chemistry
A 2.500 gram sample of a hydrate of calciumsulfate loses 0.523grams of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate
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8. A 4.00 gram sample of a hydrate of nickel(II) bromide loses 0.793 grams of water...
8. A 4.00 gram sample of a hydrate of nickel(II) bromide loses 0.793 grams of water when heated. Determine the mass percent water in the hydrate and the formula of the hydrate. 9. A 2.500 gram sample of a hydrate of calcium sulfate loses 0.523 grams of water when heated. and the fomula of the hydrate Determine the mass percent of water in the hyd rate and the formula of the hydrate.
Post lab Questions: 1. While performing the formula of hydrate laboratory experiment, the lid accidently slips...
Post lab Questions: 1. While performing the formula of hydrate laboratory experiment, the lid accidently slips over the crucible to completely seal the crucible. a. What effect this change will cause on your calculated experimental results? Explain. b. Would your calculated percent water of hydration be high, low or unaffected? Explain your answer. 2. A student was asked to identify a sample of unknown hydrate. Student was provided with the following experimental data. 3.51 g sample of the hydrate when...
- Solving applied mass percent problems Iron(II) sulfate forms several hydrates with the general formula FeSO,...
- Solving applied mass percent problems Iron(II) sulfate forms several hydrates with the general formula FeSO, XH,O, where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure FeSO, behind. Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by 42.%. Which hydrate is it? That is what is?
1. How would you determine if you have heated the sample long enough to drive off...
1. How would you determine if you have heated the sample long enough to drive off all the water from the hydrate? 2. A compound is made of 30.9% of Cu, 13.6 % Si, and 55.5% F. a. What is the empirical formula of the anhydrous salt? b. 1.00 gram of this compound is subject to high moisture environment. The resulting hydrate weighs 1.53 grams. What is the formula of the hydrate?
CHM 010 On-Line Lab, Formula of a Hydrate PURPOSE: To determine the formula of Cuso..x H20....
CHM 010 On-Line Lab, Formula of a Hydrate PURPOSE: To determine the formula of Cuso..x H20. In other words, to determine the value of "X". PROCEDURE: When copper(II) sulfate x hydrate, a blue crystalline solid containing embedded water molecules (called a hydrate), is heated in air, it loses the water molecules and the blue solid is transformed to a white anhydrous (no water) crystal known as anhydrous copper(II) sulfate. The "x" represents a whole number of water molecules attached to...
A sample of pure oxalic acid hydrate was obtained by extraction from a plant called Snake...
A sample of pure oxalic acid hydrate was obtained by extraction from a plant called Snake Tongue. A 3.000 g sample of the material was heated carefully in a vacuum oven until no more mass was lost from the sample. After heating, the final weight of the material was 2.143 g. What is the formula of the oxalic acid hydrate. (COOH)_2 middot H_2O? (mol.wt. (COOH)_2 = 90.0 g/mol) An ore sample is known to contain copper sulfate pentahydrate, CuSO_4 middot...
H20 MASS of H20 2.09 8. A sample of 8.85 g of Na2CO3 hydrate is heated,...
H20 MASS of H20 2.09 8. A sample of 8.85 g of Na2CO3 hydrate is heated, losing 1.28 g of water. Find the empirical formula 8. A sample of 8.85 g of Na2CO3 hydrate is heated, losing 1.28 g of water. Find the empirical formula.
It is often possible to change a hydrate into an anhydrous compound by heating it to...
It is often possible to change a hydrate into an anhydrous compound by heating it to drive off the water (dehydration). A 30.74 gram sample of a hydrate of Ba(ClO4)2 was heated thoroughly in a porcelain crucible, until its weight remained constant. After heating, 26.49 grams of the anhydrous compound remained. What is the formula of the hydrate? Use a period instead of a dot in the formula of the hydrate.
Please provide correct work & answers to the following, thank you!! .A student observed that when heated his...
Please provide correct work & answers to the following, thank
you!!
.A student observed that when heated his sample produced condensation on the upper walls of his test tube and changed color. When the sample was added to water it produce a solution with a color very similar to that of the original salt. Explain these observations 2. A student gets a measurement of 30.112 grams when he weighs a dry empty crucible and cover. He then adds an unknown...
Stoichiometry
It is often possible to change a hydrate into an anhydrous compound by heating it to drive off the water (dehydration).A 36.04 gram sample of a hydrate of Na2SO3 was heated thoroughly in a porcelain crucible, until its weight remained constant. After heating, 18.01 grams of the anhydrous compound remained. What is the formula of the hydrate?
8. A 4.00 gram sample of a hydrate of nickel(II) bromide loses 0.793 grams of water when heated. Determine the mass percent water in the hydrate and the formula of the hydrate. 9. A 2.500 gram sample of a hydrate of calcium sulfate loses 0.523 grams of water when heated. and the fomula of the hydrate Determine the mass percent of water in the hyd rate and the formula of the hydrate.
Post lab Questions: 1. While performing the formula of hydrate laboratory experiment, the lid accidently slips over the crucible to completely seal the crucible. a. What effect this change will cause on your calculated experimental results? Explain. b. Would your calculated percent water of hydration be high, low or unaffected? Explain your answer. 2. A student was asked to identify a sample of unknown hydrate. Student was provided with the following experimental data. 3.51 g sample of the hydrate when...
- Solving applied mass percent problems Iron(II) sulfate forms several hydrates with the general formula FeSO, XH,O, where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure FeSO, behind. Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by 42.%. Which hydrate is it? That is what is?
1. How would you determine if you have heated the sample long enough to drive off all the water from the hydrate? 2. A compound is made of 30.9% of Cu, 13.6 % Si, and 55.5% F. a. What is the empirical formula of the anhydrous salt? b. 1.00 gram of this compound is subject to high moisture environment. The resulting hydrate weighs 1.53 grams. What is the formula of the hydrate?
CHM 010 On-Line Lab, Formula of a Hydrate PURPOSE: To determine the formula of Cuso..x H20. In other words, to determine the value of "X". PROCEDURE: When copper(II) sulfate x hydrate, a blue crystalline solid containing embedded water molecules (called a hydrate), is heated in air, it loses the water molecules and the blue solid is transformed to a white anhydrous (no water) crystal known as anhydrous copper(II) sulfate. The "x" represents a whole number of water molecules attached to...
A sample of pure oxalic acid hydrate was obtained by extraction from a plant called Snake Tongue. A 3.000 g sample of the material was heated carefully in a vacuum oven until no more mass was lost from the sample. After heating, the final weight of the material was 2.143 g. What is the formula of the oxalic acid hydrate. (COOH)_2 middot H_2O? (mol.wt. (COOH)_2 = 90.0 g/mol) An ore sample is known to contain copper sulfate pentahydrate, CuSO_4 middot...
H20 MASS of H20 2.09 8. A sample of 8.85 g of Na2CO3 hydrate is heated, losing 1.28 g of water. Find the empirical formula 8. A sample of 8.85 g of Na2CO3 hydrate is heated, losing 1.28 g of water. Find the empirical formula.
Please provide correct work & answers to the following, thank
you!!
.A student observed that when heated his sample produced condensation on the upper walls of his test tube and changed color. When the sample was added to water it produce a solution with a color very similar to that of the original salt. Explain these observations 2. A student gets a measurement of 30.112 grams when he weighs a dry empty crucible and cover. He then adds an unknown...
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