Mass of empty weighing paper Mass of weighing paper + unknown Mass of unknown Trial 1 Trial II Trial III 0.849 2.90g 0.83g 2.879 2.04g 0.85g 2.90g 2.05g 2.06g Volume of H2SO4 20.00 mL 20.00 mL 20.00 mL Initial buret reading, Vinitial 0.5ml Final buret reading, 32.6ml V final Volume of NaOH used for titration (Vinitial - Vfinal) 32.1m 0.1ml 0.5ml 32.2ml 30.7ml 32.1ml 30.2ml For each trial, determine the % Na2CO3 in the sample and determine an average % Na2CO3 in the sample.

- OWLV2 | Assigr X MindTap Cen X gs MindTap - Cen x Gamu of ca Go X b My Questions static/nb/ui/evo/index.html?elSBN=9781337790840&id%3D299783426&snapshotld%3D7857658& CENGAGE MINDTAP Q sea napter 8: Chemical Composition AA e. aluminum sulfate Answer 51. For each of the following samples of ionic substances, calculate the number of moles and mass the positive ions present in each sample. a. 4.25 g of ammonium iodide, NH,I b. 6.31 moles of ammonium sulfide, (NH4), S c. 9.71 g of barium phosphide, BagP2 d. 7.63 moles of calcium phosphate, Caz (PO4)2 52. For each of the following ionic substances, calculate the percentage of the overall molar mas

B Brock Sakai : CHEM 1P91 - Fall X b My Questions | bartleby ChemTeam: Combustion Analys X G oxygen molar mass - Google S X B Brock Sakai : CHEM 1P91 - Fall x + Ims.brocku.ca/portal/site/90b45528-0b04-4bd2-85b6-897046a1e998/page/7011eaa9-4e38-4b06-9e15-1973abb58ef6 Version 264 Assign 4 1 / 2 100% + equations are: 3 KC1O (aq) → 2 KC1 (aq) + KCIO; (aq) 4 KC1O3 (aq) → 3 KC1O4 (s) + KCI (aq) What mass of KC1O4 (in kg) can be obtained from 2.80 kg of KC1O when these reactions are carried out? Molar masses (g/mol): KC1O 90.55 KC1O4 138.55 5. An organic compound containing only C, H, and possibly O was subjected to combustion analysis. A sample weighing 0.4161 g yielded 0.686 g CO2 and 0.187 g H2O. What is the empirical formula of the compound? 6. For the complete redox reaction given here, (a) break down each reaction into its half reactions; (b) identify the oxidizing agent; and (c) identify the reducing agent. 2 FeCl3 + Zn –→ ZnCl2 + 2 FeCl2 Give the oxidation number of nitrogen in each of…

M9. Readings * OWLV2 | Assig X MindTap - Cen x g.cengage.com/static/nb/ui/evo/index.html?elSBN=9781337790840&id%3D299783426&snapshotld-785765& MindTap- Cen x G amu of ca-G x b My Question x + CENGAGE MINDTAP Chapter 8: Chemical Composition L. E AA Tools Problems 45. Calculate the percent by mass of each element in the following compounds. a. HC103 b. UF4 с. СаН2 d. Ag,S e. NaHSO3 f. MnO2

Section 3 part B

Table 1: Standardization Data Trial 1 Trial 2 O145504 Mass of KHP 04536 Initial burette reading 0.05ML 12.3 ML Final burette reading 12.8 a6.omL Volume of base used ר.12 13.2 mL Data Analysis: KH Cg Hg Da (MOIAR MASS 2041ag) 1. Calculate the molarity of base for each trial. You must use dimensional analysis – show all unit conversions (hint: start with grams of KHP used). Review the balanced equation for KHP and NaOH you wrote in Expt 11 part 1. (204.29 TRIAI 1: 0.4550g. Average: Trial 2: Trial 1: with 1875 mL of your base (use the average

Help 100% 4A To Public Health Ch x * HSC 258 - Major Projec X MindTap - Cengage Lea X C The Illustration To TH d%=55750828934189288909969212&elSBN=9781305657571&id=D1061392007&nbld=21... * Q Search th References Use the References to access important values if needed for this question. For the following reaction, 24.7 grams of sulfur dioxide are allowed to react with 9.95 grams of oxygen gas . sulfur dioxide(g) + oxygen(g) → sulfur trioxide(g) What is the maximum mass of sulfur trioxide that can be formed? grams What is the FORMULA for the limiting reagent? grams What mass of the excess reagent remains after the reaction is complete? Submit Answer

dings OWLV2 | Assig X MindTap - Cen X MindTap - Cen X G amu of ca - Go X b My Questions 7/static/nb/ui/evo/index.html?elSBN=9781337790840&id%=299783426&snapshotld%=785765& * CENGAGE MINDTAP Chapter 8: Chemical Composition f. 0.000301 mole of strontium fluoride Answer + 39. Calculate the number of molecules present in each of the following samples. a. 4.75 mmol of phosphine, PH3 b. 4.75 g of phosphine, PH3 c. 1.25 × 10-2 g of lead(II) acetate, Pb(CH3CO2), d. 1.25 x 10-2 moles of lead(II) acetate, Pb(CH3CO2)2 e. a sample of benzene, C, H6, which contains a total of 5.40 moles of carbon 40. Calculate the number of molecules present in each of the following samples.

A quality-control laboratory analyzes a product mixture us-ing gas-liquid chromatography. The separation of components ismore than adequate, but the process takes too long. Suggest twoways, other than changing the stationary phase, to shorten theanalysis time

Ba(NO,l(aq) + K,SOlaq) Baso(s) + 2 KNOlaq) Volume Volume Trial 0.10 M Ba(NO)2 (ml) 0.10 M K,SO, (ml) Mass Baso4 (s) Limiting Reagent 50. 20. 0.46 50. 40. 0.92 3 50. 50. 1.15 4 50. 60. 1.15 50. 80. 1.15 • Question 8 Use the data to identify the limiting reagent for each reaction performed. V Trail 1 a. Neither/Both EV Trial 2 b. Baso4 EV Trial 3 C. KSO4 EV Trial 4 d. Ba(NO3)2 EV Trial 5 e. KNO3 Question Help: Message instructor I Calculator Submit Question • Question 9 Why is the amount of precipitate in the Data Table above the same in Trials 3 through 5? Edit Insert Formats B IVX x' A