A 10.0 mL solution of 0.050 M AgNO3 was titrated with 0.0250 M NaBr in the cell: S.C.E || titration solution | Ag(s) Find the cell voltage for 30.0 mL of titrant. (A) +0.093 V (B) -0.039 V (C) -0.093 V (D) +0.039 V
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- A 10.0-mL solution of 0.050 0 M AgNO3 was titrated with 0.025 0 M NaBr in the cell S.C.E. || titration solution | Ag(s) Find the cell voltage for 0.1 and 30.0 mL of titrant.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.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 5mL
- Given the titration reaction: Tl3+ + 2Fe2+ « Tl+ + 2Fe3+. Tl3+ + 2e- ↔ Tl+ E0 = 1.25 V Fe3+ + e- ↔ Fe2+ E0 = 0.771 VWhat is potential of 25.00 mL of 0.100 M Tl3+ after adding the following volumes of 0.100 M Fe2+:a. 10mLb. Equivalence pointc. 65mL1. 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…The phosphate in a 3.000-g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and filtrate, upon addition of 1.00 mL of 0.01 M fecl3, required 18.23 mL of 0.1377 M KSCN for titration to the end point. (a) the weight percent of phosphate in the detergent
- For the titration of 25.0 mL of 0.0100M Sn2+ by 0.0500 M Ti3+ Calculate the potential of solution after the following volumes of Ti3+ have beed added. E0 Sn4+/Sn2+ = 0.139 V, E0 Ti3+/Ti+= 0.77V A) 2.5ml B) 5.0 ml C) 6.0mLAt 25 °C, a 10.0-mL solution of 0.0500 M AGNO3 was titrated with 0.0250 M NaBr in the cell: S.C.E. titration solution | Ag(s). Find the cell voltage for 0.1 mL and 30.0 mL of titrant if the Ksp of AgBr is 5.0 x 10-13. (ESCE = 0.244 V; Ag* + e -> Ag(s) E° = 0.799 V).A 10.00 mL sample containing 8.00 g/L of a mixture of KCI and NaCl was titrated with 0.10 M standard solution of AgNO3; where 5.6 mL was needed to reach the end-point. Calculate the mass of sample (in grams). 1. O0.0033 2. O0.0800 3. O0.0083 4. O0.0337
- 0.683 grams of iron mineral dissolves with acid. Fe2+ is titrated with Ce(SO4)2 solution. Calculate the percentage of 38.5 mL of 0.161 M titrant consumed in the titration (Fe: 56 g/mol). 25.4150.82C.76,23D.32,45WARIARTAM 2. 1.2589 g of a certain brand of milk powder required 25.89 mL of 0.01873M EDTA to titrate the calcium contained in the sample. (a) What is the percent calcium in the sample? (b) Would the true result be higher, lower, or not be affected if the milk powder sample has been slightly wet?Chloride in a brine solution is determined using Volhard method. A 10.00 mL aliquot of the solution is treated with 25.00 mL standard 0.1182 M AgNO3 solution. The excess silver is titrated with standard 0.1010 M KSCN solution, requiring 12.38 mL to reach the red Fe(SCN)2+ end point. Identify the (a) indicator (b) end point color (c) molarity of the Cl- in sample.