Thursday
April 17, 2014

# Search: AgNO3 + Na2S2O3

Number of results: 960

chemistry
The universal steps: 1) balanced equation AgNO3 + NaBr >> NaNO3 (aq) + AgBr (s) balanced. So, one mole of AgBr is produced for each mole of silver nitrate and sodium bromide. 2) number moles you started with: AgNO3= .1*.150= .0150moles NaBr= .020*1= .0200 moles 3) ...
Monday, August 23, 2010 at 7:06pm by bobpursley

Chemistry
Mg + 2AgNO3 ==> 2Ag + Mg(NO3)2 mols AgNO3 = M x L mols Ag = mols AgNO3 g Ag = mols Ag x atomic mass Ag.
Tuesday, April 9, 2013 at 6:43pm by DrBob222

Chemistry
Are the following chemicals light sensitive? 1) Potassium Iodide (KI) 2) Sodium thiosulphate (Na2S2O3)
Saturday, January 8, 2011 at 9:52pm by candy

Chemistry Lab
So I did a kinetics lab on the rate of reaction of peroxydisulfate ion with iodide ion. Part 1 was the effect of concentration. One of the questions asked is to calculate the amount of thiosulfate consumed in moles. My results for trial 1 were (Times taken for consumption of 1...
Sunday, February 2, 2014 at 9:25pm by Anonymous

To Steve
BaCl2 + 2AgNO3 ==> 2AgCl + Ba(NO3)2 and KBr + AgNO3 ==> AgCl + KNO3 g BaCl2 + g KBr = 0.224g 2*mols BaCl2 + mols KBr = mols AgNO3
Friday, December 27, 2013 at 11:34pm by DrBob222

chem
millimols AgNO3 initially = 39.50 mL *0.025 M = ? mmols KSCN used to back titrate = 27.0 x 0.006 M = ? Subtract initial mmols - back titrated mmols = difference which is the amount AgNO3 used; i.e., it's the mmols AgCl produced. Convert to mols, change to grams Cl, calculate...
Wednesday, April 11, 2012 at 4:19pm by DrBob222

Chemistry
I think it was 35 mL of 0.1M AgNO3, not AgCl. When the two solutions are mixed the reaction is: 2AgNO3(aq) + MgCl2(aq) ---> AgCl(s) + Mg(NO3)2(aq) Moles of AgNO3 = (0.035L)(0.1mol/L) = 0.0035 moles of AgNO3. Moles of Ag+ ion = 0.0035 also. Likewise, moles of MgCl2 = (0.015 ...
Monday, September 1, 2008 at 10:59am by GK

Analytical Chemistry
Now that I know you are trying to calculate Ksp for Cu(IO3)2, what is the 0.28 M? Is that the molarity of the Na2S2O3 solution?
Monday, October 11, 2010 at 10:12pm by DrBob222

Chemistry
Remember Le Chatelier's Principle. When a system at equilibrium is subjected to a stress, the reaction will shift in a direction to relieve the stress. So, if we ADD NaCl to the reaction at equilibrium, it will shift (to the right or to the left) so as to use up the Cl^- added...
Wednesday, April 15, 2009 at 5:42pm by DrBob222

Chemistry
This is a limiting reagent problem as well as a solubility produce problem. 2AgNO3 + Na2S ==> Ag2S + 2NaNO3 AgNO3 initially = 20*0.1M = 2 millimols. It will produce 2 * 1/2 = 1 mmol Ag2S Na2S initially = 25 x 0.08M = 2 mmols. It will produce 2 mmols Ag2S. You will produce ...
Friday, December 7, 2012 at 8:58pm by DrBob222

chemistry
We add excess NaCl solution (58.44 g/mol) to 56 mL of a solution of silver nitrate (AgNO3 169.88 g/mol), to form insoluble solid AgCl. When it has been dried and weighed, the mass of AgCl (143.32 g/mol) is found to be 1.25 grams. What is the molarity of the original AgNO3 ...
Wednesday, September 19, 2012 at 4:42pm by cheri

Chemistry
The middle one. CaBr2 + 2AgNO3 --> 2AgBr + Ca(NO3)2 mols CaBr2 = g/molar mass Using the coefficients in the balanced equation, convert mols CaBr2 to mols AgNO3. Now convert mols AgNO3 to g. g = mols x molar mass.
Thursday, January 17, 2013 at 8:33pm by DrBob222

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

Cemistry
36% AgNO3 means 36 g AgNO3/100 g solution. 36 g = 36/170 moles = ?? 100 g solution = volume x density. Calculate volume. Then M = moles/L soln.
Wednesday, June 9, 2010 at 10:07pm by DrBob222

Analytical chemistry
The titration is: 2 Na2S2O3 + I2 = Na2S4O6 + 2 NaI moles NaOCl in 20mL aloquat = moles I2 = (1/2)moles Na2S2O3 = 0.345 L * 0.0409 M / 2 moles NaOCl in original (25mL) sample = 0.0345 * 0.0409 * (500/20) mol / 2 mass NaOCl in original (25mL) sample = 74.4424 g/mol * 0.0345 L * ...
Tuesday, July 30, 2013 at 8:55am by Graham

Chemistry
1) a = mass Fe x specific heat Fe x (Tfinal-Tinitial) 2) This is a limiting reagent problem. I know that because amounts are given for BOTH reactants. AgNO3 + NaCl ==> AgCl(s) + NaNO3 mols AgNO3 = M x L = ? mols NaCl = M x L = ? Using the coefficients in the balanced ...
Sunday, June 30, 2013 at 9:18am by DrBob222

chemistry
We add excess NaCl solution (58.44 g/mol) to 64 mL of a solution of silver nitrate (AgNO3 169.88 g/mol), to form insoluble solid AgCl. When it has been dried and weighed, the mass of AgCl (143.32 g/mol) is found to be 1.91 grams. What is the molarity of the original AgNO3 ...
Monday, September 20, 2010 at 5:40pm by Jake

chemistry
CrCl3(s) + AgNO3 (aq)= AgCl(s) + Cr(NO3)3(aq) A 0.750 g sample of impure CrCl3 was removed from a bottle that contained 1.75 g of impure sample. The removed sample was dissolved in water and required 42.5 mL of 0.215 M AgNO3 solution to react with the CrCl3 in the sample. What...
Monday, March 12, 2012 at 10:12pm by jade

chemistry
Determine the percentage composition of each of the following compounds a) NaCl b) AgNO3 c) Mg(OH)2 for NaCl i got na=23/135=0.17 x 100= 17% Cl=35/135=0.26 x 100=26% for AgNO3 i got 108/42 which im sure was wrong and i didnt get how to complete the problem.. for Mg(OH)2 i didn...
Thursday, March 13, 2008 at 6:50pm by john

CHEMISTRY
A couple of starting points for you but not finished. First, you are ok with X = AgNO3 (note you wrote Ag2NO3 a few lines below that but apparently you didn't use that formula throughout. Second, you have avoided the need for a second variable by using 0.953-X and that's ok, ...
Wednesday, January 30, 2008 at 6:05pm by DrBob222

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
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

ap chem
AgNO3 + KCl ==> AgCl + KNO3 mols KCl = grams/molar mass = about 0.01 mol but you need to do it more accurately. Convert mol KCl to mol AgNO3. That's 0.01 mol also (look at the coefficients in the balanced equation). Then M = mols/L. mol = 0.01; L = 0.026 M = 0.01/0.026 = ?
Sunday, September 29, 2013 at 5:51pm by DrBob222

Chemistry
When aqueous CuSO4 is added to aqueous Na2S2O3, why is there no reaction?
Sunday, September 25, 2011 at 6:33pm by Hannah

Chemistry
I posted before about designing a procedure to determine two unknowns (1 solid, 1 solution). The possible solutions were: NaCl, CaCl2, CuSO4, NaOH,Ba(OH)2, HCl, HNO3, or H2O. The reagents given are: NaOH, HCl, AgNO3, Zn metal, Na2SO4, and H2O. The procedure I've designed so ...
Sunday, November 11, 2007 at 5:59pm by Raj

1. You have the wrong formula for sodium thiosulfate. It is Na2S2O3 Try again 2. How about H2S + 2 KOH -> K2S + 2H2O ?
Thursday, December 6, 2007 at 11:58pm by drwls

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
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

chemistry
Let x = solubility Ag2CrO4 Ag2CrO4(s) ==> 2Ag^+ + CrO4^2- .....x..........2x.......x Ksp = (Ag^+)^2(CrO4^2-) Substitute from the chart above and solve for x b. Use the same Ksp expression. Substitute what you want CrO4^2- to be an solve for (Ag^+). That will give you Ag^+ ...
Monday, March 19, 2012 at 11:24am by DrBob222

Science
Na2S2O3*5(H2O)is hydrated sodium thiosulfate, also known as "hypo". It is a photographic darkroom chemical You need to be more careful which letters in the formula are capitalized.
Tuesday, August 11, 2009 at 3:11am by drwls

Chemistry
Refer to the net ionic equation below to answer the following questions: Co(H2O)6^+2 + 4Cl- <==> CoCl^-2 + 6H2O 1. In what direction was the equilibrium shifted by: a. Addition of HCl b. Addition of water c. Addition of AgNO3 d. Increasing the temperature e. Decreasing ...
Friday, January 21, 2011 at 11:19pm by Sharon

Chemistry
a) Add AgNO3, HCl forms white ppt of AgCl, soluble in NH3. Add BaCl2, H2SO4 forms white ppt of BaSO4, not soluble in HNO3. b) Add AgNO3, K3PO4 forms yellow ppt of Ag3PO4. Soluble in HNO3.
Friday, May 21, 2010 at 8:26pm by DrBob222

Science
What is the scentific formula for Sodium Thiosulphate? What is the mass of a 30 N rock in the school yard? Sodium thiosulfate is Na2S2O3.
Tuesday, October 10, 2006 at 8:04pm by Gina

chemistry
How many grams of I2 are present in a solution if 33.75mL of 0.140M Na2S2O3 solution is needed to titrate the I2solution?
Monday, November 18, 2013 at 11:16pm by Ellen

Science
Sorry, my apologies. After adding Na2S2O3, the Varsol layer became colorless and there was no change in the Aqueous layer.
Sunday, March 9, 2014 at 5:21pm by Karan

chemistry
This is a limiting reagent and a common ion problem rolled into one. 2AgNO3 + Na2CrO4 ==> Ag2CrO4 + 2NaNO3 385 mL x 0.380M = 146.3 mmols = 0.1463 mols AgNO3 467mL x 0.409M = 191 mmols = 0.191 mol Na2CrO4. Which is the limiting reagent? 0.1463 mols AgNO3 x (1 mol Ag2CrO4/2 ...
Thursday, January 24, 2013 at 11:17pm by DrBob222

general chemistry
2AgNO3 + BaCl2 ==> 2AgCl + Ba(NO3)2 mols AgNO3 = grams/molar mass Using the coefficients in the balanced equation, convert mols AgNO3 to mols AgCl. g AgCl = mols AgCl x molar mass AgCl = ?. This is the theoretical yield; i.e., the yield if it were 100%. Then % yield = (3.17...
Sunday, October 6, 2013 at 11:42am by DrBob222

Chemistry
AgNO3 + NaCl ==> AgCl + NaNO3 Here is a sample stoichiometry problem i posted. Just follow the instructions. moles AgNO3 = M x L. http://www.jiskha.com/science/chemistry/stoichiometry.html
Monday, September 27, 2010 at 8:37pm by DrBob222

chemistry
In a measurment 0.1M Kmno4 is used.determine the volume of solution required to react with 0.158M Na2s2o3 required?
Thursday, March 14, 2013 at 1:17pm by Abhishek Bhargav

