When 20.0 mL of 0.200 M Zn(NO3)2 is added to 30.0 mL of 6.00 M NH3, the concentrationn of Zn2+ at equilibrium is 1.00 x 10-13. What should the Kf of Zn(NH3)42+ be reported as?
See they have given equilibrium Conc of Zn+2 is 10^-13
And it is very less compared to initial value of zn+2 i.e 4*10^-3
So I assumed that zn+2 almost converted product
When 20.0 mL of 0.200 M Zn(NO3)2 is added to 30.0 mL of 6.00 M NH3,...
When 1.8 x 10-3 mol of Zn is added to 300 mL of 1.5 M NH3, [Zn2+] = ___ M when the system reaches equilibrium. For [Zn(NH3)4]2+, Kf = 2.9 × 10^9.
Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2. Then 10.0 mL of 0.300 M NH3 is added. What are the molar concentrations of Ni2+, NH3, and [Ni(NH3)6]2+ at equilibrium? Kf for [Ni(NH3)6]2+ = 2.0 x 10^8
Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2.. Then 10.0 mL of 0.300 M NH3 is added. What are the molar concentrations of Ni2+, NH3, and [Ni(NH3)6] 2+ at equilibrium? Kf for [Ni(NH3)6] 2+ = 2.0 x 10^8
Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2.. Then 10.0 mL of 0.300 M NH3 is added. What are the molar concentrations of Ni2+, NH3, and [Ni(NH3)6]2+ at equilibrium? Kf for [Ni(NH3)6]2+ = 2.0 x 108
Consider titration of 20.0 mL of 0.100 M NH3 with 0.200 M HCl solution. Calculate the pH after the addition of the following volumes of HCl solution. The Kb of NH3 = 1.8 x 10^5 a. 0.00 mL b. 6.00 mL c. 10.00 mL d. 20.00 mL
Consider a 100.0 mL sample of 0.0200 M Ni(NO3)2.. Then 10.0 mL of 0.300 M NH3 is added. What are the molar concentrations of Ni2+, NH3, and [Ni(NH3)6]2+ at equilibrium? (8 pts) Kf for [Ni(NH3)6]2+ = 2.0 x 108 PLEASE EXPLAIN, THANKS
5. A solution is made 1.1 x 103 M in Zn(NO3)2 and 0.150 M in NH3. After the solution reaches equilibrium, what concentration of Zn2 (aq) remains?
Calculate the pH when 30.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH3NH2 (Kb = 4.4 x 10-4). Calculate the pH when 90.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH3NH2 (Kb = 4.4 x 10-4).
A solution is made that is 1.5×10−3 M in Zn(NO3)2 and 0.160 M in NH3. After the solution reaches equilibrium, what concentration of Zn2+(aq) remains? Express your answer using two significant figures
A solution is made that is 1.4×10−3 M in Zn(NO3)2 and 0.150 M in NH3. After the solution reaches equilibrium, what concentration of Zn2+(aq) remains? Express your answer using two significant figures.