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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- 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. A 100 mL sample of 0.13 M trimethylamine, (CH3)3N, aqueous solution is titrated with 0.31 M HCI solution at 25 °C. Kb for (CH3)3N = 6.4 x 10-5. a. Calculate the pH of the solution after 25 mL of HCl solution has been added. b. How many mL of 0.31 M HCl need to be added to the sample to reach the equivalence point? What is the pH at the equivalence point?
- 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.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.6. HOCI is an acid in aqueous solution with Ka = 3.49 x 10-8 at 25.0 °C a. Write the chemical equation for the ionization equilibrium of HOCI in water. Include physical states and appropriate charges. b. 0.35 mol of HOCI is added to 1L of water at 25.0 °C, calculate the pH of the resulting solution. c. Write the chemical equation for the ionization equilibrium of CIO™ in water. Include physical states.6b.
- 2. The molar solubility of sulfathiazole (weak acid) in water is about 0.001 M. a. What is the lowest pH allowable for complete solubility of a 1% solution of sodium sulfathiazole? (Mw = 277) , pKa = 7.12 b. A 5% solution?The weak base propylamine (CH3(CH2)2NH2) has a Kb = 4.7 x10-4. It can be used in some pharmaceuticals and pesticides. A 25.0 mL sample of 0.185 M propylamine solution was titrated with 0.120 M HCl. What is the pH of this solution at the equivalence point? A. 2.23 B. 5.90 C. 2.03 D. 5.70 E. 5.749. Calculate the molar solubility of BaSO4 (Ksp = 1.1 x 1010) in a. water. b. a solution containing 1.0M SO,2- ions