Ascorbic acid (Vitamin C) in a 50.0mL sample of orange juice was analyzed by an electrochemical analysis, and a current of 1.78μA was detected. A standard addition of 0.400mL of 0.279M ascorbic acid increased the current to 3.35μA. Find the concentration of ascorbic acid in the juice.

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

A: Gold ion gains 3 electrons to get reduced to gold as per below equation Au3+ + 3e-  --> Au

Q: How long must constant current of 50.0 A be passed through an electrolytic cell containing aqueous…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: two grams of copper (A.W. = 63.54g g/mol, density = 8.93g/cm^3) dissolves in 500g of water to…

A: Reaction: Cu→Cu2+ + 2e- Using Nernst equation: ECell=Ecell∘-0.05912logCu2+

Q: The standard addition method is used to determine the concentration of vitamin C in apple juice by…

A: Given : Initial volume of sample of apple juice = 2.00 mL Final diluted volume of apple juice = 25.0…

Q: Calculate Current or Time How many amperes are required to deposit 0.242 grams of silver metal in…

A:

Q: How many seconds are required to deposit 0.224 grams of manganese metal from a solution that…

A:

Q: How long must a current of 20.0 amps be applied to a solution of CrCl3 to produce 175 g of Cr (s)…

A:

Q: A metal object is to be gold-plated by an electrolytic procedure using an aqueous AuCla solution.…

A: Given : Time = 3.0 min = 3.0 X 60 = 180 s                                              (Since 1 min…

Q: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

A:

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A:

Q: A baby's spoon with an area of 6.25cm2 is plated with silver from a silver nitrate solution using a…

A: Calculation of Charge: Q=I×t                                 ...... (1)    where Q=charge, I =…

Q: 10

A:

Q: A certain voltaic cell has a cell potential of 1.15 V. If the reduction potential of the cathode…

A:

Q: A solution containing a 3+ metal ion is electrolyzed by a current of 5.0 A for 10 minutes. What is…

A:

Q: A galvanic cell runs for 1 minute with a current of 0.50 A. How much charge passed through the cell…

A: The following expression shows the relationship between charge to current and time. Charge,…

Q: Calculate the mass in grams of a metal Q ( Molar mass= 88.23 g/mol) that will be deposited from a…

A:

Q: Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of…

A: Given data: Concentration of solution = 0.4 M Emf of cell = 0.015 V Formula used:…

Q: How many seconds would be required to produce 50.0 g of Mg from MgCl2 if the current is 100.0 A?

A: According to Faraday's law of electrolysis, the weight of the substance deposited on any electrode…

Q: 1.Chrome is plated from solutions of chromium (III) ions. If a particular application requires 13.7…

A: Since you have asked multiple questions in a single upload, if you want the second question to be…

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: 2) How long, in minutes, will it take to plate out 25.0g of Au from a AuCl3 solution if the current…

A:

Q: Using the Nernst equation and the table for standard electrode potentials, determine the voltage of…

A:

Q: A 17.1769 mL sample of an acid was titrated with electrogenerated OH-. It took 617s at a constant…

A: Given: Volume of acid solution = 17.1769 mLCurrent = 0.216 ATime = 617 seconds

Q: Electrolysis: Show the oxidation and reduction equations involved in the KI electrolysis Calculate…

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Ascorbic acid (vitamin C) in a 50.0-mL sample of orange juice was analyzed by an electrochemical…

A: Given: Initial Volume of juice(ascorbic acid) Vi = 50 mL Volume of Standard ascorbic acid solution…

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution the…

A: Given: Time = 3.3 hours Current = 17.8 A Atomic mass of copper = 63.5 g/mol

Q: How are standard electrode potentials measured?

A: Standard electrode potential is referred to Eo of a cell and is in an electrochemical cell at a…

Q: A 220 mL sample of a 0.500 M NaCl solution with an initial pH of 7.00 is subjected to electrolysis.…

A:

Q: How long must a current of 5.00 A be applied to a solution of Ag + to produce 10.5 g silver metal?

A: The electrolysis reaction taking place to produce Ag (s) from Ag+ (aq) solution will be  Ag+ (aq) +…

Q: If you have the reaction Fe3+ + 3e- -> Fe, how many grams of Fe will result if you apply a current…

A: Faradays first  law of electrolysis , the amount of substance  deposited at cathode   is directly…

Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

Q: How many seconds are required to deposit 0.184 grams of zinc metal from a solution that contains…

A:

Q: How long will it take to plate out 1.2 g Ni from aqueous Ni2+ with a current of 112.4 A? WHERE ARE…

A: Given,   1.2 g Ni plate out from aq Ni2+ with a current of 112.4 A

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A:

Q: A galvanic cell runs for 1 minute with a current of 0.20 A. How much charge passed through the cell…

A: Given : Current passed = 0.20 A And time = 1 min

Q: The potential of the cell Ag|AgI (s)| AgI (aq) |Ag is 0.9509V at 25C. Calculate the solubility of…

A: The half cell reactions of the Ag|AgI (s)| AgI (aq) |Ag cell are, Anode: Ag+I-→AgI++e-Cathode:…

Q: A baby's spoon with an area of 6.25cm2 is plated with silver from a silver nitrate solution using a…

A: Given: Area = 6.25 cm2Current = 2.00 ATime = 2 hours 25 minutesCurrent efficiency = 82% Density of…

Q: Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of…

A: Nernst equation as follows,

Q: For ferricyanide determination by voltammetry, 20 mL of non-electroactive KCl solution is added to…

A: Molarity = No of moles / Volume (L) Also, No of moles = Molarity * Volume (L)

Q: how many minutes are required to plate 10.0g of nickel metal from a solution of NiSO4, if the…

A:

Q: decided to deposit 55.00 g of gold over an iron medallion by electroplating it from a solution…

A:

Q: Copper metal (63.546 g/mol) is purified by electrolysis. How much copper metal (in grams) could be…

A:

Q: How long will it take to plate out 4.9 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

A: Given:: Mass of Ni= 4.9 g molar mass of Ni=58.6934 g mol-1 charge = ?

Q: How long would it take to produce 3.6 g of platinum by passing a 2.0 ampere current through a…

A: The mass of the substance (m) deposited or liberated at any electrode is directly proportional to…

Q: The limiting current of lead in an unknown solution is 5.60 μA. One milliliter of a 1.00 × 10-3 M…

A:

Q: A galvanic cell runs for 1 minute with a current of 0.25 A. How much charge passed through the cell…

A: Given : Current passed = 0.25 A And time = 1 min F=96500 C/mol

Q: How many minutes would be required to electroplate 20 g of chromium (52.00 g/mol) by passing a…

A: Let t be the time required in seconds than total charge passed in t seconds = current in ampere…

Q: Start with a battery of Au+1/ Au0 and Li+1/ Li0 at standard conditions. If you wanted to lose 2.1…

A:

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: Given-> Current (I) = 1.48 ampere  Time (t) = 37.4 min = 37.5 × 60 second = 2250 seconds Weight…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.