Question

The calculated ratio of moles water to moles anhydrous salt in CuSO4·xH2O is determined to be...

The calculated ratio of moles water to moles anhydrous salt in CuSO4·xH2O is determined to be 5.12 to 1 in an experiment. Explain why should this number be rounded off to give a hydrate formula of CuSO4 ·5H2O and not written as CuSO4·5.12H2O.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

In empirical formula of a compound, atoms are present in simple whole number ratios. So in calculation of empirical formula of a compound or number of moles of water of crystallisation in 1 mole of a hydrated salt, the number of atoms/moles of water of crystallisation is never kept as a decimal and needs to be rounded off to the nearest whole number. That is why though the calculated ratio of moles of water to moles of anhydrous salt is 5.12 to 1, it is rounded off to 5 to 1. Also this gives the formula CuSO4.5H2O which is in agreement with the known formula of the hydrated copper sulphate. The difference between the experimentally calculated ratio and the theoretical ratio (5:1) could be due to errors in carrying out the experiment.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
To obtain a high enough ratio of moles water:moles anhydrous salt for your hydrated salt: Select...
To obtain a high enough ratio of moles water:moles anhydrous salt for your hydrated salt: Select one: a. you should skip the step of heating the crucible before adding the hydrated salt b. all of the water in the hydrate salt must be driven off c. you must add water to the anhydrous salt d. you must start with a sufficiently high mass of hydrated salt prior to heating e. you should calculate the mass of water driven off from...
These are questions on the pre-lab of Synthesis and Analysis of Alum Crystals. 1. A student...
These are questions on the pre-lab of Synthesis and Analysis of Alum Crystals. 1. A student conducts an experiment on a different hydrate. The empty crucible is heated to a constant mass of 24.330. A sample of the unidentified hydrate is placed in the crucible, and the total mass is 31.571 g. The crucible and hydrate are heated to constant mass, which is measured at 29.002 g. The molar mass of the anhydrous salt is 159.609 g. a. Calculate the...
Empirical Formula of Epsom Salt Introduction Hydrates are crystalline solids that contain a fixed number of...
Empirical Formula of Epsom Salt Introduction Hydrates are crystalline solids that contain a fixed number of water molecules as an integral part of their crystalline structure. The number of water molecules bound per metal ion is often characteristic of that particular metal ion. One of the common hydrates is hydrated magnesium sulfate (Epsom salt). Epsom salt is used to reduce inflammation when applied externally. Epsom salts formula is sometimes written as MgSO4.xH2O. In this experiment, you will be trying to...
A hydrate form of copper sulfate (CuSO4x H2O) is heated to drive off all the water....
A hydrate form of copper sulfate (CuSO4x H2O) is heated to drive off all the water. If we start with 9.31g of hydrated salt and have 5.95g of anhydrous CuSO4 after heating, find the number of water molecules associated with each CuSO4 formula unit.
An empirical formula is the lowest whole number ratio of the elements in a compound and...
An empirical formula is the lowest whole number ratio of the elements in a compound and provides information about the composition of a compound. For instance, the compound sodium sulfate decahydrate has the chemical formula Na2SO4•10H2O. This formula conveys the information that there are ten water molecules per two sodium ions per one sulfate ion. You might wonder: “How were these ratios determined?” To answer the question it is necessary to recognize that the ratio of atoms (or ions) is...
1. A student was given a sample of an anhydrous salt to anazlyze, using the procedure...
1. A student was given a sample of an anhydrous salt to anazlyze, using the procedure described in this experiment. The student weighed the sample but decided to do the experiment the following day. The weighed sample was left unconvered on the bench overight. a) What error(s) might result if the student used this salt sample in a determination the following day? Briefly explain. b) Would the student avoid any error(s) desribed in (a) by reweighing the salt sample on...
1. A 5.25g sample of magnesium sulfate hydrate is heated until the masses stabilize. If the...
1. A 5.25g sample of magnesium sulfate hydrate is heated until the masses stabilize. If the residue has a mass of 2.56g, answer the following. Show your formula and then how your data is substituted into the formula. ? What is the mass of the original hydrate? ? What is the mass of the anhydrous salt? ? What mass of water was removed? ? What percentage of the compound was water? ? How many moles of water were removed? ?...
Data Table 1. Alum Data Object Mass (g) Aluminum Cup (Empty) 2.4 g Aluminum Cup +...
Data Table 1. Alum Data Object Mass (g) Aluminum Cup (Empty) 2.4 g Aluminum Cup + 2.0 grams of Alum 4.4 g Aluminum Cup + Alum After 1st Heating 3.6 g Aluminum Cup + Alum After 2nd Heating 3.4 g Mass of Released H2O 1.0 g Moles of Released H2O 18.006 g Not sure Questions: Calculate the moles of anhydrous (dry) KAl(SO4)2 that were present in the sample. Calculate the ratio of moles of H2O to moles of anhydrous KAl(SO4)2....
Given the following experimentally determined values, answer the questions. .009070 mol Cl .00565 mol Cu .00385...
Given the following experimentally determined values, answer the questions. .009070 mol Cl .00565 mol Cu .00385 mol Zn Ratio of Chloride to copper = 1.61:1 Ratio of chloride to zinc = 2.36:1 Ratio of zinc to copper = .681:1 What are your experimentally-determined formulas for (i) copper chloride, and (ii) zinc chloride? Once you have calculated the moles of each element/ion (Cu, Zn, and Cl– ), you can then determine the empirical formula of copper chloride by computing the ratio...
1. Hydrogen sulfide is composed of two elements, hydrogen and sulfur. In an experiment,6.600g hydrogen sulfide...
1. Hydrogen sulfide is composed of two elements, hydrogen and sulfur. In an experiment,6.600g hydrogen sulfide is fully decomposed into its elements. a. if 0.384g og hydrogen is obtained in this experiment, how many grams of sulfur must be obtained? b. what fundamental law does this experiment demonstrate? 2.only two isotopes of cooper occur naturally 65Cu(atomic mass=62.9296 amu; abundance=69.17%) and 65Cu(atomic mass=64.9278 amu;abundance=30.83%). calculate the average atomic mass cooper. 3. calculate the following quantities a. mass in grams of 1.223...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT