Sunday
April 20, 2014

Search: how many mL urea solution required to react with Fe3+

Number of results: 31,805

Chemistry
A 2.30 m solution of urea (CO(NH2)2; FW= 60.0) in water has a density of 1.14 g/mL. Calculate the percent mass of urea in this solution?
Tuesday, February 9, 2010 at 11:09pm by cc

Chemistry
A 2.30 m solution of urea (CO(NH2)2; FW= 60.0) in water has a density of 1.14 g/mL. Calculate the percent mass of urea in this solution
Tuesday, February 9, 2010 at 11:19pm by cc

chemistry
A 2.30 m solution of urea (CO(NH2)2; FW= 60.0) in water has a density of 1.14 g/mL. Calculate the percent mass of urea in this solution
Tuesday, February 9, 2010 at 11:21pm by CC

chemistry
The molarity of urea in a solution prepared by dissolving 16 g of urea (MW 60.0g/mol) in 39 g of H2O is ______M. The density of the solution is 1.3 g/ml.
Tuesday, March 9, 2010 at 1:32am by CC

chemistry
The molarity of urea in a solution prepared by dissolving 16 g of urea (MW = 60.0 g/mol) in 39 g of H2O is __________ M. The density of the solution is 1.3 g/mL. i get 8.9 but the practice test says the answer its 6.3
Sunday, September 26, 2010 at 2:28pm by BenY

chemistry
describe how you would prepare from the specified stock solution: 400 mL of 0.45 M urea starting with a 6 M urea stock solution
Sunday, July 24, 2011 at 4:15pm by luv2swim

AP Bio (but its a question about chemistry)
no idea how to do this... describe how you would prepare from the specified stock solution: 400 mL of 0.45 M urea starting with a 6 M urea stock solution
Sunday, July 24, 2011 at 8:02pm by katie

chemistry
the concentration of urea in a solution prepared by dissolving 16g of urea in 39 g of H2O is ________% by mass. The molar mass of urea is 60.0 g/mol
Monday, May 27, 2013 at 10:57pm by jen

Chemistry
Urea (NH2)2CO is dissolved in 100.0 g of water. The solution freezes at -0.085 degrees C. how many grams of urea were dissolved to make this solution.
Thursday, February 7, 2008 at 9:34pm by Lauren

chemistry
88.8% urea means 88.8g urea/100 g soln. I would set up [xgrams urea/(500g H2O + x g urea)] = 0.888 Solve for x to obtain grams urea needed. moles fraction = moles urea/total moles. Plug this information into delta T = Kf*m and delta T = Kb*m. You will need to convert mass ...
Sunday, December 5, 2010 at 5:04pm by DrBob222

chem
How would u prepare each of the following solutions 100 mL of a 245 ppm solution of urea, CH4N2O, in water and How would u prepare each of the following solution 100 mL of an aqueous solution whose K+ concentration is 0.084 M Write up the procedure, and I will gladly check it...
Tuesday, June 27, 2006 at 7:45pm by UTramos

Chemistry
Calculate the molarity of a solution prepared by dissolving 16 g of urea, NH2CONH2, in 39 g of H2O. The density of the solution is 1.3 g/mL. I've tried this question so many times but I keep getting it wrong please help me
Sunday, September 29, 2013 at 11:54pm by danielle

Chemistry
If the osmotic pressure of urea (CH4N20) in water is measured at 0.0259 atm at 25 degress C what is the molartiy of the urea solution?
Monday, December 10, 2012 at 6:11pm by Shelly

chemistry
Find the mass of urea needed to prepare 51.7 of a solution in water in which the mole fraction of urea is 7.80×10−2.
Sunday, January 29, 2012 at 5:58pm by amy

Chemistry
Urea, (NH2)2CO, is dissolved in 73.5 g of water. The solution freezes at -0.095°C. How many grams of urea were dissolved to make this solution? (Answer must be in grams)
Tuesday, March 29, 2011 at 10:27pm by Irma

College Chemistry
Molarity of .100 mole of urea (CH4N2O) in 250.0 mL of solution
Tuesday, February 8, 2011 at 7:15pm by Audrey

chemistry
Find the mass of urea needed to prepare 51.7 g of a solution in water in which the mole fraction of urea is 7.59×10−2. anyone have the same values?
Tuesday, January 31, 2012 at 1:25am by jazz

chemistry
Let x = mass urea. n urea = x/60.06 n H2O = 50.1-(x/18) n urea = [n urea/(n urea + n H2O)] So (x/60)/[x/60)+{50.1-x}/18] = 0.075 and solve for x. If I didn't make a math error the answer is approximately 10 g.
Saturday, January 28, 2012 at 6:06pm by DrBob222

Chemistry problem
Hi I'm stuck on these questions can you please help me A soil sample contains 0.2234 g of Fe3+ per 100g. Fe3+ is precipitated when the soil becomes alkaline as shown in the equation below. Fe3+ + 3OH- + (x-1)H2O „_ FeOOH.xH2O(s) This soil is sprayed with 40.0 wt% urea solution...
Friday, March 26, 2010 at 6:30pm by Sarah

general chemistry 2
How many grams of urea [CO(NH2)2] would be required to prepare 200 mL of a 5.0 x 10-3 molar solution? Answer
Wednesday, September 26, 2012 at 3:46pm by Anonymous

chemistry
the mole fraction of urea (molar mass = 60g/mole) in a solution prepared by dissolving 16g of urea in 39g of h2o
Monday, September 13, 2010 at 10:30pm by jessie

chemistry
Find the mass of urea needed to prepare 50.1 of a solution in water in which the mole fraction of urea is 7.50×10−2.
Saturday, January 28, 2012 at 6:06pm by Kelley

Chemistry/lab math
A stock standard of urea nitrogen contains 20 mg/mL of urea nitrogen. How much stock is needed to prepare 100 mL of a 20 mg/dL working standard? Please help!
Wednesday, August 7, 2013 at 9:36pm by Anonymous

chemistry
Hi Can sombody please help me with this problem If a soil sample contains 0.5g of iron (Fe3+) per 100g. The iron is precipitated when soil becomes alkaline as shown by equation Fe3+ + 3OH + (x-1)H2O ? FeOOH.xH2O(s) The soil is sprayed with 50 wt% urea solution with density of ...
Friday, March 26, 2010 at 3:05am by Mary

chemistry
I think the problem is that the SOLUTION has a density of 1.3 g/mL. You are assuming the water is 1.3 g/mL and it isn't. One way around that is to calculate the molality, then convert that to molarity. Or you can do it in one step like this. M = mols/L. mols = 0.2667 total g ...
Sunday, September 26, 2010 at 2:28pm by DrBob222

Chemistry
What is the molarity of a solution of Mg(OH)2 if the solution contains 1.35 g in exactly 100 mL of solution??? A 15.0 mL solution of H2SO3 is neutralized by 12.0 mL of a standradized 1.00M NaOH solution. What is the concentration of the H2SO3 solution?????? What volume of a 1....
Wednesday, December 12, 2012 at 12:24am by Tasha

cell &molecular bio
Using the Einstein-Stokes equation, calculate the time for urea to diffuse across a cuboidal kidney cell with sides of 100micrometers. Assume the diffusion coefficient (D) of urea in solution is 2 x 10^-8 m2 sec -1
Sunday, September 16, 2012 at 7:25pm by Amy

Science/Chem
1. You dissolve 157.1 g of ammonium nitrate in a 250 mL volumetric flask and add water to the mark (call this solution A). You take 30 mL of solution A and place it in a 100 mL volumetric flask and add water to the mark (this is solution B). Next you take 50 mL of solution B ...
Sunday, September 28, 2008 at 4:40pm by Kelsey

science/chem
You dissolve 157.1 g of ammonium nitrate in a 250 mL volumetric flask and add water to the mark (call this solution A). You take 30 mL of solution A and place it in a 100 mL volumetric flask and add water to the mark (this is solution B). Next you take 50 mL of solution B and ...
Sunday, September 28, 2008 at 4:41pm by Kelsey

chemistry
Hey, I am having a real hard time getting the answers to the problems. Any help would be greatly aprreciated! 1. When 11 mL of a solution containing 2.9 M AlBr3 is diluted to 33 mL, a dilute solution is formed. What is the Br- concentration in 25 mL of the dilute solution? 2. ...
Wednesday, November 7, 2007 at 5:35pm by chelsea

