A solution of dichloroacetic acid, Ka=3.6x10^-, with a molality of 0.52m, freezes at -1.2 celsius. Find the Van't Hoff factor and percent ionization for dichloroacetic acid
A solution of dichloroacetic acid, Ka=3.6x10^-, with a molality of 0.52m, freezes at -1.2 celsius. Find...
Calculate the molality of an aqueous solution of KBr whose freezing point is -4.95 degrees celsius. The Kf of water is 1.86 degrees C/m. Calculate the ideal Van't Hoff factor for KBr? Show work
The ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2, is 5.0*10^-2. What is the pH of a 0.15 molar solution of this acid?
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) the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 1.2×10−3 is 1.89. Find the percent dissociation of this solution. B) Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 0.13. Find the percent dissociation of this solution.
Part A A 0.150 M weak acid solution has a pH of 2.97. Find Ka for the acid. Part B Find the percent ionization of a 0.195 M HC2H3O2 solution. (The value of Ka for HC2H3O2 is 1.8×10−5.) Part C Find the pH of a 0.0191 M solution of hypochlorous acid. (The value of Ka for hypochlorous acid is 2.9×10−8.) Part D Find the pH of a 0.014 M solution of HF. (The value of Ka for HF is 3.5×10−4.) Part...
Question 1 : HA is a weak acid. Its ionization constant, Ka, is 1.2 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.075 M. Question 2 : We place 0.143 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.28 . Calculate the ionization contant, Ka, of HA. Question 3 : We place 0.661 mol of a weak acid, HA,...
The Ka of a monoprotic weak acid is 0.00894. What is the percent ionization of a 0.193 M solution of this acid? percent ionization:
Find the pH of a 0.100 M solution of a weak monoprotic acid having Ka= 1.2×10−3. Express your answer to two decimal places.
Determine the percent ionization of a solution of boric acid that is 61 mM (Ka = 5.4 × 10-10). percent The number of significant digits is set to 2; the tolerance is +/-4%
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.