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April 19, 2014

Search: Calculate the mass percent of a solution containing 45.6 grams ethanol (C2H6O) in 245 grams of water

Number of results: 95,928

Chem
Do my answers look correct for these? Thanks Calculate the mass percent of a solution containing 45.6 grams ethanol (C2H6O) in 245 grams of water. 15.7% You are asked to make 500.0 mL of a 4.5M solution of HCl, but the only HCl you have available to dilute is 18.0M. Describe ...
Monday, December 7, 2009 at 7:29pm by Matt

Honors Chemistry 101
Do my answers look correct for these? Thanks Calculate the mass percent of a solution containing 45.6 grams ethanol (C2H6O) in 245 grams of water. 15.7% You are asked to make 500.0 mL of a 4.5M solution of HCl, but the only HCl you have available to dilute is 18.0M. Describe ...
Monday, December 7, 2009 at 1:46am by Matt

chemistry
What is the percent by mass of 3.55 g NaCl dissolved in 88 g H2O? 2. A solution is made by adding 1.23 moles of KCl to 1000.0 g of water. What is the % by mass of KCl in this solution? 3. If you have 100.0 mL of a 25% aqueous solution of ethanol, what volumes of ethanol and ...
Thursday, February 10, 2011 at 8:53pm by Anonymous

chemistry
What is the percent by mass of 3.55 g NaCl dissolved in 88 g H2O? 2. A solution is made by adding 1.23 moles of KCl to 1000.0 g of water. What is the % by mass of KCl in this solution? 3. If you have 100.0 mL of a 25% aqueous solution of ethanol, what volumes of ethanol and ...
Thursday, February 10, 2011 at 9:49pm by Anonymous

chemistry
What is the percent by mass of 3.55 g NaCl dissolved in 88 g H2O? 2. A solution is made by adding 1.23 moles of KCl to 1000.0 g of water. What is the % by mass of KCl in this solution? 3. If you have 100.0 mL of a 25% aqueous solution of ethanol, what volumes of ethanol and ...
Thursday, February 10, 2011 at 9:49pm by Anonymous

Chemistry-Please help
(Note: I don't think the density is 1.05 g/mol; rather, I think it is 1.05 g/mL) Percent by mass means grams solute per 100 g solution. molarity = moles/L of solution. So we change molarity to grams and L of solution to total mass. 1.45 M NaCl = 1.45 moles/L. 1.45 moles NaCl x...
Monday, October 5, 2009 at 9:38pm by DrBob222

Chemistry
Please help me with these! Thanks :) Describe, in detail, how to make 5.5 liters of a 2.5 molar HCl solution from a 10.5 molar HCl stock solution. How many grams of a stock solution that is 85.5 percent H2SO4 by mass would be needed to make 150 grams of a 45.0 percent by mass ...
Sunday, February 27, 2011 at 8:50pm by Amanda

Chemistry
1. What is the percent by mass of a solution that contains 50 grams of solute dissolved in 200 grams of solution? What is the concentration of the same solution in parts per million? 2. What is the percent mass of a solution that contains 75 grams of salt dissolved in 150 ...
Friday, March 25, 2011 at 11:03am by Leora

chemistry honors
how many grams of a stock solution that is 85% H2SO4 by mass would be needed to make 150 grams of a 45.0 percent solution?
Thursday, September 30, 2010 at 12:56pm by jimmy

physical science
how much sugar is dissolved in 500 grams of a solution if the solution is 70 percent sugar by mass? Also, What is the concentration of a solution that contains 45 grams of sugar in 500 grams of solution? thank you
Sunday, December 28, 2008 at 3:55pm by Lisa

CHEM HELP ASAP
I figured all the parts of the problem except for the last one. Can you tell me what to do? In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 grams. The mustard was then dissolved in 50....
Wednesday, October 10, 2012 at 10:04am by Kelli

CHEM HELP ASAP
I figured all the parts of the problem except for the last one. Can you tell me what to do? In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 grams. The mustard was then dissolved in 50....
Wednesday, October 10, 2012 at 10:07am by Kelli

chemistry
Calculate the theoretical yield of the precipitate formed when a solution containing 1.02 grams of lithium phosphate is mixed with a solution containing 2.72 grams of strontium nitrate
Thursday, April 19, 2012 at 11:55am by Rayna

CHEM PROB MR BOB
I figured all the parts of the problem except for the last one. Can you tell me what to do? In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 grams. The mustard was then dissolved in 50....
Wednesday, October 10, 2012 at 3:14am by Kelli

Chem Problem
I originally asked you the first question and I got the answer 7.7 but theres other parts to the problem but Im not sure what to do In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 ...
Wednesday, October 10, 2012 at 12:48am by Kelli

Chem Problem
I originally asked you the first question and I got the answer 7.7 but theres other parts to the problem but Im not sure what to do In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 ...
Wednesday, October 10, 2012 at 1:16am by Kelli

Chemistry
Calculate the amount of water (in grams) that must be added to (a)5.00 g of urea (NH2)2CO in the preparation of a 16.2 percent by mass solution, and (b)26.2g of MgCl2 in the preparation of a 1.5 percent by mass solution.
Sunday, September 19, 2010 at 6:29pm by Diana

Chemistry
If 45.8 grams of MgO are dissolved in 205 grams of water, what is the concentration of the solution in percent by mass?
Monday, March 21, 2011 at 10:00am by ilyrae

Anatomy and Physiology
calculate the percent KBr in a solution containing 0.88 grams KBr per 800 mL solution.
Monday, March 7, 2011 at 1:15pm by paul durlin

Chem Problem
Help Please? In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 grams. The mustard was then dissolved in 50.0 ml. of distilled water. The total mass of the solution was found to be 49.401...
Tuesday, October 9, 2012 at 9:50pm by Kelli

Chemistry
Calculate the mass percent of a solution containing 10.5 of and 91.5 of H2O.
Saturday, November 24, 2012 at 7:50pm by Dax

chem
How many grams of a stock solution that is 87.0 percent H2SO4 by mass would be needed to make 200 grams of a 35.5 percent by mass solution? Show all of the work needed to solve this problem
Tuesday, January 17, 2012 at 5:10pm by bryan

Chemistry
How many grams of a stock solution that is 87.0 percent H2SO4 by mass would be needed to make 200 grams of a 35.5 percent by mass solution? Show all of the work needed to solve this problem.
Monday, September 2, 2013 at 5:39pm by Stephanie

Chemistry
How would you prepare 455 g of aqueous solution that is 6.50% sodium sulfate Na2SO4 by mass? percent by mass = grams/100 g solution. X grams/455 = 0.065 solve for X. Subtract 455-X to calculate how much water must be added. ok i got -454.935 is this right
Wednesday, February 6, 2008 at 9:33pm by Lauren

Chemistry
what mass of AgBr is formed when a solution containing 3.45 g of KBr is mixed with a solution containing 7.28 g AgNO3?
Saturday, April 14, 2012 at 12:06pm by David

Chemistry 1
How many grams of a stock solution that is 92.5 percent H2SO4 by mass would be needed to make 250 grams of a 35.0 percent by mass solution? Can you please teach me how to do this? I get the other stoichiometry stuff, but this one tripped me up because I don't know how to set ...
Tuesday, February 1, 2011 at 8:10am by Brittany

Chemistry
find the freezing point of a solution containing 3 grams of a compound of molar mass 125 g/mol in 45 g of camphor
Monday, March 17, 2014 at 8:12pm by Ann

Chem
What is the percent by mass of a solution if 45 grams of acetic acid is added to 90 g of H2O? Thanks.
Sunday, March 20, 2011 at 10:49pm by Jenny

Chemistry
Use mass = volume x density to calculate the mass of 1000 mL of the final solution. Then use the definition of molality = mols/kg solution. I like to calculate the mass, then put molality into a single equation, which is, kg x m x molar mass = grams. You know kg, m, and molar ...
Tuesday, February 26, 2008 at 2:58pm by DrBob222

Chemistry
I wonder if you know the implications of this problem? A solution that is 2.07 m in the solute in which the SOLVENT is 6450 g is easy enough to do. But if you want the total solution (solvent + solute) to weigh 6.45 kg, that's another ball game. m = moles/kg solvent 2.07 = ...
Monday, February 1, 2010 at 11:25pm by DrBob222

chemistry
Is that 31.45% by mass. If so, then the solution is 12.58 m. 31.45 g HCl(31.45 g HCl + 68.55 g H2O) and 31.45/36.46 = 0.8625 moles HCl in 0.06855 kg solvent which makes the solution 12.58%. Then m x grams soln = m wanted x grams wanted 12.58 m x grams soln = 0.1 m x 500 Solve ...
Saturday, October 16, 2010 at 11:01am by DrBob222

Chemistry
Calculate the percent ionizationof a 0.15 M benzoic acid solution in pure water Nd also in a solution containing 0.10M sodium benzoate. Why does the percent ionization differ significantly in the two solutions?
Monday, March 12, 2012 at 2:10am by L.Bianchessi

high school chem
How many grams of a stock solution that is 92.5 percent h2s04 by mass would be needed to make 250 grams of a 35% by mass solution?
Wednesday, March 9, 2011 at 8:37pm by Kayla

chemistry
2. 0.300 kilogram chloroform(chlorine calcium3)and 21.0grams eucalyptol(carbon10 hydrogen18 oxygen 3. what is the concentration of a solution of sodium chlorine water containing 1.170grams solute in 100moles solution 4, what is the % by volume of a solution containing 30....
Tuesday, September 14, 2010 at 12:06pm by juzen

Chemistry
percent by mass = grams/100 g solution. X grams/455 = 0.065 solve for X. Subtract 455-X to calculate how much water must be added.
Monday, February 4, 2008 at 7:07pm by DrBob222

Chemistry
A student makes a solution by dissolving 55.8 grams of potassium hydroxide in 875.0 grams of water. The resulting solution has a density of 1.07 grams per milliliter. 1. What is the volume of this solution? 2. Calculate the % concentration of this solution. 3. Calculate the ...
Monday, January 31, 2011 at 1:02pm by Paul

Chemistry
A student makes a solution by dissolving 55.8 grams of potassium hydroxide in 875.0 grams of water. The resulting solution has a density of 1.07 grams per milliliter. 1. What is the volume of this solution? 2. Calculate the % concentration of this solution. 3. Calculate the ...
Monday, January 31, 2011 at 9:59pm by Paul

Chemistry
A student makes a solution by dissolving 55.8 grams of potassium hydroxide in 875.0 grams of water. The resulting solution has a density of 1.07 grams per milliliter. 1. What is the volume of this solution? 2. Calculate the % concentration of this solution. 3. Calculate the ...
Tuesday, February 1, 2011 at 4:42am by Paul

Chemistry
A student makes a solution by dissolving 55.8 grams of potassium hydroxide in 875.0 grams of water. The resulting solution has a density of 1.07 grams per milliliter. 1. What is the volume of this solution? 2. Calculate the % concentration of this solution. 3. Calculate the ...
Tuesday, February 1, 2011 at 10:53am by Paul

Chem9
An aqueous solution containing 35.1 grams of an unknown molecular (noneolectrolyte) compound in 152.5 grams of water was found to have a freezing point of -1.8 degrees C. Calculate the molar mass of the unknown compound.
Monday, May 2, 2011 at 11:43pm by Ryan

chemistry
If im given mass percent and mass solvent how do I find mass solute and mass solution. example: Mass percent = 3.8% and Mass solvent 45.8 g. Find mass solute and mass solution
Wednesday, November 2, 2011 at 2:47pm by Monique

Chemistry
Calculate the mass of water that must be added to .45 mol of glucose to make a solution of 15 percent by mass. The molar mass of glucose is 180g/mol
Friday, March 1, 2013 at 11:24am by Dal

AP Chemistry
An aqueous sulfuric acid solution containing 571.6 g of H2SO4 per liter of solution at 20C has a density of 1.3294 g/mL. Calculate (a) the molarity, (b) the molality, (c) the percent by mass, and (d) the mole fraction of H2SO4 for the solution. (MM H2SO4 = 98.08; MM H2O = 18....
Tuesday, January 5, 2010 at 10:24pm by Beth

Chemistry
Complete the following table for aqueous solutions of caffeine, C8H10O2N4. a) molality b) mass percent solvent c) Ppm solute All we're given is Mole fraction solvent= .900. How do I solve for the other parts with only this?? It XH2O = 0.9, then Xcaffeine=0.1. Suppose we have 0...
Tuesday, March 20, 2007 at 1:30pm by Chris

