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April 23, 2014

Search: diluted pH

Number of results: 888

Chemistry
A 200 mg/dl solution was diluted 1:10. This diluted solution was then additionally diluted 1:5. What us the concentration of the final dilution?
Tuesday, March 24, 2009 at 5:51pm by Jessi

chemistry
you diluted it first by a facator of 5 (2ml to 10 ml). then you diluted it by factors of 3. dilution: 5*3*3=45 times
Tuesday, September 13, 2011 at 8:27pm by bobpursley

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
A 500 ml bottle of 16 M hydrocholric acid is diluted to a final volume of 5,0 liters .. what is the concentration of the new diluted , HLC sloution
Wednesday, May 2, 2012 at 1:29pm by Anonymous

Chemistry
Hi,can I have your help? I'm just trying to solve a few Dilution Solution problems. I'm stuck on these two,and I wish you could help. Here's one: A 500 mL bottle of concentrated acetic acid is diluted to make a 5.0% solution. Find the volume of diluted that is prepared? ...
Wednesday, December 8, 2010 at 11:36am by Cliff

Chemistry
I am hoping to receive help getting started with this problem, possibly some steps in the correct direction. Here is the question: 5.0mLs of a 6.0M solution of HCl was transferred to a 1000ml volumetric flask and diluted to volume w/ water. 50mLs of this solution was then ...
Tuesday, June 9, 2009 at 6:31pm by Juggernaut

Chemistry
Then calculate the inital ClO^- concencentrations for 1st, 2nd, and 3rd reactions. Chemical reaction: Blue dye + ClO^- -->oxidized dye +Cl^- Reaction #1: 5.0 mL or diluted bleach solution, 15.0mL of distilled water, 10.0 mL of diluted blue dye Reaction #2: 10.0mL of diluted...
Monday, February 27, 2012 at 11:36pm by Cassandra

chemistry
78.7 mL sample of a 4.81 M sucrose solution is diluted to 12.0 mL. What is the molarity of the diluted soluti?
Sunday, December 4, 2011 at 4:56pm by Aamnda

chemistry
78.7 mL sample of a 4.81 M sucrose solution is diluted to 120.0 mL. What is the molarity of the diluted soluti?
Sunday, December 4, 2011 at 10:26pm by Amanda

chemistry
78.7 mL sample of a 4.81 M sucrose solution is diluted to 120.0 mL. What is the molarity of the diluted soluti?
Sunday, December 4, 2011 at 10:26pm by Amanda

Chemistry
If 15.0ml of a 6.0M HCl solution is diluted to 75.00ml, what is the molarity of the diluted solution?
Saturday, March 5, 2011 at 4:58pm by jake

chemistry
if 25.00 mL of 1.04 M Na2CO3 is diluted to .500 L, what is the molarity of Na2CO3 in the diluted solution?
Thursday, September 6, 2012 at 8:25pm by England

Chemistry
If a 25.0 mL sample of 0.500 M HCl solution were diluted 125-fold, what would be the volume and concentration of the diluted solution?
Monday, April 4, 2011 at 8:03pm by Chris

chemistry
a 3.5L sample of a 5.8M NaCl solution is diluted to 55L.What is the molarity of the diluted solution
Sunday, November 6, 2011 at 7:08am by Monique

Chemistry
A volume of 25.0 mL of 8.0 M acetic acid is diluted with sufficient water to prepare 1.00 liter of solution. What is the concentration of the diluted solution?
Sunday, March 9, 2008 at 9:31pm by Allie

chemistry
exactly 20 mL of .0520M Pb(NO3)2 is diluted to a final volume of 100 mL. What is the molar concentration of the diluted solution?
Monday, June 13, 2011 at 8:53am by chelsea

chemistry
If 4.0L of a 4.7M SrCl2 solution is diluted to 45L , what is the molarity of the diluted solution?
Sunday, October 6, 2013 at 10:08pm by Anonymous

chemistry
If 4.0L of a 4.7M SrCl2 solution is diluted to 45L , what is the molarity of the diluted solution?
Sunday, October 6, 2013 at 10:14pm by Sean1987

Chemestry
IF 121ml of a 1.0 M glucose solution is diluted to 500.0 mL, what is the molarity of the diluted solution?
Tuesday, November 5, 2013 at 6:38pm by Earl

Chemistry
suppose a pippetting error was made when preparing the diluted vinegar, but the diluted vinigar solution was uniform and the naoh titration values were consistant. when will the student learn that the experiment result was not accurate explain
Friday, December 3, 2010 at 12:33am by andrea

