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tl See Periodic Table See Hint Calculate the equilibrium concentration of Ag (aq) in a solution...
Iul See Periodic Table See Hint Calculate the equilibrium concentration of Ag (aq) in a solution that is initially 0.120 M AgNO, and 0.840 MNH3, and in which the following reaction takes place: Ag (aq) + 2NH, (aq) (NH)2(aq) (K - 1.70.10) M Ag One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that is 0.500 M in ammonia The formation constant of Ni(NH3)2 is 5,5x10% 1st attempt Part 1 (1 point) i See Periodic Table See Hint...
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 equilibrium concentration of Ag+ (aq) in a solution that is initially 0.200 M AgNO3 and 0.200 M KCN. The formation constant for [Ag(CN)2] (aq) is Ka= 1.0 x 10^21. Show your work for each step. a. 5.6 x 10^-22 M b. 5.0 X 10^-22 M c. 3.3 x 10^-33 M d. 1.0 x 10^-30 M e. 1.3 x 10^-21 M
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).
The equilibrium constant for the equation Ag+ (aq) + 2NH, (aq) =[Ag(NH),]+(aq) is Kf = 2.5 x 103 M-2 at 25.0 °C. Calculate the value of AGixn at 25.0 °C. C AG = k Is the reaction spontaneous under standard conditions? kJ/mol J/mol no O yes Calculate the value of AGrxn at 25.0 °C when [Ag+] = 0.00138 M, (NH2) = 0.438 M, and [[Ag(NH3)2]+] = 0.00739 M. Is the reaction spontaneous under these conditions? AGrxn = kJ/mol O yes...
"calculate the concentration of Ag+ present in a solution at equilibrium when concentrated ammonia is added to a 0.010m solution of AgNO3 to give an equilibrium concentration of (NH3)= 0.20 m. Neglect the small volume change that occurs when NH3 is added
See Periodic Table See Hint The concentration of Pb2+ in a commercially available standard solution is 1.00 mg/mL. What volume of this solution should be diluted to 4.0x10 ml. to produce a solution in which the concentration of Pb2+ is 0.050 mg/L? mL
1st attempt See Periodic Table See Hint A 1.00 L solution contains 2.00x104 M Cu(NO3)2 and 2.500x10 M ethylenediamine (en). The Ky for Cu(en)22 is 1.00x1020 What is the concentration of Cu2(aq) in the solution?
We have a solution that has a concentration of 0.348 M for A(aq) and 0.619 M for B(aq). There are no other solutes initially. The reaction 2 A(aq) + B(aq) <---> 2 C(aq) + D(aq) takes place. At equilibrium, the concentration of C(aq) is 0.142 M. What is the equilibrium constant of this reaction? Please use at least 5 decimal places in calculations.
2nd attempt See Periodic Table See Hint Feedback Write a chemical equation for the hydrolysis reaction that explains why an aqueous solution of CH3NH3Cl is acidic. [Please include the states of matter with each chemical species. Remember, it is an equilibrium reaction.] xx. He (aq).