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 crystallization in the hydrated salt. You MUST Show ALL your work for full credit!

Expert Solution

queen_honey_blossom answered 1 year ago

The general formula of barium chloride hydrate is BaCl2 • n H2O, where n is the...

The general formula of barium chloride hydrate is BaCl2 • n H2O, where n is the number of water molecules. Calculate the theoretical mass percent water for each value of n – the mass of each water molecule is 18.02 amu. Report 2 decimal places for all your answers. Do NOT include units in your answer. BaCl2 BaCl2 • H2O BaCl2 • 2 H2O BaCl2 • 3 H2O Mass of anhydrous BaCl2 (amu) 208.23 208.23 208.23 208.23 Mass of H2O...

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

A 8.40-g sample of solid BaCl2·2H2O was heated such that the water turned to steam and...

A 8.40-g sample of solid BaCl2·2H2O was heated such that the water turned to steam and was driven off. Assuming ideal behavior, what volume would that steam occupy at 1.00 atm and 100.0 °C?

a) An impure barium chloride sample weighing about 0.38 g was dissolved in water and then...

a) An impure barium chloride sample weighing about 0.38 g was dissolved in water and then treated with excess sulfuric acid. Calculate the volume of 3.0 M H2SO4 needed to completely precipitate the barium ions as barium sulfate, BaSO4. (Give your answer to 2 significant figures in mL) b)The impure barium chloride sample from Part (a) was found to have a mass of 0.3821 g. The mass of barium sulfate, BaSO4, that precipitated from the addition of sulfuric acid was...

1) How many atoms are there in 51.3 g of barium chloride (BaCl2)? 2) How many...

1) How many atoms are there in 51.3 g of barium chloride (BaCl2)? 2) How many moles of carbon monoxide (CO) are in 29.3 g of the compound? 3) What is the formula for copper(II) phosphate? Capitalization and punctuation count? 4) How many atoms of phosphorus are in 2.90 mol of copper(II) phosphate? 5) How many moles of N are in 0.191 g of N2O? 6) A sample of C3H8 has 7.68 × 1024 H atoms. How many carbon atoms...

A solid hydrate of Ca(NO3)2 is to be analyzed (Ca(NO3)2 •XH2O). A sample of the hydrate...

A solid hydrate of Ca(NO3)2 is to be analyzed (Ca(NO3)2 •XH2O). A sample of the hydrate is weighed in a clean, dry and covered crucible. When empty, the crucible and cover are heated to a constant weight of 30.2016 g. The mass of the crucible and sample is 33.2255 g. The crucible with sample is heated (to drive off the water of hydration) to a final constant weight of 32.2995 g Table 1: Mass Data for the Analysis of a...

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) Water (2350 g ) is heated until it just begins to boil. If the water...

A) Water (2350 g ) is heated until it just begins to boil. If the water absorbs 5.83×105 J of heat in the process, what was the initial temperature of the water? Express your answer with the appropriate units. B) If 125 cal of heat is applied to a 60.0-g piece of copper at 22.0 ∘C , what will the final temperature be? The specific heat of copper is 0.0920 cal/(g⋅∘C) .

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?

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 ______________________________________________

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