A student wants to prepare a standard solution of BSA. They create a stock solution of BSA by add O.174 g of solid BSA powder into a 10 ml volumetric flask, then fills the flask to the line with 0.1M PBS buffer. The student uses a volumetric pipet to transfer 4 ml of stock solution into a new 10 ml volumetric flask, then fills the flask to the calibration line with 0.1M PBS buffer, and calls this Dilution 1. The student uses a micropipette to transfer 23 ul of Dilution 1 and 55 ul of 0.1M PBS butfer into a cuvette. Assuming the volumes are additive, what is the concentration of BSA in the cuvette in mg/mL? Report your answer with two places after the decimal.

A student wants to prepare a standard solution of BSA. They create a stock solution of BSA by add O.174 g of solid BSA powder into a 10 ml volumetric flask, then fills the flask to the line with 0.1M PBS buffer. The student uses a volumetric pipet to transfer 4 ml of stock solution into a new 10 ml volumetric flask, then fills the flask to the calibration line with 0.1M PBS buffer, and calls this Dilution 1. The student uses a micropipette to transfer 23 ul of Dilution 1 and 55 ul of 0.1M PBS butfer into a cuvette. Assuming the volumes are additive, what is the concentration of BSA in the cuvette in mg/mL? Report your answer with two places after the decimal.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 37QAP: An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is...

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You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
It is a solution of unknown concentration in which a solution of accurately known concentration is gradually added until the reaction is complete. Analyte Endpoint Indicator Titrant
You collected the following data from a titration experiment using a 0.129M standardized NaOH solution to titrate a 26.55 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Trial 1 0.44 19.69 ?? Trial 2 0.18 17.2 Trial 3 0.50 19.94 For just Trial 1, determine the amount of NaOH delivered for the titration with appropriate significant digits. Do not include units.
In the experiment, the amount of acetic acid in vinegar was determined by titrating with 0.1 M NaOH solution. In the analysis, three trials were performed to obtain more precise result. The table shows the initial and final burette readings for three titrations: Initial Burette Reading (mL) Final Burette Reading (mL) Trial 1 2.9 10.6 Trial 2 10.6 18.1 Trial 3 18.1 25.7 According to the given data, calculate molarity of acetic acid in the commercial vinegar. Please be sure that your answer includes followings; a) moles of NaOH for each trial b) average mole of NaOH c) average mole of acetic acid in 50 mL solution d) average mole of acetic acid in 250 mL solution e) molarity of acetic acid in vinegar.
You want to make a solution of the primary standard sodium oxalate. It has a molecular mass of 133.999 g/mol (no error). Your analytical balance has an error of 0.2 mg. You add some weighing paper to the balance and it reads a mass of 0.23626 g. You then add sodium oxalate onto the weighing paper until the mass registers as 2.8539 g. You carefully transfer this to a 250.0 ml volumetric flask with an error of 0.1 ml and dissolve the sodium oxalate in a sufficient volume of water. What is the concentration of the oxalic acid (in M) and what is the absolute error (also in M).
1. A sample of pure sodium oxalate, Na2C2O4 , weighing 0.2856 g is dissolved in water, sulfuric acid is added, and the solution titrated at 70°C , requiring 45.12 mL of a KMNO4 solution. The end point is overrun and back-titration is carried out with 1.74 mL of a 0.1032 N solution of oxalic acid. Calculate the normality of the KMNO4 solution. Hint: A redox reaction is involed between oxalate and permanganate. Look at the changes in oxidation state by determining the balanced redox reaction: 5C20,2 + + 2MN2+ 2 Mn04 + 10H* → 10CO2 + 8H20
A mixture containing KCl and NaBr was analyzed by Mohr's method. A mass of 0.31011 g of the mixture was dissolved in 50 mL of water, the Na2CrO4 indicator was added, and it was titrated with a 0.11011 mol/L AgNO3 solution. The endpoint was 36.011 mL. What are the % m/m concentrations of KCl and NaBr in the mixture?
Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution. From the procedure, find: Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84 average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)
A 5.00 mL aqueous sample containing hydrogen peroxide was diluted to 25 mL and analyzed by titration with permanganate: 2MnO4- + 5H2O2 + 6H+ → 5O2 + 2Mn2+ + 8H2O The sample required 42.8 mL of 0.0175 M permanganate to reach the end point. What is the concentration of hydrogen peroxide in the original sample?
You collected the following data from a titration experiment using a 0.123M standardized NaOH solution to titrate a 27.36 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Initial Final Vol Acid Burette Burette Delivered Concentration Reading (mL) Reading (mL) (mL) (M) Trial 1 0.56 19.20 ?? Trial 2 0.57 19.7 Trial 3 0.92 19.56 For just Trial 1, determine the Molarity concentration of the H2SO4 to 3 significant digits. Do not include units. Answer: