Use the reaction below to answer the following: CoCl2(aq) + AgNO3(aq) --> AgCl(__) + Co(NO3)2(__) A. What are the coefficients to balance this equation? B. If AgCl forms a white precipitate and compounds containing nitrate ions are always soluble in water, what are the subscripts missing from the equation above? C. What drives the reaction to occur? D. Write the net-ionic equation for this reaction? E. What are the spectator ions for this reaction? (Formula and charge)

Use the reaction below to answer the following: CoCl2(aq) + AgNO3(aq) --> AgCl() + Co(NO3)2() A. What are the coefficients to balance this equation? B. If AgCl forms a white precipitate and compounds containing nitrate ions are always soluble in water, what are the subscripts missing from the equation above? C. What drives the reaction to occur? D. Write the net-ionic equation for this reaction? E. What are the spectator ions for this reaction? (Formula and charge)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.25QAP

See similar textbooks

Similar questions

What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO3 is added to 20.0 mL of 1.00 M NaBr?
From the solution in Products 2, it was filtered and heated further until it was dried. This produced a precipitate with 0.3592 g. Calculate the molecular weight of the unknown metal cation. _______ g/mol (Hint: Is the precipitate in the second reaction a pure metal?) What is the identity of the metal in the unknown solution?
Suppose 234.3 mg of PbCl2 was added to 16.0 mL of water in a flask, and the solution was allowed to reach equilibrium at 21.0 oC. Some solute remained at the bottom of the flask after equilibrium, and the solution was filtered to collect the remaining PbCl2, which had a mass of 91.6 mg . What is the solubility of PbCl2 (in g/L)? -Express the concentration in grams per liter to three significant figures.
a. Balance the following redox in acidic media C2O42- (aq) + MnO4- (aq) → CO2(aq) + Mn2+ (aq) b. If you titrated this reaction to determine the moles of C2O42-, the colormetric endpoint is pink due to the Mn2+. How many moles of the oxalate (C2O42-) existed in solution if 12 mL of 0.791M permanganate was needed to hit the endpoint?
Shana, a student in the Analytical Chemistry class, performed a Redox Titration to determine the content of hypochlorite ions (% w/w) in an unknown solution. First, Shana prepared a primary standard solution of KIO3 by dissolving 0.4791 g dry KIO3 in 250.00 mL DI water. Next, using the procedure in your lab manual, Shana used 50.00 mL of this primary standard solution to standardize the Na2S2O3 titrant, and 26.25 mL of titrant was consumed. Next, Shana prepared the unknown solution by diluting 12.8624 g of the solution in 250.00 mL of DI water. A 50.00 mL portion of this dilute unknown solution was titrated using the procedure in your lab manual, and 19.25 mL of Na2S2O3 solution was consumed. Answer the following questions about this titration. Recall the stoichiometry of the NET chemical equation for this reaction. Note: use appropriate significant figures in your answer! A. Calculate the concentration (M) of Na2S2O3 titrant. B. Determine the amount (g) of hypochlorite ion in 50.00 mL…
Give the formula of the compound which will give a precipitate with BaCl2 but NOT with (NH4) 2CO3? SOLUBILITY RULES Solubilities of ionic substances in water: 1) All salts of Na+, K+, NH4+ are soluble in water. 2) All salts of NO3-, CH3COO- are soluble in water. 3) All salts of Cl-, Br-, I- are soluble in water (except Ag+, Pb2+, Hg22+ ) 4) All salts of SO42- are soluble in water ( except Ba2+, Pb2+, Sr2+) SO42- of Ca2+, Ag+, Hg22+ are slightly soluble in water. 5) All salts of CO32-, PO43- are insoluble in water (except Na+, K+, NH4+) 6) All salts of S2- are insoluble in water ( except Na+, K+, NH4+, Ba2+,Ca2+, Mg2+, Sr2+) 7) All salts of O2-, OH- are insoluble in water ( except Na+, K+, NH4+, (Ba2+)) OH- of Ca2+, Sr2+, (Ba2+) are slightly soluble in water OH- of Mg2+ is very very slightly soluble in water a. AgNO3 b. Zn (NO3) 2 c. KCl d. Na2 SO4
In a titration of HNO₃, you add a few drops of phenol-phthalein indicator to 50.00 mL of acid in a flask. You quickly add 20.00 mL of 0.0502 M NaOH but overshoot the end point,and the solution turns deep pink. Instead of starting over, youadd 30.00 mL of the acid, and the solution turns colorless. Then,it takes 3.22 mL of the NaOH to reach the end point. (a) What isthe concentration of the HNO₃ solution? (b) How many moles of NaOH were in excess after the first addition?
Ca2+ in a drinking water sample was analyzed by the following reactions below: Ca2+(aq) + C2O42-(aq) → CaC2O4 (s) → CaO(s) + CO(g)+ CO2(g) First an excess of C2O42- was added to 0.10 L of the Ca2+ water sample. Then CaC2O4 was precipitated, which was demcomposed into CaO with filtering and some heat. The CaO was measured to be 5.61 mg. What is the concentration of Ca2+ in the original water sample? The MW of CaO is 56.1 g/mol. 0.0100M 0.0010 M 1.00 M 0.100 M The partition coefficient (K) of methylamine (CH3NH2) is 4.50, preferring the organic layer over the aqueous layer in this extraction. The Ka of methylammonium (CH3NH3+) is 2.00 x 10-11. If 10 mL aqueous methylamine solution at pH 11.0 is extracted with 20.0 mL organic solvent, what is the fraction of solute remaining in the water (q)? HINT: methylamine is a weak base. 14.3% 10.0% 18.2% 81.8%
A precipitate of AgCl + AgBr weighs 0.8132 g. On heating on a current of Cl2, the AgBr is converted to AgCl, the mixture loses 0.1450 g in wt. Find the percentage Cl in the original sample.
I add 0.1011 g of a primary standard FAS into a volumetric flask and diluted it to the line with water. We then add 2 mL of that solution into another 100 mL volumetric flask and diluted to the line with water. What would be the concentration of the diluted solution in g/mL?
75.0 mL of 0.15 M aqueous carbonic acid is mixed with 145.0 mL of 0.25 M aqueous lithium hydroxide. What is the concentration of all ions in solution after the reaction has gone to completion?
I need help calculating the solubility. thank you C. Calcium Fluoride, CaF2 (aka, Fluorite), in a solution containing 19 mg/L of LiF (aka, Griceite),with all of the LiF being dissolved into solution. Please assume that LiF dissolves such that [Li] =[F] = 7.33 x 10-4 m. After adding CaF2 to the solution and allowing it to dissolve, what are finalvalues of [Ca], [Li] and [F]?Note: you are given the concentrations of [Li] and [F] that result from dissolving LiF. Nosolubility calculation is required for dissolving LiF; just use the concentration given above.Steps:- First, write the stoichiometric equation for dissolution of CaF2 , with the solidon the left and the two ions in solution on the right, separated by a "two-way" arrow. Hint: whenCaF2 dissolves, you get 2 moles of F for every 1 mole of Ca.- Second, set up a law of mass action equation for dissolution of CaF2. There is a common ioneffect for F, so if [Ca] = x, then [F]= 2x + [FLiF], where [FLiF] is from dissolution of the…