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°)Let an n-protic acid be an acid that can donate n hydrogen ions and has the formula HnX.If 0.900 L of 0.400 M sodium hydroxide is required to titrate 0.400 L of a 0.300 M HnX to theequivalence point, what is n in HnX?A. 1B. 2C. 3D. 4E. 5100.0 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.
- 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.what unit should my k constant be？？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.
- One strategy for dealing with the acidification of lakes is periodically to add powered limestone (CaCO3) to them, resulting in pH of 10.95. Calculate the Ca2+ concentration in the lake. CO2 in atmosphere 370 ppm KH,CO2 = 0.033 mol/(L∙atm) Ka1 = 10-6.3 Ka2 = 10-10.3 Ksp,CaCO3 = 4.57 x 10-9g.135.The solubility-product constant for Ce(IO3)3 is 3.2 X 10-10. What is the Ce3+ concentration in a solution prepared by mixing 50.0 mL of 0.0250 M Ce3+ with 50.00 mL of water?a. 0.040 M IO3- ?
- 1.Calculate the normality of the solutions containing 5.267g/L K2Cr2O7 (the Cr is reduced to Cr3+).(FW=294.19 g/mol) 2.A and B react as follows: A + B 2C. The equilibrium constant is 5.0 x 106. If 0.40 mol of Aand 0.70 mol of B are mixed in 1L, what are the concentrations of A, B and C after reaction? 3. The following data is given at a certain temperature:(1) 2N2 (g) + O2 (g) 2N2O (g) K1 = 1.2 x 10-35(2) N2O4 (g) 2NO2 (g) K2 = 4.6 x 10-3(3) ½N2 (g) + O2 (g) NO2 (g) K3 = 4.1 x 10-9Calculate the molar equilibrium constant, K for the reaction:2N2O (g) + 3O2 (g) 2N2O4 (g)5. Is Ethyl 3-Aminobenzoate more soluble in 10% HCl(aq) or 10% NaOH(aq)? Briefly explain by writing a balance equation.Consider the titration 35.0mL of 0.250M methylamine CH NH2 and 0.200 M HNO3. K. = 5.9 x 104 a. Determine the pH at the midpoint b.Determine the pH when 25.0 mL of titrant was added.