Friday
April 18, 2014

Search: A 130.0 mL sample of a solution that is 3.0×10-3 M in AgNO3 is mixed with a 225.0 mL sample of a solution that is 0.13 M in NaCN. After the solution reaches equilibrium, what concentration of Ag+(aq) remains?

Number of results: 119,211

Chemistry
I have a 7 mL solution with 3 mL of H2O added to the solution. How would I figure out the molarity of the solution?
Monday, March 31, 2008 at 11:49pm by TAG

chemistry
I worked this for you a day or so ago (two ways in fact) so you should know 429 mL is not right.In the future I will ignore any problems I've addressed previously. g x % = g x % 50g x 10% = g x 36% g = (50*10/36) = 13.89g. Use density = mass x volume to convert 13.89g to mL. v...
Saturday, August 11, 2012 at 2:29pm by DrBob222

College Chemistry
A 20.0 Ml sample of sulfuric acid is titrated with 25.0 ML of 1.0 M NaOH solution. What is the molarity of the sulfuric acid? H2SO4+ 2NaOH yields Na2SO4 + H2O
Monday, December 6, 2010 at 11:55am by Sa ndra

Chemistry
What is the pH of the solution created by combining 12.40 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? I know how to solve for HCl but not with HC2H3O2.
Saturday, May 1, 2010 at 8:43pm by Manali

Chemistry
I was just wanting to make sure I did these right. How many grams of solute are in each of the following solutions? a.) 2.5 L of 3.0 M Al(NO3)3 solution. for this one I get 1600 g of Al(NO3)3 b.) 75 ml of 0.5 M C6H12O6 solution. and for this one I get 6.8g of C6 H12 O6 How ...
Monday, November 29, 2010 at 4:12pm by Carrie

chemistry
assuming the density of a 5% acetic acid solution is 1.0g/ml, determine the volume of the acetic acid solution necessary to neutralize 25.0 ml of 0.10 m NaOH. also record this calculation on your report sheet.
Thursday, October 22, 2009 at 10:18am by janvi

Chemistry
Suppose you are going to add 450 mL of a 0.10 mol/L hydrochloric acid solution to 250 mL of a 0.2 mol/L sodium hydroxide solution. a)Which one is the limiting reactant? b)What is the theoretical yield of sodium chloride?
Saturday, December 10, 2011 at 5:05pm by Maame

Jill
State the relationship of A to B (i.e. <, >, = or can't be determined). 1. Using a 0.05 M Ag+ titrant A.VEP in titration 25-mL of 0.01 M MgCl2 B.VEP in titrating 25-mL of 0.01 M AlCl3 2. A 25.0-mL solution contains 0.015 M NaCl and 0.010 M HCl A.VEP (Mohr) B.VEP (...
Monday, February 20, 2012 at 6:33pm by Chemistry Homework Help

pharmacy calculations
500 ml of a 1:5 solution contains 500*(1/5)=100 ml. of the concentrate. So if x is the volume of 1:4, then 500-x is the volume of 1:10. Hence x(1/4)+(500-x)(1/10)=500*(1/5) Solve for x to get x=333.33 ml.
Friday, August 3, 2012 at 1:08pm by MathMate

Chemistry-Please help
11.0 g/100 mL = ?? g/mL. You took 50.0 mL of this solution and diluted to 500 mL. So the final concn is 0.11 g/mL x (50 mL/500 mL) = ?? g/mL. g glucose in 100 mL = ?? g/mL x 100 mL = xx g/100 mL.
Monday, October 5, 2009 at 7:48pm by DrBob222

chemistry
A 15.0 ml sample of an unknown HClO4 solution requires 50.3 ml if 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is: HClO4(aq)+ NaOh(aq)yields H2O(l)+ NaClO4 (aq) If anyone can help me to set this...
Saturday, December 3, 2011 at 2:35am by ben

chemistry
A 15.0 ml sample of an unknown HClO4 solution requires 50.3 ml if 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is: HClO4(aq)+ NaOh(aq)yields H2O(l)+ NaClO4 (aq) If anyone can help me to set this...
Saturday, December 3, 2011 at 1:14pm by ben16

chemistry
A 15.0 ml sample of an unknown HClO4 solution requires 50.3 ml if 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is: HClO4(aq)+ NaOh(aq)yields H2O(l)+ NaClO4 (aq) If anyone can help me to set this...
Saturday, December 3, 2011 at 1:18pm by ben16

chemistry
Give the pH of a solution containing 0.344 g of HCL in 792 mL of water. I did .344g/36.5g= .009 mols. then i times that by .792 because i changed that from ml to liters. is that right?
Thursday, May 15, 2008 at 3:14pm by Miley

chemistry
50 mL of 1.50* 10^-2 M HI(aq) is mixed with 75.00 mL of 1.10* 10^-2 M KOH(aq). What is the pH of the Final solution
Monday, February 16, 2009 at 6:30pm by reena

College Chemistry
Suppose you take 2 mL of boiling A. X = 2 mL x 200 mg/mL = 400 mg so all of X will dissolve. Y = 2 mL x 200 mg/mL = 400 mg so all of Y will dissolve. Now cool the solution to room temperature. How much X and Y will recrystallize? 2 mL x 20 mg/mL = 40 mg X will stay in solution...
Monday, January 21, 2013 at 11:49pm by DrBob222

chemistry
calculate the volume of mL of a 1.420 M NaOH solution required to titrate the following solution. 25.00 mL of a 1.500 M H3PO4 solution
Tuesday, October 11, 2011 at 8:13pm by TROUBLED

chem
A 27.4 mL sample of an unknown HClO4 solution requires 45.4 mL of 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is shown below. HClO4(aq) + NaOH(aq) H2O(l) + NaClO4(aq)
Monday, March 14, 2011 at 3:16pm by BOBBY

chemistry
The same answer as previous. mols ClO^- x molar mass NaClO = grams NaClO. If you want percent then (g bleach/g sample)*100 = ? g bleach from above. g sample = 5 mL x density g/mL = grams sample
Sunday, October 27, 2013 at 9:38pm by DrBob222

Math
A doctor needs to administer 2 mL of a 100 mg/mL solution to a 200 pound patient. However, the doctor has the solution available only in 20 mg/mL strength. What volume of the 20 mg/ml solution would be needed to administer the desired dose ?
Monday, July 21, 2008 at 8:48pm by nicole

math
A doctor needs to administer 2 mL of a 100 mg/mL solution to a 200-pound patient. However, the doctor has the solution available only in 20 mg/mL strength. What volume of the 20 mg/mL solution would be needed to administer the desired dose?
Sunday, January 1, 2012 at 12:20am by Jamie

Buffer Solution
You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 M sodium acetate (CH3COONa). What will the pH of this solution be after the addition of 93 mL of 1.00 M NaOH solution?
Wednesday, April 13, 2011 at 12:42am by Nicole

Chemistry
The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)? A) 0.40 M B) 0.10 M C) 0.20 M D) 0.25 M E) 0.36 M The answer is supposedly C, but I got A. What am I doing ...
Tuesday, December 8, 2009 at 7:17am by Charlie

Chemistry
If one were to mix 200.0 mL of an HCl solution that had a pH of 3.00 with 200.0 mL of an NaOH solution that had a pH of 10.00, what would be the pH of the final solution? Can you show me the steps please so that I can apply to questions that ask for the same type of solving? ...
Thursday, December 16, 2010 at 9:42pm by Anonymous

Math
let's try this again... A doctor needs to administer 2 mL of a 100 mg/mL solution to a 200 pound patient. However, the doctor has the solution available only in 20 mg/mL strength. What volume of the 20 mg/ml solution would be needed to administer the desired dose ?
Monday, July 21, 2008 at 8:48pm by LYNN

Chem Webwork UCI
Complete the table below: What is the pH of the solution created by combining 0.70 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH: 0.70 pH w/ HCl: 1.08 pH wHC2H3O2: 3.23 Complete the table below: What are the pH ...
Monday, April 25, 2011 at 4:50pm by Michelle

Chemistry
10 mL*x = 20*y 20*x = ?y. Wouldn't that be 40 mL of the std? If that's confusing to you (and the whole problem is confusing), just make up a number for the standard solution. Let's call that 0.1M So 10mLunk x ?M = 20mLstd x 0.1M Solve for ?M unk = (20x0.1/10) = 0.2M for the ...
Tuesday, February 28, 2012 at 6:18pm by DrBob222

chemistry
yes. The original solution is diluted from 10 mL to 15 mL.
Sunday, August 2, 2009 at 7:44pm by DrBob222

Chemistry help needed
(0.99)(1.22g.soln/ml) = 1.2078 g pure acid / mL original soln. To get 100.0 g of pure acid: (100.0g) / 1.2078 g acid / mL = 82.8 mls original solution. The total weight of that solution is: (82.8 mls)(1.22g/ml) = 101g) (Let the diluted solution contain 100.0g pure acid = m) ...
Wednesday, December 17, 2008 at 9:43pm by GK

chem
A 4.55L sample of water contains .115g of sodium ions. Determine the concentration of sodium ions in ppm if the density of the solutions is 1.00g/mL. Ok so ppm=mass of solute/mass of solution *10^-6 so we have the mass of the solute .115g and for the solution we use 4.55 L and...
Friday, May 9, 2008 at 4:16pm by natash

chemistry
A student took 100 mL of a solution of Mg(OH)2 and reacted it with HCl (aq) to calculate the concentration of hydroxide ions in the solution. If 13.75 mL of 0.010M HCl was used to react with all of the OH- (aq) in the 100-mL solution, what was the concentration of hydroxide ...
Thursday, October 3, 2013 at 7:13pm by Donna

chemistry
One can get very confused with all of the symbols; what I do is make up a problem, then substitute symbols. Let's say we have a 10% sucrose soln that has a density of 1.1 g/mL (that may not be right but it doesn't matter since we're just doing the exercise to keep symbols ...
Tuesday, January 24, 2012 at 1:05pm by DrBob222

Chemistry
A 100.0 ml sample of 0.300 M NaOH is mixed with a 100.0 ml sample of 0.300 M HNO3 in a coffee cup calorimeter. Both solutions were initially at 35.0 degrees celcius; the temperature of the resulting solution was recorded at 37.0 degrees celcius. Determine the delta H (in units...
Wednesday, November 10, 2010 at 7:34pm by Kristy

chemistry
6.67 mL of 18.0 molar sulfuric acid solution was dissolved in enough water to make 500 mL of solution. The molarity of the diluted solution is
Monday, October 31, 2011 at 12:29am by Anonymous

chemistry
how many millimeters of a 5.15 M CH3OH stock solution are needed to prepare 375 mL of a solution having 7.50 mg of methanol per mL of solution
Sunday, September 29, 2013 at 6:57pm by Anonymous

Chemistry
The specific heat of a solution is X J/g*degreesC and its density is Y g/mL. The solution was formed by combining Z mL of solution A with Z mL of solution B, with each solution initially at J degreesC. The final temperature of the combined solutions is D. The heat capacity of ...
Friday, April 2, 2010 at 10:52am by Fred

chemistry
Potassium perchlorate has a lattice energy of -599 kj/mol and a heat of hydration of -548 kj/mol. Find the heat of solution for potassium perchlorate when 10.6 g of potassium perchlorate is dissolved with enough water to make 102.7 ml of solution. (J-absorbed) find the ...
Friday, September 18, 2009 at 5:32pm by ella

Chemistry
1. A good indicator will have a(n)____ close to this volume and pH. I think it's endpoint but it's wrong. 2. (part a) What is the pH of the solution created by combining 1.70 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? ...
Saturday, April 28, 2012 at 3:38pm by Jody

chemistry
A solution is prepared by dissolving 20.2 {\rm mL} of methanol ({\rm{CH}}_3 {\rm{OH}}) in 100.0 {\rm mL} of water at 25 ^\circ {\rm C}. The final volume of the solution is 118 {\rm mL}. The densities of methanol and water at this temperature are 0.782 {\rm g/mL} and 1.00 {\rm ...
Saturday, July 14, 2012 at 10:14am by aa

BLD 414
one tryoy ounce of gold is worth 380.00. There are 33.8 grams per troy ounce. you have a stock colloidal solution of a ver fine gold dust. It's concentration is .10%. From this solution 1.0ml is placed in 9.0ml of an isotonic, pH buffered solution to make a working stock. An ...
Monday, March 19, 2012 at 2:41pm by Amber`

chemistry
Magnesium metal reacts with HCl solution, liberating H2 gas and generating Mg2+ cations in solution. A 2.335-g sample of Mg metal is added to 50.0 mL of a 4.00 M HCl solution, and the reaction goes to completion. How many grams of H2 are formed?
Thursday, September 1, 2011 at 7:53pm by ALEX

Chemistry
Magnesium metal reacts with HCl solution, liberating H2 gas and generating Mg2+ cations in solution. A 1.890-g sample of Mg metal is added to 125.0 mL of a 4.00 M HCl solution, and the reaction goes to completion. How many grams of H2 are formed?
Tuesday, September 13, 2011 at 1:49am by Mike

Chemistry
Magnesium metal reacts with HCl solution, liberating H2 gas and generating Mg2+ cations in solution. A 1.890-g sample of Mg metal is added to 125.0 mL of a 4.00 M HCl solution, and the reaction goes to completion. How many grams of H2 are formed?
Tuesday, September 13, 2011 at 1:50am by Mike

Chemistry
Magnesium metal reacts with HCl solution, liberating H2 gas and generating Mg2+ cations in solution. A 2.970-g sample of Mg metal is added to 50.0 mL of a 4.00 M HCl solution, and the reaction goes to completion. How many grams of H2 are formed?
Tuesday, September 13, 2011 at 5:26pm by Carolina

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

Statistics
This is a binomial distribution with parameters N=130, p=0.6, r=90 so P(X=90)=C(N,r)p^r(1-p)^(N-r) =C(130,90)*0.6^90*0.4^40 =5.3347282074*10^33*1.0804695562359849*10^-20 * 1.2089258196146345*10^-16 =0.00697
Friday, July 20, 2012 at 5:47pm by MathMate

Chemistry
The density of the solution is 1.17 g/mL. How much does a liter weigh? 1.17 g/mL x 1000 mL = ?? grams = mass of soln. How much of that is NaOH? 0.0357%; therefore, ?? g soln x 0.0357 = ??g NaOH.(The remainder is the mass of the water in the solution). How many mols NaOH is ...
Sunday, September 7, 2008 at 1:24pm by DrBob222

chemistry
this is a really long question. i don't understand how to answer it. help please. A 10.0% aquueous solution of sulfuric acid has a density of 1.0661 g/mL at 20 degrees celsius. A. how many grams of H2SO4 are found in 50.0 g of this solution? B. how many grams of water are ...
Sunday, April 7, 2013 at 10:58pm by Nicole

