The pH of a solution of Sr(OH)_2 solution is 7.68. Calculate the concentration of Sr(OH)_2.
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)
Calculate the hydrogen ion concentration in mol/L for a solution Sr(OH)2 of concentration 0.017 M
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?
a. Calculate the pH of the solution if 2.3 x 10-3 moles of Sr(OH)2 is dissolved in 250 mL of water? b. Calculate the pH of a 3.0000 M solution of NaOH? c. Calculate the pH if 6.5 g of HCl(g) are dissolved in 200 mL of water?
What is the pH of a 0.47 M solution of Sr(OH)2? What is the hydrogen ion concentration?
5. (4 pts) Calculate the pH of a 0.0025 M aqueous solution of strontium hydroxide, Sr(OH). 5. (4 pts) Calcula pH =
Calculate the pH of this solution molar concentration of OH− ions in a 0.085 M solution of ethylamine (C2H5NH2; Kb=6.4×10−4). [OH−] [OH−] = 7.1×10−3 M Calculate the pH of this solution. Express your answer to two decimal places.
Calculate the K_sp for hydroxide if the solubility of Sr(OH)_2 in pure water is 2.1 times 10^1 g/L. 1.16 times 10^-1 1.60 times 10^-2 1.42 times 10^1 6.40 times 10^-3 7.70 times 10^-33
Calculate the hydroxide ion concentration, [OH−] , for a solution with a pH of 5.66 . [OH−]= M
Assuming complete dissociation, what is the pH of a 4.29 mg/L Ba(OH)_2 solution? pH =