Chemistry
The standard solution were prepared by transferring exactly 1.00 mL, 2.00 mL, 3.00 mL, 4.00 ml, and 5.00 ml, respectively, of stock solution to clean 100 ml vol flads, diluting to the mark with FeCl3 solution, and then filling the aoorioruatekt kabeked cuvette. Calculate the ...
Sunday, February 3, 2008 at 11:03pm by Anonymous

chemistry
moles urea = 16g/60 moles H2O = 39/18 mole fraction urea = moles urea/total moles.
Monday, September 13, 2010 at 10:30pm by DrBob222

Chemistry
How accurately is the acetic acid solution to be made? mL x M = mL x M 80 mL x 0.1M = mL x 6.0M mL = (80*0.1/6.0) = 1.33 Technically, the way you do it is to dispense 1.33 mL of the stock solution into an 80 mL volumetric flask, then make the solution to the mark with ...
Thursday, February 24, 2011 at 12:48am by DrBob222

Chemistry
2NH3 + CO2 ==> (NH2)2CO + H2O 1a. mols NH3 = grams/molar mass 1b. mols CO2 = grams/molar mass 2a. Using the coefficients in the balanced equation, convert mols NH3 to mols of urea. 2b. Do the same to convert mols CO2 to mols urea. 2c. It is likely that these two values will...
Thursday, February 27, 2014 at 9:17pm by DrBob222

annatomy
Calculate the osmolarity of a solution that contains 0.1 M urea, 0.2 M NaCl, and 0.5 M CaCl2. Assume urea does not ionize and NaCl and CaCl2 ionize completely
Monday, November 29, 2010 at 3:42pm by russel

General Chemistry
A 230.0mL sample of a 0.275 M solution is left on a hot plate overnight; the following morning the solution is 1.50M. What volume of solvent has evaporated from the 0.275 M solution? a)42.2 mL b)63.3 mL c)187.8 mL d)230 mL e)272.2 mL
Wednesday, June 20, 2012 at 12:54pm by Kim

chemistry
a 30.0 ml solution of potassium nitrate was diluted to 125 ml and 25 ml of this solution were then diluted to 150 ml. the concentration of the final solution is 0.00307 M. Calculate the concentration of the original solution.
Thursday, July 7, 2011 at 1:33pm by Carol

math
A science teacher has a supply of 50% sugar solution and a supply of 80% sugar solution. How much of each solution should the teacher mix together to get 105 ML of 60% sugar solution for an experiment 70 ML of the 50% solution and 35 ML of the 80% solution 35 ML of the 50% ...
Tuesday, December 24, 2013 at 3:03pm by chandler

chem
MW:CH4N2O(Urea) 60g/mole x 245/1000000 x .100L = .00147g urea. So weigh out .00147g urea and mix it with water in a volumetric flask up to exactly 100mL. Since 1ppm =1mg/1kg or 1/1000000
Tuesday, June 27, 2006 at 7:45pm by regina

Chemistry (Inorganic)
Given the two substances Sodium Nitrate (NaNO3) and Urea ([NO2]2CO), why is it that urea has a lower boiling point? I thought that the nitrate would because urea has the double bond which makes it more stable. Urea is covalently bonded. NaNO3 is an ionic compound. Generally ...
Sunday, July 29, 2007 at 7:07am by Vic

chemistry
10. An aqueous solution is prepared by diluting 3.30 mL acetone, CH3COCH3, (d=0.789 g/mL) with water to a final volumeof 75.0 mL. The density of the solution is 0.993 g/mL. What is the molarity and molality of acetone in this solution?
Tuesday, April 3, 2012 at 11:46am by Anonymous

Chemistry
An unknown amount of water is mixed with 310 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 58.2 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M What volume of water ...
Monday, March 19, 2012 at 12:27am by ag

Chemistry
An unknown amount of water is mixed with 310 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 58.2 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M What volume of water ...
Monday, March 19, 2012 at 12:28am by ag

Chemistry
An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 51.2 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M What volume of water ...
Monday, May 13, 2013 at 6:07pm by Anonymous

chemistry
the density of a certain aqueous solution is 1.17g/ml, and the solution is 3.57% by mass NaOH. how many mL of this solution would you need to use in order to prepare 100.0 mL of .150 M NaOH solution?
Monday, September 6, 2010 at 6:46pm by zahra

Chemistry
How do the following solutions show the properties of a buffer? 1) 50 ml 0.10 M NH3 + 50 ml 0.10 M NH4NO3 2) 10 ml solution #1 + 5 ml H2O + 1 ml 0.10 M HCl 3) 10 ml solution #1 + 6 ml 0.10 M HCl 4) 10 ml solution #1 + 5 ml H2O + 1 ml 0.10 M NaOH
Wednesday, March 20, 2013 at 2:27pm by Jeremy

Chem3
A solution is prepared by dissolving 22.8 mL of methanol (d = 0.782 g/mL) in 100 mL of water (d = 1.00 g/mL) so that the final volume of solution is 118 mL. What is the percent methanol by mass?
Monday, May 2, 2011 at 10:12pm by Ryan

chemisry
An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52.5 mL of 6 M HCl. Calculate the concentration of the di- luted NaOH solution. Answer in units of M
Wednesday, September 19, 2012 at 5:06pm by cheri

AP Chemistry
An unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52.5 mL of 6 M HCl. Calculate the concentration of the diluted NaOH solution. Answer in units of M
Wednesday, September 11, 2013 at 6:18pm by Gabriella

CHEMISTRY
n unknown amount of water is mixed with 350 mL of a 6 M solution of NaOH solution. A 75 mL sample of the resulting solution is titrated to neutrality with 52 . 5 mL of 6 M HCl. Calculate the concentration of the di- luted NaOH solution. Answer in units of M
Friday, October 18, 2013 at 1:38pm by Maria

chemistry
What volume of a 7.00 M solution of Ca(OH)2 is needed to neutralize 37.2 mL of a 3 M solution of nitric acid? 1. 15.9 mL 2. 37.2 mL 3. 7.97 mL 4. 24.2 mL
Tuesday, November 29, 2011 at 3:13am by katie

chemistry
calculate the osmotic pressure of a solution obtained by mixing 100ml of 0.25M solution of urea and 100ml of 0.1m solution of cane sugar at 293k
Thursday, June 6, 2013 at 12:23pm by sumit

Chemistry
a 25.0 mL sample of .050 M solution of aqueous trimethylamine is titrated with a .063 M solution of HCl. calculate pH the solution after 10.0 mL, 20.0 mL, 30.0 mL of acid have been added. pKb of (CH3)_3_N= 4.19 at 25 degrees C
Sunday, November 11, 2012 at 6:29am by Elaine

Chemistry
A 10.0-mL solution of 0.30 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the following additions of the HCl solution: a) 0.00 mL b) 10.0 mL c) 30.0 mL d) 40.0 mL
Monday, May 2, 2011 at 5:27pm by Martina

chemistry
what is the molarity of a solution containing 1 mole of urea per litre of the solution ? Hw to solve this
Thursday, July 12, 2012 at 3:04pm by star

Chemistry
Calculate the concentration, in molarity, of a solution prepared by adding 9 mL of water to 1 mL of 0.1 M HCl solution. If 2.0 mL of 0.010 M NaOH is mixed with enough water to make the total volume 8 mL, what is the molarity of the resulting solution?
Monday, October 3, 2011 at 6:09pm by Nico

chemistry
3.0 WHAT stock NaOH solution? Do you mean molar? Use mL x M = mL x M. After calculating mL of the stock solution needed, transfer exactly xx mL stock solution to a 500 mL volumetric flask, then add distilled /(deionized)/(DI) water to the mark in the neck of the volumetric ...
Saturday, October 30, 2010 at 8:57am by DrBob222

Chemistry
Assignment  Calculate the pH, pOH, [H+], and [OH] for each of the following solutions. Show all work. (10 Points) Solution Composition of Starting Materials 1 0.10 M acetic acid 2. 5 mL 0.10 M acetic acid + 5 mL wa 3 1 mL 0.10 M acetic acid + 99 mL water 4 5 mL...
Monday, October 11, 2010 at 12:24pm by Brian

Chemistry
A student has 100.0 mL of an unknown solution of Vitamin C. She removes 1.00 mL of this solution, dilutes it to 50.0 mL, and titrates this second solution with an iodine solution solution that 8.5x1^-4 M. 6.60 mL of iodine solution is required to reach the endpoint. 1. How ...
Monday, March 12, 2012 at 8:26pm by Cassandra

Chemistry
A student has 100.0 mL of an unknown solution of Vitamin C. She removes 1.00 mL of this solution, dilutes it to 50.0 mL, and titrates this second solution with an iodine solution solution that 8.5x1^-4 M. 6.60 mL of iodine solution is required to reach the endpoint. 1. How ...
Monday, March 12, 2012 at 8:28pm by Cassandra

Chemistry HELP!
In order to standardize a KMnO4 solution, 0.3498 g Na2C2O4 was dissolved in 30 mL water and 15 mL 3.0 M H2SO4. The KMnO4 solution was added to the Na2C2O4 solution until a pale pink color persisted. The titration took 29.5 mL of KMnO4 solution. What is the concentration of the...
Monday, May 6, 2013 at 12:12am by Prue

Chemistry HELP!
In order to standardize a KMnO4 solution, 0.3498 g Na2C2O4 was dissolved in 30 mL water and 15 mL 3.0 M H2SO4. The KMnO4 solution was added to the Na2C2O4 solution until a pale pink color persisted. The titration took 29.5 mL of KMnO4 solution. What is the concentration of ...
Monday, May 6, 2013 at 11:25am by Prue

math
A nurse needs to make 30 ml of 5% solution of glucose. She has available bottles containing 5 ml of 7% solution and bottles containing 10 ml of 1% solution. How many 5 ml bottles and 10 ml bottles will she need to make the solution? Bottles of 5 ml of 7% solution needed: ...
Monday, March 11, 2013 at 8:40pm by Josh

CHEMISTRY
Convert 6.50 g N to g urea. 6.50 g N x (molar mass urea/2*atomic mass N) = ? g urea.
Friday, March 7, 2014 at 9:49am by DrBob222

Chemistry
An aqueous solution with a density of 0.998 g/ml at 20 degrees Celsius is prepared by dissolving 12.8 mL of CH3CH2CH2OH (p=0.803 g/mL) in enough water to make 75.0 mL of solution calculate the molarity
Saturday, October 1, 2011 at 7:32pm by Jessica

chemistry
Calculate the molar concentrations for each of the following solutions: A)1.5g NaCI in 100 ml solution B)1.5g K2Cr2O7 in 100 ml solution C)5.55g Na2SO4 in 125 ml solution D)20g MgBr2 in 250ml solution
Sunday, February 20, 2011 at 10:01am by twynna

chemistry
You were given 25.00 ml of an acetic acid solution of unknown concentration. You find that it requires 29.60 ml of a 0.1050 M NaOH solution to exaclty neutralize this sample. A) What is the molarity of the acetic acid solution? B) what is the percentage of acetic acid in the ...
Thursday, October 20, 2011 at 12:29pm by Rema

chemistry
what is the effect of concentration of urea on urea based precipitation of copper nitrate?
Wednesday, March 2, 2011 at 1:47am by zia

chemistry
mL x M = mL x M mL x 12.0 = 500 x 3.5 mL = you can do it---about 60 mL or so. The reason I worked it through is to show you what NOT to do. You DON'T use 60 mL of the concd soln (or whatever the number turns out to be) and add 500 mL of water. Instead, you take 60 (or whatever...
Thursday, March 11, 2010 at 11:00pm by DrBob222

chemisrty
Q4) Suppose you prepare 950 mL of a solution by dissolving 100 grams of NaCl in 900 mL of water. Assuming the density of pure water to be 1 g/mL, answer the following questions with regards to this solution: a) What is the mass percent of water in this solution? b) What is ...
Monday, January 16, 2012 at 4:43pm by lyan

chemistry help asap
Please check these thanks. 1. In a titration, 33.21 mL 0.3020M rubidium hydroxide solution is required to exactly neutralize 20.00 mL hydrofluroic acid solution. What is the molarity of the hydrofluroic acid solution? Answer: 0.502HF 2. A 35.00 mL-sample of NaOH solution is ...
Monday, February 6, 2012 at 8:20pm by missy

