Wednesday
April 23, 2014

Search: AgNO3+ CaCl2

Number of results: 830

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
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

College Chemistry
How many moles do you want? That's M x L = ? Then mols AgNO3 = grams AgNO3/molar mass AgNO3.
Thursday, September 27, 2012 at 6:29pm by DrBob222

AP Chemistry
Na2CrO4 + 2AgNO3 ==> Ag2CrO4 mols Ag2CrO4 = grams/molar mass = ? mols AgNO3 = 1/2 that from the coefficients in the balanced equation. M AgNO3 = mols AgNO3/L AgNO3.
Wednesday, September 11, 2013 at 6:15pm by DrBob222

Chemistry
27.8g KCl/molar mass KCl = approx 0.37 0.37/0.7 = approx 0.53M AgNO3 + KCl ==> AgCl + KNO3 mols KCl used = M x L = 0.0221 x 0.53 = ? mols AgNO3 = the same (since the ratio in the balanced equation is 1:1). Then M AgNO3 = mols AgNO3/L AgNO3.
Sunday, March 2, 2014 at 10:21pm by DrBob222

Chemistry
1M AgNO3 means 1 mol AgNO3 in 1L solution; therefore, mols AgNO3 = M x L. Then g = mols x molar mass.
Tuesday, March 26, 2013 at 3:19pm by DrBob222

chemistry
22.0% AgNO3 by mass means 22.0 grams AgNO3 per 100 g solution. That is equivalent to 220 g/1000g solution. The 1000 g solution is made of 220 g AgNO3 + 780 g water. How many moles AgNO3 in 220 g AgNO3. That will be 220/molar mass AgNO3 (approximately 1.3 moles. molality = ...
Sunday, June 12, 2011 at 4:58pm by DrBob222

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

chemistry
Technically the problem is flawed and the answer can't be calculated; however, I assume you mean that the KCl reacts COMPLETELY and stoichiometrically with the AgNO3. AgNO3 + KCl ==> AgCl + KNO3 moles AgNO3 = M x L = ?? Using the coefficients in the balanced equation, ...
Monday, April 4, 2011 at 9:12am by DrBob222

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 - Science
Ag^+ + Cl^- ==> AgCl mols AgCl = grams/molar mass =? ? mol AgCl = mols Cl^- = mols Ag^+ = mols AgNO3. g AgNO3 = mols AgNO3 x molar mass AgNO3 %AgNO3 = (g AgNO3/mass sample)*100 = ?
Tuesday, March 25, 2014 at 6:28pm by DrBob222

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

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
Write the equation and balance it. mols AgNO3 = M x L mols K2SO4 = M x L Determine the limiting reagent. I think K2SO4 is limiting but check me out on that. If so then AgNO3 is a common ion to the ppt of Ag2SO4. Ag^+ in the final solution, then, is Ag^+ from unused AgNO3 (...
Sunday, September 26, 2010 at 11:14pm by DrBob222

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

Chemistry
Suppose you wanted to find out how many milliliters of 1.0 M AgNO3 are needed to provide 169.88 g of pure AgNO3. a. What is step 1 in solving the problem? b. What is the molar mass of AgNO3? c. How many milliliters of solution are needed?
Monday, April 22, 2013 at 11:26am by Somer

Chemistry
No. 2AgNO3 + BaCl2 ==> 2AgCl + Ba(NO3)2 2 x 1 = 2 moles AgNO3 2 x 1 = 2 moles BaCl2 AgNO3 is limiting; that is 2 moles AgNO3 will use 1 mole BaCl2. At equilibrium, All of the AgNO3 has been used. BaCl2 = 2 moles initially - 1 mole reacted = 1 mole remaining. 1 mole/2L = 0.5 M.
Thursday, April 29, 2010 at 7:51pm by DrBob222

chemistry
A 30.00mL sample of a clear saturated solution of PbI2 requires 14.7mL of a certain AgNO3 for its titration. I^-(saturated PbI2)+Ag^+(from AgNO3)--> AgI(s) What is the molarity of this AgNO3? I'm not really sure where to start.
Friday, March 16, 2012 at 9:00pm by brad