Chemistry- Drbob-help
I have placed the answer I got please help. A student makes a solution by dissolving 55.8 grams of potassium hydroxide in 875.0 grams of water. The resulting solution has a density of 1.07 grams per milliliter. 1. What is the volume of this solution? 870mL 2. Calculate the % ...
Wednesday, February 9, 2011 at 11:31pm by Paul

Chemistry
If a solution containing 33.82 g of mercury(II) acetate is allowed to react completely with a solution containing 9.718 g of sodium sulfate, how many grams of solid precipitate will be formed? How many grams of the reactant in excess will remain after the reaction?
Thursday, January 17, 2013 at 6:08pm by Caitlin

please help!!
If a solution containing 33.82 g of mercury(II) acetate is allowed to react completely with a solution containing 9.718 g of sodium sulfate, how many grams of solid precipitate will be formed? How many grams of the reactant in excess will remain after the reaction?
Thursday, January 17, 2013 at 8:43pm by Caitlin

basic chem
If a solution containing 33.82 g of mercury(II) acetate is allowed to react completely with a solution containing 9.718 g of sodium sulfate, how many grams of solid precipitate will be formed? How many grams of the reactant in excess will remain after the reaction?
Thursday, January 17, 2013 at 4:59pm by Caitlin

chem please help!
If a solution containing 33.82 g of mercury(II) acetate is allowed to react completely with a solution containing 9.718 g of sodium sulfate, how many grams of solid precipitate will be formed? How many grams of the reactant in excess will remain after the reaction?
Thursday, January 17, 2013 at 7:44pm by Caitlin

Chemistry
If a solution containing 118.44 g of mercury(II) perchlorate is allowed to react completely with a solution containing 17.796 g of sodium sulfide, how many grams of solid precipitate will be formed? How many grams of the reactant in excess will remain after the reaction?
Tuesday, April 1, 2014 at 11:14pm by Noelle

Chemistry
The density of an aqueous solution containing 10% of ethanol (C2H5OH) by mass is 0.984 g/ml. A) Calculate the molality of this solution. B) Calculate its molarity. C) What volume of the solution would contain 0.125 mol of ethanol.
Wednesday, March 17, 2010 at 11:40pm by Hilavidpreet

science(chem)
The information I provided is OK. The problem is that we don't know, at least I don't know, if the 64% is a mass/mass, a mass/volume, or whatever. The site may have told you that a solution is mass/volume if it isn't specified, but the information in most texts and all the ...
Monday, May 5, 2008 at 12:14am by DrBob222

chem really need help!
If a solution containing 33.82 g of mercury(II) acetate is allowed to react completely with a solution containing 9.718 g of sodium sulfate, how many grams of solid precipitate will be formed? How many grams of the reactant in excess will remain after the reaction?
Thursday, January 17, 2013 at 9:31pm by Caitlin

chemistry
2KI+Pb(NO3)2=2KNO3+PbI2 suppose a solution containing 1.25g of KI is combined with a solution containing 2.42g Pb(NO3)2 _what mass of the yellow PbI would result what is the limiting reactant How much in grams of the excess reactant was used how much in grams of the excess ...
Sunday, February 10, 2013 at 12:20pm by may

Chemistry
A 2.304 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO3 and HCl aqueous solution. To this solution was added 1.500 grams of KI and 50.00 mL of a 0.00912 M KIO3 solution. The excess I3 was titrated with 50.00 mL ...
Tuesday, April 16, 2013 at 10:30pm by Jessica

chemistry
A 1.147 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO3 and HCl aqueous solution. To this solution was added 1.690 grams of KI and 50.00 mL of a 0.00821 M KIO3 solution. The excess I3 was titrated with 50.00 mL ...
Wednesday, April 17, 2013 at 11:31am by Lana

chemistry
A 1.857 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO3 and HCl aqueous solution. To this solution was added 1.540 grams of KI and 50.00 mL of a 0.00912 M KIO3 solution. The excess I3 was titrated with 50.00 mL ...
Thursday, May 2, 2013 at 11:44pm by Sparkle

chemistry
A solution containing 4.5 grams of non-electrolyte dissolved in 125 grams of water freezes at -0.372 degrees. Calculate the molar weight of the solute.
Sunday, September 12, 2010 at 6:01am by kareen

chemistry
2Na3PO4(aq)+3 Ba(NO3)2(aq)---->Ba3(PO4)2(s)+6NaNO3(aq) a solution containing 3.50g of Na3PO4 is mixed with a solution containing 6.40g of Ba(NO3)2 how many grams of product can be formed? and if the above reaction resulted in 3.659 g of white powder, what is the percent ...
Thursday, November 17, 2011 at 1:39pm by mckayla

chem
how would you prepare 445 grams of solution containing 13% mass HCL from 34.1 mass % of HCL solution
Monday, February 24, 2014 at 5:32pm by SDW

