The electrochemical cell shown can be used to calculate the formation constant (K) for a metal (M) and EDTA. The cell hasa potential of -0.259 V. The right half-cellcontains a metal ion (M²*) with a standard reduction potential of -0.236 V.M* + 2e M(s)E = -0.236 VVoltmeter+H.(g) Pe-0.40 barSalt bridgePi30 ml of 0.010M citric acid70 mL of 0.010M NaOH30 ml of 0.010 M M70 ml of 0.010 M EDTA (ava 0.81 at pH 11)pH 11.0 (buffered)Citric acid has three pk, values: 3.128, 4.761, and 6.396. Calculate the Kr for the metal-EDTA complex.Kr =1.96 x10Incorrect

Answered: Image /qna-images/answer/0164b470-72ca-4074-b817-48b94d652a14.jpg

The electrochemical cell shown can be used to calculate the formation constant (K) for a metal (M) and EDTA. The cell has a potential of-0.259 V. The right half-cell contains a metal ion (Mt) with a standard reduction potential of -0.236 V. M* +2e M(s) = -0.236 V Voltmeter (g) Po-0.40 bar Salt bridge 30 ml of 0.010 M citric acid 70 mL of 0.010M NAOH 30 ml of 0.010 M M 70 ml of 0.010 M EDTA (ava 0.81 at pH 11) pH 11.0 (buffered) Citric acid has three pK, values: 3.128, 4.761, and 6.396. Calculate the Kr for the metal-EDTA complex. Kr = 1.96 x10 Incorrect

The electrochemical cell shown can be used to calculate the formation constant (K) for a metal (M) and EDTA. The cell has a potential of-0.259 V. The right half-cell contains a metal ion (Mt) with a standard reduction potential of -0.236 V. M* +2e M(s) = -0.236 V Voltmeter (g) Po-0.40 bar Salt bridge 30 ml of 0.010 M citric acid 70 mL of 0.010M NAOH 30 ml of 0.010 M M 70 ml of 0.010 M EDTA (ava 0.81 at pH 11) pH 11.0 (buffered) Citric acid has three pK, values: 3.128, 4.761, and 6.396. Calculate the Kr for the metal-EDTA complex. Kr = 1.96 x10 Incorrect

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

If the Standard Potential cell for the following AgI /Ag and I/I Was -0.152vand o, suv respectively. write the total chemical reaction for the Cell ? 2) what is the Potential cell if the meterial is Standard ? 13) If the Potential cell increase with increasing Temperture of 1*104 V/KⓇ Percent Calculate AG, AS, AH at 25c
Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant x at 25.0 °C for the following reaction. CH₂OH(g) + CO(g) HCH₂CO₂ (1) Round your answer to 2 significant digits. K = 0 x10 X
Given the standard potential for hydroxide formation is -1.59V and the standard potential for Mn²*reduction is -1.18V, calculate the Ksp of Mn(OH)2
A voltaic cell is constructed from a standard Cu2+|Cu half cell (E°red 0.337V) and %D a standard H+|H2 half cell (E°red 0.000V). %3| The anode reaction is: + + The cathode reaction is: + The spontaneous cell reaction is: + + | The cell voltage is V. + ↑
Given that standard reduction potentials at 298.15 K are E° Mg*2 /Mg = -2.37 V and E° Sn2*/Sn = -0.140; then if a Mg(s) foil is soak in 1.0 M SnCl2(ag), the Mg foil be will be oxidized and eventually dissolve.
20). Calculate the cell voltage for the electrochemical cell below. Assume standard conditions. Note: Sulfate is not in any of the solutions. Ni(s) /Ni2* (aq, 1.0 M) //Pb²* (aq, 1.0 M) /Pb(s) a. +0.106 V b. +1.935 V C. +0.124 V d. +0.606 V e. None of the above
Use the standard reduction potentials given below to predict if a reaction will occur when Sn metal is put into a 1 M aqueous Mg2+ solution. Sn2+(aq)+ 2e- ---> Sn(s) E°red = -0.140V Mg2+(aq) + 2e- ---> Mg(s) E°red = -2.370V If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) _______ +_______ ------>_______ + ________
. Consider a galvanic cell with the anode containing a Zn metal electrode and a 0.10 M Zn(NO3)2solution and the other half-cell containing a Sn metal electrode and a 0.10 M Sn(NO3)2 solution. If themeasured Ecell value is +650 mV and the Zn2+/Zn reduction potential is assumed to be −790 mV, what isthe Sn2+/Sn reduction potential? Show all work.
Question 3 D Voltage Source Zn 로 salt bridge ZnSO4 Question 4 If the cell pictured above is driven as an electrolytic cell: The electrons would flow (Select ] The following statement is true: [Select] Cu The standard (assuming 1 M concentrations) cell potential is [Select ] If the salt bridge contains KCI, then [Select] CuSO4 In order to decrease (make it a smaller number) the potential necessary for electrolysis, [Select] If the current is set to a constant of 3.82 A for 5.00 min, then (Select] of metal would deposit on the cathode.
You are given an electrochemical cell where the chemical reaction involves a silver complex. A silver metal bar is used as the positive electrode. The electrochemical potential for this cell is given by E=EºAg+/Ag-0.0592(volts)*log(1/[Ag+]) For a test solution with a silver concentration of 0.001 M, the electrochemical cell potential is 0.20 volts. Find the silver electrode potential EºAg+/Ag. This same cell from (a) is used to measure the electrochemical potential for a new silver complex in equilibrium. If the measured cell potential is 0.324 volts, what is the silver concentration for this new silver complex at equilibrium?
What is the standard electrode potential for the reaction 2 Cr + 3 Pb2* →3 Pb + 2 Cr+? Standard Reduction E° (V) V Potentials Pb2+(aq) + 2e Pb(s) -0.13 1 4 6. Cr3+(aq) + 3e- - Cr(s) -0.74 8. 6. +/- 0. 2. 7.
Given the hypothetical metal samples a, B. and y were placed in an electrochemical cell as electrodes with their corresponding mettalic ions a*. B<*. and y* as their electrolytes. The following standard cell potentials were observed and recorded: E cll Trial Anode Cathode 0.72 V 0.53 V 3 1.25 V And given that the standard reduction potential of y is -2.38V, what is the standard reduction potential of a? O 1.66 V O -1.13 V O +3.10 V O +1.88 V