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
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

chem
you have 157.5 mmol of AgNO3 and 243 mmol of MgCl2. From the balanced chemical equation, 1 mol of MgCl2 would consume 2 moles of AgNO3. It would then require 315 mmol of AgNO3 to completely consume the MgCl2. Therefore, AgNO3 is the limiting reactant and it would dictate how ...
Sunday, June 7, 2009 at 9:48pm by smiley

chemistry
You can do this one of several ways, first, as a reaction to precipate the silver. The second, is just to figure out how much silver is in 5g AgNO3. This is much easier. The percent of Ag in AgNO3 is Percent silver: atomicmassSilver/formula mass AgNO3
Sunday, September 21, 2008 at 10:03pm by bobpursley

chemistry
NaCl + AgNO3 ==> AgCl + NaNO3. You have 1.91 g AgCl. How many moles is that? 1.91/143.32 = ?? How many moles AgNO3 is that? Since 1 mole AgCl is produced for every mole AgNO3 initially, moles AgCl must equal moles AgNO3. Then what is the molarity. M = moles/L. You have ...
Monday, September 20, 2010 at 5:40pm by DrBob222

Chemistry
If 10. g AgNO3 is available, what volume of 0.25M AgNO3 solution can be prepared?
Thursday, October 28, 2010 at 11:00pm by annonymous

Chemistry
If you reclaim 0.250g Ag from AgNO3, how much AgNO3 did you have to begin with?
Monday, July 16, 2012 at 11:56am by Kristin

chemistry
how many g of agno3 would you need to make a 575ml solution of 0.25 m agno3
Wednesday, August 8, 2012 at 3:01pm by sherry

chemistry
M = moles/L 0.1 = moles/0.250 L solve for moles. moles = grams/molar mass You know moles and molar mass, solve for grams (100% pure) AgNO3. grams impure AgNO3 x 0.988 = grams pure AgNO3 you want or rearrange to grams pure AgNO3/0.988 = grams you must weigh out to get grams ...
Thursday, March 25, 2010 at 4:34am by DrBob222

Chemisty
2AgNO3 + K2CrO4 -> 2KNO3 + Ag2CRO4 25mL of .1M K2CrO4 has .0025 moles Each mole of K2CrO4 reacts with 2 moles of AgNO3 So, you need .0050 moles of AgNO3 .0050moles/.050L = 0.1M AgNO3
Friday, August 10, 2012 at 1:56pm by Steve

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
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

AP Chemistry
What mass of silver nitrate (AgNO3) is required to prepare 400 g of a 3.50% solution of AgNO3
Monday, October 3, 2011 at 9:19pm by Yolanda

College Chemistry
how would you prepare 175.0ml of .150 m agno3 solution starting with pure agno3
Thursday, September 27, 2012 at 6:29pm by Anne

chem
2AgNO3 + BaCl2 ==> 2AgCl + Ba(NO3)2 How many moles AgCl were formed? That is g/molar mass = moles = 3.50/143.32 = 0.0244 moles. Since 1 mole AgCl = 1 mole AgNO3, we must have had 0.0244 moles AgNO3 in the original sample and we convert to grams by g = moles x molar mass. ...
Tuesday, December 14, 2010 at 4:39pm by DrBob222

Chemistry
NaCl + AgNO3 = AgCl + NaNO3 moles NaCl = grams/molar mass mols AgNO3 = moles NaCl M AgNO3 = mols/L Solve for L.
Monday, September 27, 2010 at 10:38am by DrBob222

chemistry
KCl + AgNO3 ==> AgCl + KNO3 mols AgNO3 = M x L = ? moles KCl = moles AgNO3 from the 1:1 ratio in the equation. g KCl = moles KCl x molar mass KCl.
Wednesday, February 29, 2012 at 7:07pm by DrBob222

Chemistry
In my math I took 8g of AgNo3/1.69.8731 g/mol=.0471 mol of AgNo3 Then since there is only one AgNO3 and one AgCL, then AgCl's has a mol of .0471, multiply that by its molecular weight of 143.321 and I recieve 6.75 grams. not 3.4, where did I did I do something wrong?
Sunday, June 7, 2009 at 1:36pm by Gweedo8

chem
You're asked to prepare 125mL of .0321 M AgNO3. How many grams would you need of a smaple known to be 99.81% AgNO3 by mass?
Saturday, February 7, 2009 at 8:20pm by Anonymous

chemistry
AgNO3 + Na2CrO4 ==> Ag2CrO4 + 2NaNO3 mols AgNO3 = M x L = ? Using the coefficients in the balanced equation, convert mols AgNO3 to mols Na2CrO4. Now convert mols Na2CrO4 to gram. g = mols x molar mass
Friday, October 18, 2013 at 5:15pm by DrBob222

chemistry
What mass of silver nitrate (AgNO3) is re- quired to prepare 400 g of a 3.50% solution of AgNO3? 1. 14 g 2. 0.00875 g 3. 114.28 g 4. 1400 g
Wednesday, September 19, 2012 at 5:05pm by cheri

chemistry
it is desired to prepare 250.0mL of a standard solution having a concentration of 0.1000M AgNo3. How many grams of a sample of AgNO3 of 98.8% purity are required for this purpose?
Thursday, March 25, 2010 at 4:33am by T

chemistry
it is desired to prepare 250.0mL of a standard solution having a concentration of 0.1000M AgNo3. How many grams of a sample of AgNO3 of 98.8% purity are required for this purpose?
Thursday, March 25, 2010 at 4:34am by T

Chemistryy
what mass of silver nitrate (AgNO3) is required to prepare 400 grams of a 3.50% solution of AgNO3? Options: 1. 0.00875 g 2. 114.28 g 3. 1400 g 4. 14 g
Tuesday, July 13, 2010 at 4:56pm by alexandra

Chemistry
Write the equation. AgNO3 ==> AgCl (obviously 1 mol AgNO3 is need to form 1 mole AgCl). 0.657 g AgCl is how many moles? moles = g/molar mass = ?? moles AgCl = moles AgNO3. Molarity = moles/L. You know molarity and moles, solve for L.
Saturday, June 12, 2010 at 5:55pm by DrBob222

Chemistry
To 40cm^3 of 1mol AgNO3 is added 20cm^3 of 0.500 AlCl3. What is the molar concentration of the resulting AgNO3 solution. The reaction, if needed, is 3AgNO3 + AlCl3 ==> 3AgCl + Al(NO3)3 I worked out the number of moles present in AgNO3 which is 0.04 mol, and the number of ...
Sunday, December 30, 2012 at 3:44pm by Matt

Science
first, identify the reactions: KCl + AgNO3 = KNO3 + AgCl CaCl2 + 2AgNO3 = Ca(NO3)2 + 2AgCl convert grams to moles for KCl and CaCl2 to get total moles of Cl involved Each mole of Cl requires one mole of AgNO3 to react. divide that no. of moles by 1.57 to get liters of AgNO3 ...
Friday, October 19, 2012 at 2:31pm by Steve

Chemistry
I assume your actual yield is 6.7496 g AgCl. Theoretical yield: AgNO3 + NaCl ==> AgCl + NaNO3. Convert AgNO3 to moles. moles = g/molar mass. Convert NaCl to moles. Now you must determine which reagent (AgNO3 or NaCl0 is in excess. Since the reaction shows a 1:1 ratio for ...
Sunday, June 7, 2009 at 1:36pm by DrBob222