Chemistry
what is the percent (m/m) of argon gas in a mixture containing 45.0 grams of argon gas and 85.0 grams of helium gas
Tuesday, May 8, 2012 at 10:25pm by Allisyn

Chemistry I
Acetone , C3H6), is the main ingredient of nail polish remover. A solution is made up by adding 35.0 ml of acetone (d=0.790g/ml) to 50.0ml of ethyl alchole, C2H6O (d=0.789 g/ml). summing volumes are additive, calculate (a). the mass percent of acetone in the solution. Using ...
Friday, February 26, 2010 at 6:37pm by DrBob222

Chemistry
If a solution containing 52.044 g of mercury(II) chlorate is allowed to react completely with a solution containing 15.488 g of sodium sulfate, how many grams of solid precipitate will be formed? How many grams of the reactant in excess will remain after the reaction? I have ...
Sunday, October 13, 2013 at 2:25pm by Chelsea

Chemistry
An aqueous KNO3 solution is made using 72.5 grams of KNO3 diluted to a total solution volume of 2.00 liters. If the molarity of the solution is .359 M and the molality of the solution is .354, what is the mass percent of the solution?
Sunday, February 19, 2012 at 9:39am by Adam

Chemistry
Calculate the mass percent (m/m) for the solute in 2 grams of KOH in 20.0 grams of H2O? How do I set this up?
Thursday, May 5, 2011 at 6:01pm by Curlyqty

Chemistry
25.0 mL of a NaCl solution (concentration unknown) was found to react with 20 drops of the chloride test solution from the PU Chloride Test Kit. Calculate the mass of NaCl (in grams) in this solution. Calculate the mass of NaCl required to prepare 0.250 L of a NaCl solution ...
Sunday, October 3, 2010 at 11:17pm by kt

gen chemistry
calculate the percent m/v concentration of a 5L solution containing 500g NaCl
Friday, May 18, 2012 at 11:01pm by ashia3

Chemistry
I am doing a lab online and have no clue on how to get started with the following questions? Please Help me! 1. Calculate and record the following (in grams): (a) mass of NaCl by subtraction of other components: (b) measured mass of NaCl after boiling away water: 2. Calculate ...
Saturday, October 23, 2010 at 10:00am by Melissa

Redox Titration questions!
Oh goodness, I'm such a pain! I need some help with these! How do I calculate the percentage? How do I start it? 2. Imagine that you ran a similar titration using a different iron sample with 0.02 M KMnO4 as the titrant. Calculate the percent of iron in the sample if the ...
Wednesday, June 11, 2008 at 9:05pm by Angel

Chemistry
I need some help with some of these questions: The action of bacteria on meat and fish produces a poisonous compound called cadaverine. As its name implies, it stinks! It is 58.77 percent carbon, 13.81 percent hydrogen, and 27.40 percent nitrogen. Its molecular weight is 102.2...
Monday, February 20, 2012 at 5:42pm by Matthew

Chemistry
I need some help with some of these questions: The action of bacteria on meat and fish produces a poisonous compound called cadaverine. As its name implies, it stinks! It is 58.77 percent carbon, 13.81 percent hydrogen, and 27.40 percent nitrogen. Its molecular weight is 102.2...
Monday, February 20, 2012 at 5:42pm by Matthew

chemistry
If 35.8 grams of LiCl are dissolved in 184 grams of water, what is the concentration of the solution in percent by mass?
Monday, November 29, 2010 at 12:10am by smith

chemistry
Calculate the freezing point of a solution contaning 5.0 grams of KCl and 550.0 grams of water. answer is -0.45 C but i don't know how to get here
Thursday, October 4, 2012 at 8:55am by Paloa

Chemistry
An isotonic solution contains 0.88% NaCl by mass per volume. Calculate the percent mass per volume for isotonic solutions containing each of the following solutes at 15 degrees C. Assume a van't Hoff factor of 1.9 for all ionic solutes. KCL NaBr Glucose
Thursday, September 17, 2009 at 9:25pm by tyler

CHemistry
C + 2NaOH ==> 2H2O + Na2C How many mols of NaOH are used in the titration? That is M x L = mols NaOH. Now convert mols NaOH to mols C using the coefficients in the balanced equation. Convert mols C to grams C. mass C = mols C x molar mass C. %C = [mass C/mass sample]*100 (...
Wednesday, October 22, 2008 at 10:17pm by DrBob222

Chemistry
How do you determine the percent composition by mass of a 100 g K2SO4 solution containing a 20-g solute. What is the mole percent composition of the solute, assuming that the solution consists of 100 g water and 20 g of K2S04? For percent composition of K2S04, I got 44.9 % K, ...
Tuesday, June 23, 2009 at 12:43pm by Sofia

college chem
For A. Assume you have enough solution to contain 10.88 moles ethanol. Therefore, you will have 1 kg water (1,000 g). 10.88 moles x (46 g/mol) = 500.48 grams ethanol. Total mass of the solution is 1000 g + 500.48 = 1500.48 grams. % ethanol = (mass ethanol/mass soln)*100 % ...
Tuesday, March 9, 2010 at 11:11pm by DrBob222

chemistry
1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution? 2. in a acid-base titration, 33.65mL of an 0.148 M HCL solution were required to neutralize 25.00mL of a NaOH solution. What is the molarity of the NaOH ...
Tuesday, October 25, 2011 at 10:55pm by djella

chemistry
M = mols/L of solution. You can calculate mols from mols = grams/ molar mass. You know molar mass CaCl2 and you know grams. Calculate mols from equation 2, and substitute in equation 1 to calculate molarity. Post your work if you need more help. I left a message for you on the...
Wednesday, May 7, 2008 at 9:02pm by DrBob222

chemistry
Can someone make sure that I am correct with my first solution? Also I need help with the 2nd problem. I am a little confused about where to begin. 1.) 1.7423g of potassium dichromate were placed in a 250.00 mL volumetric flask and water was added to the mark. Calculate the ...
Tuesday, October 7, 2008 at 5:36pm by titration

Chemistry- Drbob-help#3
I still need help with #3 I'm not sure how I got 1.14M. I have tried to do the problem over, but I not coming up with my original answer of 1.14M. Somehow I am missing a step. Please show work for the 1.14M Thanks Question#9 reads exactly as written. A student makes a solution...
Thursday, February 10, 2011 at 12:54am by Paul

science
Concentrated sulfuric acid (18.4 molar H2SO4) has a density of 1.84 grams per milliliter. After dilution with water to 5.20 molar, the solution has a density of 1.38 grams per milliliter and can be used as an electrolyte in lead storage batteries for automobiles. 1. Calculate ...
Wednesday, October 24, 2007 at 12:50am by raksha

Chemistry H
Find the molality, mole fraction, and percent by mass of a solution prepared with 500 grams of C12h22O11 in 2000 grams of H20
Thursday, June 20, 2013 at 9:39pm by c

chemistry
An aqueous solution is made using 137g of diluted to a total solution volume of 1.30L .Calculate the molarity.molality and mass percent of solution.*assume a density of 1.08g/ml for the solution..
Saturday, July 28, 2012 at 2:44pm by noor

chemistry
You don't need the density, only the definition of mass percent. mass percent = (mass solute/mass soln)*100 = ?? You have 23.7 g solute in (375+23.7 = 398.7) grams solution. (23.7/398.7)*100 = 5.94% by mass.
Wednesday, September 15, 2010 at 5:39pm by DrBob222

chemistry
calculate the percent composition or w/v% of 3x10 to the 2nd power mL solution containing 15g of glucose
Tuesday, May 4, 2010 at 8:22pm by Quentin

Chemistry
1.What mass of NaOH(s) must be added to 300 mL of HCl 0.25 M in order to completely neutralize this acid? 2.During a lab, you mix 2 solutions: a 100 ml solution containing 0.40 g of NaOH and a 100 mL solution containing 0.73 g of HCl. What is the concentration of H+ ions in ...
Thursday, May 9, 2013 at 2:22pm by Talulla

Chemistry
is there an equation to find mass percent....if know concentration and and final and initial volume of a titration lab? there isnt one then how do you find mass percent? M x L = mols of titrant. From the equation, convert to mols of unknown. Mols of unknown x molar mass = ...
Monday, May 7, 2007 at 2:31pm by Natalie

Chemistry (Check)
Classify each of these statements as always true, sometimes true, or never true. 7____AT____It is necessary to know the formula of a compound in order to calculate its percent composition. 8___ST_____If the percent by mass of carbon in methane, CH4, is 75%, then 100 grams of ...
Sunday, February 11, 2007 at 3:48pm by Bryan

ap chem
a solution is prepared by dissolving 4.87 g of sodium dichromate in 25.0 ml of water. (d=1.00g/mL).calculate a. the mass percent of sodium dichromate in the solution. b. the mass percent o water in the solution. c the mole fraction of sodium dichromate in the solution. How ...
Tuesday, February 20, 2007 at 6:16pm by just

Chemistry
H2SO4 solution containing 200.1 g of H2SO4 in 0.3500 L OF solution has a density of 1.3294 g/ml.calculate (A) Mass%H2SO4(m/m) (B)mass%H2O(m/m) (C)Molarity (D)Molality
Saturday, September 1, 2012 at 3:09am by Yeneta

Chemistry
H2SO4 solution containing 200.1 g of H2SO4 in 0.3500 L OF solution has a density of 1.3294 g/ml.calculate (A) Mass%H2SO4(m/m) (B)mass%H2O(m/m) (C)Molarity (D)Molality
Saturday, September 1, 2012 at 3:20am by Yeneta

Chemistry
Calculate the osmotic pressure of this solution. 18..6 grams of solute with molecular mass of 8940 grams are dissolved in enough water to make 1.00 dm3 of solution at 25 celsius. What is the osmotic pressure of the solution?
Monday, November 22, 2010 at 2:08pm by Jose Reyes

Chemistry
Did I do this correctly or do I need to try again? What is the mass percent of a solution when 18.6 g of table salt is added to 81.4 g of water? Mass Percent = mass of solute(g)x100 mass of solution (g) = 18.6 g x100 18.6 g + 81.4g = 18.6 g x 100 100g = 0.186 x 100 = 18.6 The ...
Friday, February 8, 2008 at 1:48pm by Lori

Chemistry
Calculate the percent ionization of 0.140 M lactic acid in a solution containing 8.510−3 M sodium lactate.
Saturday, April 27, 2013 at 12:27pm by John

chemistry
If a solution containing 34.576 g of mercury(II) perchlorate is allowed to react completely with a solution containing 10.872 g of sodium sulfate, how many grams of solid precipitate will be formed?
Friday, April 19, 2013 at 4:04pm by lee

Math
A juice concentrate containing 65% solids is added to a single-strength juice solution(containing 15% solid), in order to generate a final product which contains 45% solids. Calculate the amounts required for the concentrate and for the single strength solution to produce ...
Tuesday, February 7, 2012 at 11:17pm by Janice

chemistry
#2) Consider the preciditation reaction of a solution containing 3.50 grams of sodium phosphate mixed with a solution containing 6.40 grams of barium nitrate. How many grams of Barium phosphate can form? Ba(NO3 )2 + Na3 PO4 yields Ba3 (PO 4 )2 + NaNO3 #2b) If the actural yield...
Thursday, January 29, 2009 at 7:41pm by lyne

chemistry
A sulfuric acid solution containing 571.6g of H2SO4 per of solution has a density of 1.329g/cm3. Calculate (a) mass percentage (b)mole fraction (c) molality (d) molarity of H2SO4 in this solution.
Thursday, September 2, 2010 at 9:03am by Anonymous

chemistry needs another look plz
Posted by Lori on Tuesday, December 14, 2010 at 5:38pm. The mole fraction of an aqueous solution of potassium perchlorate is 0.125. Assuming that the density of this solution is 1.20g mL-1, calculate the following: (A) the mass percent of potassium perchlorate in the solution...
Tuesday, December 14, 2010 at 10:54pm by Lori

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