Concept explainers
Interpretation:
Spontaneity of given reaction should be explained, when addition of given buffer to the cell.
Concept introduction:
Cell potential (EMF):
The maximum potential difference between two electrodes of voltaic cell is known as cell potential.
If standard reduction potentials of electrodes are given the cell potential (EMF) is given by,
Where,
Nernst equation:
The relationship between standard cell potential and cell potential at non standard conditions and the reaction quotient are given by Nernst equation it is,
Where,
Ph of the solution is nothing but the concentration of Hydrogen ion in given solution in given condition and it is given by negative logarithm of base ten Hydrogen ion concentration.
Want to see the full answer?
Check out a sample textbook solutionChapter 19 Solutions
General Chemistry - Standalone book (MindTap Course List)
- A solution is 1.5 104 M Zn2 and 0.20 M HSO4. The solution also contains Na2SO4. What should be the minimum molarity of Na2SO4 to prevent the precipitation of zinc sulfide when the solution is saturated with hydrogen sulfide (0.10 M H2S)?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_forwardMany natural processes can be studied in the laboratory but only in an environment of controlled pH. Which of these combinations is the best to buffer the pH at approximately 7? Explain your choice. H3PO4/NaH2PO4 NaH2PO4/Na2HPO4 Na2HPO4/Na3PO4arrow_forward
- Consider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2 F(aq) (a) Calculate K for the reaction. (b) Will BaSO4 precipitate if Na2SO4 is added to a saturated solution of BaF2?arrow_forwardA solution is formed by adding 6.00 grams of solid potassium acetate, KC₂H₃O₂, to 200.0 ml of 0.0240M calcium acetate, Ca(C₂H₃O₂)₂. Calculate the pH of the resulting solution. You may assume that the potassium acetate dissolve completely and that the change in volume is negligible with the addition of the solid.arrow_forwardThe molar solubility of AgCl(s) in water at 25°C is 1.33 x 10−5 M. AgCl(s) ↔ Ag+(aq) + Cl−(aq) What is the molar solubility of AgCl(s) at 50.0°C?arrow_forward
- Calculate the solubility of aluminum hydroxide, Al(OH)3, in a solution buffered at pH 11.00.arrow_forwardLe Châtelier’s Principle is described in terms of adding/removing reactants or products. While it is easy to add reactants/products, describe how you were able to remove reactants/products from the equilibria by using the procedures in this experiment. What are the net ionic equations as appropriate for: The following reaction is examined:HSO4¯ (aq) + H2O (l) ⇌ SO42¯ (aq) + H3O+ (aq) Obtain about 5 mL (one small test tube) of “NaHSO4 solution” and “Na2SO4 solution” in two appropriately labeled test tubes. In a well plate, take 10 drops of NaHSO4 into wells A1, A2 and A3, and 20 drops to wells A4 and A5 using a pipet. Add 1 drop of Thymol Blue indicator solution to wells A1 to A5. Thymol Blue is red in very acidic solution, and changes from red to yellow between pH 1.2-2.8. Add one drop of Na2SO4 to well A1. Continue to add drops of Na2SO4 to well A1 until you see a color change, making sure to mix the solution after the addition of each drop (do not use the pipet tip to mix the…arrow_forwardWrite the expression for the solubility product constant for Pb(OH)2.arrow_forward
- A solution is formed by adding 5.20 grams of solid potassium acetate, KC₂H₃O₂, to 500.0 ml of 0.0730M calcium acetate, Ca(C₂H₃O₂)₂. Calculate the pH of the resulting solution. You may assume that the potassium acetate dissolve completely and that the change in volume is negligible with the addition of the solid.pH = ___arrow_forwardPhosphate Buffered Saline (PBS) is a commonly used buffer for experiments in biology because its pH and ion concentrations are similar to those in mammalian organisms. It works in a similar fashion to the blood plasma buffer mentioned in the textbook, but using dihydrogen phosphate ions and hydrogen phosphate ions for buffering through the following chemical reaction: H2PO4- (aq) ⇆ H+(aq) + HPO42--(aq) The equilibrium arrows depict that the phosphate ion (H2PO4- ) is dissociating further into two component ions in solution, but at the same time H+ and HPO42- ions are combining simultaneously to form phosphate in solution. So, at any given point in time, and under the appropriate conditions, there is an equal quantity of dissolved ions and combined ions in solution. There is therefore always a hydrogen ion donor and an acceptor in solution. Based on the equation above, which ion plays the role of hydrogen-ion donor (acid) and which ion plays the role of hydrogen-ion acceptor (base)…arrow_forwardBenzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. C6H5COOH(s) -> C6H5COO–(aq) + H+(aq) Ka = 6.46 x 10^-5 Calculate the pH of the solution after the following amounts of NaOH have been added… A. 0 mL B. 10 mL C. 85 mLarrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax