What is the solubility of ZnCO_3 at 25 degree C in a buffer solution with a...
The solubility of PbBr_2 is 0.427 g per 100 mL of solution at 25 degree C. Determine the value of the solubility product constant for this strong electrolyte. Lead(II) bromide does not react with water. 5.4 times 10^-4 6.3 times 10^-6 1.6 times 10^-6 3.1 times 10^-6 2.7 times 10^-4 Calculate the maximum concentration (in M) of silver ions (Ag^+) in a solution that contains 0.025 M of CO^2-_3. The K_sp of Ag_2 CO_3 is 8.1 times 10^-12. 8.1 times...
Calculate the solubility at 25 degree C of CuBr in pure water and in a 0.0170 M CoBr_2 solution. K_sp is equal to 6.27 times 10^-9. Round both your answers to 2 significant digits. Solubility in pure water in g/L: Solubility in 0.0170 M CoBr_2 solution in g/L:
Calculate the solubility at 25 degree C of Co(OH)_2 in pure water and in a 0,0020 M CoCl_2 solution. K_sp is 5.92 times 10^-15. Round both of your answers to2 significant digits. Solubility in pure water: _______ Solubility in 0.00020 M CoCl_2 solution: ________
What is the solubility in moles/liter for copper(l) chloride at 25 degree C given a K_sp value of 1 times 10^-6. Write using scientific notation and use 1 or 2 decimal places (even though this is strictly incorrect!)
Step-by-Step approach please? Calculate the solubility product of silver iodide at 25 degree C given the following data: AgI(s) + e^- rightarrow Ag(s) + I^- I_2(s) + 2e^- rightarrow 2I^- Ag^+ e^- rightarrow Ag(s) A) 2.9 times 10^- 3 B) 1.9 times 10^- 4 C) 2.1 times 10^- 12 D) 9.0 times 10^- 17 E) 2.4 times 10^- 24 E degree (V) - 0.15 + 0.54 + 0.80
can I get some help? A solution is prepared at 25 degree C that is initially 0.39 M in acetic acid (HCH_3 CO_2) a weak acid with K_a = 1.8 times 10^-5, and 0.18 M in sodium acetate (NaCH_3CO_2). Calculate the pH of the solution.
Calculate the solubility at 25°C of AgCl in pure water and in a 0.0080M AgNO3 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. The Ksp value of AgCl is 1.77 times 10 to the -10. Solubility in water: Solubility in 0.0080 AgNO3 solution:
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed at the indicated values. Ksp = 7.9 x 10-16. (a) pH 7.6 (b) pH 10.0 (c) pH 13.8
I need help with my chemistry homework :) PART 1.) A buffer solution contains 0.35 mol of hydrogen peroxide (HOOH) and 0.50 mol of sodium hydrogen peroxide (NaOOH) in 3.60 L. The Ka of hydrogen peroxide (HOOH) is Ka = 2.4e-12. (a) What is the pH of this buffer? pH = _____ (b) What is the pH of the buffer after the addition of 0.31 mol of NaOH? (assume no volume change) pH = ______ (c) What is the pH...
24. (25 points) A buffer solution was prepared by dissolving 0.500 mol formic acid and 0.060 mol sodium formate in enough water to make 1 L of solution, K, for formic acid is 1.80 x 104 a) Calculate the pH of the solution. b) If this solution was diluted to 10 times its volume, what would be the pH.