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 3.77 mg/L Ba(OH), solution? pH =
Assuming complete dissociation, what is the pH of a 4.47 mg/L4.47 mg/L Ba(OH)2Ba(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?
Calculate the [OH^-], pOH and pH of a 0.232 M solution of Ba(OH)_2. Ba(OH)_2 (aq) rightarrow Ba^2+ (aq) + 2 OH^-(aq)
What are the concentrations of OH− and H+ in a 0.00082 M solution of Ba(OH)2 at 25 °C? Assume complete dissociation. [OH−]= [H+]=
The solubility products for Mg(OH)_2 and Ca(OH)_2 are 8.9 times 10^-12 and 1.3 times 10^-4, respectively Suppose a solution contains both Mg^2+ and Ca^2+ ions, each at 0.10 M in concentration (a) At what pH Mg(OH)_2 starts to from a precipitate? (b) At what pH Ca(OH)_2 begins to from a precipitate? (C) What is the concentration of Mg^2+ when Ca(OH)_2 begins to from precipitate?
Show Mg(OH)_2 precipitate when the pH of a solution containing 0.05 M Mg^+2 is raised to 8? Show your work to justify your answer.
The pH of a solution of Sr(OH)_2 solution is 7.68. Calculate the concentration of Sr(OH)_2.