A 0.70 m aqueous solution of a monoprotic acid (HA) freezes at -1.50°C. Find the Ka of this monoprotic acid. Kf of water = 1.86 °C/m Enter to 4 decimal places.
A 0.70 m aqueous solution of a monoprotic acid (HA) freezes at -1.50°C. Find the Ka...
A 0.61 m aqueous solution of a monoprotic acid (HA) freezes at -1.11°C. Find the pKa of this monoprotic acid. Kf of water = 1.86 °C/m Enter to 3 decimal places.
A 0.595 m aqueous solution of a monoprotic acid (HA) freezes at -2.21°C. Find the pKa of this monoprotic acid. Kf of water = 1.86 °C/m
A 0.100 m aqueous solution of a weak acid, HA, is prepared. The resulting solution has a freezing point of -0.189*C. Calculate the % ionization of the acid. The Kf for water =1.86*C/m.
The experimentally measured freezing point of a 1.50 m aqueous solution of CaCl2 is -6.70°C. The freezing point depression constant for water is Kf = 1.86°C/m. Assume the freezing point of pure water is 0.00°C. The experimentally measured freezing point of a 1.50 m aqueous solution of CaCl2 is -6.70°C. The freezing point depression constant for water is Kf = 1.86°C/m. Assume the freezing point of pure water is 0.00°C. What is the predicted freezing point if there were no...
A weak acid, HA, is a monoprotic acid. A solution that is 0.250 M in HA has a pH of 1.890 at 25°C. HA(aq) + H2O(l) ⇄ H3O+(aq) + A-(aq) What is the acid-ionization constant, Ka, for this acid? What is the degree of ionization of the acid in this solution? Ka = Degree of ionization =
A monoprotic acid, HA, dissociates partially in aqueous solution. At equilibrium and 298 K, the percent dissociation of 0.50 M HA is 1.75 percent. Calculate the acid dissociation constant, Ka, of HA at 298 K. (Report your answer to 2 sig figs)
You make a 0.1 M solution with acid HA, a monoprotic acid. The Ka for this acid is 1.0E-8. If HA is mixed with a 50 M NaCl solution (no common ions with HA), determine the percent ionization of HA. So I calculated that the ionic strength of the solution is equal to 0.2 and found the activity coefficent to be 0.7469. When I plugged in the values into the Ka=(activity of A- * activity of H3O+)/activity of HA equation,...
A monoprotic acid, HA, with a Ka of 6.67 × 105 has a partition coefficient of 4.0 (favoring octanol) when distributed between water and octanol. Find the formal concentration of the acid in each phase when 100 mL of 0.100 M aqueous acid is extracted with 25 mL of octanol
Calculate the Ka of a weak monoprotic acid (HA) if the pH of a 1.0 M solution is 2.3. Ka = ___
A) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 1.5×10−5. B) Find the percent dissociation of this solution. C) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 2.0×10−3. D) Find the percent dissociation of this solution. E) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 0.14. F ) Find the percent dissociation of this solution.