Chemistry
suppose a pippetting error was made when preparing the diluted vinegar, but the diluted vinigar solution was uniform and the naoh titration values were consistant. when will the student learn that the experiment result was not accurate explain
Friday, December 3, 2010 at 9:59am by peter

Chemistry
A 3.0 -L sample of a 5.8 M NaCl solution is diluted to 65 L. What is the molarity of the diluted solution?
Tuesday, November 30, 2010 at 7:28pm by Kelsey G

Chemistry-please help
Hi, I have a queestion on Gas Chromatography(GC). The following were injected into the GC systemk: - 1) 1% sample solution in acetone 2) a 500 times dilution of item 1) The retention time of the main peak in the diluted sample solution 2) shifted by ~ 2min. The expected area ...
Sunday, September 18, 2011 at 5:06pm by jess

Chemistry
first dilution: you diluted it to 10/19 of .1M, so it is 10/190 M. Then you diluted it 10/100 of its concentration, new concentration 10/1900 M the statement <The student diluted the sample as above 1 time(s).>> makes no sense to me, it it means my first paragraph, ...
Monday, April 7, 2014 at 5:13pm by bobpursley

Chemistry
If 3.0 L of a 5.0 M SrCl_2 solution is diluted to 40 L, what is the molarity of the diluted solution?
Tuesday, October 5, 2010 at 1:11am by Lyz

Chemistry
If 4.0 L of a 4.8 M SrCl2 solution is diluted to 50 L , what is the molarity of the diluted solution?
Monday, November 1, 2010 at 2:47pm by Lisa

Chemistry
If 4.0 L of a 4.8 M SrCl2 solution is diluted to 50 L , what is the molarity of the diluted solution?
Monday, November 1, 2010 at 7:43pm by Lisa

chemistry
If 4.0 L of a 4.9 M SrCl2 solution is diluted to 40 L, what is the molarity of the diluted solution?
Saturday, November 20, 2010 at 2:14pm by Lisa

Chemistry
Then calculate the inital ClO^- concencentrations for 1st, 2nd, and 3rd reactions. Calculate [ClO^-] in a 6% bleach solution. A 6% bleach solution contains 6 grams of NaClO per 100 grams bleach. The density of 6% bleach is 1.07g/mL. Chemical reaction: Blue dye + ClO^- -->...
Tuesday, February 28, 2012 at 12:42am by Cassandra

Chem
you diluted it by a factor of 100 (added 99 parts water). then, you diluted it another factor of 100 (.005L to .5L). New concentration: .0500/1E6 M
Friday, October 14, 2011 at 9:16pm by bobpursley

chemistry
A 45.8mL sample of 5.8M KNO3 solution is diluted to 1.00L. What volume of the diluted solution contains 15.0 g of KNO3.
Sunday, November 6, 2011 at 1:35am by Monique

chemistry
An aspirin tablet weighing 0.502 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Sunday, January 27, 2008 at 4:16am by John

chemistry
An aspirin tablet weighing 0.502 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Monday, January 28, 2008 at 4:37am by Anonymous

chem
An aspirin tablet weighing 0.650 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Friday, April 18, 2008 at 12:46am by Un

chemistry
An aspirin tablet weighing 0.475 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Monday, January 26, 2009 at 1:27am by leah

Chem.
An aspirin tablet weighing 0.400 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Saturday, April 18, 2009 at 2:18am by Joanne

chemistry
An aspirin tablet weighing 0.548 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Monday, April 19, 2010 at 2:24am by Anonymous

Chemistry
An aspirin tablet weighing 0.475 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Friday, January 21, 2011 at 5:51pm by

Chemistry
A 10 mL sample of 1.5 M Potassium Phosphate is placed in a 100 mL volumetric flask and diluted to the mark. What is the Molar concentration of Potassium ions in this diluted solution?
Thursday, April 11, 2013 at 8:29pm by Jo

chemistry
How many ml of 0.05M kmn04 acidic are diluted to oxidize 2gm of fes04 is diluted solution The answer 52.63 ml I want you step by step clearly explain Thank you for Bob
Sunday, January 27, 2013 at 3:23pm by Fai

college chemistry
An aspirin tablet weighing 0.502 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Sunday, January 24, 2010 at 9:23pm by Alexander

Chemistry
use the equation CsVs=CdVd Cs = Concentration of Stock (6.0M) Vs = Volume of Stock (125mL) Cd = Concentration of Diluted (??) Vd = Volume of Diluted (250mL) you are looking for the concentration or molarity of the diluted version of the hydrochloric acid because water was ...
Wednesday, September 30, 2009 at 7:07pm by Anonymous

Chemistry-help
Hi, I have a question on Gas Chromatography(GC). The following were injected into the GC system: - 1) 1% sample solution in acetone 2) a 500 times dilution of item 1) The retention time of the main peak in the diluted sample solution 2) shifted by ~ 2min. The expected area ...
Monday, September 19, 2011 at 5:58pm by jess

Chemistry
78 mL of a 1.60M solution is diluted to a volume of a 238mL. A 119-mL portion of that solution is diluted using 133 mL of water. What is the final concentration
Friday, April 13, 2012 at 7:41pm by Sam

chem
An aspirin tablet weighing 0.650 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Sunday, April 20, 2008 at 6:01pm by un

chem
An aspirin tablet weighing 0.475 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Monday, April 18, 2011 at 4:23pm by CHEMCHEM

college math/science
A solution was diluted by a factor of 2 and then again using a 1 to 3 dilution. What is the dilution of concentrate in the final sample or If 15ul of a 4% solution is diluted up to 50ul, what is the concentration of the resulting solution? Include units with your answer
Tuesday, May 26, 2009 at 9:59pm by alyemi

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

Biochemistry
If 1/40 dilution means 1 mL diluted to 40 mL total, then multiply your final (diluted) concn by 40.
Sunday, January 25, 2009 at 9:42pm by DrBob222

Chemistry
59.0 mL of a 1.80 M solution is diluted to a total volume of 268 mL. A 134-mL portion of that solution is diluted by adding 171 mL of water. What is the final concentration? Assume the volumes are additive.
Tuesday, March 19, 2013 at 9:49pm by Robert

chemistry
53.0 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 195 mL of water. What is the final concentration? Assume the volumes are additive.
Tuesday, March 26, 2013 at 10:27pm by Jen

chemistry
59.0 mL of a 1.40 M solution is diluted to a total volume of 278 mL. A 139-mL portion of that solution is diluted by adding 129 mL of water. What is the final concentration? Assume the volumes are additive.
Wednesday, April 17, 2013 at 6:09pm by lee

Chemistry
77.0 mL of a 1.20 M solution is diluted to a total volume of 288 mL. A 144-mL portion of that solution is diluted by adding 155 mL of water. What is the final concentration? Assume the volumes are additive.
Friday, May 10, 2013 at 5:42pm by Gmp

Chemistry- dilution
51.0 mL of a 1.20 M solution is diluted to a total volume of 248 mL. A 124-mL portion of that solution is diluted by adding 125 mL of water. What is the final concentration? Assume the volumes are additive.
Sunday, October 13, 2013 at 1:51pm by Chelsea

chemistry
An aqueous solution with a pH of 3.00 is diluted from 2.0 L to 4.0 L. Wht is the pH of the diluted solution?
Tuesday, May 5, 2009 at 11:06pm by j

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
A 10.0 ml diluted chloride sample required 44.89 ml of 0.01982 M AgNO3 to reach the Fajans end point. how many moles of Cl- ions were present in the sample? What was the concentration of chloride in the diluted solution?
Monday, October 8, 2012 at 8:18pm by lin

chemistry
Solution A, while in a 1.0 cm cell, has an absorbance of 0.390 and a [Cu2+] = 0.0283 M. Then, 6.57 mL of solution A is diluted with pure water to 100.0 mL. What is the absorbance of this diluted solution? I tried but I still don't get it. Can anyone please help! :( Thanks!
Saturday, April 24, 2010 at 10:02am by hongkong

Chemistry
If 12.90 mL of a 18.2 Weight% solution of sodium chloride is diluted to a final volume of 3.00 liters, what is the Molar concentration of the diluted solution? The density of the original solution is 1.12 g/mL.
Sunday, January 23, 2011 at 9:15pm by Danielle

AP Chemistry
If you combine 2.00 ml 2.0 x 10^-3 M KSCN and 98.00 ml 2.0M Fe(NO3)3 what is the concentration of FeSCN? I know the equation (V concentrated*M concentrated)=(V diluted *M diluted) should be used, but how do you go about that when you have two initial substances?
Wednesday, March 12, 2008 at 6:55pm by Emily

