Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.660 V when [Zn2+]= 0.40 M and PH2= 0.91 atm .
Calculate the pH of the cathode compartment solution if the cell emf at 298 K is...
Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.630 V when [Zn2+]= 0.26 M and PH2= 0.99 atm . Express your answer using two decimal places
1. Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.610 V when [Zn2+]= 0.20 M and PH2= 0.92 atm . Express your answer using two decimal places. pH= Switch 8.76 Voltmeter 7n anode NO, Na +H (8) Cathode compartment (standard hydrogen electrode) Anode compartment NO, Zn2+ NO NO, Zn(s) —> Zn2+ (aq)+ 2e 2H+ (aq) + 2e →H(8)
Part A Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.640 V when [Zn240.27 M and PH = 0.85 atm. Express your answer using two decimal places. V ΑΣφ pH =$ Figure 1 of 1 Previous Answers Request Answer Submit Switch 8.76 X Incorrect; Try Again; 2 attempts remaining Voltmeter Zn anode NO Na - H2(g) Cathode compartment (standard hydrogen electrode) NO3 Zn2 Provide Feedback Next Anode compartment NO3...
A student does an experiment to determine the molar solubility of magnesium fluoride. She constructs a voltaic cell at 298 K consisting of a 0.766 M magnesium nitrate solution and a magnesium electrode in the cathode compartment, and a saturated magnesium fluoride solution and a magnesium electrode in the anode compartment. If the cell potential is measured to be 8.25x102 v, what is the value of Ksp for magnesium fluoride at 298 K based on this experiment? Ksp for MgF2-...
A voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s) + Ni2+(aq) Zn2+(aq) + Ni(s) (a) What is the emf of this cell under standard conditions? ___________ V (b) What is the emf of this cell when [Ni2+] = 2.88 M and [Zn2+] = 0.187 M? ___________ V c) What is the emf of the cell when [Ni2+] = 0.129 M and [Zn2+] = 0.961 M? ____________ V
A voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s) + Ni2+(aq) Zn2+(aq) + Ni(s) (a) What is the emf of this cell under standard conditions? V (b) What is the emf of this cell when [Ni2+] = 3.51 M and [Zn2+] = 0.191 M? V (c) What is the emf of the cell when [Ni2+] = 0.137 M and [Zn2+] = 0.878 M? V
A voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s) + Ni2+(aq) Zn2+(aq) + Ni(s) (a) What is the emf of this cell under standard conditions? V (b) What is the emf of this cell when [Ni2+] = 2.58 M and [Zn2+] = 0.101 M? V (c) What is the emf of the cell when [Ni2+] = 0.211 M and [Zn2+] = 0.837 M? V
A voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s) + Ni2+(aq) Zn2+(aq) + Ni(s) (a) What is the emf of this cell under standard conditions? V (b) What is the emf of this cell when [Ni2+] = 2.60 M and [Zn2+] = 0.194 M? V (c) What is the emf of the cell when [Ni2+] = 0.232 M and [Zn2+] = 0.979 M? V
a.) A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (P(H2) = 1 atm) immersed in a solution of unknown [H+]. If the cell potential is 0.204 V, what is the pH of the unknown solution at 298 K? b.) An electrochemical cell is constructed in which a Cr3+(1.00 M)|Cr(s) half-cell is connected to an H3O+(aq)|H2(1 atm) half-cell with unknown H3O+ concentration. The measured cell voltage is 0.366...
Use the References to access important values if needed for this question. A student does an experiment to determine the molar solubility of lead chloride. He constructs a voltaic cell at 298 K consisting of a 0.709 M lead nitrate solution and a lead electrode in the cathode compartment, and a saturated lead chloride solution and a lead electrode in the anode compartment. If the cell potential is measured to be 4.96×10-2 V, what is the value of Ksp for...