Chemistry 3A
AgNO3 + NaCl ==> NaNO3 + AgCl mols AgNO3 = M x L = ? Using the coefficients in the balanced equation, convert mols AgNO3 to mols NaCl. Then grams NaCl needed = mols NaCl x molar mass NaCl. Use the same process for grams AgCl formed.
Monday, December 10, 2012 at 9:39pm by DrBob222

Chemistry
What is the ionic equations for the following metals and aqueous substances? With the same equation what is being oxidize and what is being reduced? Zn + AgNO3 Zn + CuSO4 Zn + PbNO3 Mg + AgNO3 Mg + CuSO4 Mg + PbNO3 Cu + AgNO3
Sunday, November 21, 2010 at 9:21am by Jose-Ann

pharmacy math
2% AgNO3 ointment means 2 g AgNO3/100 g ointment. You want 1g AgNO3; 100 g ointment x (1/2) = ?g ointment.
Friday, December 7, 2012 at 1:29pm by DrBob222

chemistry
AgNO3 + NaCl ==> AgCl + NaNO3 moles AgNO3 = M x L = ? moles NaCl = moles AgNO3 grams NaCl = moles NaCl x molar mass NaCl
Friday, November 18, 2011 at 12:59pm by DrBob222

chemistry
percent what? w/w; w/v, v/v, etc. I assume this is mass percent. (g AgNO3/400 g soln)*100 = 3.50 Solve for g AgNO3.
Wednesday, September 19, 2012 at 5:05pm by DrBob222

chemistry
Have 250 mL of a 0.80 M solution of silver nitrate AgNO3 dissolved in water. how many grams of AgNO3 does the solution contain
Tuesday, October 18, 2011 at 3:38pm by mary

applied chemistry
A 50.0mL volume of AgNO3, solution contains 0.0285 mol AgNO3 (SILVER NITRATE). What is the molarity of the solution?
Wednesday, March 7, 2012 at 11:49pm by jose

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
2AgNO3 + K2CrO4 ==> Ag2CrO4 + 2KNO3 mols K2CrO4 = M x L = ? Convert to mols AgNO3. mols AgNO3 = 2*mols K2CrO4. Then M AgNo3 = mols/L. You know mols and you M from the problem. Solve for L and convert to mL.
Tuesday, September 25, 2012 at 11:24pm by DrBob222

Chemistry
An excess of aqueous AgNO3 reacts with 24.5 mL of 5 M K2CrO4(aq) to form a precip- itate. What is the precipitate? 1. AgNO3 2. Ag2CrO4 3. KNO3 4. K2CrO4
Thursday, October 14, 2010 at 3:33pm by John

ap
An excess of aqueous AgNO3 reacts with 44.5 mL of 5 M K2CrO4(aq) to form a precip- itate. What is the precipitate? 1. K2CrO4 2. KNO3 3. Ag2CrO4 4. AgNO3
Monday, October 1, 2012 at 8:19pm by cheri

Chemistry
I don't understand the question. Exposure of AgNO3 solution to light but AgNO3 solution has no chlorine in it.
Tuesday, February 8, 2011 at 11:52pm by DrBob222

Chemistry
A single mole of AgNo3 weighs 169.88 grams. In order to make a 1M solution, how many grams of AgNo3 would need to be dissolved in 5oomL?
Tuesday, November 2, 2010 at 9:26pm by Jazz

Chemistry
You have 250 mL of a 0.80 M solution of silver nitrate AgNO3 (169.87 g/mol) dissolved in water. How many grams of AgNO3 does the solution contain?
Monday, October 17, 2011 at 9:55pm by sara

science
A single mole of AgNO3 weighs 169.88 grams. In order to make a 1M solution, how many grams of AgNO3 would need to be dissolved in 1 liter?
Wednesday, July 11, 2012 at 4:30pm by yoly

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

chemistry help
The molar mass of AgNO3 is not 100. Add up atomic mass Ag, N, and three O atoms to get the molar mass (the periodic tab le will give you the atomic masss). Then 29.66 g/molar mass = moles AgNO3. Then moles AgNO3/liters of soln= M. (They tell you the solution is 100 mL. That's ...
Saturday, May 9, 2009 at 12:06am by DrBob222

Chemistry
....2AgNO3 + Na2CO3 ==> Ag2CO3 + 2NaNO3 mmols AgNO3 = 45.00*0.022 = 0.99 mmols Na2CO3 = 13.00*0.0014 = 0.0182. As a limiting reagent (LR) problem we could form 0.0182 mol Ag2CO3 with Na2CO3 or 0.495 mol Ag2CO3 with AgNO3. That makes Na2CO3 the LR. So we use up all of the ...
Friday, November 15, 2013 at 12:33pm by DrBob222

Chemistry
Since the AgNO3 have a molar mass of 169.87 g. I divided that by 0.02 g and got 0.000118 moles of AgNO3. How would I find how many moles is Ag and how many is NO3? Thanks
Tuesday, January 29, 2013 at 9:56pm by Shadow

chem
K2CrO4 + 2AgNO3 ==> Ag2CrO4 + 2KNO3 moles K2CrO4 = M x L = ? moles AgNO3 = M x L = ? Now do two stoichiometry problems. 1. How many moles Ag2CrO4 if we used all of the K2CrO4. moles Ag2CrO4 = moles K2CrO4 x (1 mole Ag2CrO4/1 mole K2CrO4) = moles K2CrO4 x (1/1) = ? 2. How ...
Tuesday, November 29, 2011 at 4:33pm by DrBob222

Chemistry UGH
Help please! I can't solve any of these, would someone be as kind as to show me the answers? How many moles of NaHCO3 are in a 125.0 g sample of the compound? 3. How many moles are in 6.73 x 1024 water molecules? 4-5. AgBr, a chemical used in photography can be made with this ...
Thursday, May 28, 2009 at 5:10pm by Daniel

Chemistry
For the following Reaction: 2AgNO3 + CaBr2 = 2AgBr + CaN2O6 If a chemist starts with 12.0g AgNO3, how many grams of CaBr2 must be added to use up all of the AgNO3?
Monday, November 14, 2011 at 1:09pm by Carrie

Science
NaBR+ AgNO3- AgBr+ NaNO3 AgNO3=reagent A NaBr=reagent B When 4.36 grams of AgNO3 react with 5.05 grams of NaBr, which is the limiting reagent? How many grams of the excess reagent remain? How many grams of AgBr are produced in the reaction?
Friday, October 5, 2007 at 11:49pm by Raz

Analytical Chemistry
why is it necessary to store AgNO3 solution in an amber bottle? Why must volhard titration be carried out in strongly acidic medium? Why is titration of AgNO3 with KSCN be done with vigorous swirling?
Friday, July 25, 2008 at 9:37pm by anonymous

Chem
AgNO3 solutions are often used to plate silver onto other metals. What is the maximum amount of silver in grams that can be plated out of 4.2L of an AgNO3 solution containing 3.1% Ag by mass?
Friday, April 18, 2014 at 7:08pm by Marianella

Chemistry
1.Calculate the Theoretical and % Yields of the following equation: 2.What is the limiting and excess reactant? 3.How much excess remains? 2AgNO3 + CaCl2 -> 2AgCl + Ca(NO3)2 mass of 2AgNO3= 1.5g mass of CaCl2= 1.1g (What I have so far): AgNO3: 1.5g(AgNO3) 2mol/170g = 0....
Thursday, January 19, 2012 at 12:50pm by Feloniz

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

Chemistry
What is the full net ionic equation for each reaction? do they form a precipitate or have a color change? CuSO4+AgNO3 CuSO4+BaCl2 CuSO4+Cu(NO3)2 CuSO4+Pb(NO3)2 CuSO4+KI CuSO4+Na2S2O3 AgNO3+BaCl2 AgNO3+Cu(NO3)2 AgNO3+Pb(NO3)2 AgNO3+KI AgNO3+Na2S2O3 BaCl2+Cu(NO3)2 BaCl2+Pb(NO3)2...
Tuesday, May 27, 2008 at 6:49pm by Joe

Chemistry
What is the full net ionic equation for each reaction? do they form a precipitate or have a color change? CuSO4+AgNO3 CuSO4+BaCl2 CuSO4+Cu(NO3)2 CuSO4+Pb(NO3)2 CuSO4+KI CuSO4+Na2S2O3 AgNO3+BaCl2 AgNO3+Cu(NO3)2 AgNO3+Pb(NO3)2 AgNO3+KI AgNO3+Na2S2O3 BaCl2+Cu(NO3)2 BaCl2+Pb(NO3)2...
Tuesday, May 27, 2008 at 6:50pm by Joe

Chemistry
Question: A solution of Silver nitrate, AgNO3, contains 1.08 grams in 250 cm3. What is its molarity? Solution: Molar mass of Silver nitrate = 108 g/mole. n(AgNO3) = 1.08 grams of AgNO3 x 1 mole of AgNO3108 grams AgNO3 = 0.01 mole. Number of moles in 1 dm3 = 0.01 mole x 1000/...
Sunday, December 30, 2012 at 3:44pm by Katie

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
You have three problems here. The first one, g AgNO3 in 1 L. M = moles/L You now M and L, solve for moles. Then moles = grams/molar mass. You know moles and molar mass, solve for grams. By the way, note that the 1 L is 1 L of solution (AFTER the AgNO3 is dissolved the final ...
Friday, July 16, 2010 at 6:15pm by DrBob222

AP Chemistry
(a) When 300.0 milliliters of a solution of 0.200 molar AgNO3 is mixed with 100.0 milliliters of a 0.0500 molar CaCl2 solution, what is the concentration of silver ion after the reaction has gone to completion? 2AgNO3 + CaCl2 ==> 2AgCl + Ca(NO3)2 initial: AgNO3 = M x L = 0....
Monday, April 5, 2010 at 6:16pm by DrBob222

Chemistry
1 mol AgNO3 = 1 mol AgBr and all of the other equalities will give several. PbBr2 and AgBr are insoluble. AgNO3 and Pb(NO3)2 are soluble in water. Etc.
Wednesday, August 1, 2012 at 4:18pm by DrBob222

Chemistry
How many moles AgNO3 do you have? That is M x L = ? moles AgNO3. Convert that to grams. g = moles x molar mass.
Wednesday, December 7, 2011 at 8:21pm by DrBob222

Chemistry
AgNO3 + NaCl → AgCl + NaNO3 . How many grams of NaCl would be required to react with 446 mL of 0.211 M AgNO3 solution? Answer in units of grams
Friday, February 21, 2014 at 12:10am by Zoey

chemistry
1.0 M x 0.060 L = moles AgNO3. 0.80 M x 0.0250 L = moles NaCl. AgNO3 + NaCl ==> NaNO3 + AgCl. This should help.
Sunday, January 10, 2010 at 5:15pm by DrBob222

chem
AgNO3 + NaCl produces AgCl + NaNo3 how much AgCl is produced when 3.10g of AgNO3 and .600g of NaCl react?
Tuesday, November 9, 2010 at 2:12pm by alex

chem
AgNO3 + NaCl produces AgCl + NaNo3 how much AgCl is produced when 3.10g of AgNO3 and .600g of NaCl react?
Wednesday, December 8, 2010 at 10:46pm by alex

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
# milliequiv AgNO3 = N x L = ? #m.e. Cl^- = #m.e. AgNO3. N Cl^- = # m.e./mL = ?
Friday, June 1, 2012 at 1:02pm by DrBob222

ap
An excess of aqueous AgNO3 reacts with 44.5 mL of 5 M K2CrO4(aq) to form a precip- itate. What is the precipitate? 1. K2CrO4 2. KNO3 3. Ag2CrO4 4. AgNO3 What mass of precipitate is formed? Answer in units of g
Monday, October 1, 2012 at 8:20pm by cheri

