Titration of Acetic Acid CH3COOH 1) Record the exact Molarity of the freshly prepared solution of NaOH by reading the label on the bottle, include all digits provided. This is the solution that will be in the buret. MB = 0.0500 M 2) Record the exact volume of acid CH3COOH that was pipetted into the Erlenmeyer mL. Note the concentration is unknown and what you will solve for. flask 10.00 (This was diluted with 50 mL of water in the Erlenmeyer flask) Trial 1 Trial 2 Trial 3 Final base (mL) 30.46 30.98 29.88 Initial base (mL)__ 0.45 0.05 0.04 Total base (mL) *Molarity (M) CH COOH *Use stoichiometry to determine the molarity of your CH,COOH solution from each of trial. Show all work including units for one. Calculate Average Molarity

Titration of Acetic Acid CH3COOH 1) Record the exact Molarity of the freshly prepared solution of NaOH by reading the label on the bottle, include all digits provided. This is the solution that will be in the buret. MB = 0.0500 M 2) Record the exact volume of acid CH3COOH that was pipetted into the Erlenmeyer mL. Note the concentration is unknown and what you will solve for. flask 10.00 (This was diluted with 50 mL of water in the Erlenmeyer flask) Trial 1 Trial 2 Trial 3 Final base (mL) 30.46 30.98 29.88 Initial base (mL)__ 0.45 0.05 0.04 Total base (mL) Molarity (M) CH COOH Use stoichiometry to determine the molarity of your CH,COOH solution from each of trial. Show all work including units for one. Calculate Average Molarity

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.101E

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Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong acid HA with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: (a) After a very small volume of titrant has been added to the initial HA solution? (b) Halfway to the equivalence point? (c) When enough titrant has been added to take the solution just past the equivalence point? (d) At the equivalence point? Nanoscale representations for Question 111.
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?
Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
Nickel(II) formate [Ni(HCO2)2] is widely used as a catalyst precursor and to make metallic nickel. It can be prepared in the general chemistry laboratory by treating nickel(II) acetate with formic acid (HCO2H). Ni(CH3CO2)2(aq) + 2 HCO2H(aq) Ni(HCO2)2(aq) + 2 CH3CO2H(aq) Green crystalline Ni(HCO2)2 is precipitated after adding ethanol to the solution. (a) What is the theoretical yield of nickel(II) formate from 0.500 g of nickel(II) acetate and excess formic acid? (b) Is nickel(II) formate paramagnetic or diamagnetic? If it is paramagnetic, how many unpaired electrons would you expect? (c) If nickel(II) formate is heated to 300 C in the absence of air for 30 minutes, the salt decomposes to form pure nickel powder. What mass of nickel powder should be produced by heating 253 mg of nickel(II) formate? Are nickel atoms paramagnetic?
Consider the titration of 100.0 mL of an unknown concentration of weak monoprotic acid with 0.550 M NaOH. If 25.00 mL is required to reach the end-point, what is the concentration of the weak acid? Answer in units of moles per litre.