8 Question#2Calculate the calculated conductivity for each solution?Given DataExperimental conductivity of 0.0500 M NaCI=5364Experimental conductivity of 0.0500 M CH3COOH=356Experimental conductivity of 0.0500 M C6H1206-95Experimental conductivity of 0.0500 M CaC12-8483Experimental conductivity of 0.0500 M CuSO4=4972Experimental conductivity of 0.0500 M FEC13=14802Calculated conductivityuS/emUnroundedCalculated conductivity uS/cmRoundedSolutionIonconcentration0.0500 M NaCI0.1000.0500 M CHCOOH0.0500.0500 M CH,Og0.0500 M CACI20.000.1500.0500 M CUSO.0.1000.0500 M FeCl30.200Calculate the percent error for each value.The Equation to calculate the percent error is shown below:% Error = {[Experimental Conductivity-Calculated Conductivity]/ Calculated Conductivity) x 100

Question#2 Calculate the calculated conductivity for each solution? Given Data Experimental conductivity of 0.0500 M NaCI=5364 Experimental conductivity of 0.0500 M CH3COOH=356 Experimental conductivity of 0.0500 M C6H1206-95 Experimental conductivity of 0.0500 M CaC12-8483 Experimental conductivity of 0.0500 M CuSO4=4972 Experimental conductivity of 0.0500 M FeC13=14802 Calculated conductivity Calculated conductivity uS/cm Rounded Solution Ion concentration uS/em Unrounded 0.0500 M NaCI 0.100 0.0500 M CHCOOH 0.050 0.0500 M CH;O, 0,00 0.0500 M CaCl2 0.150 0.0500 M CuSO, 0.100 0.0500 M FeCl3 0.200 Calculate the percent error for each value. The Equation to calculate the percent error is shown below: % Error = {[Experimental Conductivity-Calculated Conductivity]/ Calculated Conductivity) x 100

Question#2 Calculate the calculated conductivity for each solution? Given Data Experimental conductivity of 0.0500 M NaCI=5364 Experimental conductivity of 0.0500 M CH3COOH=356 Experimental conductivity of 0.0500 M C6H1206-95 Experimental conductivity of 0.0500 M CaC12-8483 Experimental conductivity of 0.0500 M CuSO4=4972 Experimental conductivity of 0.0500 M FeC13=14802 Calculated conductivity Calculated conductivity uS/cm Rounded Solution Ion concentration uS/em Unrounded 0.0500 M NaCI 0.100 0.0500 M CHCOOH 0.050 0.0500 M CH;O, 0,00 0.0500 M CaCl2 0.150 0.0500 M CuSO, 0.100 0.0500 M FeCl3 0.200 Calculate the percent error for each value. The Equation to calculate the percent error is shown below: % Error = {[Experimental Conductivity-Calculated Conductivity]/ Calculated Conductivity) x 100

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Atoms in Element 1 Atoms in Element 2 Atoms in Element 3 Atoms in Element 4 Total Atoms in Molecule Total Elements in Molecule Molecule 2 2H20 4 3CO2 3 6. 9H3PO4 27 36 72 0. 6. 1 20 4 12 20 3. 5Bas(PO4)2 15 10 40 40 105 4 2(NH2S 16 22 4Fes(SOaa 12 12 36 60 3AI(HCO.)a 3 9. 27 48 12 6. 24 42 4 10M9SO. 10 10 40 60 5NaPO. 15 5 20 60 3 7M93(PO4)2 21 14 56 91 8(NH.)PO. 24 96 8 32 160 4 4NaHCO, 4 4 12 9KCIO, 9. 9. 27 45 3 2Ca(CIO.)2 2 4 12 18 3 12Ca (PO4)2 11Ca(NO3)2 7AI(OH). 24
Consider the following reaction where an excess of water was used. AICI3(s) + 3H2O(1) → Al(OH)3(?) + 3HCI(g) Identify the physical state of Al(OH)3 and tell how you will separate it from the excess water. Select one: O A. A chemical method B. Electrolysis O C. Chromatography O D. Distillation O E. Filtration
Limestone is typically 50.0% (w/w) CaCO3. How many grams of CaCO3 are present in a limestone sample weighing 1.2 kg?
7 1 4 6.3Li +1H → 2He+. - 0²/0 O 1H 4 2He 4 4Be 3 On O
I need help with these questions (Not honor class) (Not grading)
1. What volume of 65% nitric acid with a density of 1391 kg / m ^3 can be produced from 1.5 tons of ammonia if the yield of the acid is 72%
46 gr sodium (Na) reacts with excess HCl aqueous solution according to the reaction: 2Na (s) + 2HCI(aq) → 2NaC1 (aq) + H2 According to this; which of the followings is wrong? (Na:23 21 - g/mol, ClI:35.5 g/mol, H:1 g/mol) O A) 2 gr H2 is produced B) 58.5 gr NaCl is formed O C) To consume all sodium, 2 moles of HCl is needed. D) Na atoms ionize in HCl aqueous solution. O E) 2 moles NaCl is formed
3b. An impure sample of ammonium dichromate [ (NH4)2Cr207] was analyzed to determine its purity [ %(m/m) of ammonium dichromate]. a. A 1.4325 gram sample of the impure (NH4)2Cr207 was heated and decomposed in the following (unbalanced equation) reaction: • Balance the chemical equation: [ Select ] (NH4)2Cr2O7(s) [ Select ] N2(g) [ Select ] H20(L) + + [ Select ] | Cr2O3(s) b. The decomposition of the 1.4325 g of the impure sample produces 0.1252 liters of nitrogen gas (N2(g) that were collected at a temperature of 24.7°C and a pressure of 1.032 atmospheres: o Calculate the number of moles of nitrogen (N2(g)) collected in this reaction: [ Select ] mol N2 • Calculate the mass of the ammonium dichromate [ (NH4)2Cr20, ] in the sample (1.4325 g): [ Select ] g (NH4)2Cr2O7 o Calculate the %(m/m) of the ammonium dichromate in the impure sample: [ Select ] %(m/m) (NH4)2Cr2O7
3. Which process can separate a mixture of finely powdered iron and wheat flour? A. distillation 3. B. filtration C. using a magnet D. sieving E. sublimation
2.) Five standardized dilutions of aqueous lead(11) chromate solution were prepared by adding a volume of 0.0010 M PbCrO4(ag) from a buret and then diluting the solution with deionized water to a total volume of 100.0 mL. Use the provided information to determine [CrO42] in each. Hint: enter the decimal before the scientific notation. Mixture Initial Buret Reading (mL) Final Buret Reading (mL) [Cro,?] (M) 3 2.00 7.10 ? x 105
Select the correct starting material for the reaction shown below: 1) MgBr 2) H3O+ work up OH
You have a 11.5 mg sample of blood that contains various proteins. Hemoglobin is the only protein in the sample containing Fe. Hemoglobin contains 3.83% by mass of a compound called heme (C₃₄H₃₂FeN₄O₄, MW = 616.49 g/mol). You find that your 11.5 mg blood sample contains 34.9 micrograms of Fe. What is the mass percent of hemoglobin in your protein sample? -don't prematureley round