If in separate solutions of nitrates of Sn2 +, Zn2 + and Cd2 +
we put a coin of Ag (s) in each one it is expected that Ag (s)
...
Zn2 + (ac) + 2e = Zn (s) E ° = -0.76V
Sn2 + (ac) + 2e = Sn (s) E ° = -0.14V
Cd2 + (ac) + 2e = Cd (s) E ° = -0.40V
Ag + (ac) + e = Ag (s) E ° = + 0.80V
A. React only with Zn2 + (ac)
B. React only with Sn2 + (ac)
C. React only with Cd2 + (ac)
D. Silver will react with everyone
E. Silver will not react with any
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If in separate solutions of nitrates of Sn2 +, Zn2 + and Cd2 + we put...
1. Determine the Ka value for an acid that is 0.294 M in a solution that has a pH of 2.80. A 49 x 10-14 B. 23 x 109 C. 14 x 10-5 D. 20 x 10-5 OE 3.7x 10-7 2. When titrating 25.0 mL of 0.080 M HCIO with 0.060 M NaOH, calibrate the pH after adding 25.0 mL of 0.050 M NaOH (pKa = 7.55) A. 7.43 b.7.55 C.7.77 D.10.08 E 1248 3. The correct expression for the...
Reaction Eo Ag+(aq)+ e-→ Ag(s) 0.80V Zn2+(aq)+ 2e-→Zn(s) -0.76V What would be the cathode reactant in the Voltaic Cell made from the half-reactions above? Question options: a. Zn2+(aq) b. Ag+(aq) c. Ag(s) d. Zn(s)
A voltaic cell is based on the following two half-reactions: Cd2 (ag) +2e-> Cd (s) Sn2(aq)+ 2e Sn (s) Calculate the standard cell potential. Use the date from the attached table.SRP2.docx Oa 0.13 Ob 042 Oc.027 Od-0.27
Please include solutions, thank you. Consider the voltaic cell: Zn(s) + Cd2+(aq) → Zn2+ (aq) + Cd(s). (Eºcell = 0.36V) operating at 319.351 K. If (conc. Cd2+) = 0.411 and (conc. Zn2+) = 1.101, calculate the Ecell (volts).
answer question 1 using table 1 provided bellow: 1. Generate a reactivity series for the metals tested. E° = 0.34 V for the copper half-cell. Use this value to calculate Eº for each of the other half reactions. Write each half reaction as a reduction and arrange them with the most powerful reducing agent at the top of the table. When arranged in this manner, a metal on the right side of an equation will spontaneously react with a species...
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please help me with these questions, I am having a really hard time with chemistry and this is my last assignment 1. Consider the following half-reactions: Half-reaction E° (V) Br2(l) + 2e-____>2Br-(aq) 1.080V Cd2+(aq) + 2e-____>Cd(s) -0.403V Cr3+(aq) + 3e-____>Cr(s) -0.740V The strongest oxidizing agent is: enter formula The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will Br2(l) oxidize Cr(s) to Cr3+(aq)? _____ (yes or no) Which species can be reduced...
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Using standard reduction potential in aqueous solutions at 25c Table, which substance is most likely to be oxidised by O2 (g) in acidic aqueous solution? Select one: a. Br2 (l) b. Br- (aq) c. Ni2+ (aq) d. Ag (s) e. Cu2+ (aq) Cathode (Reduction) Half-Reaction Standard Potential E° (volts) Li+(aq) + e- -> Li(s) -3.04 K+(aq) + e- -> K(s) -2.92 Ca2+(aq) + 2e- -> Ca(s) -2.76 Na+(aq) + e- -> Na(s) -2.71 Mg2+(aq) + 2e- -> Mg(s) -2.38 Al3+(aq)...
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