The Mole ConceptSulfur compounds are converted to H2SO4 while NO, compounds are converted to HNO3, and NH3 reactswith these acids to form ammonium salts. Since acidifying deposition involves different substances, oneprocess that naturally occurs is nitrification via bacterial conversion according to: (MN = 14.01 g/mol, Mo =16.00 g/mol, MH = 1.008 g/mol, Ms = 32.07 g/mol)%3DNH +202NO, + H20+ 2H+A. If 12.06 g of NH2 was found in the soil, how many ions of NH4* was present iniially?B. If 500 g of H20 was produced after nitrification, how many moles of H were co-produced?C. How many grams of O are found in 1.815 x 104* atoms of NO3 was produced?D. How many atoms of O are found in 6.88 mmol of O,?

A mole can be defined as 6.023 × 10 23 of some chemical unit be it atoms, molecules, ions, or…

The Mole Concept Sulfur compounds are converted to H2SO4 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 = 16.00 g/mol, MH %3D = 1.008 g/mol, Ms = 32.07 g/mol) %3D NH +202 - NO, + H20+2H+ A. If 12.06 g of NH4 was found in the soil, how many ions of NH4 was present iniially? B. If 500 g of H20 was produced after nitrification, how many moles of H were co-produced? C. How many grams of O are found in 1.815 x 10-4 atoms of NO3 was produced? D. How many atoms of O are found in 6.88 mmol of O2?

The Mole Concept Sulfur compounds are converted to H2SO4 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 = 16.00 g/mol, MH %3D = 1.008 g/mol, Ms = 32.07 g/mol) %3D NH +202 - NO, + H20+2H+ A. If 12.06 g of NH4 was found in the soil, how many ions of NH4 was present iniially? B. If 500 g of H20 was produced after nitrification, how many moles of H were co-produced? C. How many grams of O are found in 1.815 x 10-4 atoms of NO3 was produced? D. How many atoms of O are found in 6.88 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

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?
Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60 C), filtering to remove insoluble impurities, cooling to 0 C to precipitate solid NaHCO3, and then filtering to remove the solid, leaving soluble impurities in solution. Any NaHCO3 that remains in solution is not recovered. The solubility of NaHCO3 in hot water of 60 C is 164 g/L. Its solubility in cold water of 0 C is 69 g/L. What is the percent yield of NaHCO3 when ills purified by this method?
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?
Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
A mixture of xenon and ?uorine was heated. A sample of the white solid that formed reacted with hydrogen to yield 81 ml of xenon (at STP) and hydrogen ?uoride, which was collected in waiter, giving a solution of hydro?uoric acid. The hydro?uoric acid solution was titrated, and 68.43 mL of 0.3172 M sodium hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced Chemical equations for the reactions involving xenon.
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
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…
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
(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?
Calculate the volume (in L) of Carbon dioxide that will be formed if 25.0 grams of potassium oxalate will react with potassium permanganate in the solution. The density of the carbon dioxide is 1.98 kg/m3 K2C2O4 + KMnO4 + H2O ----> CO2 + Mn (OH)2 + KOH (Molar mass: Potassium hydroxide: 56.11 g/mol; Potassium permanganate: 158.04 g/mol; Water: 18 g/mol; Carbon dioxide: 44 g/mol; Potassium oxalate: 166.20 g/mol; Manganese (II) hydroxide: 88.96 g/mol)
Most commercial samples of K MnO contain some manganese dioxide that must be femoved prie Submit Request Answer Part B Why is the K MnO4 not stored in a rubber-stoppered bottle? Rubber doesn't make a good seal with the plastic bottles in which permanganate is usually stored. Rubber can oxidize the permanganate solution. O Rubber is made of inorganic matter and will reduce the permanganate solution. Rubber is made of organic matter and will reduce the permanganate solution. Submit Request Answer Provide Feedback P Pearson Copyright © 2020 Pearson Education Inc. All rights reserved. I Termns of Use I 40 DELL