Question

A student needs to prepare a 0.1 mg total mixture with a mole fraction of urea...

A student needs to prepare a 0.1 mg total mixture with a mole fraction of urea (Xurea) = 0.4673. How much TCA and urea (in mg) is needed for this mixture?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Tatal mixture = 0.1 mg

Urea mole fraction = 0.4673

TCA mole fraction = 1 - 0.4673 = 0.5327

mole fraction of urea = mg of urea/(mg of urea +mg of TCA)

mg of urea = mole fraction of urea (mg of urea +mg of TCA)

= 0.4673 0.1 = 0.04673 mg

mg of urea = 0.04673 mg

mole fraction of TCA = mg of TCA/(mg of urea +mg of TCA)

mg of urea = mole fraction of TCA (mg of urea +mg of TCA)

= 0.5327 0.1 = 0.05327 mg

mg of TCA = 0.05327 mg

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
Find the mass of urea needed to prepare 51.00 g of an aqueous solution in which...
Find the mass of urea needed to prepare 51.00 g of an aqueous solution in which the mole fraction of urea is 0.0751. The molar mass of urea is 60.06 g/mol. Is there a simple way to do this? I am confused with explanations for this.
A common concept that crops up in a Dalton's Law context is mole fraction. Suppose you...
A common concept that crops up in a Dalton's Law context is mole fraction. Suppose you had equal moles of two different gases in a mixture. Then the mole fraction for each would be 0.50. The mole fraction for each gas is simply the moles of that gas divided by the total moles in the mixture. Seems simple enough. How does it relate to Dalton's Law? Answer: the mole fraction also gives the fraction of the total pressue each gas...
A. What is the mole fraction of each component in a mixture of 12.63 g of...
A. What is the mole fraction of each component in a mixture of 12.63 g of H2, 66.89 g of N2, and 19.55 g of NH3? Express your answers using three significant figures separated by commas. B. A special gas mixture used in bacterial growth chambers contains 1.00 % by weight CO2 and 99.0 % O2. What is the partial pressure (in atmospheres) of each gas at a total pressure of 0.871 atm ? Enter your answers numerically separated by...
You isolate a subcellular fraction and find the protein concentration to be 40 mg/mL. a) Show...
You isolate a subcellular fraction and find the protein concentration to be 40 mg/mL. a) Show all calculations and explain how you would prepare 50 µL of a 4 mg/mL final concentration after dilution in 2X sample buffer. (Final concentration after mixing with 2X sample should be 4 mg/mL). b) You are asked to load 20 µg total proteins into a well in the polyacrylamide gel. How many microlitres of the sample prepared above should you load onto the gel?
A student needs to accurately deliver 30 mL of solution but has only a 10 mL...
A student needs to accurately deliver 30 mL of solution but has only a 10 mL pipet. From a prior calibration, the student knows that a 95% confidence interval for a single delivery from this pipet is 9.9914 ± 0.0077 mL. [Note that “accurately deliver” does not mean to pipet exactly 30 mL. The actual volume just needs to be near 30 mL and accurately known: “the exact amount doesn’t matter as long as you know exactly how much it...
1. what volume of a 5% product is required to prepare 900ml of a 1% solution...
1. what volume of a 5% product is required to prepare 900ml of a 1% solution by adding 3% of a product? a) 600ml b) 300ml c) 450ml d) none of the above 2. A prescription for 250ml of a cough mixture calls for 2mg of hydrocodone bitartrate per teaspoonful. How many tablets, each containing 5 mg of hdrocodone bitartrate, should be used in preparing the cough mixture? a) 0.20 b) 0.100 c) 6.6 d) 3.3 3) How many teaspoonfuls...
1) Use Henry's law to determine the molar solubility of helium at a pressure of 1.9...
1) Use Henry's law to determine the molar solubility of helium at a pressure of 1.9 atm and 25 ∘C. Henry’s law constant for helium gas in water at 25 ∘C is 3.70⋅10−4M/atm. 2) A 2.800×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.2 mL...
Suppose the total pressure in a bottle of soda water before it is opened is 40...
Suppose the total pressure in a bottle of soda water before it is opened is 40 psig (http://hypertextbook.com/facts/2000/SeemaMeraj.shtml) and that the gas mixture is 75% CO2 and 25% other gases. The temperature is 10°C. The Henry’s Law constant is 0.104x104 atm. a) If the system is in equilibrium, how much CO2 is dissolved in the soda? (For this problem,ignore reactions between the CO2 and the water.) I know the answer is about 6500 mg/L but I'm having trouble finding the...
Suppose the total pressure in a bottle of soda water before it is opened is 40...
Suppose the total pressure in a bottle of soda water before it is opened is 40 psig (http://hypertextbook.com/facts/2000/SeemaMeraj.shtml) and that the gas mixture is 75% CO2 and 25% other gases. The temperature is 10°C. The Henry’s Law constant is 0.104x104 atm. a) If the system is in equilibrium, how much CO2 is dissolved in the soda? (For this problem,ignore reactions between the CO2 and the water.) I know the answer is about 6500 mg/L but I'm having trouble finding the...
1.) Indicate which aqueous solution has the lowest vapor pressure: a. 0.2 M MgCl2   b. 0.1...
1.) Indicate which aqueous solution has the lowest vapor pressure: a. 0.2 M MgCl2   b. 0.1 M MgCl2   c. 0.2 M NaCl d. 0.1 M KCl e. 0.1 M Na2CO3 2.) Indicate which aqueous solution has the fastest evaporation rate. a. 0.2 M MgCl2   b. 0.1 M MgCl2   c. 0.2 M NaCl d. 0.1 M KCl e. 0.1 M Na2CO3 3.) What is the molarity of a sucrose (C12H22O11) solution that produces an osmotic pressure of 2.65 atm at 25°C?...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT