A 0.755-g sample of hydrated copper(II) sulfate (CuSO_4 \cdot xH_2O) was heated carefully until...
Question:
A 0.755-g sample of hydrated copper(II) sulfate {eq}(CuSO_4\cdot xH_2O) {/eq} was heated carefully until it had changed completely to anhydrous copper(II) sulfate ({eq}CuSO_4 {/eq}) with a mass of 0.483 g. Determine the value of x. (This number is called the "number of waters of hydration" of copper(II) sulfate. It specifies the number of water molecules per formula unit of {eq}CuSO_4 {/eq} in the hydrated crystal.)
Hydrates
Ionic compounds that contain water in their structure via hydrogen bonding are called hydrates. The number of moles of salt and the number of moles of water in a hydrate occurs in whole number ratios.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerWhen hydrated copper(II) sulfate is heated, water is removed from the hydrate as water vapor and an anhydrous form of the salt is produced.
This can...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Hydrates: Determining the Chemical Formula From Empirical Data
from
Chapter 9 / Lesson 8
337K
Learn 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
- Determine the number of grams of water in 7.00 g of copper(II) sulfate pentahydrate.
- A hydrate of copper (II) sulfate with formula CuSO_4 . x H_2O has a molar mass of 250.0 g/mol. 2.545 g of hydrate is heated and 63.85% of the residue is found after heating. a) Determine the value of
- A 2.78 g sample if hydrated iron(II) sulfate, FeSO4 \cdot X H2O, was heated to remove all of the water, the mass of the anhydrous compound was 1.52 g. Calculate the number of water molecules associated with each molecule? What is X?
- 1. Use the formula of CuSO_4.H_2O to determine the mass percent of water in copper(II) sulfate pentahydrate. 2. A 5.000-g sample of CuSO_4.5H_2O was heated several times, eventually leaving a solid residue with a mass of 3.196 g. Calculate the experiment
- A hydrate of copper(II) sulfate was thermally decomposed to 0.7981 g CuSO4 and 0.5405 G of H20. Derive the value of X for the hydrate, CuSo4 XH20. (Assume CuSo4, 159.62 amu, H20, 18.02amu
- A hydrated form of copper sulfate (CuSO4 xH2O) is heated to drive off all the water. If we start with 8.51 grams of hydrated salt and have 6.36 grams of anhydrous CuSO4 after heating, find the number of water molecules associated with each CuSO4 formula u
- 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 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?
- 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.
- A sample of a hydrate of CuSO_4 with a mass of 250 grams was heated until all the water was removed. The sample was then weighed and found to have a mass of 160 grams. What is the formula for the hydr
- Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. Mass of water = 0.95 g Mass of anhydrous copper sulfate = 2.19 g Mass of hydrate copper sulfate = 3.14 g
- When 25.0 g of copper (II) sulfate pentahydrate (bluestone) is heated, all the water of hydration is removed from the compound, leaving behind pure anhydrous copper (II) sulfate. What would its dehydrated mass (in grams) be?
- 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.
- 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 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.
- 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.
- Calculate the mass of copper(II) sulfate pentahydrate needed to prepare 0.600 M stock solution of copper (II) from solid copper (II) sulfate pentahydrate, CuSO_4 cdot 5H_2O.
- 10.0g of hydrated sodium sulphate decomposes to form 4.40g of anhydrous sodium sulfate on heating. Calculate formula mass of hydrated sodium sulphate and the value of x.
- 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.
- 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.
- Calculate the mass of CuSO_4 in 2.26 grams of CuSO_4 \cdot 5H_2O.
- One of the hydrates of MnSO4 is manganese(II) sulfate pentahydrate. A 56.0-gram sample of MnSO4 5H2O was heated thoroughly in a porcelain crucible until its weight remained constant. After heating, how many grams of the anhydrous compound remained?
- A hydrate of CuSO4 has a mass of 11.71 g before heating. After heating, the mass of the anhydrous compound is found to be 8.75 g. Explain how you would determine the formula of the hydrate and then write out the full name of the hydrate.
- 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 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
- Suppose you begin with 1.50 g of the hydrate copper(II)sulfate x-hydrate (CuSO4 xH2O), where x is an integer. After dehydration you find that you are left with 0.96 g of the an-hydrate CuSO4. What is
- What is the mass percent of copper sulfate CuSO_4 in a sample of copper sulfate pentahydrate CuSO_4.5H_2O?
