What are the concentrations at equilibrium of a 0.15 M solution of HCN? What will be the concentration of Cu2+(aq) at equilibrium? HCN(aq)<=>H+(aq) + CN–(aq) , Kc= 4.9 x 10-10
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What are the concentrations at equilibrium of a 0.15 M solution of HCN? What will be...
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
Calculate the pH and equilibrium concentrations of a 0.46M salt solution of sodium cyanide NaCN in water. Write the balanced chemical reaction(s) and show your work. Ka(HCN) = 4.0x10-10. For the concentrations, input only the numeric answer. What is the pH? What is the HCN concentration? What is the CN- concentration? What is the OH- concentration? What are the units of concentration?
What are the equilibrium concentrations? Equation
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2. (10 pts) For the reaction (aq) the equilibrium constant is Kc 3.0 x 10's at 25 oC. If the initial concentration of IHA is 0.100 M, what are the equilibrium concentrations of HA, H3o and A"?
For the reaction: N2 (g) + C2H2 (g) 2 HCN (g), Kc is 2.3x10-4 at 300 ºC. What are the equilibrium concentrations of all species if the initial concentration of HCN was 5.0 M?
5) The molecular complex Cu(CN)42- dissociates in water by the process Cu(CN) + (aq) = Cu2+ (aq) + 4 CN- Kc = 9.5 x 10-17 The initial concentration of Cu(CN)4- in an aqueous solution is 0.0390 M. No Cu?" or CN ions are initially presen. What is the concentration of Cu2+ ion present when equilibrium is achieved? [12 points)
A titration is performed on a 25 mL sample of 0.15 M HCN (Ka = 4.9 x 10–10) with 0.30 M NaOH. Which of the following is the pH of the solution after 15 mL of NaOH is added?
Acid-Base Titration: A 0.15 M solution of NaOH is used to titrate 200.0 mL of 0.15 M HCN. What is the pH at the equivalence point? Ka = 4.9 x 10-10. Please include steps/work so I can see and understand how this problem is solved.
14. What are the final concentrations of A and A, at equilibrium if the initial (A) concentration is 0.60M? K-4.2 x 10* As (g) 2A(8) Initial: 0.60 Equilibrium: 15. Find final equilibrium concentrations for HA, H', and A: HA(aq) + H20 (1) HO" (aq) + A' (aq) Initial Concentrations 0.60 M OM ом K.-2.0 x 10 **Remember to review Properties of liquids (solubility, intermolecular forces, colligative properties, concentration units), phase diagrams, phase changes and the energy associated with heating and...
Introduction to Qualitative Analysis Post-Lab Questions: (show logic for full credit) 1. Write the equilibrium-constant expression for each of the following reactions. Remember how to handle the concentrations of solids or water. a. N_(g) + 3H2(g) + 2NH,(g) b. HCN(aq) H(aq) + CN (aq) c. PbCl(s) Pb2"(aq) + 2Cl(aq) d. NH3(aq) + H2O(l) = NH,'(aq) + OH (aq) e. HF(aq) = H'(aq) + F(aq) 2. 2. What is the pH of a solution if [H'] = 2.0 x 10 M?...