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Part A A 110.0-mL sample of a solution that is 2.7 x 10- M in AgNO,...
A 130.0 mL sample of a solution that is 2.8time 10^-3 M in AgNO, is mixed with a 230 0 - mL sample of a solution that is 0.12 M in NaCN. After the solution reaches equilibrium, what concentration of AG^+ (aq) remains? Express your answer using two significant figures.
A 115.0 −mL sample of a solution that is 2.9×10−3 M in AgNO3 is mixed with a 225.0 −mL sample of a solution that is 0.11 M in NaCN. After the solution reaches equilibrium, what concentration of Ag+(aq) remains?
A 50 mL sample of 2.2 x 10^-4 M CuNO3 is added to 50 mL of a 4.0 M NaCN. Cu^+ reacts with CN^- to form the complex ion Cu(CN)3^2- according to Cu^+(aq) + 3CN^-(aq) <--> Cu(CN)3^2- , Kf= 1.0 x 10^9 determine the concentrations of CN^-, Cu^+, Cu(CN)3^2- at equilibrium
You mix a 140.0 −mL sample of a solution that is 0.0146 M in NiCl2 with a 175.0 −mL sample of a solution that is 0.250 M in NH3. Part A After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? The value of Kf for Ni(NH3)62+ is 2.0×10^8 Express the concentration to two significant figures and include the appropriate units.
When 1.24 g of AgNO3 (169.1 g mol-1) is dissolved in 245 mL of 0.150 M NaCN, what are [Ag+], [Ag(CN)2-], and [CN-] at equilibrium? Kf of Ag(CN)2- = 1.0 x 1021.
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?
You mix a 105.0 −mL sample of a solution that is 0.0130 M in NiCl2 with a 185.0 −mL sample of a solution that is 0.300 M in NH3. After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? The value of Kf for Ni(NH3)62+ is 2.0×108.
When 100 mL of 1.0 M Na₃PO₄ is mixed with 100 mL of 1.0 M AgNO₃, a yellow precipitate forms and [Ag⁺] becomes negligibly small. Which of the following is a correct listing of the ions remaining in solution in order of increasing concentration? (A) [PO₄³⁻] < [NO₃⁻] < [Na⁺] (B) [Na⁺] < [NO₃⁻] < [PO₄³⁻] (C) [Na⁺] < [PO₄³⁻] < [NO₃⁻] (D) [PO₄³⁻] < [Na⁺] < [NO₃⁻] (E) [NO₃⁻] < [PO₄³⁻] < [Na⁺]
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...
Review Constants Periodic Table You mix a 120.0-ml sample of a solution that is 0.0134 M in NiCl, with a 195.0-ml sample of a solution that is 0.500 Min NH You may want to reference Pages 778 - 783) Section 17.7 while completing this problem Part A After the solution reaches equilibrium, what concentration of Ni2+ (aq) remains? The value of K for Ni(NH4)2 | 2.0 x 10*. Express the concentration to two significant figures and include the appropriate units....