- If copper (II) sulfate pentahydrate is known to be 36% of water, how many grams of water will be lost when heating a 5.75 grams sample?
- A chemist is given a sample of a CuSO4 hydrate and asked to determine the empirical formula of it. The original sample weighed 42.75 grams. After heating to remove the waters of hydration, the sample weighed 27.38 grams. Determine the formula for this hyd
- When 20.9 g of copper (II) sulfate pentahydrate (bluestone) is heated, all the water of hydration is removed from the compound, leaving behind pure anhydrous copper (II) sulfate. What would its dehydrated mass (in g) be? The balanced chemical equation is
- 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 chemist heats a sample of copper (II) sulfate and finds that 63.9 % of the mass is copper (II) sulfate and the other 36.1 % by mass is the water. What is the formula of the hydrate?
- For the substance magnesium sulfate, anhydrous, the quantity is 0.100 g find its molar mass.
- When a 8.192 g sample of bluish-green crystals of hydrated nickel(II) sulfate is heated, all of the water of hydration is lost leaving 4.826 g of anhydrous nickel(II) sulfate. Write the formula of the hydrated crystal, showing the number of moles of water
- A 4.2039-gram sample of a hydrate of Cu(NO3)2 was heated to drive off all of the water of hydration. The remaining solid weighed 3.2635 grams. If Cu(NO3)2 xH2O represents the formula of the hydrate, what is the value of x?
- 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?
- 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 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
- Describe how to find the % by mass of water in the hydrate CuSO4 cdot 5H2O assuming that the formula is not yet known. Be specific and list the laboratory procedural steps to take.
- 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
- Determine the mass percent of water in cupric sulfate pentahydrate.
- A student heated a 1.564-g sample of a hydrate and recovered 1.333 g of an anhydrous compound. A. Calculate the percent water in the hydrate. B. The formula of the anhydrous compound was BaCl2. Calculate the number of moles of anhydrous compound recovered
- 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.
- Unknown Hydrate: CuSO_4-5H_2O Mass of test tube and hydrate, grams: 17.53, Mass of empty test tube, grams: 15.81, Mass of unknown hydrate, grams: 1.72, Mass of test tube and anhydrous hydrate (after heating), g: 17.05, Mass of empty test tube, grams: 15.8
- Write the chemical formula for copper(II) sulfate pentahydrate and calculate the formula mass.
- A chemist is given a sample CuSO_4 hydrate and asked to determine the empirical formula of it. The original sample weighed 42.75 g. After heating to remove the waters of hydration, the sample weighed 27.38 g. Determine the formula for this hydrate.
- When separated from a water solution, CuSO4 forms a hydrate with 5 water molecules per formula unit. If 45 grams of anhydrous CuSO4 are dissolved in water, what mass of the hydrate could be recovered from the solution?
- When separated from a water solution, CuSO4 forms a hydrate with 5 water molecules per formula unit. If 37 g of anhydrous CuSO4 are dissolved in water, what mass of the hydrate could be recovered from
- The number of grams required of water to dissolve 4.0g of CuSO4 * 5H2O at 100 degree C.
- Determine the percentage by mass of water in the hydrate CuSO4 5H2O.
- 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 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. What is the value of n in the formula CoBr2 nH2O for this hydrate?
- 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 6.25 gram sample of copper(II) chloride hydrate was heated until all the water was liberated. The residue massed 4.45 grams. How many water molecules are present for every formula unit of copper(II)
- What is the percent water in copper (II) sulfate pentahydrate (molar mass of copper(II) sulfate pentahydrate = 159.61 g/mol, molar mass of H_2O = 18.01 g/mol)?
- Suppose you want to know the formula of a hydrate of magnesium sulfate. If you heat 1.998 g of the hydrate until all of the water is vaporized, the mass of anhydrous M g S O 4 is 0.976 g. What is the formula of the hydrate, i.e. what is the value of x in
- 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.
- Mass of sample 0.0581 g Mass of BaSO4 0.0860 g What is the mass of sulfate?
- 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
- 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.
- 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
- A quantity of Epsom salts, magnesium sulfate heptahydrate, MgSO47H2O, is heated until all the water is driven off. The sample loses 11.8 g in the process. What was the mass of the original sample?
