Answered: How many moles of precipitate will be…

How many moles of precipitate will be formed when 30.0 mL of 0.450 M AgNO3 is reacted with excess MgCl2 in the following chemical reaction? 2 AGNO:(aq) + M9CI2(aq) → 2 AgCl(s) + Mg(NO:):(aq)

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 121AP: Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion...

See similar textbooks

Related questions

Q: An unknown base, M(OH), reacts with HCl in the following reaction: M(OH), (aq) + 21HCI (aq) => MCl,…

A: Given : M(OH)2(aq) + 2HCl(aq) → MCl2(aq) + 2H2O(l) Mass of M(OH)2 = 2.251 g Molarity of HCl…

Q: What mass of precipitate (in g) is formed when 72.8 mL of 0.500 M FeCl₃ reacts with excess AgNO₃ in…

A: From the reaction it is clear that 1 mole FeCl3 reacts with 3 moles AgNO3 to give 3 moles AgCl.…

Q: How many grams of AgCI will be formed when 60 mL of 0.500M AGNO, is completely reacted according to…

A: The balanced reaction taking place is given as, Given : Concentration of AgNO3 = 0.500 M And volume…

Q: A 18.2 ml sample of vinegar (dilute acetic acid, CH3COOH) is titrated and found to react with 91.2…

Q: An antacid tablet contains Aluminum hydroxide and an inert binding agent. The mass of the Aluminum…

A: In the chemical reaction, the number of equivalents of acid and base are equal. The number of…

Q: How many grams of precipitate are formed when 85 mL of 0.50 M FeCl, reacts with excess AGNO, in the…

Q: Consider the following chemical reaction: HBr(aq) + NaOH(aq) → H2O(l) + NaBr(aq) 25.00 mL of an…

A: Given that, Volume of HBr = 25.00 mL Volume of NaOH = 28.45 mL Molarity of NaOH = 0.1500 M The given…

Q: In the following acid-base neutralization, 1.68 g of the solid acid HC6H5O (94.12 g/mol) neutralized…

A: Moles of acid = mass / molar mass = 1.68 / 94.12 = 0.01785 approx Since from the reaction, 1 mole of…

Q: When 25.0 mL of sulfuric acid solution was completely neutralized in a titration with 0.050 M NaOH…

A: The balanced chemical reaction taking place between H2SO4 and NaOH is as follows:

Q: What mass of precipitate (in g) is formed when 85.7 mL of 0.500 M FeCl₃ reacts with excess AgNO₃ in…

A: Given precipitation reaction; FeCl3 (aq) + 3 AgNO₃(aq) → 3 AgCl(s) + Fe(NO₃)₃(aq) Given volume of…

Q: what is the molar concentration of acetic acid in the vinegar?

Q: How many grams of AgCI will be formed when 60 ml of 0.500 MAGNO: is completely reacted according to…

A: Given, 60mL of 0.500M AgNO3

Q: In the following acid-base neutralization, 1.68 g of the solid acid HC6H5O (94.12 g/mol) neutralized…

Q: What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503…

A: Given: Volume of NaCl V1= 15.00mL Volume of AgNO3 V2=20.22mL Molarity of AgNO3 M2= 0.2503M To find:…

Q: What mass of precipitate (in g) is formed when 87.2 mL of 0.500 M FeCla reacts with excess AGNO3 in…

Q: What quantity in moles of precipitate will be formed when 77.1 mL of 0.150 M AgNO3 is reacted with…

Q: AgNO₃(aq) → 3 AgCl(s) + Fe(NO₃)₃(aq)

A: This can be solved by balancing the equation.required solution is given below

Q: 2) Hydrogen peroxide (H2O2) reacts with the permanganate ion (MnO4) in acidic solution according to…

A: a.

Q: When 30.5 mL of sulfuric acid solution was completely neutralized in a titration with 0.593 M NaOH…

Q: A precipitation reaction occurs when 655 mL of 0.639 M Pb(NO2), reacts with 313 mL of 0.855 M KI, as…

A: The given volume and molarity of Pb(NO3)2 is 655 mL and 0.639 M.The given volume and molarity of KI…

Q: the following acid-base neutralization, 1.68 g of the solid acid HC6H5O (94.12 g/mol) neutralized…

A: Moles of acid = mass / molar mass = 1.68 / 94.12 = 0.01785 approx Since from the reaction, 1 mole of…

Q: 4. What volume of 0.1000 mol/L. NaOH(aq) is needed to react completely with 20 mL of 0.1805 mol/L…

Q: How many moles of precipitate will be formed when 69.3 mL of 0.300 M AgNO₃ is reacted with excess…

