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- A bare silver wire electrode is dipped into a solution 0.05M in KNO3 (supporting electrolyte) and saturated in AgBr (Ksp = 5.0 x 10-13), and connected to the back of an mV/pH meter along with a saturated calomel reference electrode. Calculate the potential of the silver indicator electrode. Calculate the cell potential.If 100mL of a pharmaceutical preparation contains 20mcL of a 50% w/v solution of benzalkonium chloride, what is the percentage strength of that agent in the solution? A. 0.1% B. 0.001% C. 0.01% D. 1%For the gaalvanic cell 2Ag+ + Mn --> 2Ag + Mn2+, which equation allows you to correctly calculate the standard cell potential? 1. E0Ag+/Ag / E0Mn2+/Mn 2. E0Mn2+/Mn + E0Ag+/Ag 3. E0Mn2+/Mn - E0Ag+/Ag 4. E0Ag+/Ag - E0Mn2+/Mn 5. E0Ag+/Ag + E0Mn2+/Mn
- A pH meter is calibrated using a pH 4.00 buffer with 174.48 mV, pH 7.00 with 0 mV and pH 10.0 buffer with (-)174.48 mV. Calculate the Molar concentration of a HCl solution with electrode potential of 396.31 mV.Consider the cell: Pt|H₂(g,p°)| HCl(aq)|AgCl(s)|Ag for which the cell reaction is 2AgCl(s) +H₂(g) → 2 Ag(s) + 2HCl(aq). At 25 °C and a molality of HCl of 0.010 mol kg⁻¹ a) Calculate ionic strength of solution and Calculate mean activity coefficient Ɣ∓?At 25C, you conduct a titration of 20.00 mL of a 0.0400 M AgNO3 solution with a 0.050 M NaI solution within the following cell: Saturated Calomel Electrode | Titration solution | Ag(s) for the cell as writted, what is the voltage after the addition of 10.00 mL of the NaI sooution? The reduction potential for the saturated calomel electrode is E=0.241 V. The standard reduction potential for the reaction: Ag++e- ® Ag(s) E0= 0.79993V. The solubility constant of AgI is Ksp=8.3x10-17 Note: the cell potential could be negative since the condditions are non-standard ones. a)0.169 b)0.354 c)0.235 d)2.360 e)0.441
- Gases in a Salt Marsh: You measure appreciable CH 4(g) andCO 2(g) partial pressures in the sediment pore fluid and you want toknow if there is equilibrium between these redox couples. The measuredpartial pressure of CO 2 (g) is 1x10 -5 atm and the measured partialpressure of CH 4 (g) is 5x10 -3 atm in the pore fluid.You measure a redox potential (E h) of pore-fluid water of Eh = -0.1 V atpH=8.3 using a platinum electrode and suitable reference electrode. Calculate a value of E h from the ratio of the measured gas partialpressuresTwo Copper strips were used to determine the effect of supporting electrolyte used on the change in mass. Three different experiments were conducted for 5mins where 0.5A current is applied throughout the experiment. In the first experiment two copper strips were immersed in 3.080g of Cu (NO3)2 dissolved in 25mL of DI water and tested for 5mins while applying current 0.5A. The weight of one copper strip act as an anode is taken before the reaction and after the reaction to calculate the change in mass due to different applied current. Same process is repeated with 25ml 0.5 M CuSO4 and25ml 0.5 M CuCl2 for 5 mins Using Faraday’s equation (Eq 1), calculate the theoretical mass and Compares the theoretical mass (mg) of copper and the actual mass deposited (obtained from the electrolysis, ∆m) by calculating the %error at different times. Discuss the observed results. Q = I x t = nFN Electrolyte Initial mass of anode (mg) Final mass of anode (mg) Cu (NO3)2 2941 2893…In an unknown sample, the amount of ascorbic acid (C6H8O6) is determined using coulometry. Analysis of a 250.0 mg sample gives an endpoint with starch after reaction with electrogenerated iodine in 384 sec using a current of 30.0 mA. What is the % ascorbic acid, (C6H8O6), (FW= 176.12 g/mol) in the sample?
- Black-and-white photographic film is coated with silver halides. Because silver is expensive, the manufacturer monitors the Ag⁺ content of the waste stream, [Ag⁺]ᵥᵥₐₛₜₑ, from the plantwith an Ag-selective electrode at 25°C. A stream of known Ag⁺ concentration, [Ag⁺](standard), is passed over the electrode inturn with the waste stream and the data recorded by a computer.(a) Write the equations relating the nonstandard cell potential tothe standard cell potential and [Ag⁺] for each solution.(b) Combine these into a single equation to find [Ag⁺]ᵥᵥₐₛₜₑ.(c) Rewrite the equation from part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ in ng/L.(d) If Eᵥᵥₐₛₜₑ is 0.003 V higher than E(standard), and the standard so-lution contains 1000. ng/L, what is [Ag⁺]ᵥᵥₐₛₜₑ?(e) Rewrite the equation in part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ for a sys-tem in which T changes and Tᵥᵥₐₛₜₑ and T(standard) may be different.How long does it take to deposit a coating of gold 1.00 μm thick on a disk-shaped medallion 4.00 cm in diameter and 2.00 mm thick at constant current of 89 A? The density of gold is 19.3 g/cm3 and the gold is from an Au(III) solution. ____ s1) Since E0 (Fe3 + / Fe2 +) = + 0.77 V, E0 (Fe2 + / Feo) = - 0.44 V and E0 (MnO4- / Mn2 +) = +1.51 VFe / Fe3 + (0.01M) // pH = 3; MnO4- (0.10M); Mn2 + (0.01M) / PtWrite down the anode, cathode and total battery reactions of the battery. Calculate the cell potential at a temperature of 25 degrees Celsius and the equilibrium constant of the spontaneous reaction in the cell with the Gibbs Free Energy Change.
