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The osmotic pressure of 0.1M sodium chloride solution at 27∘C is?

The osmotic pressure of 0.1M sodium chloride solution at 27∘C is?

WebΔT = i*K f* m where ΔT = Change in temperature in °C i = van 't Hoff factor K f = molal freezing point depression constant or cryoscopic constant in °C kg/mol m = molality of the solute in mol solute/kg solvent 1 molal urea solution freezes at -1.86 degree celsius 1.86=K f * 1 K f= 1.86 Using value of K f Find value of i ΔT=K f* m*i ie,0. ... WebTable 1. Estimated values of absolute density (g/cm 3) of aqueous sodium chloride solutions {NaCl + H 2 O) as function of electrolyte molality m and temperature T (at pressure p = 1 bar). Values in the table are consistent with the density of pure water calculated with the IAPWS-95 equation of state. ρ /g·cm −3. m /mol·kg (H 2 O) −1. comanche wells mobile home park WebDec 14, 2024 · Q). At 90 ° C, the pH of 0.1M NaCl aqueous solution is :-(1) < 7 (2) > 7 (3) 7 (4) 0.1 dr.soliman fakeeh hospital careers WebCH3COOH pKa=4.76 c=0.1 HCl pKa=-10 c=0.1 Case 2. Solution is formed by mixing known volumes of solutions with known concentrations. For each compound enter compound name (optional), concentration, volume and Ka/Kb or pKa/pKb values. For example: CH3COOH pKa=4.76 c=0.1 v=10 HCl pKa=-10 c=0.1 v=20 For strong acids … WebMar 22, 2024 · So, the pH of the solution is 11, which gives option c as the answer. Note: The dissociation constants can be changed by application of temperature and also in the presence of a catalyst. The smaller the dissociation constant, the less likely it is to be split into ions, which means there is a strong intermolecular force that holds the atoms ... dr soliman fakeeh medical center WebMay 8, 2024 · Ka = x2 0.1 −x = 1.8 × 10−5. We assume that for a Ka on the order of 10−5 or less, the small x approximation works. We can verify this by checking that the percent dissociation is less than 5 % later. 1.8 × 10−5 ≈ x2 0.1. ⇒ x ≈ √0.1Ka. = [H+] = 0.001342 M. Therefore, the pH is:

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