How do I solve the problem? If a solution containing 127.23 g of silver chlorate is allowed to react completely with a solution containing 10.77 g of lithiumchloride, how many grams of solid precipitate will be formed?solid precipitate:IHow many grams of the reactant in excess will remain after the reaction?reactant in excess:werAssuming complete precipitation, how many moles of each ion remain in solution? If an ion is no longer in solution, enter azero (0) for the number of moles.molLit =Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Science Bookscontact us helpabout us careers privacy policy terms of usehere to chatO 2011-2021 Sapling Learning, Inc.Rook Pro ResourcesGive UpO HintAssuming complete precipitation, how many moles of each ion remain in solution? If an ion is no longer in solution, enter azero (0) for the number of moles.Lit =molCl- =molmolAg*%3DmolCIO, =%3DQuestion Source: McQuarrie, Rock, And Gallogly 4e - General Chhelpcontact usterms of usecareersprivacy policyabout us) 25%

Answered: Image /qna-images/answer/94b23f86-c64c-4a9b-beda-215df1c9aa05.jpg

If a solution containing 127.23 g of silver chlorate is allowed to react completely with a solution containing 10.77 g of lithium chloride, how many grams of solid precipitate will be formed? solid precipitate: How many grams of the reactant in excess will remain after the reaction? reactant in excess: Assuming complete precipitation, how many moles of each ion remain in solution? If an ion is no longer in solution, enter a zero (0) for the number of moles. mol Lit = | Publisher: University Science Books

If a solution containing 127.23 g of silver chlorate is allowed to react completely with a solution containing 10.77 g of lithium chloride, how many grams of solid precipitate will be formed? solid precipitate: How many grams of the reactant in excess will remain after the reaction? reactant in excess: Assuming complete precipitation, how many moles of each ion remain in solution? If an ion is no longer in solution, enter a zero (0) for the number of moles. mol Lit = | Publisher: University Science Books

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 145QRT: When solutions of silver nitrate and sodium carbonate are mixed, solid silver carbonate is formed...

See similar textbooks

Similar questions

Methanol, CH3OH, is used in racing cars because it is a clean-burning fuel. It can be made by this reaction: CO(g)+2H2(g)CH3OH(l) What is the percentage yield if 5.0103gH2 reacts with excess CO to form 3.5104gCH3OH ?
Many over-the-counter antacid tablets are now formulated using calcium carbonate as die active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting die stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a burp). Write die balanced chemical equation for this process.
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
What is meant by a limiting reactant in a particular reaction? In what way is the reaction “limited”? What does it mean to say that one or more of the reactants are present in excess? What happens to a reaction when the limiting reactant is used up?
Polychlorinated biphenyls (PCBs) have been used extensively as dielectric materials in electrical transformers. Because PCBs have been shown to be potentially harmful, analysis for their presence in the environment has become very important. PCBs are manufactured according to the following generic reaction: C12H10+nCl2C12H10nCln.+nHCl This reaction results in a mixture of PCB products. The mixture is analyzed by decomposing the PCBs and then precipitating the resulting Cl asAgCl. a. Develop a general equation that relates the average value of n to the mass of a given mixture of PCBs and the mass of AgCl produced. b. A 0.1947-g sample of a commercial PCB yielded 0.4791 g of AgCl. What is the average value of n for this sample?
Nickel metal reacts with aqueous silver nitrate in a displacement reaction to produce silver metal and aqueous nickel nitrate. Consider an experiment in which the reaction starts with 12.0 g nickel metal and stops before all the nickel reacts. A total of 24.0 g metal is present when the reaction stops. Calculate how many grams of each I metal are present in the 24.0-g mixture of metals.
4-89 If 7.0 kg of is added to 11.0 kg of to form which reactant is in excess?
When solutions of silver nitrate and sodium carbonate are mixed, solid silver carbonate is formed and sodium nitrate remains in solution. If a solution containing 12.43 g sodium carbonate is mixed with a solution containing 8.37 g silver nitrate, calculate the mass of each of the four substances present after the reaction is complete.
39. Standard solutions of calcium ion used to test for water hardness are prepared by dissolving pure calcium carbonate. CaCO3, in dilute hydrochloric acid. A 1.745-g sample of CaCO3 is placed in a 250.O-mL volumetric flask and dissolved in HCI. Then the solution is diluted to the calibration mark of the volumetric flask. Calculate the resulting molarity of calcium ion.
Barium chloride solutions are used in chemical analysis for the quantitative precipitation of sulfate ion from solution. :math>Ba2+(aq)+SO42(aq)BaSO4(s) ppose a solution is known to contain on the order of 1 50 mg of sulfate ion. What mass of barium chloride should be added to guarantee precipitation of all the sulfate ion?
A 0.20 mol sample of magnesium burns in air to form 0.20 mol of solid MgO. What amount (moles) of oxygen (O2) is required for a complete reaction?