Calculate the pressure of a 0.58 M aqueous ammonia (NH3) solution at 25 degrees C. (K=...
Calculate the vapor pressure at 25 degrees C of an aqueous solution that is 5.50% NaCl by mass. The pure vapor pressure of water at this temperature is 23.78 torr.
Estimate the pH of an aqueous solution exposed to a partial pressure of ammonia (NH3) of 10-4 atm. Assume that the temperature is 25ºC, there are no other components in the water and that the Henry’s law constant for ammonia is 0.018 atm M-1. Cleary state any simplifying assumptions that you make.
Determine the osmotic pressure at 25 °C of an aqueous solution that is 0.028 M NaNO3. p = i M R T (R = 0.08206 atm L/mol K) For some reason the answer is 1.37 atm, but I am getting .685 atm.
1) Ammonia, NH3, is a monoprotic base with pKb = 4.74 at 25 °C. For 0.121 mol L−1 NH3(aq) at 25 °C, calculate (a) the percent ionization of NH3; and (b) the pH of the solution. 2) Hydrazoic acid, HN3, is a monoprotic acid with pKa = 4.72 at 25 °C. For 0.121 mol L−1 HN3(aq) at 25 °C, calculate (a) the percent ionization of HN3; and (b) the pH of the solution.
An aqueous solution of 0.23 M ammonia (NH3) has a pOH of 2.70. Determine the base-dissociation constant (Kb) of ammonia.
An aqueous solution at 25 degrees C has a OH− concentration of (1*10^-9 M). Calculate the H3O+ concentration. Be sure your answer has the correct number of significant digits.
What is the pH of 6.0 M aqueous solution of NH3 (ammonia). It's Kb = 1.8 x 10-5.
The partial pressure of ammonia in air-ammonia mixtures in equilibrium with its aqueous solution at 20°C is given in Table 2. Using these data, and neglecting the vapor pressure of water and the solubility of air in water, construct an equilibrium diagram using mole ratios with YA = moles NH3/mole air and XA = moles NH3/mole H2O as coordinates. (a) If 10 moles of gas, of composition Y = 0.3, are contacted with 10 moles of a solution of composition...
For the aqueous [Ni(NH3).]* complex K, = 2.0 x 10% at 25 °C. Suppose equal volumes of 0.0034 M Ni(NO3), solution and 0.22 M NH, solution are mixed. Calculate the equilibrium molarity of aqueous Ni2+ ion. Round your answer to 2 significant digits. | Щм x 6 ?
For the aqueous (Hg(NH3), 7°* complex K = 1.8 x 10" at 25 °C. Suppose equal volumes of 0.0090 M Hg (N 2) solution and 0.54 M NH, solution are mixed. Calculate the equilibrium molarity of aqueous Hgʻion. Round your answer to 2 significant digits. | Ом x 6 ?