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- 13.48 The cell Pt|H;(1 bar)|HBr(aq)|AgBr(s)|Ag|Pt' at 25°C with HBr molality 0.100 mol/kg has E =0.200 V. Find the activity coefficient y of HBr(aq) at this molality.The conductivity of a 0.0312 M solution of a weak base is 1.53 x 104 Scm'. If the sum of the limiting ionic conductances for BH* and OH-' is 237.0 Scm²mol·' what is the value of the base constant K6? 4.5 x 10s mol.dm (i) 2.3 x 103 mol.dm (iii) 2.89 x 10 mol.dm3 (ii) 1.37 x 10-5 mol.dm3 (iv) (v) 4.78 x 103 mol.dm3(c) 0.02 M CH3COOH solution has a resistance of 240 ohm with a cell constant of 0.366 cm'. Calculate the degree of dissociation and dissociation of CH3COOH at 0.02 M concentration. Given A° HCI, NaCl, CH3COONA are 435, 138 and 99 scm2 mol respectively.
- Calculate the ionic strength of a solution that is 0.040 mol kg−1 in K3[Fe(CN)6](aq), 0.030 mol kg−1 in KCl(aq), and 0.050 mol kg−1 in NaBr(aq).The solubility of salts that contain the conjugates of weak acids increase in acidic solution. Given the reaction of CUCN (Ksp = 3.47 x 10-20) with an acid in the form H3O+ shown below, find the equilibrium constant for this reaction given that Ka HCN = 4.9 x 10-10. CUCN(s) + H:O*(aq) = Cu"(aq) + HCN(aq) + H2O(1)Calculate the equilibrium concentration of Ag*(aq) in a solution that is initially 0.140 M AgNO3 and 0.980 MNH3, and in which the following reaction takes place: Ag*(aq) + 2NH3(aq)= Ag(NH3);(ag) (Kf = 1.70×107)
- A sample of 0.10 M CH3COOH(aq) of volume 25.0 cm3 is titrated with 0.10 M NaOH(aq). The Ka for CH3COOH is 1.8 x 10-5. (a) What is the pH of 0.10 M CH3COOH(aq)? (b) What is the pH after the addition of 10.0 cm3 of 0.10 MNaOH(aq)? (c) What volume of 0.10 M NaOH(aq) is required to reach halfway to the stoichiometric point? (d) Calculate the pH at that halfway point. (e) What volume of 0.10 M NaOH(aq) is required to reach the stoichiometric point? (f) Calculate the pH at the stoichiometric point.(a) (b) The formation constant, Kf, of Ni(CN)2(aq) Ni²+ (aq) + 4 CN¯(aq) ⇒ Ni(CN)²(aq) is 2.1 x 10³¹. We dissolve 0.0444 mol of Ni(NO3)2 in 1.000 L of a 0.777 M solution of NaCN. Make the approximation that the volume remains fixed at 1.000 L. What will be the concentrations of Ni²+ (aq), CN- (aq), and Ni(CN)2(aq) at equilibrium? The temperature is 25.0 °C. For the reaction 2 A(s) = B(g) + 3 C(g), we begin with only pure A(s). We attain equilibrium. At equilibrium, the total pressure is 8.00 atm. What is the value of AG for this reaction? The temperature is 25.0 °C throughout.A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was added
- Calculate the standard Gibbs energy change for the following reactions at 25oC: (a) C2H5OH(l) + O2(g) -> CH3COOH(l) ─+ H2O(l) (b) 2 CO2(g) -> 2 CO(g) + O2(g) Which of the above reactions, as written, is spontaneous at the standard state? Answer: [─ 362.1; +514.4]A fertilizer railroad car carrying 34,300 gallons of commercialaqueous ammonia (30% ammonia by mass)tips over and spills. The density of the aqueous ammoniasolution is 0.88 g>cm3. What mass of citric acid,C(OH)(COOH)(CH2COOH)2, (which contains three acidicprotons) is required to neutralize the spill? 1 gallon = 3.785 L.Calculate the ionic strength of a solution that is 0.2 M in AlCl3, 0.3 M in ZnCl2, 0.3 M in Fe(NO3)3 and 0.2M in Fe(NO3)2.