Assuming the base completely dissociates in water, what is the pH of a 8.05 g/L solution...
What is the pH of a 15.9 M solution of H2SO4? The first proton completely dissociates; the Ka for the second proton is 1.2×10–2.
What is the pH of a 13.5 M solution of H2SO4? The first proton completely dissociates; the Ka for the second proton is 1.2×10–2.
Assuming complete dissociation, what is the pH of a 3.77 mg/L Ba(OH), solution? pH =
The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent ionization....
Assuming complete dissociation, what is the pH of a 4.29 mg/L Ba(OH)_2 solution? pH =
Assuming complete dissociation, what is the pH of a 4.60 mg/L Ba(OH)2 solution?
Assuming complete dissociation, what is the pH of a 3.06 mg/L Ba(OH)2 solution?
Assuming complete dissociation, what is the pH of a 4.01 mg/L Ba(OH)2 solution?
Assuming complete dissociation, what is the pH of a 4.47 mg/L4.47 mg/L Ba(OH)2Ba(OH)2 solution? pH=
A solution is prepared by dissolving 0.0034 g Ca(OH)2 in enough water to prepare a 250 mL solution. what is the pH of the solution if Ca(OH)2 completely dissociates producing 2 OH for every 1 Ca