25.0 mL of 2.8 M NH3(aq) was added to 20.0 mL of 1.5 M HCl(aq) and the mixture was stirred, then tested with a pH meter. Complete the following table based on the reaction. NH3 HCI NH4CI Beginning/mol choose yo v choose ycv choose your an Reaction/mol choose yo choose y
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![25.0 mL of 2.8 M NH3(aq) was added to 20.0 mL of 1.5 M HCl(aq) and the mixture was stirred, then tested with a pH meter.
Complete the following table based on the reaction.
NH3
HCI
NH4CI
Beginning/mol
choose yo v
choose ycv
choose your an
Reaction/mol
choose yo
choose y<v
choose your anv
End/mol
choose yo
choose yc v
choose your anv
Which component(s) determines pH of the solution? choose your answer...](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb23a81c0-933d-4ab8-a309-00212bcbe2e5%2F0773fa4a-5c33-4041-978f-20eaf03c8894%2F2vp8ze_processed.png&w=3840&q=75)
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- Base Base Meid Acid CH3CH2COOH(aq) + H2O()CH3CH2COO(aq) + H30*(aq) 2. Propanoic acid, CH2CH2COOH, is a carboxylic acid that reacts with water according to the equation above. At 25°C the pH of a 50.0 mL sample of 0.20 M CH3CH2COOH is 2.79. (a) Identify a Brønsted-Lowry conjugate acid-base pair in the reaction. Clearly label which is the acid and which is the base. (b) Determine the value of Ka for propanoic acid at 25°C. (c) For each of the following statements, determine whether the statement is true or false. In each case, explain the reasoning that supports your answer. (i) The pH of a solution prepared by mixing the 50.0 mL sample of 0.20 M CH3CH2COOH with a 50.0 mL sample of 0.20 M NaOH is 7.00. (ii) If the pH of a hydrochloric acid solution is the same as the pH of a propanoic acid solution, then the molar concentration of the hydrochloric acid solution must be less than the molar concentration of the propanoic acid solution. A student is given the task of determining the…The acid dissociation constant of acetic acid in methanol is 3.02 × 10-¹0. Calculate the pH of the following solutions in acetic acid: 36. 0.035 M CH3COOH a. 3.10 b. 5.49 37. 0.035 M CH3COOH + 0.070 M CH3COONa a. 4.44 b. 5.05 38. 0.035 M CH3COONa a. 2.97 b. 4.32 c. 6.90 c. 9.22 c. 11.03 d. 8.51 d. 9.82 d. 12.38Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. What is the lactic acid concentration (in M) of the titrated sample?
- Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) Follow proper significant figure rulesa. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?Lola and Richie were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08)1.What is the lactic acid concentration (in M) of the titrated sample?2. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample.3. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?
- You are given 0.5 M solution of the amino acid Arginine. • pK1 (α-carboxyl group) = 2.17 • pK2 (α- amino group) = 9.03 and • pK3 (guanidine group) = 12.48 : Answer the following questions. a) Determine the pH of the solution if you add 15 mL 0.25 M HCl to 10 mL of the 0.5 M Arginine. Assume that Arginine is in isotonic state. Show all calculations.Amino acids have different protonation states at different pH. The protonation states of the amine and carboxylic acid functional groups can vary at different pH. In addition, the side chain can have different ionic states. Choose the protonation state of lysine at physiological pH. H₂N- H NH₂ I OH H₂N. H₂N H 0=6 NH₂ IV NH₂ || OH H₂N. H H₂N H NH₂ O V NH₂ |||Phenol is a functional group that is readily ionized by adjusting the pH of the aqueous solution during an extraction. What is the neutral and ionized form? How do you convert the neutral to the ionized form?
- Students Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?Consider the bases in the table. Which base would be the best choice for preparing a pH = 9.00 buffer?A solution contains formic and tartaric acids. A 25.00 mL aliquot portion is treated with 50.00 mL of a 0.1663 mol/L solution of cerium(IV) in 12 molL sulfuric acid; after boiling for one hour, it is cooled to room temperature and the excess cerium(IV) is titrated with 8.24 mL of iron(ll) 0.1108 molL. Under these conditions all organic acids are oxidized to carbon dioxide. Another 25.00 mL aliquot portion of the acid solution is treated with 20.00 mL of 0.2383 molL cerium(IV) in 4 molL perchloric acid and heated at 50°C for 20 minutes. The solution was then titrated with 14.65 mL of 0.1012 mol/L oxalic acid. Under these conditions all organic acids are oxidized to formic acid. (a) Calculate the concentration of formic acid in g/L (b) Calculate the concentration of tartaric acid in g/L
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