Concept explainers
In this problem, we will use material balance and chacepts (pages 761-762) to calculate the equilibrium concentrations in an extremely dilute solution of a strong acid,
(a) Write down the material balance equation for
(b) Write down the charge balance equation (an electroneutrality condition) for this solution.
(c) Use the material balance and charge balance equations, and product for water,
(d) Use the quadratic formula to solve equation in (c)
(e) Calculate
Want to see the full answer?
Check out a sample textbook solutionChapter 16 Solutions
General Chemistry: Principles And Modern Applications Plus Mastering Chemistry With Pearson Etext -- Access Card Package (11th Edition)
- 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_forwardA 0.025 M solution of an unknown organic acid has a pH of 3.23. 2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.arrow_forwardCalculate the ph of a solution prepared by dissolving 1.00g of sodium acetate,CH^3COONa, in 50.0ml of 0.15 M acetate acid, CH^3COOH(aq)arrow_forward
- 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_forwardSuppose that the solubility of Ca(OH)2 in water is 0.3g/0.1L. What is the pH of an aqeous saturated solution of Ca(OH)2?arrow_forwardUse the Henderson-Hasselbalch approximation to calculate the pH of a solution prepared by dissolving in water, to a final volume of 1.00 L, 0.200 mol of nitrous acid, 0.040 mol of sodium nitrite, 0.080 mol of HNO3 and 0.080 mol of Ca(OH)2.arrow_forward
- A rainwater sample from Mondstadt was determined to contain 1.23 x 10⁻⁷ M of hyrdonium ion. Determine the pH and pOH of the rainwaterarrow_forwardSketch the pH curve of a solution containing 0.10 M NaCH3CO2(aq) and a variable amount of acetic acid .arrow_forward134 grams of potassium sorbate KCH3 (CH)4CO2 is fully dissolved in 100.00 mL of water, which is carefully transferred to a conical flask. Then 100.00 mL of 0.240 M HNO3 is added dropwise to this solution from a burette. Given: Ka (sorbic acid) = 1.7 × 1O^-5 Showing all your calculations and reasoning, determine the pH of the solution that results after the addition of all the acid mentioned above. Suppose that the titration continues. Determine the pH of the solution in the flask at theequivalence pointarrow_forward
- Consider the following dissociation reaction of the weak acid, HA: HA + H2O ⇔ H3O+ + A- What is the name given to the equilibrium constant of this type of reaction? A. The rate constant. B. The acidity constant. C. The acid ionisation constant. D. The buffer constantarrow_forwardWhat is the significance of the Henderson-Hasselbalch equation in acid-base chemistry, and how does it relate to the pH of a solution?arrow_forwardFor a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction? Kc is the product of all reaction products (choose from: Multiplied by, added to, divided by, subtracted from) the product of the reactants, with all concentrations of reactants and products raised to their respective stoichiometric powers. As the titration proceeds, the amount of reactants (choose from: Increases, decreases, remains the same) and the amount of products (choose from: Increases, decreases, remains the same). Because the value of the numerator is (Choose from much greater than, much less than, approximately equal to) the value of the denominator, the value of Kc will be (Choose from much greater than, much less than, approximately equal to)1 for an effective titration reaction.arrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning