The Kjeldahl procedure was used to analyze 244 µL of a solution containing 38.1 mg protein/mL. The liberated NH3 was collected in 5.00 mL of 0.0375 M HCl and the remaining acid required 5.98 mL of 0.00998 M NaOH for complete titration. What is the weight percent of nitrogen in the protein?

The Kjeldahl procedure was used to analyze 244 µL of a solution containing 38.1 mg protein/mL. The liberated NH3 was collected in 5.00 mL of 0.0375 M HCl and the remaining acid required 5.98 mL of 0.00998 M NaOH for complete titration. What is the weight percent of nitrogen in the protein?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.38QAP

See similar textbooks

Related questions

Q: 10.00 mL sample of 1.20 M HNO2 (analyte) (pKa = 3.34 and Ka = 4.57x10-4) is titrated with 1.20 M…

A: Given , pka = 3.34 Molarity of HNO2 = 1.20 M Volume of HNO2 = 10 mL Mmol of HNO2 = M × V = 1.20…

Q: 0.6000 g sample contains NaHCO₃, Na₂CO₃ , and NaOH, either alone or in permissible combination.…

A: A neutralization reaction is a reaction in which an acid reacts with a base to form salt and water…

Q: A 25.00 mL sample of HCl of unknown concentration is titrated with 21.12 mL of 0.1201 M KOH to the…

A: Given :- Molarity of KOH solution = 0.1201 M Volume of KOH solution = 21.12 mL Volume of HCl…

Q: -A 0.2000-g sample containing urea is analyzed by the Kjeldahl method. The ammonia is collected in…

A: Kjeldahl nitrogen determinations are used for a variety of applications like food and beverages,…

Q: A sample containing both HCl (FW 36.45) and HNO3 (FW 62.98) had a density of 1.083 g/mL. A 10.00-mL…

Q: A titration experiment required 12.50 ml of standard hydrochloric acid solution to reach the…

A: Here, we are performing double titration. In double titration we use two indicators first…

Q: A Fajans titration of a 0.7908-gg sample required 45.32 mL of 0.1046 M AgNO3. Express the results of…

Q: A litre of solution containing 0.1 mol of CH3COOH and 0.1mole of CH3COONa provided buffer of pH…

A: Given : Moles of CH3COOH taken = 0.1 mol. Moles of CH3COONa taken = 0.1 mol. And moles of NaOH added…

Q: Which of the following is incorrect about direct titration? 1. OThe prepared solutions must be…

A: Titration is a method to determine the concentration of an unknown solution by using the solution of…

Q: 4) How many grams of potassium azide (KN3, MM = 81.118 g/mol) are present in 250.0 mL of a pH 4.20…

A: Buffer is a solution which has a specific pH and resist a change in its pH when any acid or a base…

Q: A 50.0 ml of acidic solute (Ka = 1.20 x 10 2) is titrated with a 2.50 mL of %3D 1.00 x 10-5 M NaOH…

A: Given: Ka of acid solute = 1.20 X 10-2 Volume of acid solution = 50.0 mL = 0.050 L…

Q: A solution contains NaHCO3, Na2CO3, and NaOH, either alone or in permissible combination. Titration…

Q: If all the N in 10.0 mmols urea, CO(NH2)2, is converted to NH4HSO4, and if with excess NaOH the NH3…

A: The volume of NaOH is required to be calculated.

Q: what pH range should the indicator change color to determine the endpoint of titration? Over what pH…

A: According to the given graph, the equivalence point of the given titration is at pH = 8.5. An…

Q: A student titrates 29.00 mL of 0.2250 M pyridine (Kb = 1.7*10-9) with 0.3750 M HBr. Calculate the pH…

A: Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

Q: A 50.0 ml of acidic solute (K. = 1.20 x 10-2) is titrated with a 2.50 mL of x 10-5 M NaOH solution.…

A: Given: Ka of acid solute = 1.20 X 10-2 Volume of acid solution = 50.0 mL = 0.050 L…

Q: An unknown sample containing mixed alkali (NaOH / NaHCO3 / Na2CO3) was analyzed using the double…

Q: A titration experiment required 12.50 ml of standard hydrochloric acid solution to reach the…

A: Volume of HCl required for phenolphthalein endpoint = 12.5 mL Volume of HCl required for methyl…

