Using Beer's law, calculate the molarabsorptivity (M-1 cm-1) of PNP from theabsorbance. The path length of the cuvetteis 1 cm, and the stock concentration of PNPis 0.0100 mM. Convert abs/sec to M/secusing the molar absorptivity determined inthe previous step. You will use Beer's lawagain here but will solve for concentrationinstead of molar absorptivity. ConvertM/sec to mol/sec by multiplying by the totalreaction volume (3.00 mL). Convert mol/secto nmol/sec. Convert nmol/sec tonmol/min. This value represents theamount of PNP produced (nmol) by alkalinephosphatase per minute.A=ebcA=0.163b=1cmc=0.01mMTotal Volume=3mL

The amount of substance that resides in the given volume of solvent to furnish the solution can be…

Answered: Using Beer's law, calculate the molar…

EBK A SMALL SCALE APPROACH TO ORGANIC L

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Author:Lampman

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Chapter2: Crystallization

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BC Broward Col x O Onelogin xe Expt. 6 pre-l xA "Expt. 7 Quiz X G .What is an x b ziprecruiter x O 12.628+ Par X E Login x + O File | C/Users/nerbs/Downloads/Expt.%207%20Quiz,%20Part%201.pdf 10 2) If absorptivity (the constant of how much light of a given wavelength the sample absorbs) and path length (how much solution there is for light to pass through) are the same, which is true for a Beer's Law solution? a) its concentration and absorbance are proportional b) its concentration and rate are proportional c) its absorbance and rate are proportional d) the solution is an alcoholic beverage
1 g of solute is contained in 100 mL of aqueous solution. Calculate **%E" and the amount of solute remaining in the aqueous phase after (D= 10); (i) a single extraction with 90 mL of an organic solvent. (ii) three successive batch extractions with 30 mL of an organic solvent.
2) You are tasked with determining the barium content of a sample containing barium nitrate mixed with rubidium nitrate. The sample is weighed, dissolved into 50.0mg water, and treated with xs 0.500M sodium sulfate. The acid fully ionizes in this experiment. A white precipitate forms which is washed, filtered, and weighed multiple times, according to the data given below: Mass of sample 0.425g Mass of thoroughly dried filter paper 1.462g Mass of precipitate+filter after 1st drying 1.755g Mass of precipitate+filter after 2nd drying 1.699g Mass of precipitate+filter after 3rd drying 1.698g
The scatter plot below shows the density of ethylene glycol solutions vs. the mass % of those solutions. Density (g/mL) 1.04+ 1.03- 1.02- 1.01 0.99- 0.98- 8 % 10 12 14 16 18 20 Mass % Q The equation for the line of best fit shown on the scatter plot is y= 0.001683 +0.9959. Use the equation of the trendline to determine the mass percent of an ethylene glycol solution with a density of 1.015 g/mL.
2. A on is made by mixing 1.08 g of an unknown non-volatile non-electrolyte with g of benzene. The free 10.00 zing point of pure benzene is 5.5°C. The molal reezin ng point depression constant, K for benzene is 5.12°C/molal. The following data were obtained in a freezing point depression experiment Time, min Temperature C TemperatureC 0.5 0.1 0.8 0.9 0.8 0.7 0.6 0.5 0.4 0.2 -0.5 1.2 Time min 1.0 2.0 3.0 4.0 5.0 6.0 7.0 8.0 9.0 10.0 11.0 12.0 23.8 22.1 20.2 18.5 16.6 14.8 12.7 10.8 9.1 7.2 5.5 3.6 13.0 14.0 15.0 16.0 17.0 18.0 19.0 20.0 21.0 22.0 23.0 24.0 25.0 Plot a graph of time/temperature, using the y-axis for temperature and the x-axis for time. Determine the freezing point of the solution. A. 2 De-tereine tHe alality of the solthon
> EL session.masteringchemistry.com MasteringChemistry ROSTER-2019-SPRI-PULLM-CHEM-101 blackboard wsu Google Search MasteringChemistry: HW 8 KHW 8 Applications for Dilution Calculations K8 of8 Dilution as a procedure in analysis We sometimes purposely dilute solutions if the analyte concentrations wavelengths in the visible (and sometimes uitraviolet) range. Based on the dissolved solute's properties, we can quantify that solute's concentration are too high to permit an accurate measurement. For example, a spectrophotometer can measure the amount of light that passes through a sample solution for If the solute's concentration is too high, a relatively small amount of incident light having the wavelength that corresponds to the solute's absorption behavior will less light is absorbed, and the detector in the spectrophotometer can generate more reliable data. reach the dete ctor, which results in an inaccurate measurement (consider the result if you blocked the light with an opaque…
Gravimetric determination of Ksp. Table 1 Trial Volume of solution used (ml) Mass of empty beaker (g) Mass of beaker with solid residue (g) Mass Ca(OH)2 (g) Ksp for Ca(OH)₂= % error = 10mL 92.808g 92.766g 0.042g Determine the mass of dissolved solid that was in the saturated solution. Calculate the molar solubility of the solution (M) using the mass of dissolved solid, the volume of solution used in the analysis, and the molar mass of calcium hydroxide. Substitute the molar solubility into a version of equation 4.1 [Hint: use an ICE table] to determine the Kp. Provide an annotated calculation below: 1
Based on the table below, calculate F-factor and X in the water sample. (Berdasarkan jadual di bawah, kirakan faktor-F dan X dalam sampel air.) 7. Abs nitrite concentration Standard 0.032 0.4ppm Xppm Water sample 0.067
. 100 ml boiled cooled and filtered water sample takes 9.6 ml of M/50 EDTA in titration. The Permanent hardness of the water sample in terms of ppm of CaCO3 equivalent is
16) Which of the following(s) is/are correct? I- Selectivity factor is the amount of time a solute spends in the stationary phase relative to the time it spends in mobile phase II- The retention time for an analyte is the time interval between its injection onto a column and its appearance at the detector at the other end of the column. III- Distribution constant is the ratio of the total solute concentration in the stationary phase to that in the mobile phase. A) I, II and III B) Only II C) I and III D) II and III E) Only III for GC2
In gravimetric analysis, volatile electrolyte is used in peptization step a. to form small nucleib. to easily dry precipitatec. to reprecipitate the analyteexplain please
Calculate the mass percent of the ascorbic acid in the same show full solution Situation: The pounded Vitamin C tablet was half into two below are the calculated data in the experiment. Each of the half are transfered in a 250ml erlen meyer flask and added 75ml of deionized water for the vitamin C to dissolve. Then it was prepared for titration where the burette was filled with 0.09794M standardize NaOH solution then a total of with 3 drops 2% phenolphthalein indicator was added to each erlen meyer flask l, swrill it and begin the titration. below are the following data gathered: Vitamins used: Nature Made vitamin C 500mg tablet Trial 1 Mass: 0.3108g of Vitamin C tablet Initial volume: 1.6mL Final volume: 15.4mL Trial 2 Mass: 0.3349g Initial volume: 15.4 mL Final volume: 30.2 mL

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