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April 19, 2014

Search: how many milliliters of a stock solution of 2.00m KNO3 would you need to prepare 250mL of 0.150M KNO3

Number of results: 27,020

chemistry
what is the molarity of a solution of KNO3(molecular mass=101) that contains 404 grams of KNO3 in 2.00 liters of solution? A. 1.00M b. 2.00M c. 0.500M d. 4.00M The definition of molarity is #mols/Liter of solution. Convert 404 g KNO3 to mols (mols = g/molar mass) and plug into...
Monday, March 26, 2007 at 9:34pm by Kat

New Buffalo High
how many milliliters of a stock solution of 2.00 M KNO3 would you need to prepare 100.0 mL of 0.150 M KNO3?
Wednesday, May 5, 2010 at 11:32am by Nikki

Chemistry
How many milliliters of a stock solution of 2.00 M KNO3 would yoou need to prepare 250 mL of 0.150 M KNO3? Please show work.
Friday, April 30, 2010 at 2:17pm by MEGAN!!!!

chem
You have a large amount of 7.50M stock solution. You need 1.80L of 3.00M solution for an experiment. How would you prepare the desired solution without wasting any stock solution?
Thursday, November 8, 2012 at 11:56am by chemdummy

Chemistry 2
You have a stock solution of 15.0 M NH3 . How many milliliters of this solution should you dilute to make 1200ml of 0.280 M NH3? If you take a 15.0ml- portion of the stock solution and dilute it to a total volume of 0.600 L , what will be the concentration of the final ...
Thursday, December 3, 2009 at 9:12am by Melissa

Fractions
A technician has prepared three solutions from a 600 mL stock solution. • In preparing the first solution ½ of the original volume of the stock solution was used. • The second solution required ¼ of the remaining stock solution. • Preparation of the third solution used 3/5 of ...
Monday, November 12, 2012 at 11:35pm by anna

chemistry
For dilution problems (preparing a weaker solution from a stronger stock solution) use: V1M1 = V2M2 (1.00M)(V1) = (0.240M)(2.00L) Solving for V1, V1 = (0.240M)(2.00L) / (1.00M) = ? The second part, I don't quite follow.
Wednesday, March 4, 2009 at 6:17pm by GK

Math - urgent
2. A technician has prepared three solutions from a 600 mL stock solution. • In preparing the first solution ½ of the original volume of the stock solution was used. • The second solution required ¼ of the remaining stock solution. • Preparation of the third solution used 3/5 ...
Monday, November 12, 2012 at 9:29pm by anna

chemistry
to what volume should you dilute 125mL of an 8.00M CuCl2 solution so that 50.0mL of the diluted solution contains 5.9g KNO3 I have a hard time determing the M1V1=M2V2 is
Sunday, November 6, 2011 at 1:39am by swtnblk

Chemistry
A student determined the H of neutralization of nitric acid (HN03) mixed with NaOH solution, using the procedure described in this experiment. Fifty milliliters of 1.00M HN03 was added to 50.5 mL of 1.00M NaOH solution, and the following time-temperature data were recorded. A ...
Wednesday, May 1, 2013 at 10:01pm by Mimi

chem
Describe in detail by words how to prepare 200ml of .150M HCl from a 1.00 M HCl stock solution? Need help with this please? i used C1V1=C2V2 and got volume 2 = 33L or 0.33mL. to prepare the solution i need to weigh 1 gram of HCL (from 1.00M HCl stock solution)lets say i put it...
Tuesday, November 27, 2012 at 1:22pm by vince11

chemistry
How would you prepare 2.25L of a 3.00M solution from a 15.0M stock solution?
Friday, October 18, 2013 at 4:01pm by mona

Chemistry
You wish to prepare 0.18 M HNO3 from a stock solution of nitric acid that is 18.9 M. How many milliliters of the stock solution do you require to make up 1.00 L of 0.18 M HNO3? Answer and..... HOW DO I DO IT?
Wednesday, October 1, 2008 at 12:38am by Brittany

Pharm Tech
You may find help among these links: http://search.yahoo.com/search?fr=mcafee&p=for+250ml+of+a+2%25+solution%2C+how+many+milliliters+of+a+5%25+stock+solution+are+needed Sra
Thursday, November 4, 2010 at 10:58pm by SraJMcGin

Chemistry
You wish to prepare 0.18 M HNO3 from a stock solution of nitric acid that is 18.9 M. How many milliliters of the stock solution do you require to make up 1.00 L of 0.18 M HNO3?
Wednesday, October 1, 2008 at 12:02am by Brittany

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

Pharm Tech
how many milliliters of a 5% stock solution are needed to prepare 250ml of a 2% solution?
Thursday, November 4, 2010 at 10:58pm by Kelsey

Chem
An aqueous KNO3 solution is made using 82.7 grams of KNO3, diluted to a total solution volume of 1.50 L. The density of this solution is 1.05 g/mL. What is the molality of this solution?
Monday, May 2, 2011 at 10:08pm by Ryan

Chemistry
An aqueous KNO3 solution is made using 73.4g of KNO3 diluted to a total solution volume of 1.86 L. Calculate the molarity of the solution. (Assume a density of 1.05 g/ml for the solution.)
Tuesday, January 29, 2013 at 5:46pm by Anna

chemistry
You have a stock solution of 14.0 . How many milliliters of this solution should you dilute to make 1350 of 0.280 ?
Friday, October 1, 2010 at 11:35pm by Melanie

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

Chemistry
How many milliliters of 7.00M HCl solution are needed to obtain 0.200mol of HCl?
Monday, October 15, 2012 at 7:22pm by Chris

chemistry
A KNO3 solution is made using 88.4g of KNO3 and diluting to a total soultion volume of 1.50l. Calculate the molarity and mass percent of the solution. Assume a density of 1.05 g/mL for the solution.
Sunday, November 6, 2011 at 1:30am by Monique

chemistry
how preapare 30.0ml of 0.800m HNO3 FROM A STOCK SOLUTION OF 4.00M HNO3 WHAT VOLUME IN ML OF THE 4.OOM HNO3 SOLUTION WILL YOU NEED?
Sunday, April 10, 2011 at 8:22pm by Anonymous

chem
The solubility of KNO3 is 155 g per 100 g of water at 75 degrees celcius and 38.0 g at 25 degrees celcius. What mass (in grams) of KNO3 will crystallize out of solution if exactly 100 g of its saturated solution at 75 degrees celcius is cooled to 25 degrees celcius. i found ...
Wednesday, October 15, 2008 at 8:04pm by Mischa

Chemistry
You have a stock solution of 15.0 M NH3 . How many milliliters of this solution should you dilute to make 1200ml of 0.280 M NH3 ?
Thursday, December 3, 2009 at 9:10am by Melissa

Chemistry
You have a stock solution of 16.0 M {{NH}}3. How many milliliters of this solution should you dilute to make 1500 mL of 0.200 M {{NH}}3?
Thursday, October 7, 2010 at 5:34pm by Veronica

Chemistry
You have a stock solution of 15.8 M NH3 . How many milliliters of this solution should you dilute to make 1350 mL of 0.300 M NH3
Tuesday, September 13, 2011 at 12:32am by Jennie

College 103 Chem
How many grams of Sodium Phosphate would you need to make 225ml of 8.00M of stock solution? Thank you
Wednesday, July 10, 2013 at 9:33pm by Andrew

algebra
In the lab, Jessica has two solutions that contain alcohol and is mixing them with each other. She uses times as much Solution A as Solution B. Solution A is alcohol and Solution B is alcohol. How many milliliters of Solution B does she use, if the resulting mixture has ...
Friday, February 11, 2011 at 6:48pm by Jay

chemistry
A volume of 100mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after...
Monday, August 6, 2012 at 8:00pm by Anon

Chemistry
2) To the solution in problem 1 (d) at 100 degrees celsius, 10g of water are added, and the solution is cooled to 0 degrees celsius... (problem 1d: the number of grams of water required to dissolve a mixture containing 15 g KNO3 and 3.5 g CuSO4 * 5 H20, assuming that the ...
Tuesday, September 18, 2012 at 9:50pm by Sam

chemistry
A student measures the conductivity of a KNO3 solution and determines it to be a strong electrolyte. the student incorrectly lists the species in solution as KNO3,K+, NO3. Give the correct list of species in solution? Please help I am lost
Friday, November 30, 2012 at 3:27am by Min

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
You have a stock solution of 13.4 M NH3. How many milliliters of this solution should you dilute to make 100.0 mL of 0.100 M NH3
Friday, October 15, 2010 at 12:19am by Nancy

chemistry
What volume of a 2.5 M stock solution of acetic acid (HC2H3O2) is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?
Tuesday, June 19, 2012 at 9:49am by nhfgchnr

chemistry
What volume of a 2.5 M stock solution of acetic acid (HC2H3O2) is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?
Friday, September 6, 2013 at 9:07am by delacia

chemistry
What volume of a 2.5 M stock solution of acetic acid (HC2H3O2) is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?
Thursday, September 12, 2013 at 9:01am by delacia

Chemistry
How many milliliters of a 2000.0 mg/dl stock solution are needed to prepare 100.0 ml of a 150.0 mg/dl working solution?
Tuesday, April 14, 2009 at 8:14pm by Jessi

Chemistry
How many milliliters of a 2000.0 mg/dl stock solution are needed to prepare 100.0 ml of a 150.0 mg/dl working solution?
Tuesday, April 14, 2009 at 10:16pm by Jessi

chem
What volume of a 2.5 M stock solution of acetic acid (HC¿HÀO¿) is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?
Thursday, May 10, 2012 at 4:59pm by pat

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
A chemist must dilute 55.6 ml of 1.48 M aqueous silver nitrate (AgNO3) solution until the concentration falls to 1.00M. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Round your ...
Friday, August 31, 2012 at 8:28pm by Lizzy

chem please
yes. the solubility of KNO3(s) at 0.0 degree celsius is 15g KNO3/100g H2O. Also, A 320g sample of a saturated solution of KNO3(s) in water is prepared at 25.0 degree celsius (this is part of the info given). i don't know how to solve this.
Sunday, February 1, 2009 at 10:29pm by Erin

chemistry
What mass of KNO3 in grams would be required to prepare 0.6 liters of a 1.8 M KNO3 solution?
Tuesday, November 29, 2011 at 7:39pm by Megan

chemistry
How many milliliters of a 5.0 M H2SO4 stock solution would you need to prepare 125.0 mL of 0.19 M H2SO4?
Thursday, November 4, 2010 at 3:47pm by MaryJ

chemistry
How many milliliters of a 5.0 M H2SO4 stock solution would you need to prepare 132.0 mL of 0.21 M H2SO4?
Sunday, February 26, 2012 at 6:03pm by Anonymous

Chemistry
How many milliliters of a 5.0 M H2SO4 stock solution would you need to prepare 123.5 mL of 0.48 M H2SO4?
Monday, April 7, 2014 at 9:38pm by Web

chemistry
How many milliliters of a stock solution of 5.40 M HNO_3 would you have to use to prepare 0.150 L of 0.510 M HNO_3?
Tuesday, September 27, 2011 at 10:50pm by jeff

Chemistry
Calculate the pH of a solution that is 2.00M HF, 1.00M NaOH, and 0.393M NaG (Ka=7.2 x10^-4). The answer I got was 4.76 ..
Friday, March 22, 2013 at 9:45pm by Jill

chemistry
How many moles KNO3 will you need? That is M x L = moles KNO3. Then moles KNO3 = grams KNO3/molar mass KNO3.
Saturday, February 11, 2012 at 6:03am by DrBob222

chemistry
How many milliliters of a stock solution of 12.0M HNO3 would you have to use to prepare 0.400M of 0.390 HNO3 ?
Saturday, September 25, 2010 at 4:01pm by riah

chemistry
moles AgNO3 = M x L = 0.563M x 0.0346L = 0.020 moles approximately but you need to redo all of these since I estimate all of the numbers. KI(aq) + AgNO3(aq) ==>AgI(s) + KNO3(aq) Now convert moles AgNO3 to moles KI using the coefficients in the balanced equation. moles AgNO3...
Tuesday, December 6, 2011 at 10:23pm by DrBob222

Math
How many milliliters of pure acid must be added to 150 milliliters of a 70% solution of acid to obtain a 80% solution?
Monday, February 18, 2013 at 7:15pm by Anonymous

Chemistry Lab
You are given 350 mL a stock solution of 1.66E-02 M benzoic acid, MW = 122.125 g/mol. Answer the following questions. A. What is the number of moles present in the original stock solution? B. You need to dilute the benzoic acid stock solution to 1.24E-03 M. If you need 455 mL ...
Tuesday, January 11, 2011 at 11:50pm by Natasha

Chemistry Lab
You are given 350 mL a stock solution of 1.66E-02 M benzoic acid, MW = 122.125 g/mol. Answer the following questions. A. What is the number of moles present in the original stock solution? B. You need to dilute the benzoic acid stock solution to 1.24E-03 M. If you need 455 mL ...
Tuesday, January 11, 2011 at 11:50pm by Natasha

analytical chemistry
your lab possesses a stock solution of NaOH whose concentration is approx. 0.1M. you prepare a secondary solution by diluting 15.00mL of this stock solution to a total volume of 250.0 mL. you titrate a 50.00mL aliquot of the secondary solution with a hydrochloric acid solution...
Thursday, February 21, 2013 at 2:16pm by holly

chemistry
how wold you prepare 2.00L of 1.00M HCl solution using 6.00 M HCl? i already found the volume of 6.00M HCl needed to be .333L. i am confused about how to actually prepare the solution. do i used a volumetric flask or any other glassware?
Saturday, February 26, 2011 at 5:31pm by lindy

chemistry
2) Suppose you have 5.00g of powdered magnesium metal, 1.00L of 2.00M potassium nitrate solution, and 1.00L of a 2.00M silver nitrate solution. a. Which one of the solutions will react with the magnesium powder?
Sunday, March 17, 2013 at 1:04pm by Anonymous

CHEM
Help on part "c": The forensic technician at a crime scene has just prepared a luminol stock solution by adding 19.0g of luminol into a total volume of 75.0mL of H2O. a)What is the molarity of the stock solution of luminol? anwer I got: molarity of luminol solution = 1.43M b)...
Thursday, October 18, 2007 at 3:31am by K

CHEM
Help on part "c": The forensic technician at a crime scene has just prepared a luminol stock solution by adding 19.0g of luminol into a total volume of 75.0mL of H2O. a)What is the molarity of the stock solution of luminol? answer I got: molarity of luminol solution = 1.43M b)...
Thursday, October 18, 2007 at 3:35am by K

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

UCI
A student is given a stock solution of 1.54E-04 M. How much stock solution is needed to make 100 mL of a 1.60E-05 M solution?
Friday, April 9, 2010 at 12:17am by Anonymous

math115
A chemist has 400 milliliters (mL) of solution that is 21% acid. How many milliliters of acid are in the solution?
Monday, September 14, 2009 at 9:12pm by dwayne

chemistry
How many milliliters of 16.0 M HNO3 stock solution wouuld be required to prepare 100.0mL of 3.00 M HNO3? Use the formula M1V1=M2V2
Monday, January 23, 2012 at 7:56pm by missy

chem
If there is a stock generally made up at 50x concentration, how many milliliters of stock will we need to make up 2 liters of agar medium properly?
Wednesday, September 14, 2011 at 8:19pm by ROSE

chem
how do you prepare a solution using the proper lab equipment(both from dry solid and a stock solution) i researched it but all i found was the definition for stock solution any help please!!
Thursday, February 12, 2009 at 2:25pm by lyne

Chemistry!!
A chemist wants to prepare a stock solution of H2SO4 so that a sample of 20.00mL will produce a solution with a concentration of .50 M when added to 100.0mL of water. A)what should the molarity of the stock solution be? B)If the chemist wants to prepare 5.00L of the stock ...
Monday, April 22, 2013 at 6:09pm by Anonymous

chemistry
A 355g sample of a saturated solution of KNO3(s) in water is prepared at 25.0 degrees C. If 50g H2O is evaporated from the solution at the same time as the temperature is reduced from 25.0 to 0.0 degrees C, what mass of KNO3(s) will recrystallize? i have no idea where to start...
Monday, February 22, 2010 at 12:29am by david

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

chemistery
How many milliliters of 4.00M NaOH wll react with 100 mL of 0.312 M H2SO4?
Sunday, December 9, 2012 at 7:16pm by ogb

Chemistry
I can't figure out how to set up this problem...You have a large amount of 8.00 M stock solution. You need 1.80L of 3.00 M solution for an experiment. How would you prepare the desired solution without wasting any stock solution?
Wednesday, October 5, 2011 at 10:11am by Nicole

Chemistry
The molecular mass of glucose is 180g/mol. you prepare a stock solution of glucose, by dissolving 1.8g of glucose in water to a final volume of 1.0L. The stock solution was then diluted as follows: a. 50mL of the stock solution is added to 450mL of water, b. and then 1.0mL of ...
Monday, August 29, 2011 at 1:24pm by Titania

science
HCl you need? HCl is a liquid, what is your stock solution concentration? Assuming the stock solution is 12M, then you need to dilute it 4 times, or three parts water, one part stock solution. one part of 50ml is 12.5ml HCl stock solution, then 3 parts (37.5ml) water. Add the ...
Tuesday, March 8, 2011 at 6:18am by bobpursley

Chemistry
You have 10.0 L of 1.2 M KNO3. What molarity would the KNO3 solution be if you were to take 2.5 L of it and dilute it to 10.0 L?
Wednesday, March 6, 2013 at 8:54pm by Kay

Chemistry
.12M Lactic Acid (HC3H5O3, Ka=1.4x10^-4) is mixed with .10M NaC3H5O3 to form 1.00L solution. A. Calculate the pH of the solution after the addition of 50.0mL of 1.00M NaOH. B. Calculate the pH of the solution after the addition of 120.0mL of 1.00M NaOH.
Sunday, March 28, 2010 at 12:16pm by Emma

math
A solution of alcohol and water is a% alcohol where a = 40. The solution is found to contain 32 milliliters of alcohol. How many milliliters total (both alcohol and water) are in the solution?
Monday, November 8, 2010 at 9:52am by Sabre

CHEMISTRY
HOW CAN U TELL IF HNO3 +KNO3 IS A BUFFER SOLUTION A buffer solution must contain a weak acid and its conjugate base OR a weak base and its conjugate acid. HNO3 is a strong base and KNO3 is the salt of a strong base (KOH) and a strong acid (HNO3); therefore, it doesn't qualify ...
Tuesday, February 27, 2007 at 11:05pm by CANDY

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

science
250 milliliters = 0.25 L; To make a 3.0 M NaOH solution from 6.0 M NaOH, you need equal parts of water and NaOH solution You need 0.25 Liters of the solution, so you need 1/2 * 0.25 = 125 milliliters 6.0 M NaOH, and 125 milliliters water
Thursday, November 1, 2012 at 2:15pm by Jennifer

chemistry
delta T = i*Kf*m Solve for m. m = moles KNO3/kg solvent Solve for moles KNO3. moles KNO3 = grams KNO3/molar mass KNO3 Solve for grams. i = 2
Monday, February 6, 2012 at 8:25pm by DrBob222

Chemistry
You have a stock solution of 14.4 M NH3. how many mililiters of this solution should you dilute to make 1050mL of .220 M NH3 answer 16.o mL Question if you take a 10.5mL portion of the stock solution and dilute it to a total volume of .600L, what will be the concentration of ...
Monday, February 21, 2011 at 12:56am by Natalie

Chemistry
I am having trouble answering this. please help! Q: Cereol is a newly discovered compound in corn flakes. A biologist suspects that it increases mental ability. She is making a solution to test on rats. First she makes a stock solution. She discovers that this is too ...
Saturday, March 31, 2012 at 9:25pm by Maddy

Chemistry please help!
Please help. I have no idea how to do these 4 homework problems. 1- How many milliliters of 0.140 M HCl are needed to completely neutralize 42.0mL of 0.106 M Ba(OH)2 solution? 2-How many milliliters of 0.123 M H2SO4 are needed to neutralize 0.250 g of NaOH ? 3-If 55.2 mL of ...
Monday, February 22, 2010 at 1:30pm by Robert

Math
A chemist working on a flu vaccine needs to mix a 10% sodium-iodine solution with a 60% sodium-iodine solution to obtain a 50-milliliter mixture. Write the amount of sodium iodine in the mixture, S, in milliliters, as a function of the number of milliliters of the 10% solution...
Saturday, September 6, 2008 at 4:19pm by Anonymous

Chemistry
How many moles do you need in the diluted solution? That will be M x L = ?? So you must use?? moles of the stock to obtain that. M stock = moles stock/L stock. You know moles and M, solve for L.
Monday, April 11, 2011 at 3:22pm by DrBob222

Chemistry, Urgent!
I can't solve this! I keep trying but I can't get it. Suppose 25mL of 1.00M HCl is added to 50mL of 1.00M HF. What is the pH of the HF in this solution? The pH is supposed to be 0.48 Thanks. -K.
Thursday, February 26, 2009 at 12:20am by Kearstyn

Chemistry
A stock solution is prepared by adding 20mL of 0.2M MgF2 to enough water to make 80mL. What is the F– concentration of 20 mL of the stock solution?
Thursday, November 3, 2011 at 9:29pm by aDRIAN

Chemistry
If 22.15 milliliters of 0.100 molarity sulfuric acid is required to neutralize 10.0 milliliters of lithium hydroxide solution, what is the molar concentration of the base?
Wednesday, November 28, 2012 at 12:49pm by Kaela

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

chem
Yes, unless the solubility figure is quote another way than what I listed. 60 g KNO3/100 g H2O is not the same as 60 g KNO3/100 g solution.
Sunday, May 13, 2012 at 10:18pm by DrBob222

Biochemistry
Can someone help me calculate protein concentration using the Bradford Assay? If you could show me how to do tube 2, that'd be great. Tube 1: 0 ul Protein Stock Solution, 800 ul Water, 0 ug Protein, Absorbance @595nm = 0 Tube 2: 10 ul Protein Stock Solution, 790 ul Water, 1.4 ...
Monday, October 7, 2013 at 5:29pm by OR

math
You are a lab technician and must create 250 ml of a 17% salt-solution. a. If you have 500 ml of 28% salt-solution, how many milliliters of it should you mix with water in order to create 250 ml of a 17% salt-solution? b. If you have 400 ml of 40% salt-solution, how many ...
Wednesday, February 15, 2012 at 8:45am by Fatih

Calc
You are a lab technician and must create 250 ml of a 17% salt-solution. a. If you have 500 ml of 28% salt-solution, how many milliliters of it should you mix with water in order to create 250 ml of a 17% salt-solution? b. If you have 400 ml of 40% salt-solution, how many ...
Thursday, February 16, 2012 at 10:16am by Fatih

chemistry
25 milliliters of tartaric acid solution is titrated against 31 milliliters of NH4OH. What is the normality of the NH4OH?
Wednesday, October 3, 2012 at 6:10pm by Stephen

chemistry
Hydrochloric acid is usually purchased in concentrated form with a 37.0% HCL concentration by mass and a density of 1.20g/mL. How much of the concentrated stock solution in milliliters should you use to make 2.5L of 0.500M HCL
Sunday, November 6, 2011 at 1:16am by Monique

Chemistry
You do not need the density to solve since the total volume is given Molarity=moles/liters 73.4g of KNO3/101.1032 g of KNO3/mol= moles of KNO3 Molarity=moles/liters=moles of KNO3/1.86L
Tuesday, January 29, 2013 at 5:46pm by Devron

physics
exactly what drwls said. Electric field = -(change in charge)/(change in position) So in this case in particular, you have: - (190V-120V)/(5.00m-3.00m) = - (70V)/(2.00m) = -35V/m or -35 N/C *V/m = N/C*
Friday, January 29, 2010 at 8:19am by ant

chemistry
you are conducting a freezing-point determination in the laboratory by using an aqueous solution of KNO3. The observed freezing point of the solution is -1.15 C. Using a pure water sample, you recorded the freezing point of the pure solvent of the same thermometer as .25 C. ...
Thursday, February 17, 2011 at 7:10pm by Anonymous

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