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- Part B: The Nernst Equation: E Zn ZnlCulCu (Prior to adding NH,OH) – 1.104V 1. 1980 E Zn ZnlCul Cu (After adding NH,OH) [Cu"] (From Nernst equation) inal 2. E Za Zn l cu*l Cu T (K) 270.9니 horl- 3. E° Zn Zn*ICu*l cCu (Prior to adding NaOH) Znl Zn²+ [Zn*]; nitial 0111- E Znl ZnlCuCu E Zn Zn* | Cu²t Cu (After adding NaOH) [Zv**Inmal (From Nernst equation) final 1.22E-38 K„, Zn(OH), (Equation 11) dsThe iodide in a sample that also contained chloride was converted to iodate by treatment with an excess of bromine: 3H,0 + 3Br, +-→ 6Br + 10," + 6H* The unused bromine was removed by boiling; an excess of barium ion was then added to precipitate the iodate: Ba* + 210, - Ba(10,); In the analysis of a 1.59-g sample, 0.0538 g of barium iodate was recovered. Express the results of this analysis as percent potassium iodide.Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. CH;NH2(aq) + HCIO3(aq) > 4- 3. 2+ 3+ 4+ 1 2 6 7 8 O2 4 5. ) (s) (1) (g) (aq) H N H30* CI H20 OH 4- +
- Q2:a) For the reaction: H2(ag) + I2(aq) 5 2Hl(ag) Kc = 54.8 %3D At equilibrium, the concentration of the product; HI was found to be 0.500 M, what's the concentration of Hz? {assume {H2] = X and solve for X}. Show detailed calculationsCalculate the concentration of CO32- in an aqueous solution of 0.257 M carbonic acid, H₂CO3 (aq). [CO32-] = n progress M.Write a balanced chemical equation based on the following description: aqueous potassium phosphate reacts with aqueous nickel(II) bromide to produce solid nickel(II) phosphate and aqueous potassium bromide. 2+ 3+ 4+ 3- 2. 4- 7) 4 6. 8. 9. 1 口6 0. 7 8 9. ロ2 03 4 (s) (1) (g) (aq) Br K Ph Ni Ox • x H2O Delete Reset 2.
- What is the solubility product expression for Sn(1O3)2? Ksp = [Sn2+][103-12 KSP OKsp [Sn+][21O,2-12 Ksp = [Sn2+][21O3-] 4 %3D O Ksp = [Sn4+][Io,2-j2 O Ksp = [Sn2+][2103 ?m/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take OWlw |Online teaching X [Review Topics] [References) Use the References to access important values if needed for this question. The equilibrium constant, K., for the following reaction is 2.90×102 at 1.15×10*K. 2S03(g)2s02(g) + O2(g) If an equilibrium mixture of the three gases in a 1l.0 L container at 1.15×10°K contains 0.265 mol of SOa(g) and 0.352 mol of SO2. the equilibrium concentration of O, is M. Submit Answer Retry Entire Group 8 more group attempts remaining (Previous 9:15 PM 10/14/2020 prt sc delete home end backspace unu4.) Calculate the solubility product constant, Ksp, for lead(II) chromate. Ksp = x 10-13 Hint: enter the decimal before the scientific notation.
- ensider the following equilibrium: Cu2+, *(aq) + 4NH3(ag)=Cu(NH3)42+ (Kf = 4.8e+12) (ag) solution is made by mixing 18.0 mL of 1.50 M Cuso, and 1.00 L of 0.530 M NH3. Assume additive volumes to answer the following questions. Give all answers to three sig figs. Please e Formation Equilibrium Constant for assistance. What is the concentration of NH3 in the resulting solution? [NH3] = What is the concentration of Cu(NH3)42+ in the resulting solution? [Cu(NH3),2+] = M What is the concentration of Cu2+ in the resulting solution? [Cu²+] = | MThe following salts were added to a beaker of distilled water: NaCl (NH2)2CO; Ca(NO;)2 Which of the following products will precipitate out of solution? O NH CI O CaCO, FONTHN O O NaCO;. The solubility-product constant for Ce(IO3)3 is 3.2 X 10-10. What is the Ce³+ concentration in a solution prepared by mixing 50.0 mL of 0.0250 M Ce3+ with 50.00 mL of water? a. 0.040 M I0,? b. 0.250 M IO,? с. 0.150 М IО3?