For the following reaction:
NiO2(s) + 4 H+(aq) + 2 Ag(s) → Ni2+(aq) + 2 H2O(l) + 2 Ag+(aq) ℰ° = 2.48 V
Calculate the pH of the solution if ℰ = 2.09 V and [Ag+] = [Ni2+] = 0.045 M. (See this table.)
For the following reaction: NiO2(s) + 4 H+(aq) + 2 Ag(s) → Ni2+(aq) + 2 H2O(l)...
For the following reaction: NiO2(s) + 4 H+(aq) + 2 Ag(s) → Ni2+(aq) + 2 H2O(l) + 2 Ag+(aq) ℰ° = 2.48 V Calculate the pH of the solution if ℰ = 2.39 V and [Ag+] = [Ni2+] = 0.029 M. (See this table.)
Consider the following reaction. Mg(s)+2Vo; (aq)+ 4 H* (aq)Mg2+(ag)+ 2 VO2 (aq)+ H2O(l) Ecell 3.37 V. Part A Calculate the AGo for the reaction. Express your answer to three significant figures. Consider the following reaction. Mg(s)+2Vo; (aq)+ 4 H* (aq)Mg2+(ag)+ 2 VO2 (aq)+ H2O(l) Ecell 3.37 V. Part A Calculate the AGo for the reaction. Express your answer to three significant figures.
Consider a cell based on the following reaction: GeO(s) + H2O(l) + 2 Ag+(aq) → GeO2(s) + 2 H+(aq) + 2 Ag(s) If [Ag+] = 1 M, at 25°C pH = (E - E°)/0.0592 V. pH = 2(E - E°)/0.0592 V. pH = 2(E° - E)/0.0592 V. pH = (E° - E)/0.0592 V.
A voltaic cell is constructed from an Ni2+ (aq) -Ni(s) half-cell and an Ag+ (aq)- Ag(s) half-cell. The initial concentration of Ni2+ (aq) in the Ni2+ - Ni half-cell is [Ni2+1 = 1.80x10-2 M. The initial cell voltage is +1.13 V. Part A By using data in Table 20.1 in the textbook, calculate the standard emf of this voltaic cell. V AEQ ? E V Submit Request Answer Part B. Will the concentration of Ni2+ (aq) increase or decrease as...
Consider the following reaction and its AG at 25.00 °C. Mg(s) + Ni2+ (aq) Mg2+ (aq) + Ni(s) AG = -408.0 kJ/mol Calculate the standard cell potential, Ecell for the reaction. 2.11 V Enter numeric value Calculate the equilibrium constant, K, for the reaction. K= 3.30 x1071 Incorrect
For the cell Ni(s) Ni2+(aq) || Ag+(aq) Ag(s), the standard cell potential is 1.03 V. A cell using these reagents was made, and the observed potential was 0.80 V at 25°C. What is a possible explanation for the observed voltage? The volume of the Agt solution was larger than the volume of the Ni2+ solution. The Agt concentration was larger than the Ni2+ concentration. The Ag electrode was twice as large as the Ni electrode. The Ni2+ concentration was larger...
1) Given the reaction Cd(s)+Ni2+(aq)------>Cd2+(aq)+Ni(s) Calculate the equilibrium constant (K). Ecell of +0.350 V and at 25.0 celsius 2)If 75.0mL of 0.195 M Hbr is combined with 75.0mL of 195M Ca(OH)2 at 25.0 celsius calculate the pH of this solution
1) Calculate the OH- concentration at equilibrium in the following reaction: NH3 (aq) + H2O (l) -> NH4+ (aq) + OH- (aq) (Kb = 1.8 x10^(-5). (a) 1 x10^(-14) M (b) 2.7 x10^(-3) M (c) 7.2 x10^(-6) M (d) None of the above 2) Which of the following pH values indicates the most basic solution? (a) pH=12 (b) pH=4 (c) pH=8 (d) pH=9 3) Which of the following pH values indicate the most acidic solution? ( (a) pH=11 (b) pH=2...
A voltaic cell is made from Ni(s), Ni2+(aq), Ag(s) and Ag+ a. Fill in the diagram with the chemicals associated with each part of the cell. b. Write a balanced cell reaction A voltaic cell is made from Ni(s), Niz*(aq), Ag(s) and Ag 7. a. Fill in the diagram with the chemicals associated with each part of the cell. Ni2+ + 2 e-→ Ni(s) Ag+ + e-→ Ag(s) -0.25 0.80
Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O (l) A 1.0 L buffer solution is 0.280 M in HC2H302 (acetic acid) and 0.320 M in NaC2H302 (sodium acetate). Calculate the pH of the budder and he Ka for HC2H3O2 IS 1.8 X 10-5 Calculate the pH of te solution above after the addition of 0.0400 moles of solid NaOH. Assume no volume change upon the addition of base.