Following the directions in the laboratory manual, you create Standard 2 by transferring the following volumes of 50.1 μgmL BSA, 0.1021 M NaCl, and Bradford reagent into a small test tube. Calculate the concentration of BSA (in μgmL) in the test tube. volume BSA volume NaCl volume Bradford reagent initial pipet volume 0.85 mL 0.96 mL 4.67 mL final pipet volume 0.51 mL 0.21 mL 0.58 mL

Following the directions in the laboratory manual, you create Standard 2 by transferring the following volumes of 50.1 μgmL BSA, 0.1021 M NaCl, and Bradford reagent into a small test tube. Calculate the concentration of BSA (in μgmL) in the test tube. volume BSA volume NaCl volume Bradford reagent initial pipet volume 0.85 mL 0.96 mL 4.67 mL final pipet volume 0.51 mL 0.21 mL 0.58 mL

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter5: Chemical Reactions

Section: Chapter Questions

Problem 5.93E

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A stock solution whose concentration is 25.00 mg/mL was provided. A primary standard solution was then prepared by transferring 5.00 mL of the stock solution into a 50.00 mL volumetric flask. The primary standard solution was used to prepare three standard solutions of different concentrations by taking different volumes of aliquots into three 25.00 mL volumetric flasks: Standard Solution #1 #2 #3 Amount of Primary Solution (mL) 5.00 10.00 15.00 Three 25.00 mL volumetric flasks were then diluted to mark with water. Questions #1 What is the concentration of the primary standard solutions, expressed in units of mg/ml? #2 Re-write the concentration of the primary standard solutions obtained from Q#1 in units of μg/mL. #3 Determine the concentrations of three standard solutions in units of µg/mL. #4 What is a requirement for a "blank" solution used in calibration in spectrophotometry? Page 5 (Experiment #3)
1. What is the MW of the analyte?2. What is the meq of the analyte?3. What will be the weight (in grams) of the analyte if the standardization is to be quartered?4. What will be Normality of the solution if 7.5ml of the titrant was consumed in the standardization?5. What is the average Normality if two or more trials were conducted with the values of 0.102N and 0.105N?
The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g Volume of H2C2O4•2H2O solution = 250.0mL What is the Molarity H2C2O4 standard solution ?
Based on this student data, calculate the average molarity of the NaOH solution. Standard: KHP = potassium hydrogen phthalate, MM 204.4 g/mol Student Data Trial 1 E KHP mL initial: NaOH mL final: NaOH 2.02 0.57 19.25 Trial 2 2.05 19.25 39.80 Trial 3 1.99 1.65 20.75
a 50.0 mL sample of aqueous sodium chloride was analyzed according to the experimental procedure in part E and the following data were obtained. mass of evaporating dish: 37.628 g mass of evaporating dish + solution: 86.623 g mass of evaporating dish + solid NaCl: 41.133 g A) Calculate the percent by mass NaCl in the solution. B) Calculate the Molarity of the solution. C) Calculate the molality of the solution.
The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g what is the Number of moles of H2C2O4•2H2O?
5.00 mL of stock solution is diluted to 25.00 mL, producing solution ALPHA. 10.00 mL of solution ALPHA is diluted to 25.00 mL, resulting in solution BETA. 10.00 mL of solution BETA is then diluted to 25.00 mL, producing solution GAMMA. dilution factor for ALPHA from stock solution = 0.167 dilution factor for BETA from ALPHA solution = 0.0476 part c and d?
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B. Determination of Total Acid Content in Commercial Vinegar Sample Brand of Sample: Trial 1 Trial 2 Trial 3 Volume of sample 10.00 mL Final reading - standard NaOH solution 25.63 mL Initial reading - standard NaOH 0.08 mL solution Volume consumed - standard 25.55 mL NaOH solution 0.3059 M Molarity of standard NaOH solution Total Acidity in Sample 4.69% Mean Total Acidity in Sample 4.69% BALANCED CHEMICAL EQUATION/S INVOLVED: COMPUTATIONS:
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).
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