A mixture of CuSO4 5H2O and MgSO4 7H2O is heated until all water is lost. If 5.020 g of the...
Question:
A mixture of {eq}CuSO_4 \cdot 5H_2O {/eq} and {eq}MgSO_4 \cdot 7H_2O {/eq} is heated until all water is lost. If 5.020 g of the mixture gives 2.988 g of the anhydrous salts, what is the percent by mass of {eq}CuSO_4 \cdot 5H_2O {/eq} in the mixture?
Hydrated Salt:
Salts that have water molecules within their crystals are known as hydrated salts. {eq}MgSO_4\cdot 7H_2O \space and \space CuSO_4\cdot 5H_2O {/eq} are examples of hydrated salts. When these salts are heated, they lose water and become anhydrous salts ({eq}MgSO_4 \space and \space CuSO_4 {/eq}).
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerWe are given a mixture of {eq}CuSO_4\cdot5H_2O\; \space and \space \;MgSO_4\cdot 7H_2O {/eq} and {eq}5.020 \space g {/eq} of the mixture gives out...
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
Dehydration Reaction: Definition & Examples
from
Chapter 4 / Lesson 12
24K
Learn about dehydration. Understand what a dehydration reaction is, see a comparison between hydrolysis vs. dehydration, and see examples of a dehydration reaction.
Related to this Question
- A mixture of CuSO_4 and CuSO_4.5 H_2O has a mass of 1.235 g. After heating to drive off all the water, the mass is only 0.830 g. What is the mass percent of CuSO_4.5 H_2O in the mixture?
- 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
- 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.
- Determine the percentage by mass of water in the hydrate CuSO4 5H2O.
- 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?
- What is the percent composition of water in CuSO4 5H2O?
- 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?
- 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.
- Blue copper sulfate pentahydrate (CuSO_4.5H_2O) crystals were heated to give the white monohydrate. What percentage of water was lost? (molar mass of CuSO_4.5H_2O is 250.5 g/mol)
- What is the mass percent of water in copper (II) sulfate hydrate?
- What is the mass percent of copper sulfate CuSO_4 in a sample of copper sulfate pentahydrate CuSO_4.5H_2O?
- Calculate the percentage of water in CuSO4 5H2O.
- What is the percent of water in CuSO_4 x-H_2O?
- 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
- What is the percent by mass of CuSO4 in a sample that is 74.4% CuSO4, 5H2O by mass?
- A mixture of sodium sulfate and its hydrate, sodium sulfate decahydrate has a mass of 1.8092 g. After heating to drive off all the water, the mass is only 1.6526 g. What is the weight percentage of the hydrate in the original mixture? Report your answer t
- 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
- 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.
- What is the percent of copper in CuSO_4 \cdot 5H_2O?
- 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)?
- 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
- 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
- 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?
- What is the percent copper sulfate in a mixture, if 3.21 g of copper sulfate was isolated from a 7.00 g mixture?
- 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 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?
- What is the percent by mass of copper sulfate, CuSO4, in a sample of copper sulfate pentahydrate, CuSO4, 5H2O?
- 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?
- Calculate the mass of CuSO_4 in 2.26 grams of CuSO_4 \cdot 5H_2O.
- 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. 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/
- 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 2.500 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.
- 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
- 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 sample of raw mining ore contains a hydrated salt called copper sulfate pentahydrate, CuSO4.5H2O. If a 9.854g of the ore loses 1.499g of water when heated strongly, what is the mass percentage of
- 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
- 1.) An unknown hydrate, AC XH2O, has a mass of 1.000 g before heating, and has a mass of 0.738 g after heating. What is the experimental percentage of water in the hydrate? 2.) If the anhydrous compou
- 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 chemist is given a sample of the CuSO4 hydrate and asked to determine the empirical formula of it. The original sample weighed 42.75 g, and after heating, the sample weighed 27.38. What is the formu
- 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.
- Determine the mass percent of water in cupric sulfate pentahydrate.
- 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.
- The number of grams of CuSO_4 5H_2O that will dissolve in 100g of H_2Oat 100 C.
- 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?
- Calculate the percent composition of copper in the hydrate CuSO_4 cdot 5H_2O based on atomic weight data.
- 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 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.
- Suppose you obtain 0.0166 mol for the amount of anhydrous salt and 0.1328 mol for the amount of water. What is the formula of the hydrate? Let X be the formula of the anhydrous salt.
- If you evaporated 19.568g of H_2O from a 48.001g hydrate sample, what is the percent H_2O of the compound?
- 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 mixture of NiSO4 and its hydrate NiSO4 dot 6H2O has a mass of 1.9319 g. After heating to drive off all the water, the mass is only 1.6438 g. What is the weight percentage of NiSO4 dot 6H2O in the original mixture? Give your answer to 4 significant figur
- Predict the effect of each of the following by mass of water in the hydrate CuSO4 x 5H2O and the chemical of the hydrate. a. not heating the hydrate enough b. overheating the hydrate and producing som
- 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.
- Alum, a compound used for cooking and in water filtration, is a hydrate. You heat a 4.74 g sample of the hydrated Alum and are left with 2.58 g of the anhydrous salt K A l ( S O 4 ) 2 . How many grams of water were lost? What is the formula of the hydrat
- What is the mass percent of Cu in copper (II) sulfate pentahydrate CuSO_4 \cdot 5H_2O?
- Calculate the molar mass of CuSO4 5H2O.
- 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
- 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?
- 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
- What is the empirical formula of CuSO_4 cdot 5H_2O?
- An organic extract or layer was dried by adding solid anhydrous Na2SO4 to it. About 0.542 g of water was removed and the anhydrous salt became Na2 SO4.10H2O. What mass in grams of the hydrated sodium sufate (i.e.. Na2SO4 . 10H2O) was obtained? Given the
- A sample of 5.00 grams of CaSO4 2H2O is heated to drive off water. What is the mass of the remaining anhydrous salt?
- What is the percentage composition of water in a sample of SrS2O3 + 5H2O? (this is a hydrate)
- 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
- What is the mass of one formula unit of CuSO4?
- Calculate the mass of Copper (II) sulfate CuSO_4 needed to make 3.00 L of 3.0 M solution?
- 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
- 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.
- An unknown hydrate, AC XH_2O, has a mass of 1.000 g before heating, and a mass of 0.738 g after heating. What is the experimental percentage of water in the hydrate?
- 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 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.
- A 2.50 g sample of a hydrate of calcium nitrate was heated, and only 1.70 g of the anhydrous salt remained. what is the formula of 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?
- Cobalt(II) chloride is commonly obtained from chemical suppliers as a hydrate with the formula CoCl2 6H2O. What is the percent water by weight in this hydrate?
- One hundred grams of mixture of NaSO_4.10H_2O and Na_2CO_3.10H_2O are heated to drive off water of hydration. The final weight of the mixed salts is 39.6 g. What is the ration of moles Na_2CO_3 to mol
- A thoroughly dried 1.281 g sample of Na_2SO_4 is exposed to the atmosphere and found to gain 0.383 g in mass. What is the percent, by mass, of Na_2SO_4 . 10H_2O in the resulting mixture of anhydrous N
- 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 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 5.00-gram sample of NiCl2 xH2O is heated, driving off 2.28 grams of water. What is the empirical formula of the hydrate?
- What is the percent by mass of water in the hydrate MgCl2 5H2O?
- 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.
- What is the percent of H_2O in a sample of a hydrate whose mass is 1.1290 g if the mass of water in the sample was 0.1660 g?
- When a hydrate of Na_2CO_3 is heated until all the water is removed, it loses 54.3 percent of its mass. The formula of the hydrate is (a) Na_2CO_3 cdot 10H_2O (b) Na_2CO_3 cdot 7 H_2O (c) Na_2CO_3 cdot 5H_2O (e) Na_2CO_3 cdot 3H_2O (f) Na_2CO_3 cdot H_2O
- What is the molar mass of the copper(ll) sulphate CuSO4?
- What is the percent by mass of water in MgSO4 7H2O? a. 51.1% b. 56.0% c. 195% d. 21.0%
- A mixture of MnSO_4 and MnSO_4.4H_2O has a mass of 2.005 g. After heating to drive off all the water the mass is 1.780 g. How many grams of MnSO_4.4H_2O are presented in the mixture? What is the mass percent of MnSO_4.4H_2O in the mixture?
- 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.
- What is the percentage of water in the hydrate CoCl_2 . 6H_2O?
- What is the maximum mass of copper (II) sulfate pentahydrate, CuSO4 5H2O, which could be obtained by crystallizing the solution? Ar: H = 1; O = 16; S = 32; Cu = 63.5
- The mass of water in a hydrate of MnCl2 is 36.41%. What is the empirical formula of the hydrate?
- 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 an experiment, a hydrate is heated to form an anhydrate. The masses of the before and after are measured and the percent of the water in the hydrate is calculated. If some of the hydrate spatters o
- What mass of Cu(IO_3)_2 can be formed from 0.650 g of CuSO_4 cdot 5H_2O ?
- 5 g of iron sulfate pentahydrate was dried for 30 minutes and had a 15 percent loss of total mass to the air. What is the formula after drying? How much water was lost in grams and in moles?
- Determine the number of grams of water in 7.00 g of copper(II) sulfate pentahydrate.
- 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
- When 67.5 g of an unknown hydrate CaSO_4.xH_2O was heated until all the water was driven off, the resulting mass of pure CaSO_4(s) was 53.4 g. What is the formula of hydrate?
- A 2.43 g sample of FeCl_3.H_2O is heated and 1.09 g of anhydrous residue remains. What is the mole ratio of water to anhydrate?
Explore our homework questions and answers library
Browse
by subject