Calculate the equilibrium constant (Kc) for the following reaction: CH3COOH(aq) + OH aq) CH3CO0 (aq) + H2O(1) The K, of acetic acid is 1.75 x 105; and Kw, (H2O(1) + H20() HO (aq) + H3O*(aq)) for auto-ionization of water = 1x 10 14 Hint: First write the equilibrium expressions for acetic acid and the authorization of water separately then apply manipulation rules of Kand find the answer) BIU A A I E E E x x, E 12pt Paragraph

Calculate the equilibrium constant (Kc) for the following reaction: CH3COOH(aq) + OH aq) CH3CO0 (aq) + H2O(1) The K, of acetic acid is 1.75 x 105; and Kw, (H2O(1) + H20() HO (aq) + H3O*(aq)) for auto-ionization of water = 1x 10 14 Hint: First write the equilibrium expressions for acetic acid and the authorization of water separately then apply manipulation rules of Kand find the answer) BIU A A I E E E x x, E 12pt Paragraph

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

Sodium acetate, NaCH3CO2, of mass 7.4 g is used to prepare 250 cm3 of aqueous solution. What is the pH of the solution?
The solution of total volume 0.50 L was prepared by the addition of 0.10 moles of KF to sifficient water. What are the major species of the solution and pH ?
When acidulated water (dil.H2SO2solution) is electrolysed, will the pH of the solution be affected? Justify your answer.
Estimate the fraction, f, of F6P in a solution in which G6P and F6P are in equilibrium at 25 °C given that ΔrGΘ = +1.7 kJ mo l-1 at that temperature, which implies that K=0.50.
A buffer solution of volume 100 cm3 consists of 0.10 M CH3COOH(aq) and 0.10 MNaCH3CO2(aq). (a) What is its pH? (b) What is the pH after the addition of 3.3 mmol NaOH to the buffer solution? (c) What is the pH after the addition of 6.0 mmol HNO3 to the initial buffer solution?
The standard reaction Gibbs energy for the reactionH2(g) + (1)/(2)O2(g) → H2O(I) is -237.13 kJ mol-1 at 25 °c. Determine the equilibrium constant in terms of concentration, Kc, at this temperature.
Calculate the pH, pOH, and fraction of solute protonated or deprotonated in the following aqueous solutions: (a) 0.150 M CH3CH(OH)COOH(aq) (lactic acid), (b) 2.4 x 10-4 M CH3CH(OH)COOH(aq), (c) 0.25 M C6H5SO3H(aq) (benzenesulfonic acid). The appropriate values for pKa or pKb are given inthe table.
Calculate the pH of a 2.00 M Na2CO3 given that the pKa’s of the first and second dissociation of H2CO3 (aq) acid are 6.37 and 10.32, respectively.
Estimate the pH of 1.5 x 10-4 M CH3COOH (aq), being careful to treat this solution as dilute, and not open to the approximations used as given below.
The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175mg CaCO3il? How many milliliters of concentrated sulfuric acid, 94.0% (w/w), specific gravity of 1.831 are required to prepare 1 liter of a 0.100 M solution? The solubility-product constant for Ce(IO3)3 is 3.2x1010. What is the Ce3+ concentration in a solution prepared by mixing 50.0 ml of 0.0250 M Ce3.. with 50.00 ml of water?
Estimate the pH of a solution of 0.50 M HCI(aq), assuming ideal behaviour. The mean activity coefficient at this concentration is 0.769. Calculate a more reliable value of the pH .
The dissociation vapour pressure (the pressure of gaseous products in equilibrium with the solid reactant) of NH4CI at 427 °C is 608 kPa but at 459 °C it has risen to 1115 kPa. Calculate (a) the equilibrium constant. (b) the standard reaction Gibbs energy, (c) the standard enthalpy, (d) the standardentropy of dissociation, all at 427 °C. Assume that the vapour behaves as a perfect gas and that ΔHΘ and ΔSΘ are independent of temperature in the range given.