach the stoichiometric point? (f) Calculate the pH at the stoichiometric point.arrow_forward
- A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was addedarrow_forwardA buffer is made by mixing 5.0 mL of 3.0 M NH,(aq) with 10 mL of 1.44 M NH Cl(aq). What is the pH of the buffer at 25°C, if the base ionization constant of ammonia is 1.8x10° and the ion product of water is 1.0x10-14 at this temperature?. Enter your answer in the box provided with correct units and sig. figs.: Comment : Henderson-Hasselbalch equations for acidic and basic buffers are listed on the next page. Answer: pH, 'bufferarrow_forwardQ.3: Determine the pH of the dissociation of 0.1 M HCN (aq). For which the dissociation constant is equal to 4.9 x 10-5 and the weight and volume of the conjugated base is 5 g and 2 L respectively. (Write the chemical reaction).arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning