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Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE.
Calculate the concentration of each species at equilibrium and the pH of the following solution by applying a) systematic treatment of equilibrium and b) method of succesive approximation.
b. 0.100 M methylamine (CH3NH2) (Kb = 4.35 x 10-4)
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- The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following equilibrium between 3-methylbenzoic acid (K,a-5.0x10) and its conjugate base: %3D CH3- CH3- H2O + H30* (1) Will lowering the pH shift the equilibrium to the right or to the left? (2) Calculate the ratio of the concentration of 3-methylbenzoate ion to the concentration of 3-methylbenzoic acid at a pH of 1.59. ratio [conjugate base] / [acid] Submit Answer Retry Entire Group 9 more group attempts remainingAscorbic acid (H, C,H,0,) is a diprotic acid. The acid dissocation constants for H,C,H,O, are Kal = 8.00 x 10-5 and K„2 = 1.60 x 10-12. Determine the pH of a 0.134 M solution of ascorbic acid. 2.49 pH = Determine the equilibrium concentrations of all species in the solution. [H,C,H,O,] = 0.131 M [HC,H,0G] = 3.22 x10-3 M 7.18 x10 -8 [C,H,O; = M Incorrect
- Ascorbic acid (H,C, H,0,) is a diprotic acid. The acid dissocation constants for H,C. H,O, are K - 800 x 10 and Ka- 1.60 x 10-1 Determine the pH of a 0.138 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. (H,C,H,0, = M |HC, H,0;] - C,H,O-4 F Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. R V Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. $2 CH,COO species Explanation NH3 CH₂CH(OH)COO CH₂CH(OH)COOH 5 % NH CH₂COOH H₂O G T H₂O* B Check 20 6 relative pH of 0.1 M aqueous solution Y H (Choose one) ▼ (Choose one) ▼ 8 (highest) (Choose one) ▼ 6 (Choose one) ▼ N 1 (lowest) MacBook Pro 7 U J * 8 M 1 X K ( 9 Ś O ) O L © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |…Determine the Ka for an acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 1 2 NEXT The pH for 0.0715 M solution of CC13CO2H is 1.40. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -0.032 CCI CO₂H(aq) + H₂O(1) H3O+(aq) + CCI CO₂-(aq) RESET 0 0.0715 1.40 -1.40 0.040 -0.040 0.032
- Write the appropriate equilibrium expression, set up an ICE table, solve for “x” and then proceed to calculate the concentration of all species at equilibrium. Calculate the pH of each solution. You will need to look up the appropriate ionization constants, Ka or Kb, in your book. Indicate whether the 5% rule can be applied and, if not, be sure to solve using the quadraticequation. Recalculate Ka or Kb to check.(a) 0.0092 M HClO, a weak acid (c) 0.0810 M HCN, a weak acid(b) 0.0784 M C6H5NH2, a weak base (d) 0.11 M (CH3)3N, a weak base4. What is the original molarity of a solution of formic acid (HCOOH) whose pH is 3.26 at equilibrium? 5. Calculate the percent ionization of benzoic acid having the following concentrations: (a) 0.20 M, (b) 0.00020 M. 6. Calculate the percent ionization of Ammonium hydroxide, NH4OH at the following concentrations: (a) 0.60 M, (b) 0.0046 M, (c) 0.00028 M. Comment on the trends. 7. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid.8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach?9. Calculate the [H+], [C2O4-2],…a) Why can you not prepare a solution of pH = 8 by diluting sufficiently a 0.01 M solution of HCl with water? b) You could determine Ka for benzoic acid by measuring the pH of a 0.010 M solution of benzoic acid. Why is the graphical method used in this experiment a better way of determining Ka? c) List the measurements along with their uncertainties made in the determination of the molar mass of benzoic acid. Calculate the uncertainty in the mola r mass of benzoic acid determined by the titration.
- Determine the Ka for an acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. NEXT > 5 A solution of phenol (HC H₂O) is prepared by dissolving 0.385 g of phenol in 2.00 L of H₂O. The solution has a pH = 6.29. Fill in the ICE table with the appropriate value for each involved species o determine the unknown concentrations of all reactants and products. H_O*(aq) + Initial (M) Change (M) Equilibrium (M) 1 HC,H,O(aq) + 5 H₂O(1) 2 C_H,O(aq)Write the basic equilibrium equation for HS⁻. Be sure to include the proper phases for all species within the reaction.MISSED THIS? Read Section 18.2 (Pages 788-799): Watch KCVs 18.2A, 18.28. IWE 16.2. Solve an equilibrium problem (using an ICE table) to calculate the pH of each of the following solutions. COLLA a solution that is 0.170 M in HC₂H₂O₂ and 0.105 M in KC₂H₂O₂ Express your answer to two decimal places. ▸View Available Hint(s) pH = Submit Part B ΜΕ ΑΣΦ a solution that is 0.255 M in CH, NH, and 0.135 M in CH, NH, Br Express your answer to two decimal places. View Available Hint(s) pH = 195] ΑΣΦ
