(a)
Interpretation:
The standard potential for the following reaction should be predicted.
Concept introduction:
Indicator electrode is a type of electrode that is used in potentiometric titrations. It is used as an endpoint indicator. Membrane electrode and metallic electrodes are classify as indicator electrodes
(b)
Interpretation:
The schematic representation of a cell with a copper indicator electrode and a reference SCE should be stated.
Concept introduction:
Indicator electrode is a type of electrode that is used in potentiometric titrations. It is used as an endpoint indicator. Membrane electrode and metallic electrodes are classify as indicator electrodes
(c)
Interpretation:
The equation that relates the measured potential of the cell in (b) to pBr should be predicted.
Concept introduction:
Indicator electrode is a type of electrode that is used in potentiometric titrations. It is used as an endpoint indicator. Membrane electrode and metallic electrodes are classify as indicator electrodes
(d)
Interpretation:
The pBr of a bromide-containing solution which is saturated with CuBr and consist in the cell described in (b) when the resulting potential is -0.078 V should be predicted.
Concept introduction:
Indicator electrode is a type of electrode that is used in potentiometric titrations. It is used as an endpoint indicator. Membrane electrode and metallic electrodes are classify as indicator electrodes
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Chapter 23 Solutions
Principles of Instrumental Analysis
- At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)arrow_forwardFor each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+arrow_forwardFor each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)arrow_forward
- The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.arrow_forwardFrom the standard potentials Ag2SeO4(s)+2e2Ag(s)+SeO42-E0=0.355V Ag++2eAg(s)E0=0.799V calculate the solubility product constant for Ag2SeO4.arrow_forwardHalide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.arrow_forward
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