NaOH (0.5 M) Start with 0.5 mL of [Co(OH,),]* (aq) + 2C1 (aq) Product 3 [Co(OH,)6]Cl, (0.1 M) NAOH | iconc.) Product 7 ermine the identities of Products 3 and 7. Huct 3: [Co(OH)2] luct 7 [Co(OH)2(OH2)4] [Co(OH2)4(OH)2] [Co(OH)2] [Co(OH2)6]2+ t is tl [Co(OH2)]2+ ?
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- Consider the following equilibrium: Cu²+ (aq) + 4NH3(aq) Cu(NH3)4²+ (aq) (Kf = 4.8e+12) A solution is made by mixing 15.0 mL of 0.90 M CuSO4 and 1.00 L of 0.530 M NH3. Assume additive volumes to answer the following questions. Give all answers to three sig figs. a) What is the concentration of NH3 in the resulting solution? [NH3] = M b) What is the concentration of Cu(NH3)42+ in the resulting solution? [Cu(NH3)4²+] = M c) What is the concentration of Cu²+ in the resulting solution? [Cu²+] = MYou dissolve 0.191 g of NaOH in 2.00 L of a buffer solution that has [H2PO,] = HPO, = 0.138 M. What is the pH of the solution before adding NaOH? ( %3D %3D K, for dihydrogen phosphate ion is 6.2 x 10-8.) pH %3D What is the pH of the solution after adding NaOH? pH %3D4R) Aqueous solutions of a compound did not form precipitates with Cl-, Br, I-, SO42-, CO32-, PO43-, OH", or S2-. This highly water-soluble compound produced the foul-smelling gas H2S when the solution was acidified. This compound is A) Pb(NO3)2 B) (NH4)2S С) KBr D) L12CO3 E) AgNO3 Answer: B
- HA, a weak acid, also forms the ion HA, in solution. The reaction is HA(aq) + A¯(aq) = HA, (aq) The weak acid has Ka 5.51 x 10- and the reaction has K = 2.93. Calculate the concentrations of A¯, H*, and HA, in a 1.00 M solution of HA. [A¯] = M [H*] = M [HA,] = М * TOOLSIf 316.0 mg of AgBr is completely dissolved in 144.0 mL of 0.12 M NH3, what is the equilibrium concentration of Ag+(aq) in the final solution? Kf[Ag(NH3)2+] = 1.7E7Include at least 3 significant figures in your answerWhat are the concentrations of all the species (H*, HCO;", and CO3? ) in a 0.025 M H2CO3 solution? [H* ][HCO,] K, [H,CO,] = 4.2x10-7 H,CO, (aq) z H*(aq)+HCO;(aq) [H*][Co ] K, [HCO;] 4.8x 10-11 HCO; (aq) H*(aq)+ CO3-(aq) 2H,0 2 H,O*(aq)+OH¯(aq) K, = [H* ][OH¯] =1.00× 10-14 %3D 2.
- In Questions 1 through 6, you will be calculating the initial concentrations of Fe³+ ([Fe³+]0) and SCN ([SCN]0) for each of the reactions you will perform. You should transfer the answers to these questions to the appropriate ICE table(s) on the "Data and Calculations" sheet. In all five reactions, you will be using 5.0 mL of 0.0020 M Fe(NO3)3. Each reaction mixture will be diluted to a final volume of 10.0 mL. What is [Fe³+] in all five of the reactions you will study? Type your answer, WITHOUT UNITS, in the box below. Include 2 significant figures. If you want to enter your answers in scientific notation, use the format that Blackboard recognizes: 1.5 x 10-3 would be entered as 1.5E-3 (no spaces). QUESTION 2 In Test Tube 1, you will be using 1.0 mL of 0.0020 M KSCN. Each reaction mixture will be diluted to a final volume of 10.0 mL. What is [SCN ]o in Test Tube 1? Type your answer, WITHOUT UNITS, in the box below. Include 2 significant figures. QUESTION 3 In Test Tube 2, you will be…Consider the following equilibrium: Cu²+ (aq) + 4NH3(aq) Cu(NH3)4²+₁ (aq) (Kf = 4.8e+12) A solution is made by mixing 15.0 mL of 0.90 M CuSO4 and 1.00 L of 0.530 M NH3. Assume additive volumes to answer the following questions. Give all answers to three sig figs. a) What is the concentration of NH3 in the resulting solution? [NH3] = .47 M b) What is the concentration of Cu(NH3)42+ in the resulting solution? [Cu(NH3)4²+] = 5.3e-2 X M c) What is the concentration of Cu²+ in the resulting solution? [Cu²+] = 5.3e-2 X M1. Calculate the concentration of ions in the following saturated solutions: (a) [1'] in Agl solution with [Ag'] = 9.1 x 10° M; Ksp= 8.3 x 107 (b) [A*] in Al(OH); solution with [OH] = 2.9 x 10° M; Ksp = 1.8 x 10 33 2. 2.4414 g sample containing KCI, K;SO4 and inert materials was dissolved in sufficient water to give 250 mL of solution. A Mohr titration of a 50 ml aliquot required 41.36 ml of 0.05818 M AGNO3. A second 50mL aliquot was treated with 40 ml of 0.1083M NaB(CsHs)4. The reaction is NaB(CsHs)a + + KB(CsHs)4s) + Na*. The solid was filtered, redissolved in acetone, and titrated with K* 49.98mL of the AgNO: solution according to the reaction KB(C,H;). + Ag* + AgB(CsHs)46) + K*. Calculate the percentage of KCl and K:SO, in the sample. a. As a food chemist for a major potato chip company, you are responsible for determining the salt content of new potato chip products for the packaging label. The potato chips are seasoned with table salt, NaCl. You weigh out a handful of the chips…
- and the con 2. Given the following two reactions and their equilibrium constants: Cu(H,O),*(aq) + 4 NH3(aq) =Cu(NH3),²*(aq) + 4 H,O(1) K¡ = 5 × 102 Cu(H2O),?*(aq) + CO,²-=CUCO;(s) + 4 H,O(I) K, = 7 × 10° Evaluate the equilibrium constant for the reaction (see discussion): Cu(NH3),*(aq) + CO,²-(aq)= CUCO;(s) + 4 NH;(aq) b. When 1 M concentrations of all dissolved species are present, which is more stable, CuCO3 or Cu(NH,),*? Explain your reasoning. custom pageA solution has a concentration of 1.0 x 105M of both Fe2* and Co3, If strong base (OH') is slowly added to this solution, what will precipitate first? Fe(OH)2 (Ksp = 8.0 x 10 -16 ) or Co(0H)3 (Ksp = 1.6 x 10 44) O a. neither will ever precipitate O b. Co(OH)3 O c. they will precipitate at the same time O d. Fe(OH)2Suppose you have a solution that might contain any or allof the following cations: Ni2+, Ag+, Sr2+, and Mn2+. Additionof HCl solution causes a precipitate to form. After filteringoff the precipitate, H2SO4 solution is added to the resultingsolution and another precipitate forms. This is filtered off,and a solution of NaOH is added to the resulting solution.No precipitate is observed. Which ions are present in each ofthe precipitates? Which of the four ions listed above must beabsent from the original solution?