Chemistry
the density of a certain aqueous solution is 1.17g/ml, and the solution is 3.57% by mass NaOH. how many ml of this solution would you need to use in order to prepare 100.0 ml of .150 M NaOH solution? I'm not sure where to start and what the process to go through would be... ...
Sunday, September 7, 2008 at 1:24pm by Lyndsey

chemistry
Commodity prices of NaCl and urea are about $0.033/lb for NaCl (as rock salt) and about $0.10/lb for urea. Calculate the cost of treating 1000 lb of ice on a surface to produce a solution that melts at -3.9 degrees Celsius with each chemical. I know you use to delta T= mkfi ...
Tuesday, February 26, 2013 at 9:24pm by K

chemistry
The synthesis of urea by Frederich Wöhler in 1825 began the decline of the idea that "organic" chemicals could only be made by living organisms as part of their biological processes. AgOCN(aq) + NH4Cl(aq) → AgCl(s) + NH2CONH2(aq) If you perform this reaction and collect ...
Sunday, October 16, 2011 at 10:04pm by Anonymous

Chem
Please tell me if these are right! 1.How many milliliters of 0.215 M NaOH solution are needed to completely neutralize 2.50 ml of 0.825 M H2SO4 solution? I got 19.2 ml 2. A 10.0-ml sample of vinegar which is an aqueous solution of acetic acid HC2G3O2 requires 16.5 ml of 0.500M...
Monday, December 6, 2010 at 9:17pm by Jessica

medicine
What is final concentration of a mixed solution combining 50ml of 20% solution, 150 ml of a 15% solution and 200 ml of a 35% solution?
Tuesday, July 20, 2010 at 2:15pm by Lisa

chemistry
A stock solution of 0.0100 M KMnO4 is diluted by taking 15.5 mL of it and diluting it to 100.0 mL. From this diluted solution, 5.00 mL is taken out and diluted to 100.0 mL. What is the concentration of the solution obtained in the end
Tuesday, March 13, 2012 at 7:07pm by carla

chemistry
how many moles of solute are contained in each solution? 250 mL of a 0.55 M NaNO3 solution? 145 mL of a 4.0 M HNO3 solution? 6.5 L of a 2.5 M HCl solution?
Sunday, April 11, 2010 at 5:58pm by cathy

Biochemistry
The reaction, depending on the conditions, is: (H2N)2CO ---> NH3 + HNCO The test you describe sounds like the biuret test for the peptide link. Both, urea and proteins have peptide links and give a positive test. If you have done this experiment, you should know the ...
Thursday, December 25, 2008 at 9:00am by GK

chemistry
A 25.00 mL solution of potassium nitrate (KNO3) was diluted to 125.0 mL, and 25.00 mL of this solution were then diluted to 1.000 103 mL. The concentration of the final solution is 0.00421 M. Calculate the concentration of the original solution.
Monday, October 1, 2012 at 6:11pm by Aiden

chemistry
A 25.00 mL solution of potassium nitrate (KNO3) was diluted to 125.0 mL, and 25.00 mL of this solution were then diluted to 1.000 103 mL. The concentration of the final solution is 0.00421 M. Calculate the concentration of the original solution.
Monday, October 1, 2012 at 7:00pm by Tim

chemistry dilution
This is a confusing problem. Here is another approach. We have a soln that is 200 ug/mL. We want 3 ug/100 uL. That is 0.003 ug/uL = 3 ug/mL Say we want to make 100 mL of this solution, then 3 ug/mL x 100 mL = 300 ug we need. 200 ug/mL x ?mL =300 ug ?mL = 300/200 = 1.5 mL; ...
Wednesday, February 27, 2013 at 8:54pm by DrBo222

Chemistry(reposts #1)
A solution is prepared by dissolving 5.00 g of stannic nitrate in enough water to make 250.0 mL of stock solution. A 15.0 mL aliquot (portion) of this stock solution is then removed and added to 75.0 mL of water. Calculate the concentrations of all ions in the final solution.
Friday, October 25, 2013 at 8:18pm by Anonymous

Chemistry (reposts#2)
A solution is prepared by dissolving 5.00 g of ferric chloride in enough water to make 500.0 mL of stock solution. A 50.0 mL aliquot (portion) of this stock solution is then removed and added to 75.0 mL of water. Calculate the concentrations of all ions in the final solution.
Friday, October 25, 2013 at 8:22pm by Anonymous

