# A 3.564 g of a sample of a hydrated barium chloride salt BaCl_2 cdot X H_2O is heated to a...

## Question:

A {eq}\displaystyle \rm 3.564 \ g {/eq} of a sample of a hydrated barium chloride salt {eq}\displaystyle \rm BaCl_2 \cdot X H_2O {/eq} is heated to a constant mass of {eq}\displaystyle \rm 2.641 \ g {/eq} of {eq}\displaystyle \rm BaCl_2 {/eq}.

Calculate the mass of water lost from the hydrated salt.

## Hydrates:

A hydrate can easily be determined from its chemical formula. This would contain an inorganic salt and water which has a corresponding stoichiometric ratio. The water molecules are adsorbed on the surface of the inorganic salt, with a crystalline form.

## Answer and Explanation: 1

Become a Study.com member to unlock this answer! Create your account

View this answerDetermine the mass of water, {eq}\displaystyle m_{H_2O} {/eq}, that is lost from the hydrate. We take note that, upon heating the hydrate, the...

See full answer below.

#### Ask a question

Our experts can answer your tough homework and study questions.

Ask a question Ask a question#### Search Answers

#### Learn more about this topic:

from

Chapter 9 / Lesson 8Learn the anhydrate definition and what a hydrated compound is. Understand what an anhydrate is, the hydrate formula, and how to find the formula of the hydrate.

#### Related to this Question

- A 3.564 g of sample of a hydrated barium chloride salt BaCl_2 cdot X H_2O is heated to a constant mass of 2.641 g of BaCl_2. Calculate the molar mass of water lost.
- A 3.564 g of sample of a hydrated barium chloride salt BaCl_2 cdot X H_2O is heated to a constant mass of 2.641 g of BaCl_2. Calculate the moles of anhydrous salt.
- A 2.914 g sample of a hydrated salt Barium Chloride, BaCl_2, is heated at a temperature greater than 170 degree C in a crucible until a constant mass is reached . The Mass of the anhydrous BaCl_2 salt is 2.484 g. (a) Calculate the percent by mass of wat
- A 3.564 g of sample of a hydrated barium chloride salt BaCl_2 cdot X H_2O is heated to a constant mass of 2.641 g of BaCl_2. Determine the correct value of X.
- If 4.36 g of a hydrate of the salt BaCl2 is heated and in the process losses 0.6431 g of mass, show all your work to calculate the amount of water X in the hydrate, BaCl2 XH2O.
- A 0.750 g sample of NiCl_2 is completely hydrated. Calculate the mass of the completely hydrated salt.
- A dry sample of a hydrate BaCl2-xH2O initially weighed 2.342 grams. After heating to drive off all the water of hydration, the sample (which is now BaCl2) weighed 1.997 grams. What is the value of x inBaCl2-xH2O? What is the mass of H2O that was driven
- A student measured a 6.790 g sample of hydrated salt. After heating, the mass of anhydrous salt was found to be 4.501 g. What is the mass of water in the hydrated salt?
- A student takes 4.597 g of hydrated barium chloride and heats it in a crucible. The anhydrous material weighted 3.919 g. What is the complete formula for this hydrated salt?
- An 1.803 g sample of gypsum, a hydrated salt of calcium sulfate, CaSO_4, is heated at a temperature greater than 170 degrees C in a crucible until a constant mass is reached. The mass of the anhydrous CaSO_4 salt is 1.426 g. Calculate the percent by mass
- A 1.803 g sample of gypsum, a hydrated salt of calcium sulfate, CaSO_4 is heated at a temperature greater than 170 degrees C in a crucible until a constant mass is reached. The mass of the anhydrous CaSO_4 salt in 1.426 g. Calculate the percent mass of wa
- A 1.803-g sample of gypsum, a hydrated salt of calcium sulfate, is heated at a temperature greater than 170 degree C in a crucible until a constant mass is reached. The mass of the anhydrous calcium sulfate salt is 1.426 g. Calculate the percent by mass o
- A student measured a 6.790 g sample of hydrated salt. After heating, the mass of anhydrous salt was found to be 4.501 g. What is the percent mass of water in the hydrated salt?
- A 1.994-g sample of gypsum, a hydrated salt of calcium sulfate, CaSO4, is heated at a temperature greater than 170 degrees C in a crucible until a constant mass is reached. The mass of the anhydrous CaSO4 salt is 1.577 g. What is the mass percent of water
- A 3.82-gram sample of manganese (II) sulfate hydrate lost 1.23 grams of water when heated to constant mass. A) What is the formula of the hydrated salt? Show work. B) What is the name of the hydrated salt?
- A hydrated MgSO4 salt weighing 3.211 g is heated in a crucible reaching a constant weight. The weight of the anhydrous MgSO4 is 1.570 grams. a. Calculate the percent of water in the hydrated MgSO4 salt? b. Calculate the moles of H2O removed and the moles
- In an experiment, 90.1 g of FeCl3 cdot xH_2O is heated to drive off all of the water hydration. The mass of the remaining salt is 54.1 g. What is the value of x in the formula for the hydrate?
- A 5 gram sample of a hydrate of BaCl_2 was heated, and only 4.3 g of the anhydrous salt remained. What percentage of water was in the hydrate?
- A 1.803-g sample of gypsum, a hydrated salt of calcium sulfate, CaSO4, is heated at a temperature greater than 170 degrees Celsius in a crucible until a constant mass is reached. The mass of the anhydrous CaSO4 salt is 1.426 g. Calculate the percent by ma
- Suppose 4.567 g of magnesium sulfate hexahydrate is heated to drive off the water of crystallization. a) Calculate what mass of water would be expected to be released from the salt. b) Calculate what mass of anhydrous salt would remain. c) Calculate th
- Calculate the mass of water lost from your sample? Given: Mass of crucible- 18.50g. Mass of crucible+hydrate- 19.50g. Mass of crucible+anhydrous salt 1st heating- 19.10g. Mass of crucible+anhydrous salt 2nd heating- 19.10g.
- A 2.50 g sample of a hydrate of calcium sulfate looses 0.523 g of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
- Suppose that 0.205 g of a mixture containing Na_2SO_4 and K_2SO_4 is dissolved in water. An excess of BaCl_2 is added and a precipitate of 0.298 g of BaSO_4 is produced. Calculate the percent by mass
