Homework Answers
HCN(aq) <----> H+(aq) + CN-(aq); Ka = 6.2*10-10
AgCN(s) <----> Ag+(aq) + CN-(aq); Ksp = 2.2*10-16
Ag+(aq) + 2CN-(aq) <----> [Ag(CN)2]-(aq); Kf = 1020.48 = 3.02*1020
Yes, there is a single equilibrium that describes all the above equilibria.
HCN(aq) + AgCN(s) <----> [Ag(CN)2]-(aq) + H+(aq); K = Ka * Ksp * Kf = 6.2*10-10 * 2.2*10-16 * 3.02*1020 = 4.12*10-5
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1) A solution that is 500 molar HCN, K.-6.2 x 10-10 is in equilibrium with solid...
hint: 5 rans use 3, lworth 5pts). solution that is .500 molar HCN, K= 6.2 x 10-10, is in equilibrium with solid sil...
hint: 5 rans use 3, lworth 5pts). solution that is .500 molar HCN, K= 6.2 x 10-10, is in equilibrium with solid silver (1) de, Ksp = 2.2 x 10-16. However, it is known that silver (1), Ag, can complex under certain ons with CN to produce the silver (1) dicyano complex, [Ag(CN)2]', log Kr=20.48. what are all of the equilibrium reactions that are occurring in this solution? Is there a single overall reaction that can describe the equilibria in...
Problem 2: Find the concentrations of Ag, CN, and HCN in a saturated solution of AgCN...
Problem 2: Find the concentrations of Ag, CN, and HCN in a saturated solution of AgCN whose pH is somehow fixed at 9.00. Consider the following equilibria: Ksp = 2.2 x 10-16 AgCN(s) CN + H20 Ag+ + CN- HCN(aq) + OH- Kb = 1.6 x 10-5
Problem 2: Find the concentrations of Agt. CN. and HCN in a saturated solution of AgCN...
Problem 2: Find the concentrations of Agt. CN. and HCN in a saturated solution of AgCN whose pH is somehow fixed at 9.00. Consider the following equilibria: AgCN() ► Ag+ + CN- CN + H20 HCN(aq) + OH Ksp = 2.2 x 10-16 Kb = 1.6 x 105
8. The ionization constant, Ka, for HCN(aq) is 6.2 x 10". What is the pH of...
8. The ionization constant, Ka, for HCN(aq) is 6.2 x 10". What is the pH of a 0.10 molar solution of sodium cyanide, which contains the cyanide ion? a. 5.10 b. 8.90 c. 9.21 d. 11.10 e. 11.30 9. The solubility product for Ag3PO, is: Kop = 2.8 x 101 What is the solubility of Ag,PO, in water, in moles per liter? a. 1.8 x 10M b. 2.5 x 10M c. 1.9 x 10 M d. 3.1 x 10M e....
H. Complex Ions 1. Silver chloride has very low solubility in water (Ks of 1.6 x...
H. Complex Ions 1. Silver chloride has very low solubility in water (Ks of 1.6 x 10-19), however, it is highly soluble in an ammonia solution due to the formation of the complex ion [Ag(NH3)21 (Kr" 1.7 X 10) Given this information, calculate the molar solubility of AgCl in 2.25 M ammonia. 2. Calculate the molar solubility of Cul in 0.92 M KCN. (Ksp of Cul is 1.1 x 10-12, Kp of [Cu(CN)2] is 1.0 x 1016).
Determine [Zn2 ], [CN–], and [HCN] in a saturated solution of Zn(CN)2 with a fixed pH...
Determine [Zn2 ], [CN–], and [HCN] in a saturated solution of Zn(CN)2 with a fixed pH of 2.160. The Ksp for Zn(CN)2 is 3.0 × 10–16. The Ka for HCN is 6.2 × 10–10. Hint: Use the systematic treatment of equilibrium to solve this problem. 1. Write the pertinent reactions. 2. Write the charge balance equation. 3. Write the mass balance equations. 4. Write the equilibrium constant expressions for each reaction. 5. Count the equations and unknowns. 6. Solve for...
What is the pH of a 2.50 molar solution of NaCN(aq)? KA (HCN) = 6.2×10^-10 a....