Chemistry
This is a limiting reagent problem, a common ion problem, and a Ksp problem all rolled into one. 345 mL x 0.352M AgNO3 = 121.44 mmoles. We'll round this to 121 mmols AgNO3. 443 mL x 0.511M Na2CO3 = 226.373 mmols. We'll round this to 226 mmols Na2CO3. You can round them ...
Monday, March 11, 2013 at 7:23pm by DrBob222

Chemisty
For clarity, just assign some number to the volume of a drop. Actually, a drop is between 0.03 and 0.05 mL (depending upon the size of the opening AND on the material that the buret/pipet/dropper is made). BUT, let's just make things simple by saying a drop is 1 mL. We know ...
Wednesday, January 7, 2009 at 10:39pm by DrBob222

Chemistry
Calculate the molar solubility of barium thiosulfate in 0.0045 M Na2S2O3(aq). (Hint: Check any simplifying assumptions that you make.)
Monday, April 19, 2010 at 3:07pm by Chemistry Confused

chemistry
Neither. You corrected one error from the first post to the second but not the other. moles AgNO3 = 0.2M x 0.1L = 0.02 moles. Convert to moles AgCl using the coefficients in the balanced equation. 0.02 moles AgNO3 x (2 moles AgCl/2 moles AgNO3) = 0.02 x (2/2) = 0.02 moles AgCl...
Sunday, March 13, 2011 at 10:47pm by DrBob222

chem
are these already balanced? CuSO4 + Zn ---> CuZn + SO4 AgNO3 + NaCl ---> AgCl + NaNO3 AgNO3 + NaCl ---> AgCl + NaNO3 CuSO4 + Zn ---> Cu + ZnSO4 is the correct equation I know how to balance equations but im not sure about these Yes, they are balanced. But you ...
Tuesday, March 20, 2007 at 7:57pm by Paul

chemistry
calculate the numbers of moles of sodium thiosulfate (Na2S2O3) and hence the moles of S2O3^2- ions present in the volume of 43mL can someone plz help me?
Wednesday, November 16, 2011 at 10:56pm by Yul

chemistry
calculate the numbers of moles of sodium thiosulfate (Na2S2O3) and hence the moles of S2O3^2- ions present in the volume of 43mL someone plz help
Wednesday, November 16, 2011 at 10:58pm by myu

Chem
Help! I'm not suppose to react Iron Chloride with Silver Nitrate in order to get Iron nitrate. If i'm suppose to keep one of the above ingredients and obtain a pure dry sample, what should i do? I don't know the question. Why are you not supposed to react the two? and which ...
Friday, September 8, 2006 at 12:35am by kelly

Chemisty
First determine limiting reagent. AgNO3 + NaCl ==> AgCl + NaNO3 mols AgNO3 = grams/molar mass mols NaCl = grams/molar mass Convert mols AgNO3 to mols AgCl using the coefficients in the balanced equation. Do the same for NaCl. It is likely these two values will not agree ...
Wednesday, April 24, 2013 at 10:06am by DrBob222

chemistry
Please note that nacl doesn't mean anything. kbr is nothing either. cl is nothing. Starting a sentence with a small letter makes the sentence difficult to read and interpret. Henceforth, please write your questions in good style. I'm helping because I managed to understand the...
Friday, March 27, 2009 at 10:57pm by DrBob222

Chemistry
This is a limiting reagent problem and a Ksp problem with a common ion all rolled into one. 3AgNO3 + Na3PO4 ==> Ag3PO4 + 3NaNO3 mol AgNO3 = M x L = about 0.19 but you need to do it more accurately. mols Na3PO4 = M x L = about 0.22 but you confirm. Convert mols AgNO3 to mols...
Saturday, January 19, 2013 at 9:15pm by DrBob222

Chemistry
How many moles of sodium chloride must be added to an aqueous solution that contains 2.0 moles of silver nitrate in order to precipitate 0.50 moles of silver chloride? A) 0.25 mol B) 0.50 mol C) 1.0 mol D) 2.0 mol E) 1.5 mol The answer is B. I have no idea what to do. I was ...
Sunday, March 22, 2009 at 4:59pm by Jill

chemistry
You're supposed to use your knowledge of chemistry to answer these. The first one, AgNO3 and Zn(NO3)2. Add NaCl. The AgNO3 reacts with NaCl to produce a white insoluble precipitate of AgCl. Zn(NO3)2 and NaCl does nothing. So the secret is to know the solubility tables. Where a...
Thursday, February 4, 2010 at 12:36pm by DrBob222

chemistry
What I have with is really figuring out the equation. I know that in the presence of AgNO3, the Cl- would form AgCl which forms a precipitate. The Br- would form (BrNO3)+2 or something like that. I feel like I'm on the right track here but I'm doing something wrong. The ...
Thursday, March 29, 2012 at 12:04am by Anonymous

Chem
moles AgNO3 = M x L = ?? moles CrCl3 = M x L = ?? Using the coefficients in the balanced equation, convert moles AgNO3 to moles AgCl. Same procedure, convert moles CrCl3 to moles AgCl. The two answers likely will be different which means one of them is wrong; in limiting ...
Saturday, October 9, 2010 at 5:15pm by DrBob222

CHEMISTRY
Two or three points here. If you let X = mass AgNO3 then 0.953 - X = mass Ba(NO3)2. First, if we set this up with just this information, the following is what you get. X + 0.953 - X = 0.953 and we end up with 0 = 0, which of course, is true but it doesn't help us much if the ...
Wednesday, January 30, 2008 at 6:05pm by DrBob222

Chemistry
Zn(s) + MnCl2 ==> Zn(s) + AgNO3 ==> Mn(s) + AgNO3 ==> Mn(s) + Zn(NO3)2 ==> The above four will tell you if Zn is above Mn and Ag and if Mn is above Ag and Zn. You will need two more to check where Mn is with respect to Ag
Tuesday, October 22, 2013 at 11:35pm by DrBob222

Chemistry
mols AgNO3 = grams/molar mass Convert mols AgNO3 to mols AgCl. Convert mols AgCl to g. g = mols x molar mass.
Wednesday, March 13, 2013 at 7:03pm by DrBob222

chemistry
Convert 0.1 g NaCl and 0.1 g AgNO3 (note: nacl and agno3 don't mean a thing--don't be so lazy in chemistry that you can't punch the CAPS key). Here is a worked example of a stoichiometry problem. Print this out--it will solve 99.9% of the stoichiometry problems you are likely ...
Saturday, July 16, 2011 at 10:45am by DrBob222

chemistry
CrCl3 + 3AgNO3 ==> 3AgCl + Cr(NO3)3 moles AgNO3 used = M x L = ?. moles CrCl3 = 1/3 x moles AgNO3. g CrCl3 = mols x molar mass %CrCl3 = (grams CrCl3/mass sample)*100 = ?? For mass sample use 0.750 for percent CrCl3 in the "removed" sample; use 1.75 if you want the percent ...
Monday, March 12, 2012 at 10:12pm by DrBob222

chemistry again
There are two or three methods but each is a little different and each depends upon the reaction. There is no general way to do it. If you have a limiting reagent problem (limiting reagent problems are those in which amounts are given for BOTH reactants) you do them this way. ...
Sunday, September 29, 2013 at 4:50pm by DrBob222

Chem
Which coordination compound will most likely form a precipitate when treated with silver(II) nitrate (aqueous)? [Cr(NH3)3Cl3] [Cr(NH3)6Cl3] Na3[Cr(CN)6] Na3[CrCl6] I tried the solubility rules, but that didn't work out. Any help would be great. I made a mistake about, it's ...
Saturday, April 21, 2007 at 10:53am by Londy

science
a) AgNO3
Wednesday, June 19, 2013 at 6:21am by Elena

Chemistry 101
This is a different question then asked before,I had lab where I mixed 1.365 NaCL + AgNO3-->2.6242 AgCl. The 2 questions that I need help finding the answers to are: How much salt should be used to cause all of the silver nitrate to react? How much silver chloride should be...
Monday, June 8, 2009 at 12:45pm by Gweedo8

