Answered: A current of 11.8 A is applied to 1.25…

A current of 11.8 A is applied to 1.25 L of a solution of 0.549 mol L- aqueous HBr converting some of the H+ (aq) to H2 (g), which bubbles out of solution.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.3QAP

See similar textbooks

Related questions

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2vo; (aq)…

Q: The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one…

A: Answer: 174.0

Q: Magnesium metal can be produced industrially by electrolysis of MgCl2. What mass of magnesium metal,…

Q: How long will it take for a uniform current of 6.00 A to deposit 78.0 g gold (197.0 g/mol) from a…

Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: According to the Faraday's first law of electrolysis, the amount of any substance deposited at the…

Q: How long would it take to electroplate all the Zn^ 2+ in 0.280 L of .210 M ZnSO 4 solution with a…

A: The question is based on the concept of electrochemistry. It involves application of first law of…

Q: How long will it take to plate out 3.0 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to…

A: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

Q: The passage of a current of 0.750 A for 25.0min deposited 0.369 g of copper from a CuSO4 solution.…

Q: A solution of a metal ion M 3+(aq) is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19…

A: The given data contains, current =5 A time =10 min60s1 min=600s

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

Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

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

Q: Determine the current (in A) to produce 3.10 g Ag when Ag"(aq) is electrolyzed for 2.00 h. (F =…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 210, (aq)+…

Q: A galvanic cell is based on the following reaction(at 25°C)： Cu (aq)+Sn(s) → Cu(s)+Sn (aq) If the…

A: Note - The given reaction is incorrect. So, we will use the correct reaction for the question. A…

Q: Brass, an alloy of copper and zinc, can be produced by si-multaneously electroplating the two metals…

Q: 3. The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a Cuso,…

A: The Faraday's laws are the main concepts of electrochemistry. The first law shows the connection…

Q: The galvanic cell Zn(s) | Zn2+(aq) | | Ni2+(aq)| Ni(s) is constructed using a completely immersed…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three sub-parts…

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Since in the above reaction we can see that 1 mole of Cl2 is produced with 2 moles of electrons…

Q: A solution of NaCl is neutral, with an expected PH of 7. If electrolysis was carried out on 500 mL…

Q: (a) Liquid H2O is subjected to electrolysis. One of the half-reactions is 2 H2O → O2 (g) + 4 H+(aq)…

A: We have to calculate the Faraday of electricity required and the time taken.

Q: In one process used for electroplating silver, a current of 10.23 A was passed through an…

A: Dear student, this question is related to electroplating process.

Q: How much time would it take for 325 mg of copper solid (atomic molar mass = 63.546 g/mol) to be…

A: Two moles of electrons give one mole of copper atom. Number of electrons required is determined as…

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr, converting some of the H* to…

A: Given: Current (I) = 11.3 A Volume of solution (L) = 1.25 L Concentration of HBr = 0.552 M…

Q: Molten CaCl₂ can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: For CaCl2 , the given data is- Current(I) = 2.06A Mass of Ca = 29.3g Atomic mass of Ca = 40.078 g…

Q: Copper can be electroplated at the cathode of an electrolytic cell by the half-reaction: Cur"(aq) +…

A: Given, The mass of copper is 325 mg. The current is 5.6 A. The given reaction is,

Q: ulate the potential of the following cells: a galvanic cell consisting of a lead electrode on the…

Q: The dilute sulfuric acid solution is electrolyzed with platinum electrodes with a current of 1.25 A…

A: Volume of gases evolved can be calculated from the moles of gases evolved..