What is the pH of a 2.50 molar solution of NaCN(aq)? KA (HCN) = 6.2×10^-10 a. 11.80 b. 9.60 c. 9.21 d. 4.40 e. 2.20 A. is the correct answer
1. Calculate the molar solubility of LaF; in each of the following (Ksp. LaF3 = 2.0x10-19)....
1. Calculate the molar solubility of LaF; in each of the following (Ksp. LaF3 = 2.0x10-19). a) pure water b) 0.50 M NaF c) 0.25 M La(NO3)3 The Kan of Cul is 1.1x10 and the Krfor the [Cu(CN), complex ion is 1.0x1024 Write the equilibrium reaction associated with the given K value b) Write the equilibrium reaction associated with the given Kr value. Find the final concentration of cyanide ion in a solution containing excess Cul and 0.60 M NaCN.
NH4+ ka =5.69x10 HCN ka=6.2 x 10-1 Given the follo be there following the What will...
NH4+ ka =5.69x10 HCN ka=6.2 x 10-1 Given the follo be there following the What will Laathe aqueous approximate pH of an solution of ammonium cyanide NHAEN rimonium a) slightly basic b) slightly acidic c) nearly neutral
Given that K, for HCN is 6.2 x 10-10 at 25 °C, what is the value...
Given that K, for HCN is 6.2 x 10-10 at 25 °C, what is the value of Ky for CN- at 25 °C? Given that Kh for CH, NH, is 5.0 x 10-4 at 25 °C, what is the value of K, for CHNHĨ at 25 °C? Kg =
hint: 5 rans use 3, lworth 5pts). solution that is .500 molar HCN, K= 6.2 x 10-10, is in equilibrium with solid silver (1) de, Ksp = 2.2 x 10-16. However, it is known that silver (1), Ag, can complex under certain ons with CN to produce the silver (1) dicyano complex, [Ag(CN)2]', log Kr=20.48. what are all of the equilibrium reactions that are occurring in this solution? Is there a single overall reaction that can describe the equilibria in...
Problem 2: Find the concentrations of Ag, CN, and HCN in a saturated solution of AgCN whose pH is somehow fixed at 9.00. Consider the following equilibria: Ksp = 2.2 x 10-16 AgCN(s) CN + H20 Ag+ + CN- HCN(aq) + OH- Kb = 1.6 x 10-5
Problem 2: Find the concentrations of Agt. CN. and HCN in a saturated solution of AgCN whose pH is somehow fixed at 9.00. Consider the following equilibria: AgCN() ► Ag+ + CN- CN + H20 HCN(aq) + OH Ksp = 2.2 x 10-16 Kb = 1.6 x 105
8. The ionization constant, Ka, for HCN(aq) is 6.2 x 10". What is the pH of a 0.10 molar solution of sodium cyanide, which contains the cyanide ion? a. 5.10 b. 8.90 c. 9.21 d. 11.10 e. 11.30 9. The solubility product for Ag3PO, is: Kop = 2.8 x 101 What is the solubility of Ag,PO, in water, in moles per liter? a. 1.8 x 10M b. 2.5 x 10M c. 1.9 x 10 M d. 3.1 x 10M e....
H. Complex Ions 1. Silver chloride has very low solubility in water (Ks of 1.6 x 10-19), however, it is highly soluble in an ammonia solution due to the formation of the complex ion [Ag(NH3)21 (Kr" 1.7 X 10) Given this information, calculate the molar solubility of AgCl in 2.25 M ammonia. 2. Calculate the molar solubility of Cul in 0.92 M KCN. (Ksp of Cul is 1.1 x 10-12, Kp of [Cu(CN)2] is 1.0 x 1016).
1. Calculate the molar solubility of LaF; in each of the following (Ksp. LaF3 = 2.0x10-19). a) pure water b) 0.50 M NaF c) 0.25 M La(NO3)3 The Kan of Cul is 1.1x10 and the Krfor the [Cu(CN), complex ion is 1.0x1024 Write the equilibrium reaction associated with the given K value b) Write the equilibrium reaction associated with the given Kr value. Find the final concentration of cyanide ion in a solution containing excess Cul and 0.60 M NaCN.
NH4+ ka =5.69x10 HCN ka=6.2 x 10-1 Given the follo be there following the What will Laathe aqueous approximate pH of an solution of ammonium cyanide NHAEN rimonium a) slightly basic b) slightly acidic c) nearly neutral
Given that K, for HCN is 6.2 x 10-10 at 25 °C, what is the value of Ky for CN- at 25 °C? Given that Kh for CH, NH, is 5.0 x 10-4 at 25 °C, what is the value of K, for CHNHĨ at 25 °C? Kg =
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