Chemistry
Quantitative anaylsis of cl- ion is often performed by a titration with silver nitrate, using sodium chromate as an indicator. As standardized AgNo3 is addded, both white AgCl and red Ag2CrO4 precipitate, but so long as some cl- remains, the Ag2CrO4 dissovles as the mixgture ...
Sunday, October 31, 2010 at 1:42pm by MEG

Chemistry
Your answer is close to a factor of 10 off but I don't understand most of what you did. Here is how I would do it, following DrWLS' response. moles AgNO3 = M x L = 0.32 x 0.120 = 0.0384 moles. moles K2CrO4 = M x L = 0.32 x 0.040 = 0.0128 moles. How much AgNO3 must we have if ...
Friday, January 29, 2010 at 1:50am by DrBob222

All I have is the concentration of S2O3^-2 which is 3.33e^-3M. How would I find moles? For the experiment we used 2.50mL of Na2S2O3. Do I use this to find moles?
Sunday, February 26, 2012 at 9:14pm by Hannah

Chemistry
Li2SO4+AgNO3= ???
Tuesday, February 22, 2011 at 10:56pm by Artie

Chemistry
How many grams of I2 are present in a solution if 38.55ml of 0.160M Na2S2O3 solution is needed to titrate I2 the solution?
Monday, November 19, 2012 at 2:12am by Michi

Chemistry
How many grams of I2 are present in a solution if 39.85mL of 0.160M Na2S2O3 solution is needed to titrate the I2 Solution
Friday, March 14, 2014 at 1:43am by Jackie

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

Chemistry
A. Standardization of Na2S2O3 -Mass of KIO3 in 100mL = 0.09600g -Calculate Molarity of KIO3= ? Please check: 0.09600g/(214.0g/mol)=4.486x 10^-4 mol -4.486 mol/0.1L= 0.004486 M This looks ok to me except for the -4.486. I don't know why the - sign is there unless it's just a ...
Sunday, March 6, 2011 at 11:42pm by DrBob222

Standardization of the Sodium Thiosulfate Solution Make up a standard solution of potassium iodate by accurately “weighing by difference” about 0.1 g of KIO3 and placing it in your 100 mL volumetric flask. Fill the flask to mark with distilled water. Potassium iodate reacts ...
Sunday, October 19, 2008 at 9:35pm by Sara

Stoichiometry problem
NacI and AgNo3
Saturday, September 9, 2006 at 10:04pm by ali

chemistry
agh3+no3
Monday, February 4, 2008 at 6:14pm by agno3+nh3

General Chem
What do you call a solution that is maid by mixing solid Na2S2O3 5H20 with NaOH? Also, what is the complete balanced equation for mixing the above solution with an aqueous solution of NaClO? Thanks anyone!
Wednesday, June 22, 2011 at 7:14pm by Mark

Chemistry
A- a water soluble salt forms a precipitant during Group 3 analysis. An acidic solution of this precipitant and NaBiO3 yields a pinkish color. This same salt has no reaction to concentrated H2SO4 or AgNO3, what is the chemical formula for this salt? B- a brown colored salt ...
Monday, April 2, 2012 at 7:29pm by Mima

Chemistry
A- a water soluble salt forms a precipitant during Group 3 analysis. An acidic solution of this precipitant and NaBiO3 yields a pinkish color. This same salt has no reaction to concentrated H2SO4 or AgNO3, what is the chemical formula for this salt? B- a brown colored salt ...
Tuesday, April 3, 2012 at 2:32pm by Mima

Chemistry
In the future, PLEASE tell us what you are doing. I am guessing that you have added AgNO3 to a Cl solution to ppt AgCl. The reason you add HNO3 is because you want an acid solution from which to ppt AgCl. AgOH and/or Ag2O (actually a hydrated silver oxide) ppts from a neutral ...
Tuesday, March 9, 2010 at 5:28am by DrBob222

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
A solution was prepared by adding 15mL of 0.129 M KI, 5mL of 0.1 M Na2S2O3, 1mL of starch solution, and 15mL of 0.125 M (NH4)2S2O8. Calculate the concentration of (M) of I in the final mixture before the chemical reaction.
Friday, October 3, 2008 at 1:36pm by Brian

Chemistry (Stoichiometry)
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 8:36pm by Jennifer

chemistry
AgNO3 + KOH formula and name
Monday, March 23, 2009 at 5:39pm by molly

chemistry
How many moles are in 1.18g of 4.7x10^-4 M AgNO3?
Wednesday, October 12, 2011 at 1:31am by christopher

chemistry
why is AgNO3 stored in an amber bottle
Monday, February 13, 2012 at 11:08pm by faith

Chemistry
What is the chemical equation for AgNO3 + NaCI?
Monday, February 27, 2012 at 10:12am by Tia

chemistry
See the AgNO3 problem before.
Wednesday, September 19, 2012 at 4:55pm by DrBob222

Science
How do i calculate this? 5 ml of 0.1% (w/v) AgNO3 2 L of 1% (w/v) NaCl
Sunday, June 9, 2013 at 7:49pm by Kayla

chemistry
1gm of AgNO3 is dissolved in 50ml of h2o. it is titrated with 50ml od sol. agi is precipitated is filtered of.the exces of ki is then titrated with 1/10M KIO3 in the presence of acidic medium until all I->>ICl. it reqires 50ml of the 1/10M KIO3 sol. 20ml of same KI sol ...
Sunday, March 28, 2010 at 12:55am by debby

Chemistry
How many milliliters of 0.230 M Na2S2O3 solution are needed to titrate 2.349 g of I2 according to the equation below? I2(aq)+2S2O3^2-(aq)->S4O6^2-(aq)+2I^1-(aq)
Wednesday, October 6, 2010 at 10:29pm by Drew

science
Any advice on how to figure out solubillty of Agno3?
Saturday, October 27, 2007 at 1:14pm by julia

Chemistry
Does Pb(NO3)2 + AgNO3 form a precipitate?
Wednesday, November 19, 2008 at 4:26pm by Mackenzie

chem
You need to know the molarity of the AgNO3 being added.
Thursday, April 22, 2010 at 1:32pm by DrBob222

Chemistry -
Zn + AgNO3 Produced Ag + ZnNO3
Saturday, May 29, 2010 at 12:58pm by nomso

Chemistry 101
what is the number of atom in each compound of AgNO3
Monday, June 8, 2009 at 12:45pm by maryann

Chemistry
Sorry the question is What is the molarity of this AgNO3(aq)?
Sunday, March 18, 2012 at 5:18pm by Ash

science
what is the product or reaction between H3O + AgNO3?
Tuesday, May 28, 2013 at 11:52am by glen

science
what is the product or reaction between H3O + AgNO3?
Tuesday, May 28, 2013 at 11:53am by glen

Science (chemistry)
I suppose you could do these if you knew how to do the MgCl2, AgNO3 etc.
Wednesday, April 2, 2014 at 11:41pm by DrBob222

chemistry
Al(OH)3 + 3HCl ==> AlCl3 + 3H2O is already balanced. I think you may have made a typo in the first one. I suspect it is S2O3^2- on the right which is the way I will balance it. 6NaOH + 4S ==> 2Na2S + Na2S2O3 + 3H2O
Sunday, August 28, 2011 at 7:41am by DrBob222

Chem.
Excuse me but I just now reread the question and I had not seen the first line. To extract Ag from AgNO3 is a slightly different reaction. I guess it all depends upon how much silver you want and in what form. If you just want to plate out some silver, the easy way to do it to...
Monday, November 24, 2008 at 11:00pm by DrBob222

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