Q 1. At 291 K, the equivalent conductivities at infinite dilution of HCl „NaCl and CH3COONA are 369.3, 101.7 and 1.7 S cm2eq-1 respectively. If equivalent conductivity of centinormal solution of acetic acid is 14.3 S cmzeq-1, [H+]in solution of acetic acid is Xx104. Calculate of Value of X?
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- Q 1. At 291 K, the equivalent conductivities at infinite dilution of HCI NaCl and CH3COONA are 369.3, 101.7 and 1.7 S cm2eq-1 respectively. If equivalent conductivity of centinormal solution of acetic acid is 14.3 S cmzeq 1, [H+] in solution of acetic acid is Xx10 . Calculate of Value of X?Q1. Dissolved 0.273 grams of pure sodium oxalate (Na,C,O.) in distilled water and added sulfuric acid and titration the solution at 70 ° C by using 42.68 ml of KMNO, solution and has exceeded end point limits by using 1.46 ml of standard oxalic acid (H; C;O.) with 0.1024 N. Calculate the normlity of KMN0.. Note that the molecular weight of sodium oxalate (Na,C,O.) = 134 and its equivalent weight = 67Average activity coefficient for HBr at 25oC for three different diluted solutions is 0.930 (at m = 5.0 mmol kg-1), 0.907 (at m = 10.0 mmol kg-1), and 0.879 (at m = 20.0 mmol / kg-1) has been given. Calculate the approximate value of the constant B in the expanded Debye Hückel law.
- The mean activity coefficient in an 0.050 molKg-1 LaCl3 (aq) solutions is 0.303 at 25 o C. What is the percentage error in the value predicted by the debye – Huckel limiting law?Q: The concentration of the sulphate ion in a mineral water can be determinedby the turbidity which results from the addition of excess BaCl2, to a quantityof measured sample. A turbidometer used for this analysis has been standardisedwith a series of standard solutions of NaSO4. The following resultswere obtained:Standard solution Conc. (SO4)2− (mg/L) Reading of turbidometerS0 0.00 0.06S1 5.00 1.48S2 10.00 2.28S3 15.00 3.98S4 20.00 4.61i. In supposing that a linear relationship exists between the readings takenfrom the apparatus and the sulphur ion concentration, derive an equationrelating readings of the turbidometer and sulphate concentration(method of least squares).ii. Calculate the concentration of sulphate in a sample of mineral waterfor which the turbidometer gives a reading of 3.67.Calculate the mean ionic molality for 0.25m LaCls. [Ans. 1.1914 m] 570 nsmer For aqueous HCl solutions, it can be determined: Y- =0.72515 + 0.029188m + 0.055959m Determine the molality at which auCi= 1. (Note: This is the molality for the standard state of HCL in Water; pHCI) [Ans. 1.1914 m] %3D
- 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.dm3Calculate the solubility of silver acetate.1 (CH;COOA9) in water at 25 °C, assuming * .the DHLL to apply; Ksp = 0.004 M²9. The molar conductivity values at infinite dilution, in units of Sm?mol1, of NHẠCI, NaCl and N2OH are 1.497 x 10², 1.2645 x 10² and 2.478 x 10², respectively. (a) Calculate the molar conductivity at infinite dilution of NH4OH. (b) The molar conductivity of 0.0100 moldm3 NH,OH is 1.13 x 103 Sm?mol. What is the degree of dissociation and the dissociation constant, Kp, of 0.0100 moldm3 NHẠOH?
- Calculate the molar concentration of FeSCN2+ in solution #3. The determined molar absorptivity of the solution at 448 nm is 333 L mol-1 cm-1.The mean activity coefficients of HBr in three dilute aqueous solutions at 25 °C are 0.930 (at 5.0 mmol kg-1), 0.907 (at 10.0 mmol kg-1), and 0.879 (at 20.0 mmol kg-1). Estimate the value of B in the Davies equation.Calculate the values expected for the total alkalinity and for the phenol- phthalein alkalinity of a 25°C saturated solution of calcium carbonate in water, and compare them to the values for a solution that also is in equilib- rium with atmospheric carbon dioxide. Use the concentrations quoted in the last column of Table 10-4.