- A 2.500-g sample of a hydrate of calcium sulfate loses 0.524 g of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
- A 1.1000-gram hydrate sample chosen from Na2CO3 10H2O, AlCl3 6H2O, MgCl2 6H2O, and BaCl2 2H2O was heated and found to lose 0.4919 grams of H2O. a. Show the calculation of the % H2O in the unknown hydrate sample. b. Show the calculation of the % H2O in eac
- A sample contains BaCl2 2H2O and NaCl. After 0.678 grams of the sample was heated, the residue weighed 0.648 grams. What is the percent of BaCl2 2H2O in the sample?
- A 2.50-gram sample of a hydrate of calcium sulfate loses 0.523 grams of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
- A 2.500 gram sample of hydrate of calcium sulfate loses 0.532 grams of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
- A 5.00 g sample of a hydrate of barium chloride was heated, and only 4.30 g of the anhydrous salt remained. What is the formula of the hydrate?
- A 0.8046-gram sample of impure BaCl_2 * 2H_2O weighed .7082 grams after it was dried at 200 degrees C for two hours to drive off H_2O. Calculate the % water in the sample.
- Anhydrous barium iodide has a mass of 9.52 grams. What is the name of its hydrate if the hydrated sample has a mass of 10.41 grams?
- A student heated a 4.901 g sample of hydrated iron chloride. After heating, the anhydrous iron chloride has a mass of 3.010 g. Calculate the percentage by mass of water in the hydrated compound.
- 0.2356 g sample containing only NaCl and BaCl2 yielded 0.4637g of dried AgCl. Calculate the percent of each compound in the sample.
- A hydrated salt is a solid that includes water molecules within its crystal structure. A student heated a 9.10-g sample of a hydrated salt to a constant mass of 5.41 g. What percent by mass of water d
- When 1.42g of M_2SO_4 were dissolved in water and treated with excess aqueous BaCl_2, all of the sulfate precipitated as BaSO_4, 2.33 of BaSO_4 were formed. Find the atomic mass and the identity of M.
- A 1.803-gram sample of gypsum, a hydrated salt of sulfate (CaSO4), is heated at a temperature greater than 170 degrees Celsius in a crucible until a constant mass is reached. The mass of the anhydrous CaSO4 salt is 1.426 grams. Calculate the percent by ma
- 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 3.592-gram sample of hydrated magnesium bromide is dried in an oven. When the anhydrous salt is removed from the oven, its mass is 2.263 grams. What is the mass percent of the water in this hydrated salt?
- A 2.914-g sample of gypsum, a hydrated salt of calcium sulfate, CaSO4, is heated at a temperature greater than 170 degrees C in a crucible until a constant mass is reached. The mass of the anhydrous C
- A 4.0-gram sample of hydrate nickel(II) bromide loses 0.793 grams of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
- calculate the percentage of the water in sample CuSO4.5H2O Given: Mass of crucible- 18.50g. Mass of crucible+hydrate- 19.50g. Mass of crucible+anhydrous salt 1st heating- 19.10g. Mass of crucible+anhydrous salt 2nd heating- 19.10g.
- A 1.803-g sample of gypsum, a hydrated salt of calcium sulfate, CaSO_4, is heated at a temperature greater than 170 C in a crucible until a constant mass is reached. The mass of the anhydrous CaSO_4
- A sample of 5.00 grams of CaSO4 2H2O is heated to drive off water. What is the mass of the remaining anhydrous salt?
- An 8.24 gram sample of a hydrated salt is heated until it has a constant mass of 6.20 grams. What is the percent by mass of water contained in the original sample?
- A 2.914 g sample of gypsum, a hydrated salt of calcium sulfate, CaSO_4 , is heated at a temperature greater than 170 degree C in a crucible until a constant mass is reached. The mass of the anhydrou
- A sample of a hydrated salt weighs 8 grams. After heating, the anhydrous sample weighs 5 grams. How many grams of water were present in the original sample?
- A sample of iron(II) chloride hydrate, FeCl2 nH2O, weighs 1.025 grams. After carefully removing the water from the compound, the mass of the anhydrous salt is 0.653 grams. Find the empirical formula of this hydrate.
- Suppose 2.3754 g of CuSO4 5H2O is heated to drive off the water of crystallization. Calculate what weight of anhydrous salt will remain. The molar mass of CuSO4 5H2O = 249.70 g/mol and the molar mass of CuSO4 = 159.60 g/mol.
- When 1.40 g of hydrated magnesium sulfate is heated to constant mass, 0.68 g of the anhydrous salt remains. Find the formula for the hydrated magnesium sulfate.
