Friday
April 18, 2014

Search: if 10 mL of 0.004M AgNO3 is added to 10mL of 0.0024M K2CrO4, is eitheR Ag+ or CrO42- in stoichiometric excess? if so, which is in excess?

Number of results: 86,493

chemistry
1. if 10mL of 0.004M AgNO3 is added to 10mL of 0.0024M K2CrO4, is either Ag+ or CrO4(2-) in stoichiometric excess? if so, which is in excess? 2. the Ksp for BaCrO4 is 1.2x10-10. will BaCrO4 precipitate upon mixing 10 mL of 1x10-4M Ba(NO3)2 with 10mL of 1.0x10-4M K2CrO4?
Monday, October 19, 2009 at 11:22am by millie

chemistry lab titration
I don't understand how I would have to find the pH at 0mL or at 5 mL added or at 10 mL added. are the equivalence points at 10mL, 20mL, 30 mL? and the k3 that you are referring to did you get that from the pK3?
Wednesday, April 7, 2010 at 5:55pm by tara

chemistry
For which of the following mixtures will Ag2SO4(s) (Ksp=1.20E^-5)precipitate? More than one answer can be selected. a.) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq) b.) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.30 M AgNO3(aq) c.) 150.0 mL of 0.10 M Na2SO4(...
Tuesday, November 6, 2012 at 12:23am by chem question

Bio (please help me, important)
In my bio lab we are creating serial disk dilutions (100mg, 300mg, 500mg) from a plant extraction sample. Wood sample #1 (7mL of hexane) Hexane 0.6651g so .6651g of the plant was dissolved in 7mL of hexane. Then I did dilution calculations so 0.6551g/7 mL = 0.095g/ml so I ...
Wednesday, January 3, 2007 at 8:13pm by Ali

chemistry
mix 10ml NaBr 3.i000M wth 10ml water & 10ml AgNo3 3.3.1000M KspAgBr=5.25.1000 .what is the situation at equilibrium
Tuesday, November 22, 2011 at 6:24am by rene

Chemistry
1.Calculate the pH of a solution prepared by mixing 20mL of the .07222M aspirin solution with 10mL of .2M NaOH. 2. Calculate the pH for the titration of 40mL of .1M solution of C2H5NH2 with .1M HCl for a)0 mL added and b)20 mL added c)40 mL added d)50mL added. Kb= 6.4x10^-4
Saturday, November 26, 2011 at 8:14pm by Jessica

chemistry
A solution prepared by mixing 16.7 mL of 0.760 M NaCl and 16.7 mL of 0.760 M KI was titrated with 0.380 M AgNO3 in a cell containing a silver indicator electrode and a saturated calomel reference electrode. (a) What is [Ag+] when 16.2 mL of 0.380 M AgNO3 have been added? ...
Tuesday, March 11, 2014 at 9:30pm by Bobz

College Chemistry/Lab Math
Why did you multiply 0.0001g of gold/mL by 0.10mL? Shouldnt it be .50 mL? I say this because .10 is the volume of serum added, which does not contribute to the total amount of gold in the final solution.
Sunday, March 17, 2013 at 1:46pm by James

Chemistry
The activity of a stock isotope is 10,000 DPM/0.10mL. If 0.25 ml of this stock is placed in 2.50 ml of water, what is the activity in the diluted specimen? My guess is that I just multiply the 10,000 DPM by the 1/10 dilution factor. I then come up with 1,000DPM/0.10ml. Does ...
Wednesday, April 17, 2013 at 5:34pm by Maranda

chemistry
I have no idea. You didn't give a mass of AgNO3 used. I can give you a template to use, however, if we assume the mass AgNO3 used initially was 1 gram. Then the original concn was 1 g/10 mL = 0.1 g/mL. Then you took 3 mL of that and diluted to 1000 mL so the new concn is 0.1 g...
Monday, October 5, 2009 at 3:47pm by DrBob222

chemistry
A= 100 g AgNO3/50 mL B = 100 mL H2O C = 200 mL H2O D = 100 g KCl/100 mL. Now we take 25 mL (1/2 of it) A and add to B. Then we take 25 mL (1/2 of it) D and add to C. Then B+C are added. What do we have? 50 g AgNO3 is 1/2 of A. 50 g KCl is 1/2 of D. We had 25 mL H2O (1/2 of 50...
Thursday, April 24, 2008 at 11:38pm by DrBob222

science(chem)
I'm making different concentrations of ethanol and I just wanted to check my calculations and method. Making ethanol concentrations of: 0.40% 0.30% 0.20% 0.10% 0.05% To make the 0.40% ethanol from stock solution using 100ml volumetric flask: (xg ethanol)/(100ml) x 100= 0.40% ...
Wednesday, October 1, 2008 at 10:40pm by ~christina~

chemistry
A stock solution's hypochlorite activity was determined as follows: . - 2.00g of liquid sodium hypochlorite (NaOCl) was weighed into a flask and diluted with 50mL deionized water.10mL of 10% sulfuric acid and 10mL of 10% potasssium iodide were added, followed by titration with...
Wednesday, August 4, 2010 at 8:17pm by angela

Chemistry
The question doesn't make sense to me. The 50 mL of the AgNO3 solution has a mass of 50.0 g assuming the density of water and the AgNO3 soln is the same; however, that is the mass before an excess of Zn metal is added. I have no idea how much the total material weighs. It all ...
Wednesday, June 30, 2010 at 4:34pm by DrBob222

Chemistry (AP)
5 drops of AgNO3 must be added to 1 L of a water sample: 46.1 mg SO42-/L and 30.6 mg Cl -/L. What will be the precipitate that forms? the molarity of AgNO3 is 0.0010 M (mol/L) 1 drop = 0.05 mL
Thursday, April 22, 2010 at 2:28pm by Tommy

chem
If 60.0 mL of 0.150 M CaCl2 is added to 50.0 mL of 0.100 M AgNO3, what is the mass in grams of AgCl precipitate?
Monday, March 2, 2009 at 1:15pm by ash

chemistry
If 30.0 mL of 0.150 M CaC12 is added to 15.0 mL of 0.100 M AgNO3, what is the mass in grams of AgC1 precipitate?
Wednesday, September 29, 2010 at 2:22am by Michael

bio
You have a sample of NaCl that contains 100 mg/ml NaCl. You are trying to perform an reaction that requires 10ml of 20 mg/ml. Enter in the correct amount (in ml) of Stock NaCl solution you need to use to make 10ml of 20 mg/ml NaCl
Tuesday, March 1, 2011 at 11:28pm by mina

Chemistry
When 50 mL of 1.0 M AgNO3 is added to 50 mL of 0.50 M HCl, a precipitate of AgCl forms. After the reaction is complete, what is the concentration of silver ions in the resulting solution? (a) 0.50 M (b) 1.0 M (c) zero (d) 0.25 M (e) 0.75 M How do I go about solving this? I ...
Monday, February 1, 2010 at 8:30pm by Anonymous

chemistry
Ag^+ + Cl^- ==> AgCl mols NaCl = 0.05g/molar mass = ? mols AgNO3 = mols NaCl M AgNO3 = mols AgNO3/L AgNO3 You know M and mols, solve for L AgNO3 and convert to mL.
Tuesday, March 25, 2014 at 2:37pm by DrBob222

CHEMISTRY
1. You have 88.8 mL of 2.50 M solution of Na2CrO4 (aq). You have 125 mL of a 2.50 M solution of AgNO3 (aq). Calculate the concetration of Na+ when the two solutions are added together. 2. You have 75.0 mL of 2.50 M solution of Na2CrO4 (aq). You have 125 mL of a 1.84 M solution...
Monday, August 30, 2010 at 8:23pm by Alex

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
Net ionic equations for: Br- + AgNO3 CO3 + AgNO3 Cl-+ AgNO3 I + AgNO3 PO4^-3 + AgNO3 SO4^-2 + AgNO3 S^-2 + AgNO3 They all formed ppt,but I don't know where to go from here. Even a couple to get me started would be greatly appreciated!
Sunday, July 14, 2013 at 12:41pm by Ann

Chemistry
1. I don't know the details of your experiment but I suspect AgNO3 is, indeed, a primary standard. How you explain that is up to you. 2. Too basic and you have problems with Ag(OH)2. 3. moles KCl = grams/molar mass moles KI = grams/molar mass Total Cl and I = sum of the two. ...
Friday, December 2, 2011 at 2:59am by DrBob222

Chemistry
(NO3^-) = 0.1/2 = 0.05M. If you don't see that, then assume a volume (any value) of AgNO3 and NaCl and mix them together. For example, 100 mL of each, then millimoles AgNO3 = 100 x 0.1 = 10 Then M NO3^- = 10mmoles/200 mL = 0.05M.
Wednesday, May 25, 2011 at 6:55am by DrBob222

chemistry
how many mL of watel should be added to yeild a soultion that has a concentration of .125 M when you start with a 250 mL soultion of 1 M AgNO3?
Wednesday, January 26, 2011 at 12:01pm by nancy

math
1a. 100ml / 10min = 10ml/min. W = 10ml/min * 60min/hr * 24hr/da = 14400ml/da. 1b. W = 14400ml/da * 7da/wk = 100800ml/wk. 1c. W = 14400ml/da * 365da/yr = 5256000 ml/yr. 2. 1000000 ml * 1/10 min/ml * 1/60 hr/min * 1/24 da/hr = 69.4 days.
Thursday, August 19, 2010 at 5:01pm by Henry

chemistry
What volume of WATER MUST BE ADDED to 10.0 mL of 6.0 M NaOH to make a solution that is 0.30 M in NaOH? Assume that the volumes are additive. a. 10 mL b. 190 mL c. 200 mL d. 210 mL e. 500 mL
Monday, March 29, 2010 at 6:30am by lawrence

Chem
mass of empty cylinder is 87.470g 97.470g w/10mL of water 107.470g + 10mL of water 117.470g + 10 more mL of water need to know the total volume of water (in mL or cm3) total mass of water density of water calculate the average of the 3 densities of water.
Saturday, June 19, 2010 at 8:29pm by dra

Analytical Chemistry
A solution prepared by mixing 51.4 mL of 0.340 M AgNO3 and 51.4 mL of 0.340 M TlNO3 was titrated with 0.680 M NaBr in a cell containing a silver indicator electrode and a reference electrode of constant potential 0.175 V. The reference electrode is attached to the positive ...
Thursday, April 11, 2013 at 3:32pm by Micki

chemistry
What is the concentration of this solution? If you added 10mL of water to the 10mL of 0.010M CaCl2 solution.
Monday, September 13, 2010 at 12:55am by fredy

Chemistry
10 mL of 0.1 HCl was added to 9mL of water. 10 mL of that solution was added to another 90 mL of water. The student diluted the sample as above 1 time(s). What is the pH of the solution?
Monday, April 7, 2014 at 5:13pm by Keyatta

Science(Chemistry)
Suppose that 23 mL of 0.6 M K2CrO4(aq) reacts with 13.7 mL of AgNO3(aq) completely. What mass of NaCl is needed to react completely with 38.5 mL of the same AgNO3 solution? Answer in units of g
Thursday, April 18, 2013 at 2:33pm by Joseph

chemistry
A solution prepared by mixing 47.1 mL of 0.4 M AgNO3 and 47.1 mL of 0.4 M TlNO3 was titrated with 0.8 M NaBr in a cell containing a silver indicator electrode and a reference electrode of constant potential 0.175 V. The reference electrode is attached to the positive terminal ...
Saturday, November 9, 2013 at 5:45am by martini

Quaid university usmanlatif3@gmailcom
50 ml of sample solution+10ml of 6M acetic acid+10ml of 3M of Ammonium acetate+heat to boiling+slight excess of 10% ammonium chromate solution+cool+filter+wash the ppt+weight+calculate the ba % in bacro4
Monday, January 16, 2012 at 5:53pm by usman

chemistry
We are doing a lab that requires finding the molarity of an unknown AgNO3 solution after reacting NaCl + AgNO3 --> NaNO3 and AgCl and collecting/massing the precipitate. We will be using 10.00 mL of an NaCl solution and 10.00 mL of the AgNO3 solution. We know that the AgNO3...
Wednesday, October 4, 2006 at 7:03pm by Chris

Chemistry
A 30.0-ml sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. What is the pH at 5 ml of added base, at 10 ml of added base?
Tuesday, March 19, 2013 at 8:22pm by Annie

Chemistry
2AgNO3 + Na2CrO4 ==> Ag2CrO4 + 2NaNO3 I see it differently. Initial: 20 mL x 0.1 M = 2 millimoles AgNO3 80 mL x 0.01 M = 0.8 mmoles Na2CrO4. Ag2CrO4 = O NaNO3 = 0 final: Ag2CrO4(s) = ppt = 0.8 mmoles. Na2CrO4 = 0 (all of it used--the only chromate from the solution will ...
Thursday, May 6, 2010 at 1:40am by DrBob222

College Chemistry/Lab Math
This is good, but mass/volume %= (g/mL)*100 So, (0.10 % w/v)/100 = 0.001 g gold (in 1 ml) And so, (0.001g gold)/(1 ml + 9 ml) = 0.0001g of gold/mL ****Don't worry about mass/volume % at this point. But now you have a solution that is 0.0001g of gold/mL You remove 0.5mL of ...
Sunday, March 17, 2013 at 1:46pm by Devron

Chemistry
Hi Can someone please help me undersand how to get the answer to this question A 15.0 mL solution of 0.050 mol/L AgNO3 was titrated with 0.0250 mol/L NaBr in the cell SCE || titrated solution | Ag(s) Find the cell voltage for 10.0 mL of titrant added. (a) -0.0312 V (b) 0.194 V...
Monday, April 26, 2010 at 6:53am by James

college chemistry
How do you calculate the pH when the following substances are added to a buffer.(all of the solutions are at .10M conc.) The buffer: 50mL NH3 + 50mL NH4NO3 1) 10mL buffer + 6mL water 2)10mL buffer + 5mL water +1mL HCl 3)10mL buffer + 6mL HCl 4)10mL buffer + 5mL water + 1mL ...
Monday, April 13, 2009 at 11:19pm by Mary

college chemistry
How do you calculate the pH difference when the following substances are added to a buffer.(all of the solutions are at .10M conc.) The buffer: 50mL NH3 + 50mL NH4NO3 1) 10mL buffer + 6mL water 2)10mL buffer + 5mL water +1mL HCl 3)10mL buffer + 6mL HCl 4)10mL buffer + 5mL ...
Monday, April 13, 2009 at 7:30pm by Mary

Chemistry
A 25.00 mL sample of a clear saturated solution of PbI2 requires 14.3 mL of a certain AgNO3(aq) for its titration. I^-(from satd PbI2)+ Ag^+(from AgNO3)= AgI(s) So, this is where I am. using the Ksp equation for PbI2: 7.1*10^-9=4x^3 solving for x gives me 0.00121 Giving the ...
Sunday, March 18, 2012 at 5:18pm by Ash

chemistry
you are diluting it 20 times? Add 1 part original, 19 parts water. Now if you want to do it the hard way: molesacid=10ml*6M=V*.3 Volumetotal=200ml so water added =200-10ml
Monday, March 29, 2010 at 6:30am by bobpursley

chemistry
In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 10 mL 4.0 M acetone + 10mL 1.0 M HCL + 10 mL 0.0050 M I2 + 20 mL H2O A student found that it took 250 seconds for the color of the I2 to disappear. What was the ...
Monday, July 26, 2010 at 7:15pm by Paul

Chemistry
Nitrate never enters into the reaction. Na2CrO4 + 2AgNO3 ==> Ag2CrO4 + 2NaNO3 (AgNO3) = 1.74M x 125 mL = 217.5 mmoles. (NO3^-) at the end is 217.5 mmoles/total mL volume. That is 125 mL AgNO3 + 75 mL from the Na2CrO4. So nitrate = mols/L = or 217.5 mmoles/200 mL ??.
Sunday, February 27, 2011 at 6:52pm by DrBob222

chemistry
suppose i want to find out how many mL of 1.0M AgNO3 are needed to provide 169.9g of pure AgNO3. what is step one in solving this problem? How many mL of solution are needed?
Wednesday, November 18, 2009 at 12:04pm by lynda smith

Chemistry
When 20.0 mL of 0.100 M AgNO3 are mixed with 80.0 mL of 0.0100 M Na2CrO4, what is the chromate ion concentration (CrO4^2-)? Ksp for Ag2CrO4 = 9.0 x 10^-12. I think it's 1.0 x 10^-9. Am I right?
Thursday, May 6, 2010 at 1:40am by Cory

Physical chemistry 2
50 ml of 0.02M acetic acid is titrated with 0.1M NaOH.Calculate the pH of the solution when 10ml of NaOH is added
Tuesday, March 12, 2013 at 12:41am by Anonymous

chemistry
How do you calculate the pH when the following substances are added to a buffer.(all of the solutions are at .10M conc.) The buffer: 50mL NH3 + 50mL NH4NO3 1) 10mL buffer + 6mL water 2)10mL buffer + 5mL water +1mL HCl 3)10mL buffer + 6mL HCl 4)10mL buffer + 5mL water + 1mL ...
Tuesday, April 14, 2009 at 6:15pm by Mary

Cemistry
A solution is 36% silver nitrate (AgNO3) by mass. The density of this solution is 1.44 g/mL. The formula weight of AgNO3 is 170 g/mol. Calculate the molality of AgNO3 in this solution.
Wednesday, June 9, 2010 at 10:07pm by Swagato

Chemistry
I need help with this problem: 50.0 mL of 4.4 g/L AgNO3 is added to a coffee-cup calorimeter containing 50.0 mL of 4.4 g/L NaI, with both solutions at 25°C. a).What is ΔTsoln (assume the volumes are additive and the solution has the density and specific heat capacity of ...
Monday, October 13, 2008 at 3:44pm by CJ

Chemistry
Find the Qsp when 9 drops of 0.014 M Na2CO3(aq) are added to 25 mL of 0.003 M AgNO3(aq). The solubility product of Ag2CO3 is 6.2 10−12. Assume 20 drops per milliliter.
Saturday, March 30, 2013 at 2:47pm by Alice

Chemistry
an acid base titration is conducted in which 20 ml of LiOH is added to 10ml of .200M HBr to reach the equivilance point. what is the molarity of the LiOH solution?
Monday, April 12, 2010 at 12:55am by Elf

Chemistry
a. Calculate mols AgNO3 needed. mols AgNO3 = grams/molar mass b. 169.87 c. mols AgNO3 = M x L. You know M and mols solve for L and convert to mL.
Monday, April 22, 2013 at 11:26am by DrBob222

math
you want 1200/(1500/10ml)= 4/5 * 10 ml=8ml
Tuesday, December 13, 2011 at 10:35pm by bobpursley

Chemistry lab
I mixed 10 mL of 9mM KI with 5 mL of 0.9mM in a flask, and then added it to a beaker that contained 10 mL of 45 mM KBrO3, and 10 mL of 90mM HCl. This reaction took 61.60 seconds to complete. I think I need to find the change in concentration, but don't know how to do this. I'...
Tuesday, April 8, 2014 at 12:43pm by Calley

Chemistry
Suppose you are studying coordination compounds of Co(II) with the ligand pyridine (py, C5H5N, MW = 79.10). You isolate a crystalline compound and since the only available ions are chloride and nitrate, you hypothesize the empirical formula of the coordinaton compound must be ...
Friday, April 20, 2007 at 8:14pm by Ray

Environmental Chemistry
Calculate the pH when the following volumes of 0.20 M LiOH are added into 50 mL of a 0.1 M HCl solution. Both LiOH and HCl are strong electrolytes. a) 0 mL b) 10 mL c) 24.6 mL d) 25 mL e) 25.6 mL f) 30 mL g) 40 mL
Tuesday, May 8, 2012 at 11:50am by Dauren

Chemistry
You have 20mL of a solution of concentration 0.015mg/mL of x in test tube #1. Prepare serial dilutions of your stock solution, and calculated the concentration of x as follows: Add 10mL of distilled water and 10mL of stock solution from test tube 1 to test tube 2. Add 10mL of ...
Wednesday, November 3, 2010 at 3:36pm by Jon

Chemistry
A 50.0 mL sample of 0.12 M formic acid, HCOOH, a weak monoprotic acid, is titrated with 0.12 M NaOH. Calculate the pH at the following points in the titration. Ka of HCOOH = 1.8 multiplied by 10-4. What is the pH when 50.0 mL NaOH is added 60.0 mL NaOH is added 70.0 mL NaOH is...
Sunday, April 3, 2011 at 5:13pm by George

Chemistry
What is the Qsp when 59.0 mL of 2.00 multiplied by 10-4 M AgNO3 are mixed with 70.0 mL of 1.00multiplied by10-4 M Na2CrO4? Assume the volumes are additive. Ksp = 1.1 multiplied by 10-12.
Monday, December 6, 2010 at 1:20am by Anonymous

Chemistry
If you mix 20.0 mL of 1.00 x 10-4 mol/L NaCl with 20.0 mL of 2.00 x 10-6 mol/L AgNO3 will a precipitate form ? If it does it will be AgCl, which has a Ksp of 1.80 x 10-10. i'm not quite sure how to figure this out...
Tuesday, February 21, 2012 at 10:32pm by Aria

Analytical Chemistry
Unfortunately, my KIO3 was given to me in mL from my professor so i have no clue what the grams of KIO3. I tried to figure out the moles of Na2S2O3 solution but looking over it i believe that 0.28 M is incorrect. The info I have is: 2.6g of Na2S2O3 was added to roughly 1 mL of...
Monday, October 11, 2010 at 10:12pm by Max

chemistry Molarity
mL x M = mL x M Substitute and solve for mL. 353 x 1.25 = mL x 0.5 Solve for mL and this will be the FINAL VOLUME. To find how much water must be added requires a. That we assume the volumes are additive. b. Then final volume in mL - 353 mL = mL to be added.
Saturday, December 11, 2010 at 2:17pm by DrBob222

Chemistry
Is 10.0 mL of 0.10 M NH4Cl added to 10.0 mL of 0.10 M HCl a basic buffer? I think Yes. Right?
Thursday, May 6, 2010 at 11:11pm by Jim

Chemistry
Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 10-6) by 0.200 M HNO3. Calculate the pH of the resulting solution after the following volumes of HNO3 have been added. a)0.0 mL b)20.0 mL c)25.0 mL d)40.0 mL e)50.0 mL f)100.0 mL
Saturday, March 23, 2013 at 4:37pm by Jeff

Chemistry
Even if you can help answer one that would be a great help! 1. How many liters of NO(g) are produced when 0.85L of 2.00M HNO3 solution is added to 216g according to the equation. Which reactant is the limiting reactant? 3 Ag + 4 HNO3 -> 3 AgNO3 + NO + 2 H2O3 2. Calculate ...
Sunday, October 20, 2013 at 5:06pm by P.

chemistry
Silver nitrate (AgNO3) reacts with sodium chloride as indicated by the equation AgNO3 + NaCl ! AgCl + NaNO3 . How many grams of NaCl would be re- quired to react with 511 mL of 0.38 M AgNO3 solution? Answer in units of grams
Wednesday, September 19, 2012 at 4:40pm by cheri

Chemistry
Calculate the number of moles of ag in 5ml of .004m agno3 and the number of moles of cr04 in 5ml of .0024m k2cro4
Wednesday, March 19, 2014 at 10:33am by Candice

Chemistry
Consider the titration of 41.5 mL of 0.213 M HCl with 0.123 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. (Assume that all solutions are at 25C.) (a) 0.0 mL (b) 10.0 mL (c) 40.0 mL (d) 80.0 mL (e) 100.0 mL
Wednesday, March 13, 2013 at 2:55am by Margaret

Chemistry
Calculate the amount (in grams) of AgNO3 needed to prepare 250.0 mL of 0.25 M of AgNO3.
Sunday, March 9, 2008 at 9:29pm by Allie

Chemistry
How many grams of AgNO3 (silver nitrate) are contained in 425 mL of a .15 M solution of AgNO3?
Tuesday, January 29, 2013 at 2:37pm by Jessica

Chemistry
Silver nitrate (AgNO3) reacts with sodium chloride as indicated by the equation AgNO3 + NaCl ! AgCl + NaNO3 . Howmany grams of NaCl would be required to react with 518 mL of 0.543 M AgNO3 solution? Answer in units of grams
Tuesday, October 4, 2011 at 8:45pm by Broy

Chemistry
You can't understand if you don't try. You could help by explaining exactly what you don't understand instead of leaving me hanging out there with no idea of which direction to go to help. mols = M x L. You have M = 0.15M in the problem. You have 425 mL (0.425L) volume in the ...
Tuesday, January 29, 2013 at 2:37pm by DrBob222

health
Pharmacist dilutes a vial containing 1gm of antibiotic with 10ml of water. The solution is then added to 100ml of d5w. What is the concentration, in mg/ml, of the antibiotic in the d5w?
Tuesday, August 16, 2011 at 5:07pm by Arlene

Chemistry
Can someone please help me answer these questions? Is additional information other than what is given needed to solve? Thanks in advance. 1) Calculate the PH of a buffer containing 0.100 M propanoic acid, HC3H5O2 and .100 M NaC3H502 after the following have been added. Ka for ...
Friday, December 13, 2013 at 1:39am by Charles

chemistry
HNO2 + NaOH ==> NaNO2 + H2O moles HNO2 = M x L = 0.025 x 0.108 = 0.00270 moles HNO2 initially. moles NaOH added = 10mL x 0.162 = 0.00162 moles HNO2 remaining after reacction = 0.00270-0.00162 =0.00108. M HNO2 = moles/L (L = 25 mL + 10 mL) So this problem becomes determine ...
Sunday, October 2, 2011 at 9:42pm by DrBob222

Chemistry
I would convert 575 mg Na to mmols Na. mmoles Na = mmols NaCl = 575 mg Na/23 = ?? Titrate with AgNO3 = 0.1M x 25.00 mL = 2.50 mmols AgNO3 which will equal 2.50 mmoles NaCl. (You should write the NaCl + AgNO3 equation to confirm that.) You have a soy sauce that is 25.00 mmols/...
Friday, January 21, 2011 at 11:30am by DrBob222

chemistry
10g of nacl were added to 10ml of water. the resulting solution was diluted to be a final volume of 250ml. Given the density of the solution is 0.9864g/ml. Calculate the molality of the solution. Who helps
Tuesday, December 25, 2012 at 3:14pm by Fai

chemistry
what mass of AgNO3(MW 169.87) is required to make 25 mL of 0.100 M AgNO3?
Monday, August 30, 2010 at 8:50am by jayson

chemistry
calculate the Ph in the titration of 50.00 ml of 0.100 M ammonia with 0.100 M HCl after 0,24.00,50.00, and 74.00 ml acid have been added Ka((NH3)= 1.8x10^(-5) PH= ............ when 0 ml added. PH= ............ when 24.00 ml added PH= ............ when 50.00 ml added PH...
Friday, December 2, 2011 at 6:50pm by saud

chemistry
When 25 mL of 0.24 mol/L CaCl2 is mixed with 45 mL of 1.5 mol/L AgNO3, a precipitate of AgCl forms because the Ksp of AgCl is 1.8 x 10^-10 Is this true or false?
Thursday, April 3, 2008 at 10:48pm by MikeSo

science
A solution is prepared by mixing 100.0 mL of 0.0500 M AgNO3 with 75.0 mL of 0.0500 M CaCl2. What is the equilibrium concentration of Ag+ in solution? Ksp for AgCl is 1.6 x 10^-10
Friday, July 26, 2013 at 4:29pm by luna

chemistry
24.8 mL sample of a 4.63 x 102 M solution of NaCl is mixed with a 30.0 mL sample of a 3.67 x 102 M solution of AgNO3. What is the mass, in grams, of AgCl precipitate that forms?
Monday, September 30, 2013 at 8:19pm by pratibha

Chemistry
2a. Adding 1 mL of 10M NaOH to HOW MUCH of the buffer. Since the problem gives molarities, I will assume 1L. millimols HPO4^2- = 1000 mL x 0.058 = 58 mmols H2PO4 = 1000 mL x 0.042 = 42 mmols NaOH added = 1 mL x 10M = 10 .......H2PO4^- + OH^- ==> HPO4^2- + H2O I......42...
Sunday, January 27, 2013 at 11:00pm by DrBob222

Chemistry
I have interpreted this problem differently than Bob Pursley. I think the problem states that 85 mL HCl and 89 mL NaOH WERE LEFT when the accident was discovered; therefore, we have added 100-85 = 15 mL HCl and 100-89 = 11 mL NaOH. Therefore, mmoles HCl added = 15 mL x 0.06 M...
Thursday, July 9, 2009 at 3:16am by DrBob222

Analytical Chemistry
What is the cell voltage when the following volumes of 0.680 M NaBr have been added? (b) 1.0 mL (c) 13.2 mL (d) 24.7 mL (e) 25.6 mL (f) 26.0 mL (g) 38.9 mL (h) 51.4 mL (i) 52.0 mL
Thursday, April 11, 2013 at 5:51am by Micki

Chemistry
What is the (H30) concentration when 40 mL of 0.10 M nitrous acis, HNO2, are added to 10.0 mL of 0.10 M HCl? Ka for HNO2 is 4.0 x 10^-4. I get 1 x 10^-3. Is this right?
Wednesday, May 5, 2010 at 9:53pm by Mary