Chemistry
A 25 mL sample of waste water was treated with acid and SCN- to form an intense red complex. This complex was diluted to 100.0 mL and put in a variable pathlength cuvet. For comparison, a 10.0 mL reference sample of 6.8 x 10-4 M Fe3+ was treated with acid and SCN-, and diluted...
Sunday, November 27, 2011 at 3:49pm by Ken

chemistry
Aqueous solution with a pH of 10.6 is diluted from 1 L to 1.5 L. What is the pH of the diluted solution?
Sunday, March 14, 2010 at 6:39pm by elizabeth

Biochemistry
An acid diluted DOES change the pH. A base diluted DOES change the pH. For example, 0.1 M HCl has a pH of 1. Dilute that by a factor of 2 and the concn = 0.05. The pH of that solution is -log(0.05) = 1.30
Friday, June 24, 2011 at 12:47am by DrBob222

chemistry
20.0mls of a bulk solution was transferred to a 100ml volumetric flask and diluted to volume with water. 2.00mls of this solution was then found to have a concentration of 0.15M/l. What is the concentration of the bulk solution. The bulk solution has been diluted from 20 ml to...
Tuesday, June 9, 2009 at 8:15pm by MathMate

CHEMISTRY
Before investigating the scene, the technician must dilute the luminol solution to a concentration of 4.0010−2 . The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many moles of luminol are present in 2.00 L of the diluted...
Monday, September 28, 2009 at 1:29am by STEVE

Chemistry
Before investigating the scene, the technician must dilute the luminol solution to a concentration of 4.0010−2 . The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many moles of luminol are present in 2.00 L of the diluted...
Tuesday, October 13, 2009 at 7:26pm by boston

Chemistry
Before investigating the scene, the technician must dilute the luminol solution to a concentration of 4.0010−2 . The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many moles of luminol are present in 2.00 L of the diluted...
Tuesday, October 13, 2009 at 7:32pm by boston

Chemistry!
Before investigating the scene, the technician must dilute the luminol solution to a concentration of 6.0010−2 M. The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many moles of luminol are present in 2.00 L of the ...
Wednesday, March 28, 2012 at 10:43pm by Gabe

chemistry (Pls Bob check for me)
A 150 mg/dl glucose solution was diluted 1:2. Then 0.5ml of it was added to 4.5ml saline 2 ml of this solution was diluted to 10ml. What is the final concentration of glucose? 1L= 10dl 1dl =100mL Answer 0.015mg/dl
Saturday, March 16, 2013 at 2:30pm by Fai

Lab Math
A stock solution of inulin has a concentration of 500mg/ml. From this stock 0.05ml is diluted with 0.05ml of sterile saline. After 30 min blood is sampled and produces a result of 50ug/ml. What is total extravascular volume? I just need to find what the diluted part is so I ...
Wednesday, September 5, 2012 at 9:05pm by Morgan

Chemistry
A: A student must make a five-fold dilution of a 2.15 M HCl solution. If the student wishes to make 75.0 mL of the diluted solution, what volume of the 2.15 M solution will he need to dilute? B: What is the concentration of the diluted substance?
Monday, March 21, 2011 at 2:16pm by Anonymous

Chem
I erred. Goodness. You diluted it 100 times, then diluted it 100 times again. new concentration=.05M/(100x100)=.05/10,000 or .05*10^-4 or 5*10^-6 M
Friday, October 14, 2011 at 9:16pm by bobpursley

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

Chem (ques 2)
The analysis of some household cloudy ammonia cleaner involved diluting a 50.0mL sample of the cleaner to a volume of 250.0mL then titrating this diluted solution. The diluted sample was found to have an NH3 (aq) concentration of 0.350 mole per L. What is the percentage by ...
Saturday, January 27, 2007 at 9:14am by atriletz

Biochemistry
BSA stock solution A has a concentration of 3.50 mg/mL. 1.00mL of stock solution A is diluted to a final volume of 5.00mL to prepare solution B. 1.00mL of stock solution B is diluted to a final volume of 5.00mL to prepare solution C. 1.00mL of stock solution C is diluted to a ...
Monday, November 18, 2013 at 9:37pm by S

Chemistry
A. The forensic technician at a crime scene has just prepared a luminol stock solution by adding 13.0 g of luminol into a total volume of 75.0 mL of H2O. -What is the molarity of the stock solution of luminol? B. Before investigating the scene, the technician must dilute the ...
Sunday, October 12, 2008 at 11:00am by Irvin

P. Chemistry
A student added solid K2O to a 750.0 mL volumetric flask. The solid was dissolved in water and then the flask filled with water to the mark. This formed 750.0 mL of the initial KOH solution. 20.0 mL of the initial solution was transferred to another flask and diluted to 200.0 ...
Tuesday, February 23, 2010 at 5:32pm by Mark

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
Can someone please check to see if I am doing this correctly. Thank you :) Q) Calculate the new molarity of a 35mL sample of 0.450 M CaCl2 solution that is diluted with enough water to make 250 mL of solution. A) 0.450 m CaCl2 x 35mL/250mL = 0.063 mL diluted solution
Monday, April 1, 2013 at 5:21pm by Kishwa

chemistry
pH = -log(H^+). Plug in 3.00 for pH and calculate (H^+). Since the solution is diluted by a factor of two, then (H^+) in the diluted solution will be 1/2 of the initial value. Plug in the new (H^+) and solve for the new pH. Hint: it will NOT be 1/2 of 3.00.
Tuesday, May 5, 2009 at 11:06pm by DrBob222

chemistry
15.0 mL of 8.00 M NaOH was diluted with water to 500 mL. Calculate the molarity of the diluted NaOH solution. My calculations: 0.015L x 8.00moles/1L x 39.997/1mole = 4.8g M= (4.8g x 1mole/39.997) / 0.500L = 0.24M is my workings correct? Is there another way to get to this?
Monday, April 22, 2013 at 5:55am by alex

chem
a 45.8mL sample of a 5.8 M KNO3 solution is diluted to 1.00L. What volume of the diluted solution contains 15.0g KNO3? how do you do this? moles of solution: 5.8*.0458 moles Grams of solute= moles*molmassKNO3 Volume of 15g= 1000ml*15/gramssoluteabove
Thursday, April 5, 2007 at 11:40am by kyle

molarity
An aspirin tablet weighing 0.475 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Friday, February 16, 2007 at 12:54pm by christine

chemistry
An aspirin tablet weighing 0.548 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...
Thursday, May 10, 2007 at 10:08pm by jared

Chem 1
The forensic technician at a crime scene has just prepared a luminol stock solution by adding 15.0g of luminol into a total volume of 75.0 \rm mL of \rm H_2O. What is the molarity of the stock solution of luminol? 1.13M Before investigating the scene, the technician must ...
Wednesday, March 13, 2013 at 4:32pm by Chris

Food Analysis
1.If 0.5l of 5M solution of CU(NO3) is diluted to a volume of 0.80l by adding water, what is the molarity of the resulting diluted solution? 2.How many ml of water will be required to dilute 11ml of 0.45Macid solution to a molarity of 0.1M? 3.Calculate the weight CuSO4.5H2O ...
Tuesday, March 8, 2011 at 9:07am by Sarah

Science
A 5.0ml aliquot of a sample was transferred to a 25.0ml flask and acidified by addition of 2.5ml of 0.1M HClO4 and diluted to mark. 1.0ml of that solution was mixed with 5.0ml of 1 X 10-4M AYR(Aluminum)dye and 15.0ml ethanol in a 25.0ml flask and diluted to mark. What is the ...
Thursday, September 2, 2010 at 3:17pm by Eileen

oops--typo--Chemistry
This is the corrected copy. An equal sign I typed as a - sign. millimoles HCl = 6M x 51.2 = 3072. mmoles NaOH solution (75 mL) = 3072. M NaOH soln = mmoles/mL = 3072/75 = 4.096M That's the molarity of the diluted solution. The diluted solution started out as 6M and it was ...
Monday, May 13, 2013 at 6:07pm by DrBob222

Chemistry
You diluted the first one from 5 mL to 100 mL; therefore, the new concn will be = 0.01 M x (5 mL/100 mL) = ?M Or you can say you diluted it by a factory of 100/5 = 20 times; therefore, it is 1/20th as strong. Then 0.01 x 1/20 = ?
Tuesday, November 13, 2012 at 12:09am by DrBob222

Biochemistry
A protein sample is diluted 5-fold before measuring the protein concentration in a protein assay. In the protein assay, the concentration of the diluted protein is determined to be 0.27 mg/mL. What is the concentration of the original protein sample?
Tuesday, November 19, 2013 at 7:57am by S

Analytical chemistry
A 25 ml sample of household bleach was diluted to 500 ml in a volumetric flask. An unmeasured excess of potassium iodide was aded to a 20 ml aliquot of the diluted sample; the iodine liberated in the reaction: OCl- + 2I- -> I2 + Cl- + H2O required 34.5 ml of 0.0409 M ...
Tuesday, July 30, 2013 at 8:55am by Gloria

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

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