help please! 4. You added 0.05 mL of 0.10 M AGNO3 to 4.0 mL of 2.0...
4. You added 0.05 mL of 0.10 M AgNO, to 4.0 mL of 2.0 M NaCl, and formed a saturated solution of AgCl (s): AgCl (s) 7 Ag+ (aq)+CF (aq) K=Ksp Using this saturated solution as the test solution you set up the following cell AgAg (test solution after reaction)||Ag (1.0M) Ag and measured Ecell = 0.61 V. (a) Using the measured value of Ecell and Eq (15), calculate the equilibrium (Ag l (i.e. of the test solution after reaction)....
PRELAB ASSIGNMENT (CO 4. You added 0.05 mL of 0.10 M AgNO, to 4.0 mL of 2.0 M NaCl, and formed a saturated solution of AgCl (s) AgCl (s) Ag+ (aq)+ Cl-(aq) Using this saturated solution as the test solution you set up the following cell and measured Ecell = 0.61 V (a) Using the measured value of Eell and Eq (15), calculate the equilibrium [Ag'] (i.e. of AglAg' (test solution after reaction)lAg (1.0M)Ag the test solution after reaction). (1...
Help please! The subscript c on the E and n refers to the cathode and a refers to the anode and EP, E, ne and n, are obtained from the Chemistry Data Sheet. Combining (13) and (14) with Eq. (11) gives Een – Es – Ex = {E: -0.0592 109 Reumot} - {E:- 0.092 108 Quote} (15) V-12 EXPERIMENT V: VOLTAIC CELLS, AND THE NERNST EQUATION PRELAB ASSIGNMENT (CONTINUED) 4. You added 0.05 mL of 0.10 M AgNO3 to 4.0...
Muyuulin (1JJ. Part III: Determination of a Solubility Product In Part Ill you will prepare a saturated solution of silver carbonate (Ag2CO3) and deten solubility product constant of Ag2CO3. Ag2CO3(s) = 2 Agt(aq) + CO32-(aq) (17) In making the solution, 1.0 mL of 0.10 mol/L AgNO3 will be added to specified volume mol/L Na2CO3. The limiting reagent in this reaction will be the silver ions. Use of an excess an of anion allows for a relatively simple calculation of the...
Suppose that 51.0 mL of 0.11 M AgNO3 is added to 50.0 mL of 0.048 M NaCl solution. (a) What mass of AgCl will form? g AgCl the tolerance is +/-2% (b) Calculate the final concentrations of all of the ions in the solution that is in contact with the precipitate. [Ag+] = × 10 M [NO3−] = × 10 M [Na+] = × 10 M [Cl−] = × 10 M (c) What percentage of the Ag+ ions have precipitated?...
5. In the hood, form solid AgCl by adding 1 mL of 6 M HCI (aq) to 1 mL of 0.1 M AgNO3 (aq) in a medium test tube, and then add 1 drop of 15 M NH3 (aq) to establish the equilibrium shown below. AgCI (s) +2 NH3 (aq)Ag(NH3)2 (aq)+CI (aq) Stress 1. Add reactant. Stress 2. Add product. action observation shift right or left Stress 1 Stress 2 What happens to the concentration of CI as reactant is...
4) When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.500 M NH4CI, how many grams of AgCl are formed? (MM AgCI =143.32 g/mol) AgNO3(ag)+ NH4C| (aq) AgCl(s)+ NH4NO3(aq)
A 50.0 mL sample of 0.0639 M AgNO3(aq) is added to 50.0 mL of 0.100 M Naloz(aq). Calculate the (Ag") at equilibrium in the resulting solution. The Kp value for AglO3(s) is 3.17 x 10-8 (Ag"]= [ mol/l
A 100.00mL solution of 0.100 M NaCl was titrated with 0.100 M AgNO3. A SCE indicator electrode (E+=0.241V) was the anode and an Ag wire was the cathode for this precipitation titration. Calculate the voltage after the addition of 65 mL of AgNO3 given that Ksp(AgCl)=1.8x10^(-10). Answer=0.081 V. Please show steps, thank you! :)
hen 170. mL of 0.209 M NaCl(aq) and 170. mL of 0.209 M AgNO3(aq), both at 21.6°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 24.2°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 3.68 ✕ 103 J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the...