If 2.000 g of hydrated magnesium chloride are heated to remove the water of hydration, the...

If 2.000 g of hydrated magnesium chloride are heated to remove the water of hydration, the anhydrous salt that remains has a mass of 0.9366 g. Determine the following:(A)The mass of water that was lost upon heating. (B)The moles of water that were lost upon heating. (C)The moles of magnesium chloride that remained after heating. (D)The mole ratio for the magnesium chloride and the water. (E)The formulas for this hydrate is ___________________________________________(F)The name for this hydrate is ______________________________________________

Expert Solution

queen_honey_blossom answered 1 year ago

A solution is prepared from 4.5750 g of magnesium chloride and 43.248 g of water. The...

A solution is prepared from 4.5750 g of magnesium chloride and 43.248 g of water. The vapor pressure of water above this solution is found to be 0.3626 atm at 348.0 K. The vapor pressure of pure water at this temperature is 0.3804 atm. Part A Find the value of the van't Hoff factor i for magnesium chloride in this solution. Express your answer using four significant figures.

The salt magnesium chloride is soluble in water. When 0.630 g of MgCl2 is dissolved in...

The salt magnesium chloride is soluble in water. When 0.630 g of MgCl2 is dissolved in 114.00 g of water, the temperature of the solution increases from 25.00 to 27.29 °C. Based on this observation, calculate the enthalpy of dissolution of MgCl2 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. ΔHdissolution = ? kJ/mol

A 1.250 g sample of barium chloride hydrate, BaCl2.xH2O, was heated until all the water had...

A 1.250 g sample of barium chloride hydrate, BaCl2.xH2O, was heated until all the water had been driven off. The remaining anhydrous salt weighed 1.060g. Use this data to calculate the value of x, the number of moles of water of crystallization in the hydrated salt. You MUST Show ALL your work for full credit! 5. 0.0185 mol of hydrated magnesium sulfate MgSO4.xH2O has a mass of 4.56g. Calculate the value of x, the number of moles of water of...

a 3.592 g sample of hydrated magnesium bromide, MgBr2. xH20, is dried in an oven. when...

a 3.592 g sample of hydrated magnesium bromide, MgBr2. xH20, is dried in an oven. when the anhydrous salt is removed from the oven, it's mass is 2.263 g. what is the value of x?

a hydrated form of copper sulfate (cuso4·xh2o) is heated to drive off all the water if...

a hydrated form of copper sulfate (cuso4·xh2o) is heated to drive off all the water if we start with 9.57 g of hydrated salt and have 7.15 of anhydrous CuSo4 after heating find the num. of water molecules associated with each CuSo4 formula unit

A sample of hydrated barium chloride (BaCl2) has a mass of 8.26 g. After dehydration, the...

A sample of hydrated barium chloride (BaCl2) has a mass of 8.26 g. After dehydration, the anhydrous sample has a mass of 7.04 g. What is the correct name for the hydrate

One way to remove magnesium (Mg2+) from water is to precipitate it with a strong base...

One way to remove magnesium (Mg2+) from water is to precipitate it with a strong base such as sodium hydroxide (NaOH). Assuming the following unbalanced reaction describes the process. (a) Calculate the concentration of NaOH (in mg/L) needed to completely remove 20 mg/L of Mg2+. (b) Calculate the mass (in lb) of solid Mg(OH)2 that will be produced (and must be disposed of) if this reaction is performed in 250,000 gallons of water. MgSO4 + NaOH = Mg(OH)2¯ + Na2SO4

34.62 g of ferrous bromide reacts with 29.25 g of potassium chloride in a heated vessel....

34.62 g of ferrous bromide reacts with 29.25 g of potassium chloride in a heated vessel. Write a balanced chemical equation for this double replacement reaction. What is the percent yield of ferrous chloride if the actual yield is 10.25 g? How much excess remains?

A hydrated nickel chloride compound was found to contain 24.69% Ni, 29.83% Cl, and 45.48% water....

A hydrated nickel chloride compound was found to contain 24.69% Ni, 29.83% Cl, and 45.48% water. Determine the empirical formula of this hydrated compound

A 10.00 g sample of a hydrate of magnesium chloride (MgCl2•x H2O) contains 5.317 g of...

A 10.00 g sample of a hydrate of magnesium chloride (MgCl2•x H2O) contains 5.317 g of H2O. What is the value of x?

Question