Calculate the molar conductivity of NH4OH at infinite dilution if the following data are known: A° (NaOH) = 248 x 104 siemen mol1 m?, A° (NaCl) = 126 x 104 siemen mol1 m? win ww m A° (NHẠCI) = 150 x 1044 siemen mol1 m? %3D win
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- A solution is made by dissolving 0.455 g of PbBr2 in 100 g of H2O at 50C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated9. 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?6. If molar conductivity of HCl solution at 25° C is 425 Scm? mol'at infinite dilution. The specific conductance is 3.824 Scm", if degree of dissociation is 90%, what is the concentration of the solution? a) 1 mol/L c) 0.10 mol/L e) 0.9 mol/L b) 10 mol/L d) 0.8 mol/L
- Calculate the molar conductivity of NH4OH at infinite dilution if the following data are known: Λo (NaOH) = 248 x 10-4 siemen mol-1 m2, Λo (NaCl) = 126 x 10-4 siemen mol-1 m2 Λo (NH4Cl) = 150 x 10-4 4 siemen mol-1 m2The equivalent conductance of a 0.0140N solution of chloroacetic acid is 109.0 at 25 degrees C. What is the ionization constant (Ka) of chloroacetic acid?ality al, g. on te ew led ed in X= A solution was prepared by dissolving 140.0 g of KCl in 315 g of water. Calculate the mole fraction of KC1. (The formula weight of KCl is 74.6 g/mol. The formula weight of water is 18.0 g/mol.) Express the mole fraction of KCl to two decimal places. View Available Hint(s) Submit 5 ΑΣΦ Part B - Use the definition of molality 001 mol/ka 12 of 33 ? P Pearson Review I Constants I Periodic Table A solution was prepared by dissolving 140.0 g of KCl in 315 g of water. Calculate the molality of KC1. (The formula weight of KCl is 74.6 g/mol. The formula weight of water is 18.0 g/mol.) Express the concentration of KCl in molality to two decimal places. ▸ View Available Hint(s) >
- D A S cm² mol-¹ Q CH34 8. Which of these electrolyte solutions is expected to give the highest ionic molar conductivity, A? (KCI A°= 150 S cm² mol-¹) (CH3COOH A°= 391 S cm² mol-¹) 0 y=-2219.8x + 150 1 A (mol/cm³)¹2 (c) ¹² A) 5.00 x 10 mol/cm³ KCI B) 5.00 x 105 mol/cm³ KC1 C) 1.00 x 10 mol/cm³ KC1 D) CH3COOH solution with a degree of dissociation of 0.01 E) CH3COOH solution with a degree of dissociation of 0.1 지금 0 y-654.104x+0.00256 CAAccording to the table below answer the following question: Salt pair NaC KC NaNO 3 KNO 3 Equivalent Conductance (mho cm Vequiv) 108.90 130.10 105.33 126.50 KBr 132.30 NaBr is ? 143.8 106.7 153.5 111.10KMnO4 and Na2C2O4 solutions were used in the reactions that took place in a back titration to determine the amount of H2O2 in a sample. Calculate the concentration of H2O2 in the sample (w / v) as% by making appropriate assumptions for the volumes and normality of all these solutions.
- A solution of 1.50 g of solute dissolved in 25.0 mL of H₂O at 25°C has a boiling point of 100.45°C. (a) What is the molarmass of the solute if it is a nonvolatile nonelectrolyte and thesolution behaves ideally (dof H₂O at 25°C= 0.997 g/mL)? (b) Conductivity measurements show the solute to be ionic ofgeneral formula AB₂ or A₂B. What is the molar mass if the solu-tion behaves ideally? (c) Analysis indicates an empirical formulaof CaN₂O₆. Explain the difference between the actual formulamass and that calculated from the boiling point elevation. (d) Find the van’t Hoff factor (i) for this solution.ST5H.1- Suppose the mean ionic activity coefficient for the ions M2* and X- of the ionic compound M1X2 is Y+ = 0.791. If we could somehow magically know that y+ = 0.888 then what is y_? Type your answer..Q3 A: Calculate the equivalent weight of H;PO4 ,Na,CO3, Ca(OH), . Awt H=1 ,0=16 , Na=23 .C=12 ,Ca=40 ,P=30. B: Write properties of standard solution.