- A student had a sample of BaCl_2 * 2H_2O. He heated a sample the mass did not change. From this data, calculate the percentage of BaCl_2 in the original sample. mass of crucible + cover = 26.39 g mass
- 1. A 2.914-g sample of gypsum, a hydrated salt of calcium sulfate, CaSO_4, is heated at a temperature greater than 170 degrees C in a crucible until a constant mass is reached. The mass of the anhydro
- Calculate the percent mass for water in the following hydrates. a. Barium chloride dihydrate b. Calcium sulfate dihydrate c. Copper (II) sulfate pentahydrate d. Iron (II) sulfate heptahydrate e. Magnesium sulfate heptahydrate f. Sodium sulfi
- A 6.165-gram sample of an unknown hydrate of cobalt(II) bromide is heated until all the water of hydration is removed. The CoBr2 that remains has a mass of 4.637 grams. How many grams of water were lost in the dehydration?
- You have a 1.00 g sample of a hydrate of Na2CO3. By heating the compound, you drive off the water and are left with 0.3704 g of the anhydrous compound. a. What mass of water has been driven off? b. What is the percent by mass of Na2CO3 in the hydrate? c.
- A 4.00-gram sample of a hydrate of nickel (III) bromide loses 0.79 grams of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
- Suppose a student performs a similar experiment to determine the empirical formula of a barium chloride hydrate. Given the data collected in the table below, what is the formula of the hydrate? The molar mass of water is 18.015 g/mol and the molar mass of
- A 1.000 g sample of a metal chloride, MCl2, is dissolved in water and treated with excess aqueous silver nitrate. The silver chloride that forms weighs 1.286 g. Calculate the atomic mass of M.
- Calculate the percent mass for water in the following hydrates. a. Barium chloride dihydrate b. Calcium sulfate dihydrate c. Copper (II) sulfate pentahydrate d. Iron (II) sulfate heptahydrate e. Magnesium sulfate heptahydrate f. Sodium sulfide
- A hydrate of sodium sulfide has the following formula: Na_2S* x H_2O. The water in a 3.41-g sample of the hydrate was driven off by heating. The remaining sample had a mass of 1.58 g . A) Find the nu
- A 2.50 g sample of a hydrate of calcium sulphate losses 0.523 g of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
- After 0.69 g of CoCl2 6H2O is heated, the residue has a mass of 0.333 g. Calculate the % H2O in the hydrate.
- A 6.165-gram sample of an unknown hydrate of cobalt(II) bromide is heated until all the water of hydration is removed. The CoBr2 that remains has a mass of 4.637 grams. How many moles of water were lost in the dehydration?
- A student had a sample of BaCl2.2H2O. He heated a sample until the mass did not change. From this data, calculate the percentage of BaCl2 in the original sample. Mass of crucible+cover=26.39g Mass
- Suppose a student performs a similar experiment to determine the empirical formula of a barium chloride hydrate. Given the data collected in the table above, what is the formula of the hydrate? The molar mass of water is 18.015 \dfrac{g}{mol} and the mola
- A 0.386-gram sample of a sodium sulfate hydrate with the general formula Na2SO4 xH2O is heated. The mass after heating is 0.170 grams. What is the full formula and name of the hydrate salt?
- Mass of evaporating dish 22.34, mass of evaporating dish+hydrate 24.64, mass of evaporating dish+anhydrous salt 23.85. CuS04XH2O=CuSO4+XH2O. 1. Determine the mass of the water lost. 2. Determine the number of moles of the water lost.
- A hydrate of copper (II) chloride has the following formula: C u C l 2 x H 2 O . The water in a 3.41 g sample of the hydrate is driven off by heating. The remaining sample has a mass of 2.69 g. Find the number of waters of hydration ( x ) in the hydrat
- A chemist has a sample of hydrated FeCl_3 and it weighs 5.0 grams. He heats it strongly to drive off water of hydration, and after heating, he found that the anhydrous compound has a mass of 3.0 grams
- Write the formula and calculate the molar mass of barium chloride.
- An 8.2420-gram sample of an unknown hydrate of cobalt(II) bromide is heated until all the water of hydration is removed. The CoBr2 that remains has a mass of 6.2000 grams. a. How many moles of CoBr2 are in the sample? b. How many grams of water were lost
- How do you calculate the empirical formula of the barium hydroxide hydrate if a sample consists of 3.70 grams of barium hydroxide and 2.64 grams of water?
- Calculate percent water in the following hydrates: 1. BaCl_2 \cdot 2H_2O \\2. CaCO_3 \cdot 6H_2O
- If 25 grams of CoCl2 H2O was heated to constant weight, what mass of anhydrous salt would remain?
- 3.592 g sample of hydrated m anhydrous salt is removed from the oven, its mass is 2.263 g. What is the value of x?
