10. (12 pts) Formic acid, HCCOH, ionizes according to the following equation:HCOOH(aq)+H,O(l)=HCOO (aq)+H,O* (aq)You have 500.0 mL of 0.200 M forming acid. Calculate the volume of NaOH, 0.0500 M, thatshould be added to formic acid to form a buffer that has a pH of 4.00. Ka = 4.0 × 104.14. (12 pts) Calculate the pH of 0.200 M Barium acetate, Ba(CH3COO)2. Ka for aceticacid, CH3COOH, is 1.8 × 10-5.

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Answered: 10. (12 pts) Formic acid, HCCOH,…

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...

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||| O crosoft O 3 Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq) + NaHCO3(aq) NaCl(aq) + H₂O(l) + CO₂(g) The CO₂ gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 200. mL of a 0.072 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits. W CHEMICAL REACTIONS Solving for a reactant in solution Microsoft Microsoft 6.52.210... 08 g Explanation 10 Check 280 x10 X 2 NOV 13 Ś ||| - K Jay SETMANES tv ♫ MacBook Pro DZA . E © 2022 McGraw Hill…
6. a) What is the pH of pure water at 35.0 °C? At this temperature Kw = 2.042 x 10-14. b) Based on the information in part a) above, is the self-ionization of water an endothermic or exothermic process? Explain why. c) The net ionic equation for the reaction of a strong acid with a strong base is: H3O*(aq) + OH(aq) 2 H-ОФ What is the equilibrium constant for this reaction at 35.0 °C?
A common indicator ionizes in solution according to the equation: HA(aq) → H"(aq) + A (aq) reaction (1) red yellow When the indicator is dissolved in distilled water, the solution is yellow. If excess HCl is added to the solution, the solution turns (or stays) v as the v reaction predominates to establish equilibrium. We know that the dissociation of water takes place in the same solution: H2O(1) + H*(aq) + OH"(aq) reaction (2) If excess NaOH is added to the solution, the equilibrium in reaction (2) shifts to the v, thereby v H". The consequent effect on reaction (1) would be that the color is
6. a) What is the pH of pure water at 35.0 °C? At this temperature Kw = 2.042 x 10-14. b) Based on the information in part a) above, is the self-ionization of water an endothermic or exothermic process? Explain why. c) The net ionic equation for the reaction of a strong acid with a strong base is: H;O*(aq) + OH(aq) → 2 H2O1) What is the equilibrium constant for this reaction at 35.0 °C?
5.
Chemistry (Part -3) =============
A student prepares three solutions, X, Y, and Z, as described in the table above. The values of Ka for the acidic species in the solutions are given in the table below.
5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5
ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called Xcitingpartic acid (HXp). She prepared a solution of the weak acid by diluting 2.7 ml of 0.20 M HXp with 19.3 mlL of water. Upon measuring the conductivity of the solution and a blank, she obtained 205.0 µS/cm and 2.0 uS/cm, respectively. She also measured the pH of the solution and got a pH of 3.49. Help her find the following: 1. Concentration of the weak acid (HXp) after dilution 2. Corrected conductivity 3. Molar conductivity of the solution 4. Equilibrium concentration of H30, and Xp 5. a 6. Equilibrium concentration of the weak acid (HXp) 7. K, 8. Ao
A chemist titrates a 25.0 mL sample of 0.239 M benzoic acid (C6H5COOH) against a 0.100 M solution of NaOH.The overall reaction is shown by the equation below: C6H5COOH(aq)+NaOH(aq)C6H5COONa(aq)+H2O(l) The Ka value for benzoic acid is 6.28 × 10–5. Calculate the pH at the start of the titration, before any NaOH has been added. Give your answer correctly to two places after the decimal.
For 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.
Consider exactly one litre of a propanoic acid buffer solution, containing 0.600 M C3H5OOH and 0.252 M C3H5OO- . 3.1 Determine the pH of the buffer solution. 3.2 Determine by means of a full calculation the change in pH of the buffer solution that will result when 100. mL of a 1.00 × 10−2 M HCℓ solution is added to it. You must indicate all the relevant reaction equations in your working.

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