Question

Suppose a student performs a similar experiment to determine the empirical formula of a barium chloride...

Suppose a student performs a similar experiment to determine the empirical formula of a barium chloride hydrate. Given the data collected in the table above, what is the formula of the hydrate? The molar mass of water is 18.015 g/mol and the molar mass of barium chloride is 208.23 g/mol. (2 points)

mass of empty crucible

55.060 g

mass of crucible and hydrate

57.083 g

mass of crucible and anhydrous salt

56.434 g
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
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...
Please show the work. Thank you Formula of a Hydrate Data: Mass of the crucible and...
Please show the work. Thank you Formula of a Hydrate Data: Mass of the crucible and cover                                              51.729g Mass of crucible, cover and sample                                       52.388g Mass of crucible, cover and salt after first heating               52.258g Mass of crucible, cover and salt after second heating          52.254g Calculations: Chemical formula of anhydrous salt (given)                          CaSO4 Mass of hydrate (sample)                                                      0.659g Mass of anhydrous salt                                                          ______ ? Mass of water liberated                                                         ______ ? Percentage H2O in the hydrate                                              ______ ? Moles...
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...
• Using the dehydration equation of hydrated barium chloride, answer the following question: a) If 3...
• Using the dehydration equation of hydrated barium chloride, answer the following question: a) If 3 moles of hydrated barium chloride was heated, how many moles of anhydrous barium chloride, and how many moles of water vapor will be produced? b) 20 g of sand was mixed with 5 g of a hydrate. Calculate the percentage of the hydrate in this mixture. c) If you know that the real percentage of the hydrated barium chloride was exactly 25% out of...
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? ?...
A student performs an experiment similar to experiment 1 using hydrochloric acid (HCl) and potassium hydroxide...
A student performs an experiment similar to experiment 1 using hydrochloric acid (HCl) and potassium hydroxide (KOH). The mass of the hydrochloric acid solution is 250.000 g. After combining the HCl and KOH, the final combined mass is 400.000 g. Given what you have learned about the conservation of mass in this experiment, what must have been the mass of the KOH solution?
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 student performed the Separation by Fractional Crystallization experiment described with the following results: Initial mass...
A student performed the Separation by Fractional Crystallization experiment described with the following results: Initial mass of sample mixture: 9.58 g, mass of salicylic acid recovered, 4.35 g; mass of CuSO4•5H2O recovered, 4.68 g. The recovered CuSO4•5H2O was then heated for 20 minutes at 120 °C. The mass of the new hydrate was 3.83 g. (The molar mass of H2O = 18.015 g/mol, and the molar mass of CuSO4= 159.61 g/mol) Calculate the mass of water in the new hydrate...
1. While performing the formula of hydrate laboratory experiment, the lid accidently slips over the crucible...
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 anwer. 2. A student was asked to identify a sample of unknown hydrate. Student was provided with the following experimental data. [ 3.51g sample of the hydrate when heated loses water...
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....
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT