For the following reaction in aqueous solution, identify all those species that will be spectator ions. Select all that apply. Na,SO4+1 + Hg(NO3)2 HgSO,+ 2NANO3 >
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- A redox titration is performed to investigate iron content in an alloy sample. The potential of titration is monitored against a standard hydrogen electrode at 25 °C. All materials needed for redox titration were prepared accordingly. The half reactions involved in his experiment are:Fe3+ + e ̄ → Fe2+ E° = 0.771 V I3 ̄ + 2e ̄ → 3I ̄ E° = 0.535 Va) Construct a balanced titration equation.b) Assess the E° for this redox reaction.c) Depict whether the name of pH indicator that could be used to determine the endpoint of thistitration.d) Given a 25 mL portion of 0.5 M Fe3+ was titrated with 1 M titrant. Calculate the volumeof titrant required to reach equivalence point.e) Evaluate the cell potential at this point if over-titrated by 2.50 mL.Balance the reaction below; determine the sum of the coefficients; this is in a basic solution! Include co-efficients for any unshown species(such as water and hydroxide)._CrO42- + _I- ↔ _Cr(OH)3 + _I3- 30 17 34 38a. Balance the following redox in acidic media C2O42- (aq) + MnO4- (aq) → CO2(aq) + Mn2+ (aq) b. If you titrated this reaction to determine the moles of C2O42-, the colormetric endpoint is pink due to the Mn2+. How many moles of the oxalate (C2O42-) existed in solution if 12 mL of 0.791M permanganate was needed to hit the endpoint?
- Calculate E0 that would be developed by the cells using the following reactions (all concentrations 1M) 1. Ni + 2Ag+↔ Ni2+ + 2Ag2. 2Cr + 3Cu2+ ↔ 2Cr3+ + 3CuBelow are the reduction half reactions for chemolithoautotrophic nitrification, where ammonia is a source of electrons and energy and oxygen is the terminal electron acceptor. NO2- + 6e- -> NH4+ (E0 = +0.34 volts) O2 + 4e- -> 2H2O (E0 = +0.82 volts) If you balance and combine the reactions so that 293 moles of NH4+are oxidized to NO2-, how many moles of electrons will be transferred from Nitrogen to Oxygen?A 1.000 g sample containing chlorides, iodides and inert materials was treated with dilute nitric acid followed by AgNO3. A precipitate of AgCl (143.32) and AgI (234.77) was produced and weighs 0.9238 g. On heating in a current of Cl2, the AgI is converted to AgCl, and the resulting product weighs 0.7238 g. Find the percentage of a) NaI (149.89) and b) NaCl (58.44) in the sample
- A potentiometric titration was done using a solution containing 200 mL of water, 20 mL of 3 M sulfuric acid, 5 mL of concentrated phosphoric acid and 10.00 mL of 0.5964 N K2Cr2O7. The amount of titrant added was 19.24 mL of 0.3355 N Fe2+ solution. [H+] = 1.41 x 10-3 M during the titration. Find the concentrations of all species relevant to the redox chemistry present in solution at this point in the titration.The concentration of NO3- in a water sample was determined using ion-selective electrode. A 25.00 mL of the sample is placed in a beaker and a potential of 0.102 V is obtained. A 1.00 mL aliquot of a 200.0 mg/L standard solution of NO3- is added to this sample which gave a potential reading is 0.089 V. What is the concentration (ppm) of NO3- (FW = 62.00 g/mol) in the water sample?Which is more reducing, a solution with 20 mM sufide (HS-; assume S0 as product of sulfide oxidation), or a solution with 40 mM Mn2+ (assume MnO2 as product of Mn(II) oxidation).
- Which of the statements below are true for the titration of Fe2+ with standard Ce4+?I The indicator electrode potential before the addition of Ce4+ solution is calculated using the Fe3+ half-reaction after calculating the equilibrium concentrations of Fe3+ and Fe2+ in solution.II Before the equivalence point, the indicator electrode potential is calculated using the Fe3+ half-reaction because only [Fe3+] and [Fe2+] are known.III At the equivalence point, the indicator potential is the average of Eo for Fe3+ and Ce4+.IV After the equivalence point, the indicator electrode potential is calculated using the Ce4+ half-reaction because only [Ce4+] and [Ce2+] are known. A. I, III, and IV B. I, II, and IV C. II and IV D. II, III, and IV E. I, II, III, and IVWhich species from below is oxidized? Write the half reaction. Which species from below is reduced? Write the half reaction. 10 grams of Ag in 0.1M Cu(NO3)2 Ag (g) Cu (g) Ag+ Cu2+ Max. Temperature Color Observation 10 g 5.88641e-14 3.70529e-14 0.100000 25o C Blue 10 grams of Cu in 0.1M Cu(NO3)2 Cu (g) Cu2+ Max. Temperature Color Observation 10 g 0.100000 250 C Blue and orange at the bottom of flask 10 grams of Zn in 0.1M Cu(NO3)2 Zn (g) Cu (g) Zn2+ Cu2+ Max. Temperature Color Observation 9.67310 g 0.317730 g 0.100000 Around 0 Around 300 C White/ transparent 10 grams of Pb in 0.1M Cu(NO3)2 Pb (g) Cu (g) Pb2+ Cu2+ Max. Temperature Color Observation 8.96400 g 0.317729 g 0.0999996 3.92983e-7 About 270 C White/ transparent 10 grams of Mg in 0.1M Cu(NO3)2 Mg (g) Cu (g) Mg2+ Cu2+ Max. Temperature Color Observation 9.87850 g 0.317730 g 0.100000…IWrite balanced equations for the following reactions in basic solution: SO2 + I2 resulting in SO2 + SO3 +1 to the -1 Zn + NO3 to the -1 resulting in NH3 +Zn to the +2 ClO to the -1 + 4CrO2 Write balanced equations for the following reactions in acid solution: Ni to the +2 + IO4 to the -1 resulting in Ni to the =3 + 1 to the -1 O2 + Br to the -1 resulting in H2O + Br2(I) Ca + Br to the 1 resulting in H2O (I) + Br2 (I) Ca + Cr2O7 to the -2 resulting in Ca to the +2 + Cr to the +2