- What is the variable x in the following hydrate formula NaCl.xH_2O, if the mass of sodium chloride is 58 g and the mass of the water is 36 g?
- What is the expected mass of anhydrous salt formed after the waters of hydration of CoCl_2.6H_2O are driven off completely by heating, resulting in a mass loss of 2.000 g water?
- A 1.543 g sample containing a sulfate ion was treated with barium chloride reagent, and 0.2243 g of barium sulfate was isolated. Calculate the percentage of sulfate ions in the sample.
- Suppose 2.3754 grams of copper (II) sulfate pentahydrate is heated to drive off the water of crystallization. Calculate the weight of anhydrous salt that will remain.
- In hydrated copper sulfate, the chemical formula is CuSO_4 cdot 5H_2O, while that of hydrated cobalt (II) chloride is CoCl_2 cdot 6H_2O. Describe how to determine the number of moles of water needed to hydrate any salt. Is there a pattern or formula?
- The following data were collected from the gravimetric analysis of a hydrated salt: Mass of crucible and lid (g) 19.437 Mass of crucible, lid, and hydrated salt (g) 21.626 Mass of crucible, lid, and anhydrous salt (g) 21.441 Determine the percent water in
- A sample of a hydrated salt weighs 10 grams. After heating, the anhydrous sample weighs 7 grams. What is the percentage of water in the original sample?
- A sample of hydrated copper (II) sulfate has a mass of 4.56 g. After heating, it has a mass of 2.92 g. What is the percent by mass of water in the hydrate?
- After 0.6523 g of CoCl_2 cdot 6H_2O is heated, the residue has a mass of 0.3423 g. Calculate the percent H_2O in the hydrate. What is the formula of the hydrate?
- 3.05 g of hydrated copper sulfate produces 1.94 g of anhydrous salt. Assuming complete removal of water of crystallization, determine the formula of hydrated copper sulfate.
- A 3.05 g of hydrated copper sulfate produces 1.94 g of anhydrous salt. Assuming complete removal of all water of crystallization, determine the formula of hydrated copper sulfate.
- A 204.2 g sample of a mixture contains 22.3% sodium chloride. What mass (g) of sodium chloride is present in the sample?
- A sample of a hydrate of NiCl2 with a weight of 0.235 grams is heated to drive off the water leaving a weight of 0.128 grams. Determine the formula of the hydrate, i.e. what is the value of X in NiCl2X(H2O)?
- A 15.67 g sample of hydrate of magnesium carbonate was carefully heated, without decomposing the carbonate to drive off water. The mass was reduce to 7.58 g. What is the formula of the hydrated?
- A 10.000 grams sample of a hydrated sodium salt gives off 6.035 grams of water when it is heated. When the dehydrated sample is analyzed, it is found to contain 1.284 g Na, 0.865 g P, 0.028 g H, and 1.787 g O. Calculate the empirical formula of the hydrat
- 1) Calculate the mole fraction of each component in a solution with 6.87 g of sodium chloride (NaCl) dissolved in 65.2 g of water. 2) Calculate the mass-to-mass ratio of 25.0 g of salt in 105 g of water.
- After 0.6523 g of hydrate is heated, the residue has a mass of 0.3423 g. Calculate the % H_2O in the hydrate.
- When 3.761 g of a hydrate of strontium chloride is heated to 60 degree C it forms strontium chloride dihydrate of mass 2.746 g. What is the formula of the original sample?
- 1.2008 g of a hydrate of CuSO_4 . XH_2O after heated has a mass of 0.7676 g. Calculate the mass percent of water, and determine the chemical formula of this hydrate.
- The thermal decomposition of 1.826 g of a hydrate of MnCl2 produces 1.161 g of anhydrous MnCl2. Calculate the mass percent of water in the hydrate.
- What is the mass of the anhydrous salt in 64 grams of cobalt(ii) chloride hexahydrate?
- A hydrate of iron (II) fluoride has the following formula: FeF2 x H2O. The water in a 3.41-g sample of the hydrate was driven off by heating. The remaining sample had a mass of 1.93 g . Find the number of waters of hydration (x) in the hydrate.
- Based on the following information, calculate the percent by mass of salt in the mixture. Mass of beaker = 75.000 g Mass of beaker + unknown = 85.175 g Mass of beaker + salt = 75.175 g Mass of salt = 0.175 g
- If 4.02 g of a hydrate of magnesium sulfate loses 2.06 grams of water when heated, what is the formula for the hydrate?
- Calculate the mass-to-mass ratio of 25.0 grams of salt in 105 grams of water.
- One hundred grams of mixture of NaSO4-10H2O and Na2CO3-10H2O are heated to drive off water of hydration. The final weight of the mixed salts is 39.6g. What is the ration of moles Na2CO3 to moles Na2SO4 in the original hydrated salts?