Inorganic Chemistry
1) 5.0 mL of 6.0 x 10^-4 potassium 5.0 mL of the solution prepared above are then mixed with
Monday, July 30, 2012 at 10:28pm by Katheryn

chemistry
What is the molarity of a potassium hydroxide solution if 38.65 mL of the KOH solution is required to titrate 25.84 mL of 0.1982 M hydrochloric acid solution?
Wednesday, November 10, 2010 at 8:48am by Anonymous

chemistry
What is the molarity of a potassium hydroxide solution if 38.65 mL of the KOH solution is required to titrate 25.84 mL of 0.1982 M hydrochloric acid solution?
Wednesday, November 10, 2010 at 9:08am by Anonymous

science
A solution contains 2 mEq/mL of KCL (Molecular weight 74.5). If a 20 mL ampule of this solution is diluted to 1 liter what is the percent strenght of the resulting solution?
Monday, January 14, 2013 at 6:59pm by Felix

chemistry
A solution contains 2 mEq/ml of KCL (Molecular weight 74.5). If a 20 ml ampule of this solution is diluted to 1 liter what is the percent strength of the resulting solution?
Thursday, February 21, 2013 at 2:10pm by Ann

Chemistry
In a titration of 26.0 mL of 0.840 M H2SO4, __________ mL of a 0.200 M KOH solution is required for neutralization. Express your answer to the nearest 1/10 mL. Hint: remember H2SO4 is a diprotic acid
Wednesday, March 10, 2010 at 3:12pm by Camarra

Chemistry
A student placed 17.0 g of glucose (C_6H_{12}O_6) in a volumetric flask, added enough water to dissolve the glucose by swirling, then carefully added additional water until the 100 mL mark on the neck of the flask was reached. The flask was then shaken until the solution was ...
Wednesday, July 7, 2010 at 8:31pm by Tiffany

College Chemistry
The density of a 0.0122 M KMnO4 is 1.037 g/mL. Suppose 26.35 g of 0.0122 M KMnO4 are required to titrate 1.072 g of a household H2O2 solution. a)Calculate the mL of MnO4^- added to reach the endpoint. b)Calculate the moles of MnO4^- added to reach the endpoint. c)Calculate the...
Tuesday, February 25, 2014 at 3:47pm by Kelsey

Chemistry
Mass of an aspirin tablet is 0.42g and contains 77.38% ASA by mass. I dissolved the tablet in hot naOH and cooled the solution with distilled water to the mark of 250 volumetric flask. Then I pipetted 5.0 mL of the solution to the 100 mL volumetric flask and I diluted it with ...
Wednesday, April 25, 2007 at 7:34pm by Brissa

Chemistry
1. What is the pH of the solution created by combining 0.50 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? 2. What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of...
Monday, November 1, 2010 at 12:14am by Kyo

CHEMISTRY
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 ...
Thursday, October 17, 2013 at 9:41pm by Anonymous

chemistry
a student synthesized 6.895g of barium iodate monohydrate, Ba(IO3)2.H2O, by adding 30.00 mL of 5.912*10^-1M barium nitrate, Ba(NO3), to 50.00 mL of 9,004*10^-1 M sodium iodate, NaIO3 (1) write the chemical equation for the reaction of solutions of barium nitrate and sodium ...
Monday, March 1, 2010 at 1:32pm by aymal

chemistry check 2
I know you've read this question too many times already but I just want to make sure I did the last part (Ksp) correctly. 50.0 ml of a 0.0500 M solution of lead (II) nitrate is mixed with 40.0 ml of a 0.200 M solution of sodium iodate at 25°C. Calculate the Pb2+ and IO3- ...
Thursday, May 17, 2007 at 1:32pm by mel

Chemistry
when 20 ml of a .10 M silver nitrate solution is mixed with 25 ml of a 0.080 M solution of sodium sulfide, producing a precipitate of silver sulfide, what is the final concentration of sulfide ion?
Friday, December 7, 2012 at 8:58pm by Helga

chemistry
If a saline solution has a concentration of 0.25 g per mL, calculate the following. a) The concentration of this solution in %w/v. b) The concentration of this solution in grams per litre (g/L). c) The concentration of this solution in milligrams per mL (mg/mL).
Wednesday, November 7, 2012 at 6:10pm by Hannah

Analytical Chemistry
A 22.617 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is diluted with 70.407 g of water. A 10.883 g aliquot of this solution is then titrated with 0.1072 M HCl. It required 29.32 mL of the HCl solution to reach the methyl red ...
Thursday, February 28, 2013 at 5:04pm by Sam

chemistry
An aqueous solution of phosphoric acid, H3PO4, contains 285 g H3PO4 in 400 mL solution, and has a density of 1.35 g/mL. Calculate a. the weight % H3PO4 in this solution. b. the concentration in mol/L of this solution
Wednesday, November 10, 2010 at 4:12pm by princess

chem
A 26.8 mL sample of an unknown HClO4 solution requires 46.8 mL of 0.101 M NaOH for complete neutralization. What was the concentration of the unknown HClO4 solution? The neutralization reaction is shown below. HClO4(aq) + NaOH(aq) H2O(l) + NaClO4(aq) i got .00473 M HClO4 but ...
Friday, March 18, 2011 at 10:24am by hannah

Chemistry
How many grams of Na2CO3 can be found in a 273 mL sample of 0.5 M solution
Monday, April 8, 2013 at 3:40pm by Linzy

chemistry
b) what is the pH after the addition of 1.0 mL of 0.10 M HCL to 15.00 mL of the solution?
Wednesday, October 13, 2010 at 11:04pm by anon

Math
Theoretically they need 90ml & 3% = 2.7ml of 100% solution. Let x=volume of 10% solution, then 90-x = volume of 1% solution. x*10% + (90-x)*1% = 2.7 Multiply by 100: 10x + (90-x) = 270 Solve for x and check. I get 20ml 10% and (90-20)ml 1%.
Sunday, December 5, 2010 at 10:05pm by MathMate

Chemistry
5.00 mL of 2.00x10^-3M Fe(NO3)3 is mixed with 4.03 mL of 2.00x10^-3M NaSCN and 1.08 mL of 0.1M HNO3, for a total volume of 10.11 mL. a) What is the initial concentration of the Fe(NO3)3 in the mixed solution? b) What is the initial concentration of the NaSCN in the moxed ...
Wednesday, February 26, 2014 at 2:36pm by Dan

Chemistry
Is my answer in 3 sig fig or 4 sig fig?? A solution is prepared by dissolving 12.80 g of magnesium chlorite in enough water to make 200.0 mL of stock solution. A 25.0 mL aliquot (portion) of this stock solution is then removed and added to 250.0 mL of water. Calculate the ...
Sunday, October 20, 2013 at 8:21pm by Anonymous

chemisty
a 10.00ml diluted chloride sample required 44.89 ml of 0.01982 m abno3 to reach the fajans end point. how many moles of cl ion were present in the sample
Thursday, October 25, 2012 at 9:47pm by lisa

CHEM HELP?!
A particular household ammonia solution (D= 0.97g/ml) is 6.8% by mass. How many milliliters of this solution should be diluted with water to produce 650 mL of a solution with pH= 11.65?
Monday, February 16, 2009 at 7:54pm by i need help!

CHEM
A particular household ammonia solution (d= 0.97g/mL) is 6.8% NH3 by mass. How many milliliters of this solution should be diluted with water to produce 650 mL of a solution with pH = 11.55?
Monday, February 16, 2009 at 11:20pm by help!!!

chem
A particular household ammonia solution (d= 0.97g/mL) is 6.8% NH3 by mass. How many milliliters of this solution should be diluted with water to produce 650 mL of a solution with pH = 11.55?
Tuesday, February 17, 2009 at 12:10am by help!!!

chem
If you have a .045 M solution of sodium hydroxide, how many mL of the solution do you need to neutralize 6.5 mL of a .055 M sulfuric acid solution? do i use the equation M1V1 = M2V2?? or is that for dilutions
Sunday, September 6, 2009 at 5:01pm by sam

CHM 152
10 ppm = 10 g/10^6 g H2O. If water has density of 1.00 g/mL, then 10^6 grams H2O will be 1,000,000 mL. 10 ppm = 10 g/1,000,000 mL. So divide the 1,000,000 ml by 1,000,(to obtain 1,000 mL total or 1L) and to keep things equal we divie 10 g by 1000 = 10/1000 = 0.01 g Fe^+3
Tuesday, June 8, 2010 at 12:05am by DrBob222

Chemistry
A solution is prepared using 15.0 mL of 1.0 M HCl and 20.0 mL of 0.5 M HNO3. The final volume of the solution is 1.25 L. What are the [H3O+] and [OH-] in the final solution? What is the pH of the final solution?
Saturday, May 22, 2010 at 12:31pm by Heather

Chemistry
A solution is prepared by dissolving 50.0 g of pure HC2H3O2 and 20.0 g of NaC2H3O2 in 975 mL of solution (the final volume). what is the ph? What would the pH of the solution be if 50.0 mL of 0.900 M NaOH were added? What would the pH be if 30.0 mL of 0.30 M HCl were added to ...
Monday, November 12, 2012 at 8:39pm by Bella

Chemistry
A 1.00 g sample of enriched water, a mixture of H2O and D2O, reacted completely with Cl2 to give a mixture of HCl and DCl. The HCl and DCl were then dissolved in pure H2O to make a 1.00 L solution. A 25.00 mL sample of the 1.00 L solution was reacted with excess AgNO3 and 0....
Friday, September 21, 2012 at 11:34am by Adam

Chemistry revision
all these questions I got wrong on my homework today ...I'm trying to find out why and what the correct answers were .. please help How many grams of solute are required to make a 504 mL solution of copper (I) nitrate with a concentration of 1.3317 M? before I had help and was...
Monday, April 29, 2013 at 2:32pm by Tif

chemistry
Calculate the concentration of each solute and each ions when 25.0 mL of 18.0 M H2SO4 is mixed with 130.0 mL water
Monday, May 6, 2013 at 11:46pm by Anonymous

chem
If 50.0 mL of a 0.10M solution of sodium chloride is mixed with 50.0 mL of 0.10 M magnesium chloride, what is the molar concentration of chloride in the resulting solution?
Tuesday, October 6, 2009 at 8:54am by Amanda

Chemistry
Sorry about that The chemical 5-amino-2,3-dihydro-1,4-phthalazinedione, better known as luminol, is used by forensic scientists in analyzing crime scenes for the presence of washed-away blood. Luminol is so sensitive that it can detect blood that has been diluted 10,000 times...
Wednesday, February 11, 2009 at 8:03pm by HELP PLEASEEE

chemistry
A stock solution was prepared by dissolving exactly 0.4000 g of pure ASA (180.16 g/mol) in 10.00 mL of NaOH and heating the solution to a gentle boil. After cooling to room temperature, the solution was poured into a 250-mL volumetric flask and diluted to the mark with DI ...
Thursday, January 28, 2010 at 1:44am by Tasha

Chemistry
Solution x has a pH of 4.35. Solution y has 10- times high [OH-] compared to solution x. Solution z has a pH 4.0 units higher than that of solution x. calculate the ration of [H3O+] between solutions x&y and between x&z. What is the pH of solutions y and z? classify each ...
Tuesday, March 19, 2013 at 2:12pm by mary

Chemistry
A 50.0 mL sample containing Cd2 and Mn2 was treated with 49.1 mL of 0.0700 M EDTA. Titration of the excess unreacted EDTA required 17.5 mL of 0.0300 M Ca2 . The Cd2 was displaced from EDTA by the addition of an excess of CN–. Titration of the newly freed EDTA required 10.9 mL ...
Thursday, October 25, 2012 at 11:26pm by Chris

chemistry
50.0 mL of a 0.00200 M Cd^2+ solution is titrated with 0.00400 M EDTA in the presence of 0.0750 M NH3 buffered at pH = 9.00. Determine pCd^2+ when 28.5 mL of EDTA solution have been added. Cd^2+ + Y^4- ? CdY^2- Kf= 3.16 x 10^16 Cd^2+ + NH3 ? CdNH3^2+ ß1 = 3.24 x 10^2 Cd^2+ + 2...
Tuesday, August 13, 2013 at 5:22am by raghu

