Part A
MgF2, magnesium fluoride
Part B
Ca(OH)2, calcium hydroxide
Part C
C4H8O4. erythrose, a carbohydrate
7.39 Calculate the mass percent composition of each of the following: a. MgF2, magnesium fluoride b. Ca(OH)2, calcium hydroxide c. C4H204, erythrose, a carbohydrate d. (NH4)3PO4, ammonium phosphate, fertilizer e. C17H 9NO3, morphine, a painkiller
A saturated solution of magnesium fluoride , MgF2, was prepared by dissolving solid MgF2 in water. The concentration of Mg2+ ion in the solution was found to be 1.18
A chemist prepares a solution of magnesium fluoride (MgF2) by measuring out 0.03 g of magnesium fluoride into a 350. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's magnesium fluoride solution. Round your answer to 1 significant digit molL
Part A Calculate the molar solubility of magnesium fluoride (MgF2) in a solution that is 0.350 M in NaF. For magnesium fluoride, Ksp = 5.16 x 10-11. 02.05 x 10-5 M o 4.21 x 10-10 M O 2.35 x 10-4 M O 1.47 x 10-10 M Submit Request Answer
What is the solubility in mole per liter for magnesium fluoride, MgF2, in a 2.4 mM solution of magnesium chloride, MgCl2? Hints: Use the 'small x' approximation and assume that magnesium chloride is fully soluble at this concentration. Ksp=5.16×10-11 for MgF2
A chemist makes 820. mL of magnesium fluoride (MgF2) working solution by adding distilled water to 130. ml. of a 2.02 mm stock solution of magnesium fluoride in water. Calculate the concentration of the chemist's working solution. Round your answer to 3 significant digits. MM х ? Dilution A chemist makes 820, ml. of magnesium fluoride (MgF2) working solution by adding distilled water to 130. ml. of a 2.02 mm stock solution of magnesium fluoride in water Calculate the concentration...
Calculate the mass percent composition of each of the following @ Mg F2, magnesium fluoride 16 C4 H ₂ O4, erythrose, a carbohydrate
What is the molar solubility of magnesium fluoride in a solution that is 0.40 M F− ions? The Ksp of MgF2 is 6.4 × 10−9. What is the molar solubility of magnesium fluoride in a solution that is ions? The Ksp of MgF2 is 6.4x10^-9 8.0 × 10−5 8.0 × 10−9 4.0 × 10−8 1.6 × 10−8
Calculate the [F-] present in a satuated solution of magnesium fluoride if Ksp= 7.4 x10^-11 MgF2(s) <—-> Mg 2+ (aq)+ 2F-(aq)
A thin coating of Magnesium Fluoride (MgF2) is deposited on the surface of some eyeglasses which have an index of refraction of 1.6. The MgF2 has an index of refraction of 1.38. (a) What is the minimum thickness of the coating so that green light of wavelength 500 nm has minimal reflectance (i.e. maximum transmission for anti-reflective coating)? (b) What is the minimum thickness of the coating so that green light of wavelength 500 nm has maximum reflectance?