A: Given, 69.3 mL of 0.300 M AgNO₃

Q: When 80.5 mL of 0.642 M Ba(NO3)2 are mixed with 44.5 mL of 0.743 M KOH, a precipitate of Ba(OH)2…

A: Molarity: Molarity is defined as the number of moles of solute per litre of solution. It is given…

Q: mass of 0.284 g. The limiting reactant in the salt mixture was later determined to be CaCl2·2H2O.…

A: since you have posted a question with multiple subparts we are entitiled to answer only first 3…

Q: How many grams of AgCI will be formed when 60 ml. of 0.500 MAGNO, is completely reacted according to…

A: Given: Volume of AgNO3= 60 mL = 60×10-3 L Concentration of AgNO3 = 0.500 M Molar mass of AgCl =…

Q: How many grams of AgCI will be formed when 60 mL of 0.500M AGNO: is completely reacted according to…

A: Given: Volume of AgNO3 = 60 mL Concentration of AgNO3 = 0.500 M molar mass of AgCl = 143.32 g/mol

Q: The acid H2A reacts with the base M(OH)3 in the following ratio: 3H2A + 2M(OH)3 → products. What…

A: Given data,Volume of H2A=0.852LMolarity of M(OH)3=0.500MVolume of M(OH)3=0.197L

Q: How many grams of AgC will be formed when 60 mL of 0.500 MAGNO, is completely reacted according to…

A: The number of moles of AgNO3 is calculated as shown below. The number of moles of AgNO3 is 0.03 mol.

Q: 3. With 85 % H2SO, by volume in water being used in the reaction, how many moles of water will be…

A: Since you have asked multiple questions, we will solve one question for you. If you want any…

Q: How many grams of precipitate are formed when 85 mL of 0.50 M FeCl, reacts with excess AGNO, in the…

A: Given, 85mL of 0.50M FeCl3

Q: How many grams of AgCl will be formed when 60 mL of 0.500M AGNO, is completely reacted according to…

A: It is given that 60mL of 0.500 M AgNO3 is reacting completely (limiting reagent) to form AgCl and…

Q: Solutions of magnesium sulfate and potassium phosphate react to form a precipitate. What volume, in…

Q: What mass of precipitate (in g) is formed when 80.0 mL of 0.500 M AlCl₃ reacts with excess AgNO₃ in…

Q: Suppose you are titrating vinegar, which is an acetic acid solution of unknown concentration, with a…

Q: A 5.00 g sample of vinegar (contains acetic acid) is titrated (reacted) with 0.108 M NaOh. If the…

A: Mass percent is the proportion of mass of a solute of a substance which is divided by the whole mass…

Q: A cup of coffee may contain 300. mg of caffeine (C 8H10N4O2).Calculate the molarity (M) of caffeine…

A: Molar Mass of caffeine (C 8H10N4O2) =194 g Mass of caffeine given =300 mg= 0.3 g Mole = Mass Given/…

Q: If 50.0 mL of NaOHNaOH solution is required to react completely with 0.44 gg KHPKHP, what is…

A: Given :- Volume of NaOH = 50.0 mL Mass of KHP = 0.44 g To calculate :- Molarity of NaOH solution

Q: The amount of chloride anion in a solution can be determined via titration with AgNO3(aq), according…

A: The reaction given is Cl–(aq) + AgNO3(aq) → AgCl(s) + NO3–(aq)

Q: What mass of precipitate (in g) is formed when 80.0 mL of 0.50 M AlCl₃ reacts with excess AgNO₃ in…

A: The balanced reaction taking place is given as, => AlCl₃ (aq) + 3 AgNO₃ (aq) → 3 AgCl (s) +…

Q: Liquid pentanal reacts with potassium permanganate solution in sulfuric acid to produce pentanoic…

A: Given data,Volume of pentanal=2.634mLDensity of pentanal=0.811g/mLVolume of KMnO4=26.43mL

Q: What mass of precipitate (in g) is formed when 61.2 mL of 0.500 M AlBr₃ reacts with excess AgNO₃ in…

Q: Vinegar Vinegar is a dilute solution of acetic acid, often represented by the symbol "HAc" in…

Q: A 1.280 g sample of oxalic acid, H2C2O4, is placed in a 100.0-mL volumetric flask, which is then…

Q: How many grams of AgCI will be formed when 60 mL of 0.500M AGNO, is completely reacted according to…

Q: Vinegar contains (among other things) acetic acid. What is the molarity of acetic acid (HC2H3O2) in…

A: Solution stoichiometry involves the calculation of concentration of solutions in the given…

