1.7. Calculate the concentration of free Ca2+ in a solution of 0.10 M CaY² at pH 6. Kf for CaY2 is 4.9x1010 and a = 0.36. a. 1.76 x 1010 b. 6.8 x 104 c. 2.4 x 10-6 d. 3.0 x 10 4
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- 5. What concentration of acetate ion (CH3CO2') in 0.500 M CH3CO2H produces a buffer solution with pH = 5.00? (Ka = 1.8 x 10-5) CH;CO2H (aq) H20 (I) CH;CO, (aq) H30* (aq) + 6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH;CO2H) to 1.00LH,0. What is the pH of the solution at equilibrium? (K, 1.8 x 10°)100.0 mL of a 0.50 M aqueous NH3 solution is mixed with 200.0 mL of 0.25 M aqueous HCl. At 25 °C the mixture will have a pH of OA.7.00 O D. Cannot be predicted without the K values.5. a. Write an equation to show that HPo, (aq) can act as a Brønsted base in water. b. Label the species in (a) as acid, base, conjugate a cid and conjugate base respectively c. For the following equilibrium at 298 K, the equilibrium constant К- 2.84 х 10 2 М. Ag PO45) + H,O() = 3Agʻ(aq) + HPO, (aq) + OH (aq) Calculate the concentration of Ag in 0.10 M HPO. solution at pH 10.
- 6. Consider the equation: 2A(aq) + B(aq) = 2C(aq)+ 3D(aq) When 25.0 mL of 0.065 M B is combined with 35.0 mL of 0.0900 M A and allowed to reach equilibrium, the concentration of D is observed to be 0.0395 M. Calculate the equilibrium constant.thermodynamics3. The solubility of CsF2(s) in water is 2.1 x 104 M. Calculate its Kap.
- 3. Calculate the solution pH and the species concentrations for a solution containing 1 mM Na:CO; when the followings are added to the solution in a closed system. Assume that the volume change as a result of the acid addition is negligible. a. 1 mM HNO3 is added b. 2 mM HNO, is addedAt a certain temperature 0.0050 g of BaF2 dissolves in 100.0 mL of water. A. Calculate the molarity of this solution. (S) B. Calculate the Ksp of BaF2 at this temperature.what unit should my k constant be？？
- GW 17 1. A 0.36 M hydrocyanic acid (HCN) solution has a pH of 4.87. Give: (a) the balanced equation for the ionization of hydrocyanic acid; (b) K, of HCN; (c) % ionization of HCN. a. b. 114 с.1. A. Determine Ksp for silver phosphate, Ag.PO4, given a molar solubility of 2.7 x 10“ M. B. Calculate the molar solubility of lead (II) chloride, P6C12, in a 0.250 M solution of CaCl2(aq). Ksp for PbCl2 = 1.6 x 10%. C. Describe the effect on the solubility of lead (II) chloride and silver phosphate by the acidification of solution. Discuss both salts in your answer.A buffered solution containing dissolved aniline, C,H,NH,, and aniline hydrochloride, C,H;NH,CI, has a pH of 5.50. A. Determine the concentration of C,H,NH in the solution if the concentration of C,H,NH, is 0.305 M. The pKp of aniline is 9.13. 0.07 |C,H,NH¡] = M Incorrect B. Calculate the change in pH of the solution, ApH, if 0.374 g NaOH is added to the buffer for a final volume of 1.05 L. Assume that any contribution of NaOH to the volume is negligible. 11.95 ApH =| Incorrect