Q: 3, Calculate the pH of a solution prepared by mixing 150.0 mL of 0.200 M hydrobromic acid and 150.00…

A: (3)

Q: In order to determine the concentration of benzylamine (pKa = 9.33) in a urine sample, acid-base…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A titration of 100.0 mL of 1.00 M malonic acid (H2A) was done with 1.00 M NaOH. For malonic acid,…

A: Answer -

Q: A titration experiment required 12.50 ml of standard hydrochloric acid solution to reach the…

A: Volume of HCl required for phenolphthalein endpoint = 12.5 mL Volume of HCl required for methyl…

Q: A 250.0-mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and…

A: When acid is neutralized by a base then equivalent of both acid and base will be equal. We should…

Q: sample containing both HCl (FW 36.45) and HNO3 (FW 62.98) had a density of 1.083 g/mL. A 10.00-mL…

Q: Consider the titration of 50.00 mL of 0.100 M CH3CO2H with 0.200 M KOH, calculate the pH after…

Q: 50 mL of benzoic acid (HC7H5O2) 0.1 mol L-1 are titrated with NaOH 0.1 mol L-1. Calculate the pH…

A: Given: Volume of benzoic acid = 50.00 mL Concentration of benzoic acid = 0.100 mol/L Concentration…

Q: 36. Titrating a 10.00 mL aliquot of 0.150 M NaOH with 0.120 M HCl will require a. 8.00 mL b. 0.18…

A: Calculation is given as follows

Q: A 100 mL sample contains H3PO4 and NaH2PO4. A 10 mL aliquot was taken and methyl orange was added as…

A: The sample contains a mixture of H3PO4 and NaH2PO4.

Q: Derive the titration curve when titrating 100.0mL of 0.100M weak base aniline (pka = 4.601) with…

Q: Consider the titration of 50.00 mL of 0.100 M CH3CO2H with 0.200 M KOH, calculate the pH after…

A: The question is based on the concept of titrations. we are titrating a weak acetic acid with a…

Q: A sample containing both HCl (FW 36.45) and HNO3 (FW 62.98) had a density of 1.083 g/mL. A 10.00-mL…

Q: A 50.0 ml of acidic solute (Ka = 1.20 x 10-2) is titrated with a %3D 2.50 mL of 1.00 x 10-5 M NAOH…

A: Given: Ka of acid solute = 1.20 X 10-2 Volume of acid solution = 50.0 mL = 0.050 L…

Q: If 12.35 ml of 0.4967N NaOH were required in the titration after the ammonia from the sample had…

A: Normality of NaOH = 0.4967 NNormality of NaOH = Molarity of NaOH = 0.4967 MVolume of NaOH required =…

Q: A mixture of NaOH (M.wt = 40) and Na2CO3 (M.wt = 106) is titrated with 0.3 M HCl, requiring 30 mL…

A: The equations of titration are : For the titration using phenolphthalein indicator,…

Q: Suppose that you titrate 50.0 mL of 0.15 M HNO2 with 0.20 M NaOH. Given that the Ka for HNO2 is 4.0…

A: Since you have asked a question with multiple sub-parts, we will solve first three sub-parts for…

Q: 2.0 g of mixture involving Na3PO4, Na2HPO4 or NaH2PO4 or involving three of them. The solution is…

A: Please find the answer attached.

Q: A 0.200-g sample containing urea (FM 60.05) is analyzed by the Kjeldahl method. The ammonia is…

A: Given, mass of sample containing urea = 0.200 g = 200 mg molar mass of urea = 60.05 g/mol…

Q: 0.7980-g sample of chloride was titrated using the Fajans method and required 45.32 mL of 0.1046 M…

A: We have given that 0.7980g sample of chloride was titrated using the Fajans method and required…

Q: A solution of an unknown weak base (0.495 g in 100 mL of water) was prepared and titrated with…

A: Here we have to select which of the following bases is weak based on the given data. Data: Molarity…

Q: The retention of a carboxylic acid analyte in HILIC will decrease as the pH of the buffer component…

A: Answer The retention of a carboxylic acid analyte in HILIC will decrease as the pH of the buffer…

Q: If all the N in 10.0 mmols urea, CO(NH2)2, is converted to NH4HSO4, and if, with excess NaOH, the…

A: MilliMoles of urea = 10 mmol 1 mole of urea = 2 moles of nitrogen 10 mmol of urea =(2 ×10) mmoles of…