Q: Aspirin, acetylsalicylic acid, C9H8O4, reacts with basic substances. If the titration of an aspirin…

Q: 3) A solution of silver nitrate (AgNO3) and then prepared by dissolving 1.26 g of salt in a…

A: Given: Mass of AgNO3 = 1.26 g Volume of solution = 250 mL Molar mass of AgNO3 = 169.9 g/mol

Q: An antacid tablet contains Magnesium hydroxide and an inert binding agent. The mass of the Magnesium…

A: As per the mole concept, the amount of substance in moles is equal to the ratio of its mass to the…

Question

How many moles of precipitate will be formed
when 30.0 mL of 0.450 M AgNO3 is reacted with
excess MgCl2 in the following chemical reaction?
2 AGNO:(aq) + M9CI2(aq) → 2 AgCl(s) +
Mg(NO:):(aq)

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

Glycerol (C3H8O3) is commonly used as an additive to moisturizers. The amount of glycerol added can be determined by titration with permanganate in basic solution. 14MnO4(aq)+C3H8O3(aq)+20OH(aq)14MnO42(aq)+3CO32(aq)+14H2O How many milliliters of 6.15 M KMnO4 are required to completely react with 7.25 mL of an aqueous solution of glycerol (d=1.144g/mL) that is 51.6% by mass?
A student tries to determine experimentally the molar mass of aspirin (HAsp). She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is HAsp(aq)+OH(aq)Asp(aq)+H2OWhat is the molar mass of aspirin?
Gold metal will dissolve only in aqua regia, a mixture of concentrated hydrochloric acid and concentrated nitric acid in a 3:1 volume ratio. The products of the reaction between gold and the concentrated acids are AuCl4-(aq), NO(g), and H2O. The equation for this reaction where HNO3 and HCl are strong acids is Au(s)+4Cl(aq)+4H+(aq)+NO3(aq)AuCl4(aq)+NO(g)+2H2O(a) What stoichiometric ratio of hydrochloric acid to nitric acid should be used? (b) What volumes of 12 M HCl and 16 M are HNO3 required to furnish the Cl- and NO3- ions to react with 25.0 g of gold?
Bone was dissolved in hydrochloric acid, giving 50.0 mL of solution containing calcium chloride, CaCL2. To precipitate the calcium ion from the resulting solution, an excess of potassium oxalate was added. The precipitate of calcium oxalate, CaC2O4, weighed 1.437 g. What was the molarity of CaCl2 in the solution?
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?
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?
The substance KSCN is frequently used to test for iron in solution, because a distinctive red color forms when it is added to a solution of the Fe3+ cation. As a laboratory assistant, you are supposed to prepare 1.00 L of a 0.200 M KSCN solution. What mass, in grams, of KSCN do you need?
You are given a solid mixture of NaNO2 and NaCl and are asked to analyze it for the amount of NaNO2 present. To do so, you allow the mixture to react with sulfamic acid, HSO3NH2, in water according to the equation NaNO2(aq) + HSO3NH2(aq) NaHSO4(aq) + H2O() + N2(g) What is the weight percentage of NaNO2 in 1.232 g of the solid mixture if reaction with sulfa-mic acid produces 295 mL of dry N2 gas with a pressure of 713 mm Hg at 21.0 C?
The molarity of iodine in solution can be determined by titration with arsenious acid, H3AsO4. The unbalanced equation for the reaction is H3AsO3(aq)+I2(aq)+H2O2 I(aq)+H3AsO4(aq)+2 H+(aq)A 243-mL solution of aqueous iodine is prepared by dissolving iodine crystals in water. A fifty-mL portion of the solution requires 15.42 mL of 0.134 M H3AsO3 for complete reaction. What is the molarity of the solution? How many grams of iodine were added to the solution?
Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
An unknown monoprotic acid reacts with NaOH according to the net ionic equation HA(aq) + OH(aq) A(aq) + H2O(l) Calculate the molar mass of HA if 0.856 g of the acid requires 30.08 mL of 0.323 M NaOH.
A 10.00-mL sample of a 24.00% solution of ammonium bromide (NH4Br) requires 23.41 mL of 1.200 molar silver nitrate (AgNO3) to react with all of the bromide ion present. (a) Calculate the molarity of the ammonium bromide solution. (b) Use the molarity of the solution to find the mass of ammonium bromide in 1.000 L of this solution. (c) From the percentage concentration and the answer to part b, find the mass of 1.000 L ammonium bromide solution. (d) Combine the answer to part c with the volume of 1.000 L to express the density of the ammonium bromide solution (in g/mL).

SEE MORE QUESTIONS

Recommended textbooks for you

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS