bAnswered: 101 Chem 101 b X G how many kilograms in a p x(274) Ésta Es Tu Canció101 Chem 101XHomeXapp.101edu.coOregon Scholarship....Unofficial Transcript...myClackamas LoginDocument Require...Apps WLogonWelcome to the OS...Home - FAFSA on t...The National Societ...>SubmitQuestion 19 of 20A particular medication dosage is 45.0 mg/kg of body weight. How manymg of the medication should a child weighing 30.1 lbs. receive?mg123X56C78+-0x 1005:53 PMType here to searchENG11/21/2019+LO4t

Given, weight of child = 30.1lbs.Conversion of pounds (lbs) into kilograms:

Answered: bAnswered: 101 Chem 101 b X G how many…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter8: Sampling, Standardization, And Calibration

Section: Chapter Questions

Problem 8.8QAP

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A. B. and C. already solved (https://www.bartleby.com/questions-and-answers/chemistry-question/a89691d6-2162-4677-b0cc-dc84fcceda08). Please answer E, F and GCircle in pencil in the image on th eirght cide of the diagram is a "2"( Pb(NO3)2 ).
1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)pls compelete the 2nd table given the data
Data Given. no Trial 3 information needed
It is estimated that uranium is relatively common in earth's curst, occuring in amounts of 4g/metric ton. A metric ton is 1000 kg. At this concentration, what mass of uranium is present in 1.0 mg of the earth's curst? (The answer is suppose to be 4X10-9 grams)
is 1.52 correct? pls prove
Parts G and H. I thought the answers were 56.21 and 115.21 but it says they're wrong.
In Part B, you used a similar procedure to that of Part A to determine the mass percent of CaCO3 in an antacid tablet. The commercially accepted range of CaCO3 in an antacid tablet is 25–35% by mass. Miranda obtained the data below from her Part B trial: TRIAL PRESSURE (torr) MASS OF TABLET (g) TEMPERATURE (°C) VOLUME CO2 RECOVERED (mL) 1 750.5 0.5702 21.3 69.6 2 750.5 0.5622 21.2 68.2 Miranda determined her average % Recovery of CO2 to be 65.0% from Part A. Based on her data collected from Part A, was the average percent mass of CaCO3 in her antacid tablet within the commercially accepted range? Yes, her mass percent does fall within the commercially accepted range. No, her mass percent does not fall within the commercially accepted range.
using exactly 5.00 mL of 0.0400 M stock CuSO4 solution. Add 100 mL of water. Data for Part IMass of empty dish: 32.470 g empty dishVolume of 0.0400 M solution: 5.00 mL CuSO4 solution.Mass of dish and 0.0400 M solution: 37.497 g dish and solutionMass of dish and CuSO4 solid: 32.503 g dish and CuSO4 solidCalculations for Part I1. Calculate the mass of solution2. Calculate the mass of solid CuSO4 dissolved in the solution.3. Calculate the number of moles of solid CuSO4 dissolved in the solution.4. Calculate the mass of water evaporated from the solution.5. Calculate the density of solution, (g solution/mL solution).6. Calculate the % by mass, CuSO4 in solution (100 x g CuSO4/g solution).7. Calculate the molality of solution (moles CuSO4/kg solvent).8. Calculate the molarity of solution (moles CuSO4/L solution).9. Given that the true molarity is 0.0400 M, calculate the percent error of your result.
Enter the units of r when the amount is measured in mol L-1 and time in min (use the backslash / but be sure to use () when more than one unit is is the denominator and a space or * to mean the product, for example: L/(mol s) or L/(mol*s) or L/(s mol) or L/(s*mol) )
Propagate the error in the following expression:(0.5847(±0.0002)mole / 250.0(0.1)??) ×(1000 ml / 1 L)
A volumetric calcium analysis on triplicate samples of the blood serum of a patient believed to be suffering from a hyperparathyroid condition produced the following data: mmol Ca/L = 3.55, 3.65, 3.14. What is the 95% confidence interval for the mean of the data, assuming(a) No prior information about the precision of the analysis?(b) s → σ = 0.056 mmol Ca/L?
In a river with a constant flow rate, the factory releases wastewater containing NaCl at a concentration of 200 mmol / L to the river at 20.0 L / s. The Na+ and Cl- concentrations at the downstream observation point were 1.00 mmol / L and 0.800 mmol / L, respectively. What is the river flow Q and Cl- concentration before the inflow of drainage? The river originally contains 0.500 mmol / L of Na+.

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