Express the concentration of a 0.0800 M aqueous solution of fluoride, F
0.0800 M solution means 1.00 L of solution contains 0.0800 moles of solute.
The mass of solute is the product of the number of moles and the molar mass.
The mass of the solution is the product of its volume and density.
The mass percentage is the ration of the mass of solute to the mass of solution multiplied by 100.
%
The concentration in ppm is the ratio of the mass of solute to the mass of solution multiplied by 1 million.
Express the concentration of a 0.0800 M aqueous solution of fluoride, F
Express the concentration of a 0.0880 M aqueous solution of fluoride, F, in mass percentage and in parts per million. Assume the density of the solution is 1.00 g/mL. Number Number 0 0 ppm
Express the concentration of a 0.0550 M0.0550 M aqueous solution of fluoride, F−,F−, in mass percentage and in parts per million (ppm). Assume the density of the solution is 1.00 g/mL. mass percentage: ppm:
A student measures the F- concentration in a saturated aqueous solution of barium fluoride to be 1.46×10-2 M. Based on her data, the solubility product constant for barium fluoride is .
M. A student measures the Mg2+ concentration in a saturated aqueous solution of magnesium fluoride to be 1.15X10 Based on her data, the solubility product constant for magnesium Muoride is
A student measures the Ca2+ concentration in a saturated aqueous solution of calcium fluoride to be 2.18x10-6 M. Based on her data, the solubility product constant for calcium fluoride is Submit Answer Retry Entire Group 9 more group attempts remaining
What is the pH of a solution with a fluoride concentration of 0.16 M ? The Kb for F– is 1.47×10-11 .
A student determines that an aqueous solution that contains 0.196 M potassium fluoride and 0.206 M hydrofluoric acid, also has an H3O+concentration of 8.48×10-4 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: HF(aq) + H2O H3O+(aq) + F-(aq) Calculate K as is usually done, omitting the solvent, water, from the expression for K: K = and A student determines that an aqueous solution that contains 0.365 M potassium nitrite and 0.125 M nitrous...
An aqueous solution contains 0.100 M fluoride ions and 0.126 M hydrogen fluoride. 5.00 mL of 0.0100 M HCl is added to 25.0 mL of this solution. What is the pH of the final solution? The given value for Ka of HF is 3.5 x 10-4.
An aqueous solution of sodium fluoride is slowly added to a water sample that contains barium ion (4.65x10-2 M) and calcium ion (7.40x10-2 M).The Ksp of barium fluoride is 1.00x10-6. The Ksp of calcium fluoride is 3.90x10-11. What is the remaining concentration of the first ion to precipitate when the second ion begins to precipitate?
An aqueous solution is prepared to be 0.31S M in sodium fluoride and 0.190 M in acetic acid. Is this solution a buffer solution? What is the pi I of this solution? If 0.119 moles of nitric acid are added to one liter of this solution, what is the pH of the resulting solution? pH =