d) x*n e) char Q7: To prepare [Co(NH)SCIJC2, the following procedure was wsed 17 g of CoCl2.6H20 powder was portion-wise added to a solution of 10 gof concentrated aqueous ammonia. To the obtained brown Co slurry, 16 ml S0 wise added. When the effervescence has ceased, add 60 mL conc. HCl slowly than 70 C. Hold the temperature between 55 C and 65 C for 15 min. Add 50 the solution to cool to room temperature. Collect the product by suction filration Calculate the theoretical yield 15.1g 20.0 g 17.9 g 22.4 g 21.1 g

d) x*n e) char Q7: To prepare [Co(NH)SCIJC2, the following procedure was wsed 17 g of CoCl2.6H20 powder was portion-wise added to a solution of 10 gof concentrated aqueous ammonia. To the obtained brown Co slurry, 16 ml S0 wise added. When the effervescence has ceased, add 60 mL conc. HCl slowly than 70 C. Hold the temperature between 55 C and 65 C for 15 min. Add 50 the solution to cool to room temperature. Collect the product by suction filration Calculate the theoretical yield 15.1g 20.0 g 17.9 g 22.4 g 21.1 g

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Give the expression for the solubility product constant for Ca3(PO4)2- Select one: O a. B Ca2+PR PO43-P Ca3(PO4)2 O b. [ Ca2+P[ PO43-P Ca3(PO4)2 O c. R Ca2+P[3 PO43-3 Ca3(PO4)2 O d. [ Ca2+j?[ PO43-73 O e. [Ca2+j³[PO43-12
For Baf, K- 1.0 x 10 What is the molar solubility of BaF in a solution containing 0.10M NaF? O 0.000010M O 0.0063M O 0.000025M O a.00010M Question 18 Calculate the standard Gibbs free energy change at 298K for the reaction FejOun + 4CO 3Fen + 4CO AG; () -1372 Cole) 394.4 1014 O 757 mol 0957 /mal 14/mal O148/mol 2pm
27) Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products): (a) AgI (b) Ag2SO4 (c) Mn(OH)2 (d) Sr(OH)2·8H2O (e) the mineral brucite, Mg(OH)2
Q7) what is the pH at the equivatent point in the titration of 5 mmol Potassium acid ph thalate dissolved in 100 mel of water and titrat ed with 0.1M NaoH 9 K, = 4 +r56 %3D Ans. : 8.46
. 29) The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated: (a) TlCl: [Tl+] = 1.21 ×× 10–2 M, [Cl–] = 1.2 ×× 10–2 M (b) Ce(IO3)4: [Ce4+] = 1.8 ×× 10–4 M, [IO3−][IO3−] = 2.6 ×× 10–13 M (c) Gd2(SO4)3: [Gd3+] = 0.132 M, [SO42−][SO42−] = 0.198 M (d) Ag2SO4: [Ag+] = 2.40 ×× 10–2 M, [SO42−][SO42−] = 2.05 ×× 10–2 M (e) BaSO4: [Ba2+] = 0.500 M, [SO42−][SO42−] = 4.6 ×× 10−8 M
the ksp for the Fe(OH)3 is 4.0x10^-38 10. According to the background information the Group III reagent is to be buffered at pH 10 to procuce a nign enough (OH- to precipitate the Group III ions, but not high enough to precipitate the group IV ions. a. If a solution contained Fe" ions at a concentration of 0.1 M, what pH would have to be reached to precipitate 99% of the Fe" as Fe(OH)s? Hint: Determine (Fe") after precipitation and use it and the Keo to determine (OH b. If a solution contained Ni* ions at a concentration of 0.1 M, what pH would have to be reached to precipitate 99% of the Ni as Ni(OH)2? c. Based on your answers to a. and b., if enough OH- was added to reach a pH of 10, would the Fe3 be selectively precipitated, leaving the Ni2 in solution? Explain? No
9:55 AM | 0.0KB/s Chegg Home Student question Expert Q&A My solutions Skip question Vo LTE 4G Start Solving JA In the determination of chloride by the Mob method, what will be the equiliblium concentration of silver ions in mgil, on the basis of the solubility - product principle, when the chloride concentation has been reduced to 0.2 ma? (b) If the concentration of chromate indicator used is 5X M, how much excess silver ion in mgiL must be present before the formation of a red precipitate will begi(a) In the defermination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in meL., an the basis of the solubility. pcoduct principle, when the chloride concencration has beea reduced to 0.2m? (b) If the concentration of chromate indicator ased is 5 × 10³ M, bow much excess silver ion in mel, must be present before the formatice of a red precipitate will begin? (b) If the concentration of chromate indicator used is 5 x 10-3 M, how much excess silver…
Give ONLY the formula of a compound which will a)dissolve AgCI, but not MgCl2 b)dissolve Pbo , and also Ag,0 c)dissolve Al , but not Mg d) dissolve Zn(OH)2 and Nio but not Ca(OH)2 e)give ppt.with Co(NO:)2 and also with Ba(NO:)2 soln.
Answen the folllowing queotions a. Whats is the dissociation equeation of AgCl b. What is the expression tör the solubitity product [ Ag+³][ci'] con stant for Ag Cl A. Ksp: [Ag+²J[c"] B. Ksp = TAgc1]/[Ag+I][CI"] tAgCl], C.Ksp = CAg+2] [CI] %3D
The formation constant* of [M(CN) 2 ]^ - is 5.30 * 10 ^ 18 , where M is a generic metal. A 0.140 mole quantity of M(NO 3 ) is added to a liter of 0.750 M solution. What is the concentration of mathcal W ^ + at equilibrium?[M^+2]=
At 15 °C, the solubility product of PbCrO4 is 1.69 × 10-14 mol2dm-6. (a) Write an expression for the solubility product of PbCrO4.(b) Calculate the solubility of PbCrO4.(c) On adding concentrated aqueous lead(II) nitrate dropwise to 0.010 moldm-3 potassium chromate (VI), what is the concentration of lead(II) ions when the first trace of precipitate appears?
It is required to know the concentration of an aqueous solution of H2SO4 that appeared in the laboratoryChemistry III and it's unlabeled. To this end, a student of analytical chemistry carried out the followingProcedure: He took 5.00 mL of a fresh and standardized solution of 0.525M NaOH and brought them to a250.0 mL balloon to be completed with distilled water. Subsequently, he poured 15.00 mL of the solutionH2SO4 of unknown concentration in an Erlenmeyer flask and added 2 drops of phenolphthalein.Using a burette filled with the last NaOH solution, he noticed that when adding 39.40 mL of the hydroxidethe Erlenmeyer solution reached a faint but permanent pink. With the above dataDetermine the concentration and pH of the H2SO4 solution.