3. The following image is a scheme for serial dilutions prepared for spectrophotometric analysis.If the stock solution concentration is 0.05 % (v/v) can you calculate the other tube'sconcentrations in v/v?10.0 mL. 100% dye 2.0 mL H₂O2.0 mL H₂O2.0 mL. H₂O 2.0 mL H₂O2.0 mL H₂O4.0mL4.0mL4.0 4.0 mL4.0/fil4.0mLN1.8 mL1.8 ml1.8 mL1.8 mL1.8 mL1.8 mLDilution tableTest tube #12345623Volume of food coloring stockadded to beaker from preceding, mL10.0 stock solution4.0Volume of distilled wateradded to beaker, mL4.04.04.04.0n.a.2.02.02.02.02.0

Step 1:Step 2:Step 3:Step 4:Step 5:

Answered: 3. The following image is a scheme for…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter11: Properties Of Solutions

Section: Chapter Questions

Problem 109AE: Patients undergoing an upper gastrointestinal tract laboratory test are typically given an X-ray...

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Patients undergoing an upper gastrointestinal tract laboratory test are typically given an X-ray contrast agent that aids with the radiologic imaging of the anatomy. One such contrast agent is sodium diatrizoate, a nonvolatile water-soluble compound. A 0.378-m solution is prepared by dissolving 38.4 g sodium diatrizoate (NaDTZ) in.l.60 102 mL water at 3 1.2C (the density of water at 31.2C is 0.995 g/cm3). What is the molar mass of sodium diatrizoate? What is the vapor pressure of this solution if the vapor pressure of pure water at 31.2C is 34.1 torr?
Precipitimetry The chloride in a 4.321-g food sample was precipitated through the addition of 50.00 mL of a standard AgNO3 solution (10.00 mL AgNO3 = 11.22 mL KSCN). The precipitate was coated with nitrobenzene and the mixture was diluted to 250.0 mL. A 50.00 mL aliquot was taken from the diluted solution and required 4.56 mL back titration with a %3D standard KSCN solution (22.33 mL KSCN = 0.9758 g AgNO3). %3D Formula Masses: AgNO3 = 169.87; CI = 35.45 Calculate the following: 1. Molar concentration of KSCN solution M %3D 2. Molar concentration of AgNO3 solution M %3D 3. % (w/w) chloride in the original sample =
C. Electrolytes in Body Fluids 1. Type of IV Solution 5% Isolute P (mEa/L) Plasnalyte (mEg/L) Lactated Ringer's (mEg/L) Nal+ = 130 Klt = 4 Ca2+ = 3 Nal+ = 25 K+ = 20 Nal+ = 140 Kl+ = 5 2. Cations %3D %3D Mg+ = 3 Mg2+ = 3 CI- = 22 HPO- =3 Acl- = 23 CI- = 98 Glu'-= 23 Acl- = 27 3. Anions CI'- = 109 %3D HPO = 28 %3D %3D 4. Total Charge of Cations (+) 137 137 5. Total Charge of Anions (-) 6. Sum of the Charges Copyright 2014 Pearson Education, Inc.
What mass of MgCl₂ 6H₂O is required to make a 0.200 dm³ stock solution containing 25.0 ppm Mg(II)? What volumes of this stock solution are required to make 10.0 cm³ standard solutions containing 5.00, 1.00 and 0.10 ppm Mg(II)?
Q5/ Calculate the concentration of sodium ion in grams per liter after mixing 150mL of 0.200 M NaCl and 250ml of 0.250 M Na,S04. (20M) Atom weight = Na = 22.9897, Cl = 35.453, O = 16 H=1S = 32.065, Ca = 40.078 Ba = 137.327, C= 12.0107, N = 14.0067
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.
Recall that the test solutions were prepared according to Table KEQ.2. Table KEQ.2:Volumes for the Test Solutions Test Solution 6 7 8 9 10 2.00x10-3 M Fe(NO3)3 5.00 mL 5.00 mL 5.00 mL 5.00 mL 5.00 mL Molar concentration of Fe(NO3)3 stock solution:2.00 × 10¯¹ M Molar concentration of KSCN stock solution:2.00 × 10–³ M 2.00x10-³ M NaSCN 1.00 mL 2.00 mL 3.00 mL 4.00 mL 5.00 mL 0.100 M HNO3 4.00 mL 3.00 mL 2.00 mL 1.00 mL 0.00 mL Use the ICE tables below to calculate the equilibrium concnetrations for each solution. You will use your absorbance reading and best-fit line from the calibration curve to determine the equilibrium concentration of Fe(NCS)2+
As part of this experiment you will need to determine the concentrations of Fe* and SCN ions present in test tubes 1-9. These values can be calculated using the volumes and concentrations provided in Tables 1 and 2 of the Equilibrium Lab - Procedure and the dilution equation (M,V1 = M2V2). Note: the solutions provided in the lab, and therefore the tables in the lab document, are the compounds used to prepare the solution. You must determine the concentration of the ions based on how these compounds díssociate in solution Complete the following table by filling the the calculated initial concentrations of each substance. Be sure to: Pay attention to significant figures • Round appropriately Use decimal notation (not scientific) Do not include units Test Initial [Fe3*] (M) Initial [SCN'] (M) Tube 1 3 4. 6. 7 8. 2.
2- 150 mg of NazC2O4 containing solution is titrated with a KMNO4 solution with the corretion factor 1.03. The consumption of KMNO4 is found as 29 mL. Find the theoretical molarity (M) and real concentration (Mreal) of the KMNO4 solution.
1. A solution is known to contain 38.04 ± 0.03 mM KCl, and you have taken an aliquot of this solution using a pipette calibrated to deliver 20.013 ±0.006 mL. Determine the number of moles of KCl that are delivered in the aliquot, including the absolute uncertainly in that value. 2. You deliver the aliquot taken in problem 1 into a volumetric flask with a volume of 250.00 mL ± 0.02 % and dilute the solution to volume in the flask using Dl water. What is the concentration of KCl in this flask, report your answer with the absolute uncertainty. 3. Tabulated below are replicate titration volumes for an analysis. What is the error (both absolute and percent) for the average titration volume?
SO4 -two content in 7689mL of a water sample was precipitated as Na2SO4. The precipitated was filtered, washed and calcined in an empty crucible with a mass of 27.0234g. The mass of the crucible plus Na2SO4 (142g/mol) was 27.7708g. Calculate the %m/v of Na (23g/mol) and the concentration of Na in the sample in ppm.
A sample of an infusion was diluted 10 ml to 250 ml and then 10 ml to 200 ml. It was thenanalysed and was found to contain sodium at 0.789 mg/100 ml. Calculate the concentrationof sodium in the original sample in %w/v. The sample was composed of a mixture of sodiumlactate and sodium carbonate in equimolar amounts. Calculate the amount of sodiumlactate and sodium carbonate in mg/10 ml of the sample (Na = 23, lactate = 89, carbonate =60)

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