Chemistry
density is mass/volume. Since they give you the mass of 55.81g already, you need to find the volume which is 24.7mL-17.6mL=7.10mL. 55.81g/7.10mL= 7.86 g/mL. mL=cm^3 so it becomes 7.86 g/cm3 or 7.86 gxcm^-3. The metal that matches this density is Iron.
Thursday, March 8, 2012 at 2:34pm by Thien

Chemistry
12 mL x 0.4M AgNO3 = 4.8 millimols. 8 mL x 0.8M NaCl = 6.4 mmols. AgNO3 + NaCl => AgCl + NaNO3 This is a limiting reagent problem since amounts are given for BOTH reactants. You can tell, since the reactants and products are 1:1:1:1 that AgNO3 is the limiting reagent so you...
Monday, April 23, 2012 at 1:53pm by DrBob222

chemistry
how many grams of Ag2CO3 will precipitate when excess Na2CO3 solution is added to 64.0 mL of 0.554 M AgNO3 solution?
Saturday, March 23, 2013 at 7:12pm by mya

chemistry
A 40.0 mL sample of 0.150 M Ba(OH)2 is titrated with 0.400 M HNO3. Calculate the pH after the addtion of the following volumes of acid, and plot the pH versus millimeters of HNO3 added. a. 0.00 mL b. 10.2 mL c. 19.9 mL d. 30.0 mL e. 39.8 mL
Monday, June 27, 2011 at 9:02pm by Cindy

Chemistry
Yes, there is a volume for HCl; in fact, that's what the problem is all about. That is, what is the pH after the addition of each of those quantities of 0.1M HCl. You have 10.00 mL of 0.3M NH3 initially which is 3. mmole. After 0 mL, that is 0 mmole HCl added. After 10 mL x 0....
Monday, May 2, 2011 at 5:27pm by DrBob222

Chemistry
You want to make an ICE chart and use the Henderson-Hasselbalch equation. Let's simply our typing by calling CH3COOH just HAc and CH3COONa will be NaAc. mmoles HAc = 0.400 M x 100 mL = 40.0 mmoles Ac^- = 0.200M x 100 mL = 20.0 mmoles HCl added = 1.00 mL x 10.0 M = 10.0...
Sunday, June 26, 2011 at 11:34pm by DrBob222

organic chemistry
Partition (distribution) coefficient, k, of benzyl alcohol in hexane and water is 12.0. Choose for the correct equation for the amount of benzyl alcohol as x that you should use to calculate the amount of benzyl alcohol extracted with one 10mL portion of hexane from 500mg of ...
Tuesday, November 25, 2008 at 9:44pm by Jenn

Chemistry
Heres a balanced equation: Na2CO3(aq)+2AgNO3 (aq) --> 2NaNO3(aq)+Ag2CO3 (s) From this equation, 10 mL of AgNO3 in this contains 34 grams of AgNO3. Calculate the grams of solid product, Ag2CO3. Part 2: 10 mL of Na2CO3 in this experiment contains 21 grams of Na2CO3. ...
Wednesday, February 6, 2013 at 8:58pm by Sarah

Analytical Chemistry
Then i did 3 more trials consisting of 10 ml of Cu(IO3)2, 25 ml of H20, 10ml of Acetic acid, and 1.3g of KI I now need to find (M) of IO3 so i can find the Ksp of the reaction
Monday, October 11, 2010 at 10:12pm by Max

Chemistry
Silver nitrate is AgNO3. You made a typo. 47.8 mg = 0.0478 g = ? mols. mols = 0.0478/molar mass AgNO3 = approximately 0.00028 in 10 mL = 0.00028/0.01 = about 0.028M Then 0.028 x (3.00/1000) = ? M.
Tuesday, June 26, 2012 at 6:02pm by DrBob222

college chemistry
Consider the titration of a 50.0 mL sample of a 0.100 M solution of the triprotic weak acid citric acid (H3C6H5O7) with 0.100 M KOH. For citric acid, the three (3) acid dissociation constant values are ka1 = 7.40x10-3, ka2 = 1.70x10-5, and ka3 = 4.00x10-7, respectively. Given ...
Wednesday, April 21, 2010 at 5:59pm by Aubree

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