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To find the molar mass of copper (II) sulfate pentahydrate, calculate the individual molar masses of each element present (Cu, S, O, and H) from the Periodic Table, and then multiply by the respective subscript in the formula. Add up the molar masses of copper (II) sulfate (CuSO₄) and five water molecules (5H₂O) to get the molar mass of copper (II) sulfate pentahydrate.
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How many grams of copper(II) sulfate pentahydrate would you need to measure in order to have 10.0 grams of anhydrous copper (II) sulfate?
To calculate this, you would need to consider the molar masses of copper(II) sulfate pentahydrate and anhydrous copper(II) sulfate. Copper(II) sulfate pentahydrate has a molar mass that includes water molecules, so you need to determine the molar mass difference between the two compounds. Using this information, you can calculate the amount of copper(II) sulfate pentahydrate needed to obtain 10.0 grams of anhydrous copper(II) sulfate.
What mass of anhydrous copper 2 sulfate can be obtained by heating 125g of cuper 2 sulfate pentahydrate?
To find the mass of anhydrous copper(II) sulfate obtained: Calculate the molar mass of each compound: CuSO4·5H2O (pentahydrate) and CuSO4 (anhydrous). Use the molar ratio between CuSO4 and CuSO4·5H2O to find the amount of anhydrous CuSO4. Convert the amount to mass using the molar mass of CuSO4. The mass of anhydrous CuSO4 will be less than the initial 125g due to the loss of water upon heating.
Suppose 2.3754g of copper-II sulfate pentahydrate is heated to drive off the water of crystallization Calculate what mass of anhydrous salt will remain?
The gram formula unit mass of copper (II) sulfate pentahydrate is 249.68. The gram formula unit mass of water is 18.015. Therefore, the mass of water of crystallization present in 50.0 g of copper (II) sulfate pentahydrate is: 50[5(18.015)/249.68] or 18.0 g, to the justified number of significant digits. (Note that the prefix penta- means five)
What is the weight in grams of 3.36 1023 molecules of copper sulfate?
What is the weight in grams of 3.36 × 1023 molecules of copper sulfate (CuSO4)?
How many grams of copper sulfate would you heat to produce 29.8g of water?
Well, darling, to produce 29.8g of water, you'd need to heat 249.9g of copper sulfate pentahydrate. When you heat it, the water molecules will be driven off, leaving you with just the copper sulfate. Just make sure to wear your safety goggles, we don't need any accidents in the name of science!
How many grams of copper(II) sulfate pentahydrate would you need to measure in order to have 10.0 grams of anhydrous copper (II) sulfate?
To calculate this, you would need to consider the molar masses of copper(II) sulfate pentahydrate and anhydrous copper(II) sulfate. Copper(II) sulfate pentahydrate has a molar mass that includes water molecules, so you need to determine the molar mass difference between the two compounds. Using this information, you can calculate the amount of copper(II) sulfate pentahydrate needed to obtain 10.0 grams of anhydrous copper(II) sulfate.
What mass of anhydrous copper 2 sulfate can be obtained by heating 125g of cuper 2 sulfate pentahydrate?
To find the mass of anhydrous copper(II) sulfate obtained: Calculate the molar mass of each compound: CuSO4·5H2O (pentahydrate) and CuSO4 (anhydrous). Use the molar ratio between CuSO4 and CuSO4·5H2O to find the amount of anhydrous CuSO4. Convert the amount to mass using the molar mass of CuSO4. The mass of anhydrous CuSO4 will be less than the initial 125g due to the loss of water upon heating.
Suppose 2.3754g of copper-II sulfate pentahydrate is heated to drive off the water of crystallization Calculate what mass of anhydrous salt will remain?
The gram formula unit mass of copper (II) sulfate pentahydrate is 249.68. The gram formula unit mass of water is 18.015. Therefore, the mass of water of crystallization present in 50.0 g of copper (II) sulfate pentahydrate is: 50[5(18.015)/249.68] or 18.0 g, to the justified number of significant digits. (Note that the prefix penta- means five)
How many grams of copper sulfate pentahydrate CuSO4 5H2O would you heat to produce 29.8 g of water?
29.8g H2O = 1.66 mol H2O Molar Mass CuSO4 * 5H2O = 249.6 g mol CuSO4 * 5H2O --> 5 mol H2O 249.6 g CuSO4 * 5H2O/1 mol CuSO4 * 5H2O Times * 1mol CuSO4 * 5H2O/5mol H2O Times* 1.66 mol H2O = 82.6 g CuSO4 * 5H2O
What is the molar absorption of copper-II sulfate pentahydrate whose absorbance is 0.17 at 650nm?
Depends on the length the light traveled through the solution and the solution concentration. molar absorption = absorbance/(length x concentration) length is typically in cm and concentration is typically in mol/L
What is the weight in grams of 3.36 1023 molecules of copper sulfate?
What is the weight in grams of 3.36 × 1023 molecules of copper sulfate (CuSO4)?
How many grams of copper sulfate would you heat to produce 29.8g of water?
Well, darling, to produce 29.8g of water, you'd need to heat 249.9g of copper sulfate pentahydrate. When you heat it, the water molecules will be driven off, leaving you with just the copper sulfate. Just make sure to wear your safety goggles, we don't need any accidents in the name of science!
What is the molar weight of copper sulfate?
159.61 grams per mole.
How many grams of copper ii sulfate are required to produce 0.48 mol of aluminum iii sulfate?
To find the amount of copper (II) sulfate needed to react with 0.48 mol of aluminum (III) sulfate, start by writing a balanced chemical equation for the reaction between the two salts. From the balanced equation, determine the molar ratio between copper (II) sulfate and aluminum (III) sulfate. Then, use this ratio to calculate the amount of copper (II) sulfate needed to produce 0.48 mol of aluminum (III) sulfate.
If add water to a copper sulfate crystal will it get larger?
Copper(II) sulfate can fom 3 hydrates; the molar mass increase from the anhydrous salt to heptahydrate.
How you can prepare 18 mmol of copper sulfate tetrahydrate?
Hi MW (CuSO4.4H2O)= 64+32+(4*16)+(4*18)= 232 g/mol 18mmol= 18*10^-3 mol= 0.018 mol ?gr (CuSO4.4H2O)= 0.018mol * (232 g/mol )= 4.176 gr so, you need (4.17 gr (CuSO4.4H2O)) in 1000 ml solvent or (0.417 gr (CuSO4.4H2O)) in 100 ml solvent for example, solvent is deionized water
How many moles of anhydrous copper sulfate is produced when 6.4 moles of hydrated copper sulfate is heated?
When hydrated copper sulfate is heated, it loses its water molecules to form anhydrous copper sulfate. Since the molar ratio between the two forms is 1:1, if 6.4 moles of hydrated copper sulfate is heated, 6.4 moles of anhydrous copper sulfate will be produced.