- A 4.1045-gram sample of a hydrate of NiSO4 was heated to drive off all of the water of hydration. The remaining solid weighed 2.2616 grams. If NiSO4 xH2O represents the formula of the hydrate, then what is the value of x?
- The calculated ratio of moles of water to moles of anhydrous salt in CuSO4 xH2O is determined to be 5.12 to 1 in an experiment. Explain why this number should be rounded off to give a hydrate formula of CuSO4 5H2O and not written as CuSO4 5.12H2O. What co
- 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?
- 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?
- 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
- 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
- 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 sample of MgSO4 7H2O weighs 15 grams. After heating, the anhydrous sample weighs 7 grams. What is the percentage of water in the original sample?
- A 2.634 g sample containing impure CuCl_2 cdot 2H_2O was heated. The sample mass after heating to drive off the water was 2.125 g. (a) What was the mass percent of CuCl_2 cdot 2H_2O in the original sample?
- Hydrated calcium sulfate contains 55.8 % sulfate by mass. Calculate the value for n.
- Calculate the mass of Copper (II) sulfate CuSO_4 needed to make 3.00 L of 3.0 M solution?
- a. If an unknown hydrate, AC XH2O, has a mass of 1.555 g before heating and a mass of 0.994 g after heating, what is the experimental percentage of water in the hydrate? b. If the anhydrous compound (AC) in the preceding problem has a molar mass of 160 g/
- Given: Na_2SO_4.nH_2O, the molar mass of sodium sulfate is 142.05 g/mol. Upon heating 8.5 g sample of Sodium Sulfate hydrate, it loses 4.776 grams after heating. Find the n for the hydrate?
- 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?
- 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.
- What is the mass percent of Cu in copper (II) sulfate pentahydrate CuSO_4 \cdot 5H_2O?
- A solid hydrate weighing 2.682 grams was heated to drive off the water. A solid anhydrous residue remained, which weighed 1.420 grams. a. Calculate the percent of water in the hydrate. b. If the anhydrous residue has a formula weight of 142, how many mole
- If 125 grams of magnesium sulfate heptahydrate is completely dehydrated, how many grams of anhydrous magnesium sulfate will remain?
- One of the hydrates of Ba(ClO4)2 is barium perchlorate trihydrate. A 59.7-gram sample of Ba(ClO4)2 dot 3 H2O was heated thoroughly in a porcelain crucible until its weight remained constant. After heating, how many grams of the anhydrous compound remained
- 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
- 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
- 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?
- 45.3 g of magnesium sulfate heptahydrate is heated in an oven until all the water is driven off. What is the mass of the anhydrous compound?
- 76.2 g of magnesium sulfate heptahydrate is heated in an oven until all of the water is driven off. What is the mass of the anhydrous compound?
- What is the mass percent of water in copper (II) sulfate hydrate?
- If the mass percentage of water in FeSO_4 \cdot XH_2O is 45.3%, find the number x?
- The following questions deal with copper(II) sulfate. (a) In part B of this experiment, you will use copper(II) sulfate pentahydrate. What is the molar mass of this compound? .....g/mol (b) How much
- Calculate the molar mass of CuSO4 5H2O. A. 159.62 g/mol B. 249.70 g/mol C. 177.64 g/mol D. 185.72 g/mol E. 446.48 g/mol
- 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. What is the percent by mass of water in iron(II) sulfate heptahydrate, FeSO_4 \cdot 7H_2O (or what percent of the molar mass of FeSO_4 \cdot 7H_2O is due to the waters of crystallization)? b. What mass due to waters of crystallization is present in a
- An ore sample is known to contain copper sulfate pentahydrate,CuSO_4\cdot5H_2O. If a 10.000 g sample of the ore loses 0.336 g of water when heated strongly, what is the maximum quantity of CuSO_4\cdot5H_2O that could be in the sample? (Molar Mass CuSO_4 \
- 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 3.82-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 3.564 g of a 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 mass of water lost from the hydrated salt.
- What is the molar mass of the copper(ll) sulphate CuSO4?
- The formula of a hydrate is CaSO4 5H2O. How do you calculate the number of moles of water removed by heat from a sample of the hydrate?
- 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.
Explore our homework questions and answers library
Browse
by subject