The Mole Concept Sulfur compounds are converted to H,SO4 while NO, compounds are converted to HNO3, and NH3 reacts with these acids to form ammonium salts. Since acidifying deposition involves different substances, one process that naturally occurs is nitrification via bacterial conversion according to: (MN = 14.01 g/mol, Mo = %3D 16.00 g/mol, MH = 1.008 g/mol, Ms = 32.07 g/mol) NH + 202 – NO, + H20+2H+ A. If 10.15 g of NH4* was found in the soil, how many ions of NH4* was present initially? B. If 256 g of H2O was produced after nitrification, how many moles of H were co-produced? C. How many grams of O are found in 7.40 x 1024 atoms of NO3 was produced? D. How many atoms of O are found in 9.30 mmol of O2?

The Mole Concept Sulfur compounds are converted to H,SO4 while NO, compounds are converted to HNO3, and NH3 reacts with these acids to form ammonium salts. Since acidifying deposition involves different substances, one process that naturally occurs is nitrification via bacterial conversion according to: (MN = 14.01 g/mol, Mo = %3D 16.00 g/mol, MH = 1.008 g/mol, Ms = 32.07 g/mol) NH + 202 – NO, + H20+2H+ A. If 10.15 g of NH4* was found in the soil, how many ions of NH4* was present initially? B. If 256 g of H2O was produced after nitrification, how many moles of H were co-produced? C. How many grams of O are found in 7.40 x 1024 atoms of NO3 was produced? D. How many atoms of O are found in 9.30 mmol of O2?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 39P

See similar textbooks

Similar questions

Silver ions can be found in some of the city water piped into homes. The average concentration of silver ions in city water is 0.028 ppm. (a) How many milligrams of silver ions would you ingest daily if you drank eight glasses (eight oz/glass) of city water daily? (b) How many liters of city water are required to recover 1.00 g of silver chemically?
When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
A chemist dissolves a 1.497-g sample of a type of metal (an alloy of Sn, Pb, Sb, and Cu) in nitric acid, and metastannic acid, H2SnO3, is precipitated. She heats the precipitate to drive off the water, which leaves 0.4909 g of tin(IV) oxide. What was the percentage of [in in the original sample?
When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part of the engine block. Why?
(Last Day Promotio... Kronos Worktorce... Maame Acheampo... MIDTERM M [Review Topics] [References] Use the References to access important values if needed for this question. How many grams of Ag,CO3 will precipitate when excess Na,CO3 solution is added to 77.0 mL of 0.690 M AGNO, solution? 2AGNO3(aq) + Na,CO3(aq) Ag,CO3(s) + 2NAN03(aq) + 2NaNO3(aq) Submit Answer Retry Entire Group 9 more group attempts remaining
(a) In 20 or less of yourown words define the term “leachate”and describe how it forms. (b) Previous records had shown that to prevent acute toxicity to organisms, the maximum mass of CdSO4 that should be allowed into the landfill was determined to be 0.1 kg. This was calculated using a standard concentration of Cd in mg/L where the volume of the leachate pond was used as 500 000L. (i) Provide the name of the CdSO4 compound. State the oxidation number of Cd in this compound (ii) You need to ensure that the concentration used to determine the mass of Cd allowed in the landfill, meets the current regulatory standard. Assuming that previous calculations determined that all of the CdSO4 would be deposited in the leachate pond, what standard concentration of Cd in mg/L was used to determine the maximum mass of allowable CdSO4?
A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.
3 Bal, (aq)+ 2 Nag POq Caq) 7 BalPO42 + l6 Nal laq • Consider the reaction of 30.0mL of 0.270M Balz with 20.0 mL of 0.3ISM Naz PO4. Lwhat quantity in meles of Balz are preset in the solution? are produced /What quantitg in moles of precipitate E ali Bal were consumed based on the balanced chomical equation? 6) What auantity in males of Na3 Pla aro present in soluction? d) What quantity in moles of precipitate are paduced if all the Naz PO, were cansumed based on the balanced chemi.cal equation? e) which reactant is limisting f What mass (in g) of precipitate is firemed when the limiting reactant is considered?
/viewer.html?state=%7B"ids"%3A%5B"1EMYPODX_-Kkn4ZIB78ytQoncxrZHwVo7%5D%2C"from"%3A'C e Kami Export - Bryce Carrington-$TOICHIOMETRY WORKSHEET#1 paf 6. Silver bromide can be precipitated through the following reaction. What mass of precipitate can be produced starting with 34.3 g of NaBr? NaBr + AGN03 NaNO3 + AgBr 7. How many moles of sodium bromide could be produced from 25.0 g of liquid Bromine? Bromine + Sodium iodide Sodium bromide + lodine
Foreattt part of iTIS qtestfoni; tonsider FOHOWIHg Btetat: You need to make a stock solution of Ca( C2H3O2 )2 with a concentration of 6.50 M. You have a 850.0 mL volumetric flask available to make this stock solution in. You are then tasked with using this stock solution to prepare a sample for use in an experiment. The experimental sample should have a final volume of 15.0 mL and a concentration of 0.350 M Ca(C2H3O2)2. a) What is the molar mass of Ca(C2H3O2)2? b) How many moles of the solute would be needed to create the stock solution using the volumetric flask available? c) How many grams of the solute should be added to the volumetric flask to create the stock solution? d) What volume, in mL, of the stock solution should be used to prepare the experimental solution through dilution? US 目 M
Caustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?
coulbonug9 oinihe olni bouogmoOB QU llaa of word Solubility Rules: Water Soluble Compounds EXSube sCHcood) or etosiq 1. Salts of ammonium (NH4*) and Group IA are always soluble. 2. Salts containing nitrate (N03-), acetate (C2H3O2-), or chlorate (CIO3-) ions are always soluble. enoiteo 1ol ooJ 3. Salts of the halides are soluble with the following exception: a. Compound containing Ag*, Hg2*, Pb²* prirdolaw Jon er Es i olnol the exception of: 4. Salts containing the sulfate ion (SO42-) are soluble elgmsx3 a. Compounds containing Ag*, Hg2*, Pb²+, Ca2*, Sr2*, or Ba2+ Water Insoluble Compounds Juloe ent! 1. Salts of the carbonate (CO32-), phosphate (PO43-), chromate (CrO42-), or sulfides (S2-) ions are insoluble with the exception of compound containing group 1A or ammonium cations. 2. Salts containing the hydroxide ion (OH-) are insoluble with the exception of compounds containing group 1A, ammonium cations, or Ba2+. biup Inot luo tneioliteoo belon Soluble means that it dissolves in water…