Chemistry
Question: A 0.400 g sample of propionic acid was dissolved in water to give 50.00 mL of solution. This solution was titrated with 0.150 M NaOH. what was the pH of the solution when the equivalence point was reached? I'm not really sure how i would go about setting this up. ...
Wednesday, April 15, 2009 at 10:07pm by Eliz

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
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! URGENT
A standard solution is prepared for the analysis of fluoxymesterone (C20H29FO3), an anabolic steroid. A stock solution is first prepared by dissolving 10.0 mg of fluoxymestrone in enough water to give a total volume of 500.0 ml. A 100.0 micro liter aliquot (portion)of this ...
Wednesday, December 7, 2011 at 1:39am by Lindsay

chemistry
A particular household ammonia solution (d = 0.97 g/mL) is 6.8% NH3 by mass. How many milliliters of this solution should be diluted with water to produce 650 mL of a solution with pH = 11.50?
Sunday, March 28, 2010 at 5:27am by anonymous

Chemistry
Sorry about that The chemical 5-amino-2,3-dihydro-1,4-phthalazinedione, better known as luminol, is used by forensic scientists in analyzing crime scenes for the presence of washed-away blood. Luminol is so sensitive that it can detect blood that has been diluted 10,000 times...
Wednesday, February 11, 2009 at 7:22pm by Chemistry

College Chemistry
A 30.00 mL volume of a weak acid, HA, (Ka = 3.8 x 10^-6) is titrated with 39.00 mL of 0.0958 M NaOH to the equivalence point. A.) What is the pH of the acid solution, before any base is added to it? B.) What is the pH of the acid solution after exactly 19.50 mL of NaOH is added?
Tuesday, April 13, 2010 at 1:11am by Shell

algebra
let the amount of the 20% solution used be x ml then the amount of the 50% solution used is 300-x m. solve for x .... .2x + .5(300-x) = .3(300) times 10 2x + 5(300-x) = 3(300) take it from there
Tuesday, February 21, 2012 at 3:54pm by Reiny

chemistry
Titration of 50.00 mL of 0.0521 M sodium oxalate, Na2C2O4, required 38.71 mL of a potassium permanganate solution: 5 C2O42- + 2MnO4- + 16H+ = 2Mn2+ + 10 CO2 + 8H2O Calculate the molarity of the potassium permanganate solution.
Saturday, June 23, 2012 at 1:03pm by mary

BioChem
If you want to determine the actual salicylate concentration for a sample that gives you a darker color than the highest standard, you would need to make a dilution of it. If you dilute it by mixing .25 mL of sample with .75 mL of water and then find that this mixture has a ...
Monday, October 31, 2011 at 10:38pm by Dreamland11

Chemistry
Q1: You wish to prepare a buffer solution with pH = 11.10. What volume of 6.0 M HCl would you add to 500 mL of 0.10 M (C2H5)2NH to prepare the buffer? You may assume that the solution’s volume remains constant. Q2: What is the resulting pH when 20 mL of 0.20 M NaOH is added to...
Sunday, February 24, 2013 at 1:49pm by David

Chemistry
Q1: You wish to prepare a buffer solution with pH = 11.10. What volume of 6.0 M HCl would you add to 500 mL of 0.10 M (C2H5)2NH to prepare the buffer? You may assume that the solution’s volume remains constant. Q2: What is the resulting pH when 20 mL of 0.20 M NaOH is added to...
Sunday, February 24, 2013 at 2:16pm by Anonymous

Pages: <<Prev | 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | Next>>

Search
Members