Chemistry
24.5 ml of water are added to a 1.20 molar solution of nitric acid. If the concentration decreases to 0.55 molar, what volume of the concentrated solution was used? 1.20 M x mL = (24.5 mL + mL) x 0.55 M Solve for mL. Check my thinking. When you finish the calculation, check it...
Friday, April 20, 2007 at 5:41pm by Veronica

chemistry
I don't know how to explain or if Ive got my homework answer correct. The question is: A patient on dialysis has a high level of urea, a high level of sodium and a low level of potassium in the blood. Why is the dialyzing solution prepared with a high level of potassium but no...
Thursday, April 14, 2011 at 8:27am by Connie

Analytical Chemistry
25.0 mL of a 0.1067 M Solution of nickel (II) sulfate is diluted to 250 mL with water. 10 mL of this solution is taken and diluted to 1.0 L. Calculate the concentration of [Ni2+] in the final solution in ppm.
Tuesday, February 11, 2014 at 2:53pm by Anonymous

CHEMISTRY
An ethanol-water solution is prepared by dissolving 10.00 ml ethanol C2H5OH (density=0.789g/ml) in sufficient water to produce 100.00 ml of solution with a density of 0.982g/ml. What is the concentration of ethanol in this solution? Expressed as ml. a.)%volume b.)%mass c.)%m/v...
Wednesday, November 13, 2013 at 8:00am by ADRIAN

Chemistry
A 16.6 mL portion of an HBr solution of unknown strength is diluted to exactly 247 mL. If 102.1 mL of this diluted solution requires 87.8 mL of 0.37 M NaOH to achieve complete neutralization, what was the strength of the original HBr solution?
Sunday, May 1, 2011 at 11:00pm by Sam

chemistry
Finding molarity and molality(best answer)? An aqueous solution is prepared by diluting 3.30 mL acetone,(d= 0.789g/mL) with water to a final volume of 75.0 mL. The density of the solution is 0.993 g/mL. What is the molarity, molality and mole fraction of acetone in this solution?
Friday, October 7, 2011 at 3:11am by sam

chemistry
if the pH of a half-neutralized acid solution is 5.4, how would you find the [H+] of the the solution. There is 1.0 g of L-ascorbic acid which was dissolved in 100 ml of water. That solution was split in two and 50 ml of the solution was titrated with 0.2 M NaOH (13 ml NaOH). ...
Thursday, April 17, 2008 at 3:04pm by tom

Chemistry
54.0 mL of a 1.50 M solution is diluted to a total volume of 258 mL. A 129-mL portion of that solution is diluted by adding 165 mL of water. What is the final concentration?
Saturday, February 2, 2013 at 3:01pm by Sara

Chemistry
72.0 ml of a 1.50 M solution is diluted to a volume of 288 mL. A 144 mL portion of that solution is diluted using 185 mL of water. What is the final concentration?
Monday, January 24, 2011 at 7:34pm by Anonymous

Chemistry
72.0 ml of a 1.50 M solution is diluted to a volume of 288 mL. A 144 mL portion of that solution is diluted using 185 mL of water. What is the final concentration?
Tuesday, January 25, 2011 at 1:29am by Anonymous

Chemistry
75.0 mL of a 1.80 M solution is diluted to a volume of 258 mL. A 129-mL portion of that solution is diluted using 187 mL of water. What is the final concentration?
Sunday, August 26, 2012 at 5:50pm by Amanda

Chemistry
75.0 mL of a 1.80 M solution is diluted to a volume of 258 mL. A 129-mL portion of that solution is diluted using 187 mL of water. What is the final concentration?
Sunday, August 26, 2012 at 5:50pm by Amanda

Chemistry
61.0 mL of a 1.50 M solution is diluted to a volume of 258 mL. A 129-mL portion of that solution is diluted using 167 mL of water. What is the final concentration?
Sunday, September 19, 2010 at 10:23pm by jack

Chemistry
67.0 mL of a 1.50 M solution is diluted to a volume of 258 mL. A 129-mL portion of that solution is diluted using 163 mL of water. What is the final concentration?
Tuesday, October 2, 2012 at 5:09pm by Anonymous

Chemisty
74.0 mL of a 1.80 M solution is diluted to a volume of 248 mL. A 124-mL portion of that solution is diluted using 135 mL of water. What is the final concentration?
Monday, January 14, 2013 at 5:09pm by Paul

Biology 20
The removal of urea is a critical function of the Kidney. Explain th origin of urea and the mechanism by which the kidneys ensure its secretion.
Wednesday, June 4, 2008 at 5:07pm by Laurie

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