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.
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?
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 1.1 x 10-3 M in Zn(NO3)2 and
0.150M in NH3. After thw solution reaches equilibrium, what
concentration of Zn2+ (aq) remains? Look up the values
of Kf in your book on page 779 (Table 17.3).
Complex Ion K Complex Ion K 1.7 x 1013 Ag(CN)2 1 X 1021 Cu(NH3)4 Ag(NH3)2+ 1.7 x 107 1.5 x 1035 Fe(CN)64 Fe(CN)63 Ag(S203)23 2.8 x 1013 2 x 1043 AIF 3 7 x 1019 Hg(CN). 1.8 X 1041 Al(OH)4 3...
Question 2 A solution contains 1.1 x 10-4 M in Zn2+ and 0.150 M in NH3. If the Kf for (Zn(NH3)4]2+ is 2.8*10%, how much zinc ion remains at equilibrium? Zn2+ + 4NH3 + [Zn(NH3)412+ A 8.9x10-12M B. 7.8 x1011 M C 8.7x10-10M 0.4.7x10-13 1.1x1019M
3. The Ksp for silver chloride is 1.8 x 10-10 at 25 °C. What is the solubility of silver chloride (in mol L"?) in 0.025 M tin(IV) chloride solution? a) 8.5 x 10-5 b) 6.7 x 108 c) 7.2 x 10-9 d) 1.8 x 10-9 e) 1.3 x 10-5 4. What is the concentration of Zn2+(aq) ions in the solution made by adding water to zinc nitrate (0.10 mol) and ammonia (3.0 mol) so that the final volume of solution...
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.
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?
5. A solution is made by mixing 200.0 ml of 1.5 x 10-4 M Cu(NO3)(aq) with 250.0 ml of 0.20 M NH3(aq). Calculate the concentration of copper ion (Cu? (aq)) in the solution when it reaches equilibrium. (Kr for [Cu(NH3)4]2+ = 1.7 x 1013)
15.0 mL of 0.50 M NaOH is added to a 100.-mL sample of 0.442 M NH3 (Kb for NH3 = 1.8 x 10–5). What is the equilibrium concentration of NH4+ ions?
Consider the cell: Zn(s)ǀ(Zn2+(0.20 M)ǁCu2+(0.20 M)ǀCu(s) with Eº(Cu2+/Cu = 0.34 v and Eº(Zn2+/Zn) = –0.76 v a) Write the cell reaction which occurs when the cell produces current and calculate Ecell. b) If each cell compartment contains 25.0 mL of the corresponding metal salt solution and 25.0 mL of 3.00 M NH3(aq) is added to the Cu2+ solution, Ecell = 0.68 v. Use these data to calculate Kf for Cu(NH3)42+. Cu2+(aq) + 4 NH3(aq) ⇄ Cu(NH3)42+