Table A: Standard NaCl used to make primary standard solutionMass of weighing bottle + NaC1 (g)21.8720Mass of weighing bottle after transfer (g)21.772Mass of NaCl used in solution (g)0.6948Purity of NaCl (%)100.03Table A: unknow used to make primary standard solutionMass of weighing bottle + unknow (g)16.8777Mass of weighing bottle after transfer (g)16.20010Mass of unknow used in solution (g)0.6776Purity of unknow (%)Table C: Titration of 25.00 mL aliquots of NaCl with AGNO3Trial 1Trial 2Trial 3Final Burette Reading (mL)28.2924.7925.11Initial Burette Reading (mL)4.991.491.69Volume Added (mL)23.3023.3023.42Table C: Titration of 25.00 mL aliquots of unknow with AGNO3Trial 1Trial 2Trial 3Final Burette Reading (mL)Initial Burette Reading (mL)23.9922.4526.912.891.255.61Volume Added (mL)21.1021.2021.30 Standard Sodium ChlorideWeighed mass of NaCIg in 250.0 mLPurity of NaCIMolar concentration of NaCl using weighed mass and purity =mol L-Titrations of standard NacI (25.00 mL aliquots) with the provided AGNO;Volume of AGN0, required (mL)Precise Titration #12Mean volume AgNO,mLMedian volume AGNO,mLStandard deviation in the mean titration volumemLConfidence limit for the titration volumemLRelative confidence limit for the titration volume (standardization) =pptConcentration of AGNO, from mean titration volumemol L-3.

Concentration of solution refers to amount of solute present in a given amount of solution or…

Mean volume AgNO, Median volume AgNO, Standard deviation in the mean titration volume Confidence limit for the titration volume Relative confidence limit for the titration volume (standardization) - Concentration of AgNO, from mean titration volume mL ml. mL mL ppt mol L

Mean volume AgNO, Median volume AgNO, Standard deviation in the mean titration volume Confidence limit for the titration volume Relative confidence limit for the titration volume (standardization) - Concentration of AgNO, from mean titration volume mL ml. mL mL ppt mol L

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter2: Crystallization

Section: Chapter Questions

Problem 3Q

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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.
逐步解决不使用人工智能出色完成工作非常感谢您的支持 SOLVE STEP BY STEP IN DIGITAL FORMAT DON'T USE AI | DON'T USE AI | DON'T USE AI | DON'T USE AI | 2. An ethyl alcohol solution that is 75% alcohol by weight is to be used as a bactericide. The solution is to be prepared by adding water to a 95% ethyl alcohol solution. How many grams of each should be used to prepare 400 grams of the bactericide?
Connected to DESKTOP-VKHKVG3 A solute added to a solvent raises the boiling point of the solution because Molal Boiling-Point Elevation Constants (Kb) and Freezing-Point nts the temperature to cause boiling must be great enough to boil not only the solvent but also the solute. Disconnect the solute particles raise the solvent's vapor pressure, thus requiring a higher temperature to cause boiling. 06:28 / 31:54 "TRU the solute particles lower the solvent's vapor pressure, thus requiring a higher temperature to cause boiling. the solute increases the volume of the solution, and an increase in volume requires an increase in the temperature to reach the boiling point (derived from PV = nRT]).
chri www. CHE100-lab 5 A N alt S X Molarity 11/13 Lab 5-Solution Preparation Purpose: Perform both the calculations and hands-on procedure involved in preparing solutions. Weight/Volume Percent F Background information: Consider the different concentration definitions (listed below) that have been discussed. Also consider the procedure described for preparing a solution with a volumetric flask. Volume/Volume Percent H (w/v%) = mass solute (g)/volume of solution (mL) x 100% سال (v/v%) = volume solute (mL)/volume of solution (mL) x 100% M = moles solute /volume of solution (L) Procedure: Experiment 1. Prepare one of the following solutions: (a) 100mL of aqueous 0.10M NaCl, (b) 50mL of aqueous 0.10M KCI, (c) 100mL of aqueous 0.05M MgSO4, (d) 50mL of aqueous 0.05M NaHCO3 1. Determine how many grams of solid are required. Show all steps for this calculation, using dimensional analysis with units clearly identified. 2. Prepare this aqueous solution, using a volumetric flask for the precise…
A 0.25g nonelectrolyte solute (MW=124.5g/mol) is dissolved in 100g solvent (MW-82.90g/mol) have a freezing point depression of 0.209degC. If an electrolyte (i = 2.95) solution is dissolved in the same amount of solvent and results to a freezing point lowering of 0.357degC, what is the concentration of the electrolyte)? 1.1627m 0.0116m 0.1016m 1.1672m
(Preparation of 0.1 N HCI solution in 250 ml D.W) Procedure: Preparation of approximately (0.IN) HCI from 37% and 1.2 Sp.g • Calculate the Normality of the concentrated HCl from the law: To prepare (500ml) of 0.IN HCL: NI VI = N2 V2 NI x ? = 0.1 x 500 • Transfer some of distilled water to 500ml volumetric flask and add the calculated volume of conc. HCI. Mix the content thoroughly. Complete to the mark with distilled water and make a label.
b Success Confirmation of Qu X < + с app.101edu.co Aktiv Chemistry X D2L Bar Graph Report - Spring x G The let-down reflex allows XCA. Fill words to blanks: Lon X Time's Up! The enthalpy of solution (AH) of KOH is -57.6 kJ/mol. If 1.56 g KOH is dissolved in enough water to make a 150.0 mL solution, what is the change in temperature (°C) of the solution? (The specific heat capacity of the solution is 4.184 J/g °C and the density of the solution is 1.02 g/mL). 1 4 7 +/- Untitled document - Google + 2 5 8 | °℃ 3 6 9 0 Update: Submit X C x 100
A sodium sulfate solution is measured at 2.2 molal in pure water at a source company. (sodium sulfate molar mass = 142.05 g mol) The lab needs to report the concentration in molarity. What is the final molarity of the sodium sulfate solution? (density of water = 1.0 g mL¯' ; density of the solution = 1.2 g uestion 4 %3D mL-1). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Question 4 of 29> AMoving to another question will save this response. 888. P11 64 F12 eIC " 24 4 & 7\ 3 5 6. 8. %3D dele E R T Y A S D L F G K Z C N alt alt option command command option
Solubility of an Unknown Solute 08 60 Solubility (g solute / 100g H,0) 40 10 20 30 40 50 60 70 80 90 100 Temperature (°C) According to the solubility curve above, dissolving 20 grams of solute in 100g of water at 50°C would make a solution that was [ Select] Dissolving 50g of solute in 100g of water at 60°C would [ Select] [Select] saturated unsaturated supersaturatcd 20
100 Solute per 100 g of H₂O (g) 8888GBAGO 90 80 70 60 50 40 30 20 KI 10 KNO3 V NHẠCI KCIO3 0 0 10 20 30 40 50 60 70 80 90 100 Temperature (°C) Round to the nearest 5 grams. The solution holds 85 g at 50 °C and 40 g at 25°C. What mass of KNO3 will precipitate out if the solution is disturbed? mass KNO3 = [?] g Enter
> 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…
4. If the amount of solvent was doubled to 200 grams, the solubility would: * O increase O decrease Ostay the same