Question in image belowplease show all needed steps and solution Agl (silver iodide, Kep " 8.51 x 1017) is a low solubility/insoluble salt. Ag(CN)2 has a formation constant (K¢) - 1.0 x 1021.a. Would a solution prepared from 1.0 x 10 M AGN03 and 2.0 x 105 M Nal form a precipitate or stay in solution? A complete answer willinclude the calculation of Q and its comparison to Ksp-b. Show the complete equation for the formation of Ag(CN)2- from the addition of KCN and Agl. (you may leave out the K* cation in yourequations if you choose)c. What is the equilibrium constant K for the formation of Ag(CN)2-from Agl and KCN?

a) Reaction of AgNO3 and NaI is as follows: AgNO3 + NaI →AgI + NaNO3 As per the reaction 1 mole…

Agl (silver iodide, Ksp " 8.51 x 1017, is a low solubility/insoluble salt. Ag(CN)2 has a formation constant (Ke) - 1.0 x 1021. a. Would a solution prepared from 1.0 x 10 M AGNO3 and 2.0 x 10 M Nal form a precipitate or stay in solution? A complete answer will indude the calculation of Q and its comparison to Ksp- b. Show the complete equation for the formation of Ag(CN)2-from the addition of KCN and Agi. (you may leave out the K* cation in your equations if you choose) c. What is the equilibrium constant K for the formation of Ag(CN-from Agi and KCN?

Agl (silver iodide, Ksp " 8.51 x 1017, is a low solubility/insoluble salt. Ag(CN)2 has a formation constant (Ke) - 1.0 x 1021. a. Would a solution prepared from 1.0 x 10 M AGNO3 and 2.0 x 10 M Nal form a precipitate or stay in solution? A complete answer will indude the calculation of Q and its comparison to Ksp- b. Show the complete equation for the formation of Ag(CN)2-from the addition of KCN and Agi. (you may leave out the K* cation in your equations if you choose) c. What is the equilibrium constant K for the formation of Ag(CN-from Agi and KCN?

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter16: Solutions

Section: Chapter Questions

Problem 37E

See similar textbooks

Similar questions

A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. a. Write a balanced chemical equation for any reaction that occurs. b. What precipitate forms? c. What mass of precipitate is produced? d. Calculate the concentration of each ion remaining in solution after precipitation is complete.
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?
Consider a 1.50-g mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture in water, 0.500 M silver nitrate is added dropwise until precipitate formation is complete. The mass of the white precipitate formed is 0.641 g. a. Calculate the mass percent of magnesium chloride in the mixture. b. Determine the minimum volume of silver nitrate that must have been added to ensure complete formation of the precipitate.
Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is added to 50.0 mL of 2.45 M barium chloride. (a) What is the expected precipitate? (b) How many grams of precipitate are obtained? (c) What is the chloride concentration after precipitation is complete?
Relative solubilities of salts in liquid ammonia can differsignificantly from those in water. Thus, silver bromide issoluble in ammonia, but barium bromide is not (thereverse of the situation in water). Write a balanced equation for the reaction of anammonia solution of barium nitrate with an ammoniasolution of silver bromide. Silver nitrate is soluble inliquid ammonia. What volume of a 0.50 M solution of silver bromidewill react completely with 0.215 L of a 0.076 M solutionof barium nitrate in ammonia? What mass of barium bromide will precipitate fromthe reaction in part (b)?
A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.400 M HCl. The solution was then treated with an excess of aqueous chromium(III) nitrate, resulting in formation of 2.06 g of precipitate. Determine the concentration of the NaOH solution.
68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.
42. a. Fill in the following table as if it is a well plate and you are mixing two aqueous compounds at a time to see if a precipitate forms. If a precipitate is expected to form, indicate that by writing the correct formula for the precipitate in the corresponding box in the table. If no precipitate is expected to form, write “NO” in the box. CaCI2 Pb(NO3)2 (NH4)3PO4 Na2CO3 AgNO3 K2SO4 b. How do you prepare 300.0 mL of a 0.250 M CaCl2 solution using an available 2(X) M solution? Support your answer with calculations, but also make sure you describe how to prepare the solution.
A 50.00-mL sample of 0.0250 M silver nitrate is mixed with 0.0400 M chromium(III) chloride. (a) What is the minimum volume of chromium(III) chloride required to completely precipitate silver chloride? (b) How many grams of silver chloride are produced from (a)?
One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and then to titrate the remaining NaOH. The reaction of aspirin with NaOH is as follows: A sample of aspirin with a mass of 1.427 g was boiled in 50.00 mL of 0.500 M NaOH. After the solution was cooled, it took 31.92 mL of 0.289 M HCl to titrate the excess NaOH. Calculate the purity of the aspirin. What indicator should be used for this titration? Why?