A student prepared three nickel samples in the lab but forgot to label them. Thesamples that were prepared were [Ni(H₂O)6]2+, [Ni(NH3)612+, and[Ni(H₂NCH₂CH₂NH₂)3]2+. The sample vials were coloured violet, blue, and green.Which sample corresponded to which coloured vial?O[Ni(H₂O)6]2+ = green; [Ni(NH3)6]2+ = blue; [Ni(H₂NCH₂CH₂NH2)3]²+ = violetO[Ni(H₂O)6]2+ = violet; [Ni(NH3)%]2+ = green; [Ni(H,NCH,CH,NH,)3]2+ = blueO[Ni(H2O)%]2+ = violet; [Ni(NH3)%]2+ = blue; [Ni(H,NCH,CH,NH2)3]2+ = greenO[Ni(H2O)%]2+ = green; [Ni(NH3)]2+ = violet; [Ni(H2NCH,CH,NH,)3]2+ = blueO [Ni(H,O),]2+ = blue; [Ni(NH3)%]2+ = green; [Ni(H,NCH,CH,NH2)2+ = violet

Answer: Solutions of different complex ions show different colors due to absorption of lights of…

A student prepared three nickel samples in the lab but forgot to label them. The samples that were prepared were [Ni(H₂O)6]2+, [Ni(NH3)612+, and [Ni(H₂NCH₂CH₂NH2)312+. The sample vials were coloured violet, blue, and green. Which sample corresponded to which coloured vial? O [Ni(H2O)%]2+ = green; [Ni(NH3)%]2+ = blue; [Ni(H2NCH,CH,NH2)3]2+ = violet O [Ni(H2O)%]2+ = violet; [Ni(NH3)%]2+ = green; [Ni(H2NCH,CH,NH2)3]2+ = blue [Ni(H2O)%]2+ = violet; [Ni(NH3)%]2+ = blue; [Ni(H2NCH2CH,NH2)3]2+ = green [Ni(H,O)%]2+ = green; [Ni(NH3)%]2+ = violet; [Ni(H,NCH,CH,NH2)3]2+ = blue O [Ni(H2O)%]2+ = blue; [Ni(NH3)%]2+ = green; [Ni(H,NCH,CH,NH,\3]2+ = violet

A student prepared three nickel samples in the lab but forgot to label them. The samples that were prepared were [Ni(H₂O)6]2+, [Ni(NH3)612+, and [Ni(H₂NCH₂CH₂NH2)312+. The sample vials were coloured violet, blue, and green. Which sample corresponded to which coloured vial? O [Ni(H2O)%]2+ = green; [Ni(NH3)%]2+ = blue; [Ni(H2NCH,CH,NH2)3]2+ = violet O [Ni(H2O)%]2+ = violet; [Ni(NH3)%]2+ = green; [Ni(H2NCH,CH,NH2)3]2+ = blue [Ni(H2O)%]2+ = violet; [Ni(NH3)%]2+ = blue; [Ni(H2NCH2CH,NH2)3]2+ = green [Ni(H,O)%]2+ = green; [Ni(NH3)%]2+ = violet; [Ni(H,NCH,CH,NH2)3]2+ = blue O [Ni(H2O)%]2+ = blue; [Ni(NH3)%]2+ = green; [Ni(H,NCH,CH,NH,\3]2+ = violet

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

Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 7.750 mL V2, volume of standard NaOH required for second equivalence point : 19.70 mL Calculate the mass of iron in the sample :
bot 3. Iron(II) ion (Fe°*) reacts with thiocyanate ion (SCN¯) to form a red complex ion with the formula [FESCN]2+. The net ionic equation describing this reaction is given in Equation 10. eH MC () Fe+ (aq, It. yellow) + SCN (aq, colorless)=[FESCN]²+ (aq, red) 12+ (Eq. 10) A student studying this equilibrium begins with an equilibrium mixture that is light pink. (1) What change will the student observe when a solution containing Fe³+ ion is added to this mixture?
Although KOH, R6OH, and CSOH have little association between metal and hydroxide in aqueous solution, Lit and Na+ do form complexes with OH : [LIOH(aq)] Lit + OH- = LIOH(aq) K1 [Li* ][OH¯] = 0.83 [NAOH(aq)] Na+ + OH = NaOH(aq) K1 = [Na+ ][OH ] = 0.20 Prepare a table showing initial and final concentrations of Lit, OH, and LIOH(aq) in 1.00 F LIOH solution. Calculate the fraction of lithium in the form LİOH(aq) at equilibrium. fraction as LIOH(aq):
Nitrogen of ammonia can be determined by treatment of the sample with chloroplatinic acid; the product is slightly soluble ammonium chloroplatinate: H₂PtCl 6 + 2NH4+ → (NH4)2PtCl6 + 2H+ The precipitate decomposes on ignition, yielding metallic platinum and gaseous products: (NH4)2PtCl6 3 → Pt(s) + 2Cl₂(g) + 2NH3(g)↑ + 2HCl(g)↑ Calculate the percentage of ammonia in a sample if 0.2115 g of the impure sample gave rise to 0.4693 g of platinum. Given: M(NH3) = 17.0306 g/mol; M(Pt) = 195.08 g/mol. O O b. 14.25% O O d. 82.38% a. 56.52% c. 38.74%
10) Ce³+ exhibits pH dependent solubility. If Ce(NO3)3 is dissolved in an acidic solution to a concentration of 0.025 M, at what pH has 95% of the cerium been removed as the insoluble hydroxide salt? Ce(OH)3 pKsp=21.2
In the following chemical reaction what is the concentrations of [H3O+] in a solution that is 0.00045 M [Al(H2O)6]3+. Assume that the [Al(H2O)6]3+ dissociates 100% completely and assume 1 Liter of solution. [Al(H2O)6]3+ + 3H2O ↔ [Al(H2O)3(OH)3]2+ + 3H3O+
Mass of KxFe(C2O4)y · zH2O : 5.60 g Mass of sample : 0.155 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 9.000 mL V2, volume of standard NaOH required for second equivalence point : 15.90 mL Calculate the percent of potassium in the sample :
Given the reaction: 2X + Cr2O3 → X2O3 + 2Cr Which of the following could be X? A Al B Ni C Sn D Pb
How many unpaired electrons are there in the high-spin state of Co2+ in an tetrahedral field?
Mass of KxFe(C2O4)y · zH2O : 5.60 g Mass of sample : 0.155 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 9.000 mL V2, volume of standard NaOH required for second equivalence point : 15.90 mL Calculate the mass of potassium in the sample :
Consider the equilibrium reaction below. [Cu(H₂O)6]²+ (aq) + 4 Cl (aq) light blue [CuCl4]² (aq) + 6 H₂O (1) orange A test tube contains a solution of Cu(NO3)2 which is light blue. What is the major species present in the solution responsible for the color?
[Co(H2O)6]2+ (aq) + 4 Cl-(aq )⇆ [CoCl4]2-(aq) + 6 H2O Explain why the addition of water changes the equilibrium position even though the concentration of water is essentially constant and normally not included in the equilibrium constant expression. What are two functions that water performs in this reaction?