0.02 g (=20 mg) of MgF2(s) is added into 1.0 L of pure water containing no Mg2+ and F-. MgF2(S)↔ Mg2+ + 2F- Ksp = 3.7 x 10-11 (AW: Mg=24, F=19)
(a) What would be the concentration (in M) of F- in solution at equilibrium?
(b) How much solid (if any) would remain (in mg/L) after the system reaches equilibrium?
0.02 g (=20 mg) of MgF2(s) is added into 1.0 L of pure water containing no...
0.02 g (=20 mg) of MgF2(s) is added into 1.0 L of pure water containing no Mg 2+ and F- MgF2(S) ↔ Mg2+ + 2F- Ksp= 3.7 x 10^-11 (AW: Mg=24, F=19) (a) What would be the concentration (in M) of F- in solution at equilibrium? (b) How much solid (if any) would remain (in mg/L) after the system reaches equilibrium?
MgF2(s) <--> Mg2+(aq) + 2 F–(aq) In a saturated solution of MgF2 at 18 0C, the concentration of Mg2+ is 1.21 x 10–3 molar. The equilibrium is represented by the equation above. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 0C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 liter of saturated MgF2 solution at 18 0C to which 0.100 mole of solid KF has been added. The KF dissolves completely. Assume...
In a saturated solution of MgF2 at 16 °C, the concentration of Mg2+ is 1.44x10 –3 M The equilibrium is represented by the equation MgF2 -->Mg 2+ + 2 F-. A.Write the expression for the solubility product constant, Ksp. B.Calculate the value of Ksp at 16°C for MgF2 Note: Your answer is assumed to be reduced to the highest power possible. C.Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 16°C to which 0.450 mole of...
4. Calculate the pH of a solution of pure water containing 1.0 mg/L of sulfuric acid.
5.0 g of barium fluoride is added to 1.0 L of water. After a sufficient amount of time, the saturated solution is filtered and the solid is dried and weighed and found to have a mass of 3.6g. What is the solubility product constant, Ksp Bato Bar + 2 Flag) (BaFz)? Ksp = [B2[F]?
In pairs; Let’s say you add 10.0 g PbCl2 (s) to 1.0 L of water. Even though PbCl2 is ‘insoluble’, a fraction of the solid will dissolve. Write out the chemical equilibrium for the dissolution of PbCl2 in water. The Ksp for PbCl2 is 1.7 x 10-4. Calculate how many grams of PbCl2 will dissolve in the solution. Your lab partner claims that by adding NaCl to the solution, thus increasing [Cl-] and forcing the equilibrium back toward PbCl2 (s),...
If 1.2 moles of CaF2 (s) are added to 2.7 L of water what will the concentration of F- be at equilibrium? The Kop - 3,9 x 10-11 CaF, (s) = Ca (aq) + 2F (aq) O(A) 5.38 x 10 M (B) 3. 12 x 10-6 M (C) 2.14 x 10- M (D) 7.91 x 10-M (E) 4.27 x 10-4 M
The department of health and human services recently recommended the concentration of fluoride in drinking water be limited to 0.7mg/L (the current policy allows for a range of 0.7 to 1.2 mg/L). The concentration of fluoride in natural water depends on The presence of fluoride-containing minerals 9. (7 points) The Department of Health and Human Services recenty recommended oe concentration of fluoride in drinking water be limited to 0.7 mg (the current poley wws t a range of 0.7 to...
What mass of solid NaOH must be added to 1.0 L of water at 25*C in order to dissolve 10.0 g of Zn(OH)2 (Ksp=4.5x10-17) according to the following reaction? Zn(OH)2 (s) + 2OH- (aq) ------> Zn(OH)42- (aq) The formation constant for Zn(OH)42- is Kf=2.8x1015.
(aq) (1) Mg(OH)2 is partially dissolved in water: Mg(OH), (s) = Mg2+ (aq) + 2OH Write the Kop expression for Mg(OH)2 : Kp = (2) Solid AgCl is partially dissolved in water: AgCl 2 Ag+ + CI''. If the molar solubility is known as [Ag +) = [CI''] = 1.3x 10 M, AgCl Kip =- (a) 1.3 x 10 (b) 1.69 x 10-10 (c) 2.6 x 10 (d) none of these (3) At 25 °C, the solubility of solid AgCl...