Q: (a) In the electrolysis of aqueous Na2O2, how many liters of H2(g) (at STP) are generated by a…

A: The reaction taking place is given as, => Na2O2 (aq) + H2O (l) ↔ H2 (g) + O2 (g) + NaOH (aq)…

Q: How many minutes would it take to plate 12g of silver from an aqueous Ag(l) solution using a current…

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: A cell is set up with copper and lead electrodes in contact with CuSO4(aq), and Pb(NO3)2(aq). If…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Cu*…

A: Answer :- Ecell = 1.09 (V) The cell voltage (Ecell) for given cell = 1.09 V…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu?* (aq)…

Q: Determine the current (in A) to produce 3.00 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A: The half reaction when Ag+ (aq) is electrolyzed. Ag+ (aq)…

Q: Calculate the cell potential for the galvanic cell (in volts) in which the following reaction occurs…

A: In order to figure the cell potential of any reaction in an electrochemical cell, first derive…

Q: A pure organic acid sample (0.1516 g) is neutralized with OH- ions produced in a constant current of…

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

Q: Copper metal (63.55 g/mol) is purified by electrolysis. How much copper metal (in grams) could be…

Q: Copper is electroplated from CuSO4 solution. A constant current of 5.79 A is applied by an external…

Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: Given values:I = 0.912 ATime = 18.5 h It is known that 1 h = 3600 sec.Therefore, 18.5 h = 18.5×3600…

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: 1. Consider the reaction: MnO2(s) + 4H*(aq)+ 2B1¯(aq) → Mn2+(aq) + Br,(l)+2H,O(1) At what pH will…

A: The electrochemical cell is the one that generates electrical energy from chemical energy. It is…

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au³+(aq) =…

A: In this question, we will calculate the cell potential for this given Reaction in the Question. How…

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

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 210, (aq) +…

Question

100%

Can someone please help with question with question 8

1302 - 4.3 - Exercise 18.121 - Copy - Copy
8 of 15
I Review | Constants I Periodic Table
A current of 11.8 A is applied to 1.25 L of a solution of 0.549 mol L¯' aqueous HBr converting some of the
H+(aq) to H2 (g), which bubbles out of solution.
Part A
What is the pH of the solution after 76 minutes? (Assume the volume of solution to be constant.)
Express your answer using two decimal places.
ΑΣφ
pH =
Submit
Request Answer

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A 0.0712-g sample of a purified organic acid was dissolved in an alcohol-water mixture and titrated with coulometrically generated hydroxide ions. With a current of 0.0392 A, 241 s was required to reach aphenolphthalein end point. Calculate the equivalent mass of the acid.
The limiting current of lead in an unknown solution is 5.60 μA. One milliliter of a 1.00 × 10-3 Mlead solution is added to 10.0 mL of the unknown solution and the limiting current of the lead isincreased to 12.2 μA. What is the molar concentration of lead in the unknown solution?
A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to H2( g), which bubbles out of solution. What is the pH of the solution after 73 minutes?
A pH meter equipped with an electrode that respond to (H3O+ in a solution/OH- in a solution/ Voltage of solution / or all of them)?
Calculate the pOH of 0.716 M anilinium hydrochloride (C6H5NH3Cl) solution in water, given that Kb for aniline is 3.83 × 10-4.
The pOH of 0.0200 M solution of Sr(OH)2 is
Calculate [ OH− ] for a solution where [H3O+]=0.00605 M .
In regions where there is acid industrial dumping (pH: 4.0), show whether there will be more or less aluminum than in rivers (pH: 7.0) far from the industrial region? Justify the answer by determining the aluminum concentration in these waters.Kps = Al (OH) 3 = 1.0x10-33
calculate the poh of 0.00010405M solution of H plus
An aqueous solution of a weak base, B, has a concentration of 0.110 M and degree of hydrolysis of 6.85%. Sample reference equation B(aq) + HOH( ) BH+(aq) + OH (aq) What is the pH of this solution ?
Calculate the pOH of a 9.44 X 10-8 M Mg(OH)2 solution. I need the work otherwise I wont understand it
Balance the equation below assuming it occurs in a basic solution :Al(s) + CrO42−(aq) ⟶ Al(OH)3(s) + Cr(OH)4−(aq) You may use the template below or submit your own file as a response