DAI Fill in the formulas, ions, equilibrium equations and expressions, constants, and measured pH's for the solutions in the tables below. Value of Equilibrium Constant 0.10 M Solution Ion Expected to Hydrolyze Spectator Ion Net-Ionic Equation for Hydrolysis Equilibrium Expression pH of Solution (Specify Ka, Kb, Kw) (Specify Ka, Kb, Kw) Distilled water None None None H₂O Example: Sodium acetate C2H3O2 (aq) + H₂O (1) C₂H₂O₂ Na+ - NaC₂H3O2 HC2H3O2 (aq) + OH (aq) Kb [HCHO][OH] [C2H3O2] Kb 5.6 x 10-10 Sodium chloride Sodium carbonate Ammonium chloride

DAI Fill in the formulas, ions, equilibrium equations and expressions, constants, and measured pH's for the solutions in the tables below. Value of Equilibrium Constant 0.10 M Solution Ion Expected to Hydrolyze Spectator Ion Net-Ionic Equation for Hydrolysis Equilibrium Expression pH of Solution (Specify Ka, Kb, Kw) (Specify Ka, Kb, Kw) Distilled water None None None H₂O Example: Sodium acetate C2H3O2 (aq) + H₂O (1) C₂H₂O₂ Na+ - NaC₂H3O2 HC2H3O2 (aq) + OH (aq) Kb [HCHO][OH] [C2H3O2] Kb 5.6 x 10-10 Sodium chloride Sodium carbonate Ammonium chloride

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.
Q.3: Determine the pH of the dissociation of 0.1 M HCN (ag). 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).
Coral structures found in the Great Barrier Reef are composed of calcium carbonate, CaCO3, and are under threat of dissolution due to ocean acidification. Consider the following equilibrium reaction equation. CaCO3(s) + CO2(aq) + H2O(l) ⇌ Ca2+(aq) + 2HCO3–(aq) Write the expression for the equilibrium constant, Kc for this reaction. Predict whether the pH of the ocean will increase or decrease as a result of a decrease in the partial pressure of carbon dioxide in the atmosphere (circle your answer). Calculate the molar solubility (s) of calcium carbonate in water at 25 °C when Ksp = 4.5 ´ 10–9.
HA, a weak acid, also forms the ion HA, in solution. The reaction is HA(aq) + A (aq) = HA, (aq) The weak acid has K, = 8.64 × 10-7 and the reaction has K = 3.80. Calculate the concentrations of A, H*, and HA, in a 1.00 M solution of HA. [A¯] = M [H*] = M [HA,] = M
Use the Acid-Base table to write net equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed. (Use the lowest possible coefficients. Omit states-of-matter in your answer. Your reaction arrow may be either a right arrow (-->) or an equilibrium arrow (<=>), depending upon the value of Keq for the reaction.
Write the concentration equilibrium constant expression for this reaction. 312(s)+2 Cr³* (aq)+7H2O(l) →Cr₂O²½˜¯(aq)+61¯ (aq)+14H*(aq) ☑ ==
What is the pH of a grapefruit that contains 0.007 M citric acid solution (C;HgO;)? CH3O;(aq) + H2O(2) = CGH;0, (aq) - H30ʻ(aq) K, = 7.5 x 104 2.71 3.62 5.35 4.54
In some natural systems the pH must be maintained within very narrow limits. e.g. in human blood the pH must remain close to 7.4 or cell deterioration occurs. Blood contains several weak acid/conjugate base equilibria called buffers, which control the pH.One weak acid present in blood is the dihydrogen phosphate ion, H2PO4-(aq), for which the equilibrium in aqueous solution is H2PO4-(aq) +H2O(l) <--> HPO42-(aq) + H3O+(aq). a) What would be the effect on this equillibrium of adding hydrochloric acid solution?b) Write the expression for the equilibrium constant of this reaction.c) If 0.5 mol H2PO4- and 0.5 mol HPO42- are in equilibrium in 1.0L of aqueous solution, calculate the pH of the solution. (Ka for H2PO4-= 6.4 x 10-8)d) 0.010 mol HCl is now added to the 1.0L of the solution in c). Assuming that all the added H+ ions are used up in the equilibrium shift, calculate the concentrations of H2PO4- and HPO42-. Hence calcuate the pH of this solution.e) 0.010 mol HCl has been added…
42. A buffer is prepared using acetic acid, CH3COOH, (a weak acid, pKa = 4.75) and sodium acetate, CH3COONa (which provides acetate ions, the conjugate base), according to the following proportions: Volume of CH3COOH(aq): 139.0 mL Concentration of CH3COOH(aq): 1.103 M Volume of CH3COONa(aq): 127.0 mL Concentration of CH3COONa(aq): 1.259 M Calculate the pH of this buffer after the addition of 20.00 mL of 3.00 M sodium hydroxide, NaOH, a strong base. 4.38 5.90 4.69 4.81 5.12
A 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, 'buffer
Calculate the equilibrium Molarity of HPO4^2-
Give detailed answer with explanation needed