Chem.
What kind of single replacement do you want to do. You don't need silver METAL to a s.d. reaction. Here are two using a silver salt. Mg + AgNO3 ==> Ag + Mg(NO3)2 Al + AgNO3 ==> Ag + Al(NO3)2 OR if it's the silver you want to do, Ag + Au(NO3)3 ==> Au + AgNO3 None of ...
Monday, November 24, 2008 at 11:00pm by DrBob222

chemistry
Your answer of 3.75 would be correct if the limiting reagent were NaBr. AgNO3+NaBr=AgBr↓+NaNO3 No. of moles of AgNO3 = 0.1*0.15 = 0.015 M No. of moles of NaBr = 0.02*1 = 0.02 M The limiting reagent is AgNO3, so the No. of moles of AgBr produced = 0.015 Mass of AgBr = 0....
Monday, August 23, 2010 at 6:50pm by MathMate

chemistry
what is the equation for C6H12O6+NaOH+Cu(OH)2 C6H12O6+AgNO3+NH4OH AgNO3+NH4OH+ galactose when heated
Saturday, October 16, 2010 at 12:39pm by flans

chemistry
By means of what single reagent could you distinguish between the following? (Tell what happens to each substance.) Solutions: AgNO3 and Zn(NO3)2 H2SO4 and HNO3 Ag(NH3)2Cl and AgNO3 Solids: AgCl and ZnCl2 AgCl and Hg2Cl2 PbCrO4 and K2CrO4
Thursday, February 4, 2010 at 12:36pm by Becky

Chemistry
In my problem i need to find the mass of Ag in AgNO3. I have 3.489g of AgNO3. Help please! Determine the percentage composition from the formula. PercentAg= atomicmassAg/molmassAgNO3 Then, mass Ag= 3.489 * decimal percent above.
Sunday, January 28, 2007 at 7:49pm by Jason

chemistry
M = moles/L You know M and L, calculate moles. Then moles = g/molar mass. You know moles and molar mass, calculate g AgNO3 (theoretical AgNO3) but since it isn't 100%, you must correct for that. grams to weigh *0.9981 = theoretical AgNO3. Solve for grams to weigh.
Tuesday, February 16, 2010 at 3:41am by DrBob222

Chemistry
Convert 13.38 g Of Ag to moles by dividing by the gram-atomic mass of Ag. 1 mole of Ag produces 1 mole of AgNO3 1 mole of AgNO3 + 1 mole NaCl ---> 1 mole AgCl so..... Moles of Ag = Moles of AgNO3 = moles of NaCl (Moles of NaCl) / (molarity of NaCl) = liters NaCl
Tuesday, September 30, 2008 at 9:33pm by GK

Solution Stoichiometry
If 75.0 mL of an AgNO3 solution reacts with enough Cu to produce .25g Ag by single displacement, what is the molarity of the initial AgNO3 solution if Cu(NO3)2 is the other product?
Sunday, March 29, 2009 at 5:10pm by Anonymous

Analytical chemistry
a .2280g sample contained only NaCl and KBr. it was dissolved in water and titrated with a 0.04799M of AgNO3. complete titration of both halides was found to require 51.27mL of the AgNO3 solution. Calculate the weight percent of Cl in the solid sample.
Sunday, April 7, 2013 at 6:58pm by Lana

Chemistry
AgNO3 solutions are often used to plate silver onto other metals. What is the maximum amount of silver in grams that can be plated out of 3.8 L of an AgNO3 solution containing 3.2% Ag by mass? (Assume that the density of the solution is 1.02 g/mL.)
Tuesday, November 30, 2010 at 7:24pm by Kelsey G

Chemistry
Do you mean AgNO3? AgNO3(aq) + NaCl(aq) ==> AgCl(s) + NaNO3(aq) The beginning mass = final mass.
Wednesday, November 28, 2012 at 10:31pm by DrBob222

Pages: 1

Search
Members