Q: if all the N in 10.0 mmols urea, CO(NH2)2, is converted to NH4HSO4, and if, with excess NaOH, the…

Q: A 50.0 mL of acidic solute (Ka = 2.6 x 10-2) is titrated with a 25.0 mL of 0.001 M NaOH solution.…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: 1. A 250.0-mg sample of an organic weak acid was dissolved in an appropriate solvent and titrated…

A: Given Mass of sample = 250 mg 1 mg = 10 -3 gram 250 mg = 250 × 10-3 gram…

Q: A 300 mg sample containing Na2CO3, NaHCO3 and NaOH and inert material either alone or in some…

A: Given, mass of sample = 300 mg = 0.3 g sample contains Na2CO3, NaHCO3, NaOH and inert material…

Q: 2. A 7.5 mL sample required 28.5 mL of a 0.15 M NaOH to titrate to endpoint. a) What is the mass of…

A: Given Volume of acetic acid ( V1 ) = 7.5 mL Volume of NaOH ( V2 ) = 28.5 mL Molarity of NaOH (…

Q: A 0.5000 g sample contains NaHCO₃, Na₂CO₃ , and NaOH, either alone or in permissible combination.…

A: The percentage composition of a given compound is the ratio of the amount of each substance to the…

Q: calculate the pH after addition of 0.00, 5.00, 15.00, 25.00, 40.00, 45.00, 49.00, 50.00, 51.00,…

Q: A 100 mL solution of 0.1 M amino acid (AA) at pH 1.0 was titrated with 10 M NaOH solution. The pH…

A: Inorganic chemistry

Q: What is the pH of a buffer solution prepared by mixing 20.0 mL of 0.0600 mol L-' NaOH with 20.0 mL…

Question

The Kjeldahl procedure was used to analyze 244 µL of a solution containing 38.1 mg protein/mL. The liberated NH₃ was collected in 5.00 mL of 0.0375 M HCl and the remaining acid required 5.98 mL of 0.00998 M NaOH for complete titration. What is the weight percent of nitrogen in the protein?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider the following two acids: pKa1 = 2.98; pKa2 = 13.40 HO2CCH2CH2CH2CH2CO2H Adipic acid pKa1 = 4.41; pKa2 = 5.28 In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
A 0.5843-g sample of a plant food preparation was analyzed for its N content by the Kjeldahl method, the liberated NH3 being collected in 50.00 mL of 0.1062 M HCl. The excess acid required an 11.89 mL back-titration with 0.0925 M NaOH. Express the results of this analysis in terms of (a) %N (b) %urea, H2NCONH2 (c) %(NH4)2SO4 (d) %(NH4)3PO4
A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample. Please use the factor label method in answering.
A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample.
A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCI and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample.
A sample containing the amino acid alanine, CH3CH(NH2)COOH, plus inert matter is analyzed by Kjeldahl method. A 2.00 g sample is digested, the ammonia is distilled and collected in 50.0 ml of 0.150 M H2SO4, and a volume of 9.0 ml of 0.100 M NaOH is required for back titration. Calculate the percent alanine in the sample.
Sulfur containing compound weighing 4.8670 grams was digested and purified to form H,SO4. A 25.00-mL of 0.0090 M NaOH was added to the collected H,SO4, and the excess base was then back titrated with 13.45 mL of 0.0100 M HCl. Calculate the sulfur content in the sample in parts per million. This problem involves back titration. Write the two chemical equations involved in the analysis. Identify the analyte, “bridging" reagent and titrant. Solve for the mole of the analyte using the titration values and the stoich relationships. One mole of H2SO4 is equal to one mole of sulfur in the sample. Solve for the mass of S then the ppm S.
A 250.0-mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.0663 M NaOH, requiring 35.18 mL to reach the end point. Determine the compound’s equivalent weight
A 100 mL sample contains Na2CO3 and NaOH. A 25 mL aliquot was taken and phenolphthalein was added as indicator into the solution. The sample solution was titrated with 13.0 mL of 0.10 M HCl. After the disappearance of the pink color, methyl orange was added and the sample solution was titrated with 4.0 mL of 0.10 M HCI. Calculate the amounts of Na2C03 and NaOH in the sample as mg/100 mL. (write all chemical reactions, Na:23, C:12, 0:16, H:1 g/mol).