Calculate B₂ for Ag(CN)₂ if the following cell develops a potential of +0.600 V. The pK₂ of HCN is 9.21. Ag(s)IKAg(CN)₂ (7.50× 10-³ M), NaCN(0.100 M, buffer pH 9.21) || S.C.E.
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- A 50.00 mL of 0.100 M Fe(II) is to be analyzed by redox titration with suitable reagents For the redox titration of 50.00 mL of 0.100 M Fe(II) with 0.100 M Ce(IV) in1 M H2SO4, (i) What is the reaction involved? (ii) Explain how the potential at the equivalence point can be determined.Calculate the potential at the equivalence point as measured by a platinumindicator electrode against a standard hydrogen electrode.- (a) Suppose you wanted to make a buffer of exactly pH 7.00 using KH,PO, and Na,HPO,. If the final solution was 0.1 M in KH,PO,, what concentration of Na,HPO, would you need? (b) Now assume you wish to make a buffer at the same pH, using the same substances, but want the total phosphate molarity ([HPO,²]+ [H;PO, ]) to equal 0.3. What concentrations of the KH,PO4 and Na;HPO, would be required?4. Two RND Engineers were assigned to create buffer solutions for two separate product lines that were susceptible to degradation if their pH was not maintained at a certain level. [a.] Engr. Baylon prepared the buffer for the product that requires a pH of around 4.0 by mixing 0.225 M of phosphoric acid and 0.414 M of sodium dihydrogen phosphate [b.] 0.640 M of ethanolamine, HOC,H,NH, were mixed with 0.750 M of its chloride salt, HOC,H4NH3CI, by Engr. Samonte for the alkali goods that requires a pH of 9.5 max. Are the prepared buffers solutions applicable for their intended use? Take the acid ionization constant of phosphoric acid to be 7.1x10-3 while the base ionization constant of ethanolamine is 2.68x10-5
- Q1) In titration of the solution containing 0.1 Molar of I'and 0.1 Molar of Cro,", with the solution of 0.1 molar of Ag+ , what is the titration error in first step? if the end point of first titration will be taken on the precipitation of Ag.Cro. KSP(Ag.Cro.)=10112 KSP(Agl) = 10.1(f). Following are the titre values of two students when 25 mL of KIO3(aq) is titrated against Na2S2O3(aq).Titration no. Student 1 Student 21 2 3 24 24.9 25.7 25 24.1 24.0Which student is best in doing titration and why do you say so?(g). Taking the values of best student, calculate the concentration of the solution for which molarity is not known.(Note: first calculate moles of pipet solution in 25 mL, then moles of I2 and then moles of solution of unknown concentration and then its molarity by using average titre)For the reaction of hydrazine (N2H4) in water, H,NNH, (ag) + H20(1) = H,NNH,+(aq) + OH¯(@ag) K, is 3.0 x 10-. Calculate the concentrations of all species and the pH of a 1.6-M solution of hydrazine in water. [H,NNH,] =| %3D [H,NNH, !3! JOH |= %3D [H*]=[ ]M pH= %3D
- The Ka expression for the H, PO,/HPO?- buffer is given Ionic strength (µ, M) 0.005 0.010 0.050 | 0.10 by the equation YH+ 0.933 0.914 0.86 0.83 [HPO] YHPO;- [H*] YH* Ka = [H,PO;] YH,PO; YHPO; - 0.740 0.660 0.445 0.355 10-7.20 YH,PO, 0.928 0.902 0.82 0.775 What is the pH of a 1:1 mixture of H, PO, to HPO?- at an ionic strength of 0.005 M? Activity coefficients can be found in the table. pH 6.7712. The following quantities of salts were added to a volume of water to make 1 liter of solution: 1 x 10-2 moles NaCl 2 x 10-2 moles CaCl, 2 x 10-2 moles BaCl, (a) What is the ionic strength of the solution? (b) A small amount of phosphate salt is added to the same solution with negligible change in ionic strength. Given K = 10-7.2 for the reaction H,PO, = H+ + HPO,?- Calculate (H*][HPO,2-1/[H,PO,"), called °K, using the Güntelberg ap- proximation of the DeBye-Hückel law. (c) Calculate the "salting-out" coefficient, k,, for a nonelectrolyte in the same solution if its activity is 10-3 M and its concentration is 9.5 x 10 4 M.13.53 For the cell (13.71), the observed emf at 25°C was 612 mV. When solution X was replaced by a standard phos- phate buffer solution whose assigned pH is 6.86, the emf was 741 mV. Find the pH of solution X. Pt|H;(g)|soln. X;KCI(sat.)|Hg,Cl,(s)|Hg|Pt' (13.71)
- The reaction Cu(s) + HNO3(ag) Cu(NOsh(ag) + 2 NO:) +2 H;O() is used to dissolve the copper metal Ifa 1.000 g sample of copper is used, and instructions say to use four times as much acid as the required amount, how many mL (to the nearest mL) of 15.0 M nitric acid would be used in the procedure for this sample? Select one: O a 10mL Ob 17ml O c.4mL O d 25ml O e 5mLFor 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 2pmA chemistry graduate student is given 125. mL of a 1.50M diethylamine ((C,H, NH solution. Diethylamine is a weak base with K,=1.3 × 10 °. What mass (HIN %3D of (C,H5), NH,Br should the student dissolve in the (C,H,) NH solution to turn it into a buffer with pH =10.79? 2. You may assume that the volume of the solution doesn't change when the (C,H) NH, Br is dissolved in it. Be sure your answer has a unit symbol, and round 12 it to 2 significant digits. 10