Calculate the number of moles of Ag+ in 2.00 mL of 0.0049 M AgNO3
Part A Calculate the number of moles of Ag+ in 5.00 mL of 4.00x10-3 M AgNO3 and the number of moles of Crof. in 5.00 mL of 3.50x10-3 M K Cr04. Input your answers separated by a comma. PO AJO O O ? Submit Request Answer - Part B If 5.0 mL of 4.00x10-3 M AgNO3 is added to 5.0 mL of 3.50x10-3 M K, CrO4, is either Ag+ or CrO2 in stoichiometric excess? If so, which is in excess?...
Part A Calculate the number of moles of Ag+ in 5.00 mL of 2.00x10-3M AgNO3 and the number of moles of Crok in 5.00 mL of 3.50x10-3 M K Cr04. Input your answers separated by a comma. IPO AQ R o 2 ? mol Submit Request Answer
Calculate the number of moles of Ag^+ in 6.0 mL of 0.004M AgNO_3 and the number of moles of CrO_4^- in 6.0 mL of 0.0024 M K_2CrO_4.
Calculate the equilibrium concentration of Ag+(aq) after 10.0 mL of 0.100 M AgNO3(aq) have been mixed with 10.0 mL of 1.00 M NaCN(aq).
We want to determine the concentrations of Ag+, CN-, and Ag(CN)2- when 10.0 mL of 2.00 M KCN is mixed with 10.0 mL of 0.0200 M of AgNO3. Kf for Ag(CN)2- = 1.0 x 1021 a) What is the initial concentration of Ag ion (in M) after mixing but before reaction or equilibrium is established? b) What is the initial concentration of Ag ion (in M) after mixing but before reaction or equilibrium is established?
Consider the titration of 25.00 mL of 0.07920 M KI with 0.05410 M AgNO3. Calculate pAg+ at a) 25.00 mL > ?? b) Ve > M1V1 = M2V2 (0.07920)(0.025)=(0.05410)(Ve) --------> Ve = 36.60 mL c) 45.00 mL > ?? of AgNO3 added (Ksp= 8.3*10-17). Show ALL work. pAg+ = -log[Ag]
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 solution is prepared by mixing 47.00 mL of 0.024 M AgNO3 with 11.00 mL of 1.0×10-3M Na2CO3. Assume that volumes are additive. Calculate [Ag+], [CO32–], [Na+], and [NO3–] after equilibrium is established. [Ag+]= [CO32+]= [Na+]= [NO3-]=
Calculate the equilibrium concentration of Ag (aq) in a solution that is initially 0.140 M AgNO3 and 0.600 MNH3, and in which the following reaction takes place: Ag (ag)+2NH3 CaAg(NH3(aq) (K-1.7010) M Agt
Calculate the number of moles of solute in 2.00 L of 15.0 M H2SO4, concentrated sulfuric acid.