5 c) Benzoic acid, HC¬H5O2, is a weak monoprotic acid. A stock HC-H;O2 solutionwith unknown concentration was prepared.A 25.00 mL sample of the stock HC,H5O2 solution was titrated with0.1234 M sodium hydroxide to the equivalence point, using phenolphthalein as anindicator. The titration took 20.26 mL of titrant (sodium hydroxide).(c) Write a balanced net ionic equation for the chemical reaction that occurs in thistitration.

The net ionic equation shows ions which are only present directly in the reaction all spectator ions…

Answered: 5 c) Benzoic acid, HC;H5O2, is a weak…

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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1) A 25.0 ml solution of an unknown concentration of phosphoric acid, H3PO4, is titrated with0.250 M solution of magnesium hydroxide (Mg(OH)2). The equivalence points are reached with 35.5 ml of magnesium hydroxide is added. What is the concentration of the unknown phosphoric acid? Type of problem? How do you know What are you looking for? What substance do you want and what units do you want it in? Solve
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5 b) Benzoic acid, HC7H5O2, is a weak monoprotic acid. A stock HC,H5O2 solution with unknown concentration was prepared. A 25.00 mL sample of the stock HCH5O2 solution was titrated with 0.1234 M sodium hydroxide to the equivalence point, using phenolphthalein as an indicator. The titration took 20.26 mL of titrant (sodium hydroxide). (b) Write a balanced complete ionic equation for the chemical reaction that occurs in this titration.
15.00 mL of 0.214 M oxalic acid, H2C2O4 ,solution was placed in an Erlenmeyer flask. 0.237 M KOH solution was used to titrate the solution in the flask. H2C2O4 is a diprotic acid and the Hs that are shown in blue are the Hs that will react with the hydroxide ion of a base. During the titration, KOH solution was added until ________ moles of H2C2O4 were in the reaction flask.
5mL of 0.150 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl) The Kb for ammonia is 1.75 x 10-5 1)Write a balanced chemical equation for the reaction of ammonia and hydrochloric acid and a balanced chemical equation for the equilibrium of ammonia in water. 2) What is the pH of the ammonia solution prior to the addition of any HCl?
A 0.434 g sample of a monoprotic acid is dissolved in water and titrated with 0.170 M KOH. What is the molar mass of the acid if 18.5 mL of the KOH solution is required to neutralize the sample? molar mass: g/mol 19 || ||| |
The formula H₂SO4 + 2 KOH --> K₂SO4 + 2 H₂O describes the reaction between sulfuric acid and potassium hydroxide. In the titration done, 20 mL of KOH with an unknown concentration is put into a flask with bromthymol blue indicator. The KOH solution was titrated with a 0.25 M H₂SO4 solution. Three trials were performed and each trial yielded to an endpoint of yellow-colored solution, which is the desired endpoint. After three trials, the following readings were obtained: 15.5, 15.1, and 14.9 mL respectively. Calculate the molarity of Potassium hydroxide. (Answer must be rounded off to 2 decimal places)
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An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution? 2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution? 3. What is the concentration of Ag+ in solution?
7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. H3C6H5O7 (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?
Suppose that 42.00 mL of 0.150 M NaOH is added to 0.360 g of a weak acid, H3A. The excess NaOH is then titrated with 23.40 mL of 0.120 M HCl. What is the molar mass of the acid? a) 103 g/mol b) 241 g/mol c) 190 g/mol d) 310 g/mol
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