What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample?
Q. please help me out asap!!! Suppose a 1.441-g sample is known to contain 12.5 % chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample? What mass of silver chloride will be obtained?
Asked by angela - Tue Dec 23 15:39:47 2008 - - 4 Answers - 0 Comments

A. Hi angela...im stuck on the same problem...hahahaha Silver nitrate is highly soluble salt and when it is dissolved it forms silver and nitrate ions: AgNO3(aq) ---> Ag^+(aq) + NO3^-(aq) Silver ions react with chloride ions present in the solution and forms insoluble silver chloride: Ag^+(aq) + Cl^-(aq) ---> AgCl(s) This is the net ionic equation of the reaction. Mass of the sample:1.441 g Mass of Cl- ions in the sample: 1.441 x (12.5/100) = 0.180125 g Molar mass of Cl = 35.5 g /mol Mole of Cl- ions = 0.180125 g / 35.5 g/mol = 0.0050739mol According to net ionic equation; 1 mol Ag^+ ion is necessary to precipitate 1 mol Cl^- ion, therefore for 0.0050739 mol Cl^- ion we will need 0.0050739 mol Ag^+ ion. According to dissolving equation;… [cont.]
Answered by Karan K - Wed Dec 24 11:59:31 2008

What is the best way to get the silver out of silver nitrate?
Q. What is the easiest and cheapest way to get silver (Ag) out of silver nitrate (AgNO3). I dont mean by just dissolving it in water I need to get actual solid silver.
Asked by Dylan N - Tue May 15 20:57:51 2007 - - 3 Answers - 0 Comments

A. Add copper wire, and crystals of silver will form on the wire. Cu gets oxidized and Ag gets reduced.
Answered by mrfarabaugh - Tue May 15 21:00:18 2007

What happens in a reaction between Zinc and Silver Nitrate when the Zinc ends up having a silver cloating?
Q. How would I calculate the mass of the zinc with the silver coating? Starting with 5.00g of zinc and adding that to .1L of a .1M silver nitrate solution. Assume all silver is reduced.
Asked by mylo - Fri Oct 9 04:41:46 2009 - - 2 Answers - 0 Comments

A. Zinc is higher than Ag in the reactivity seies. If you add Zn to a solution of AgNO3, the following occurs: Zn + 2AgNO3 Zn(NO3)2 + 2Ag The zinc become a positive ion, it has lost electrons, so it has been oxidised.
Answered by Trevor H - Fri Oct 9 06:04:38 2009

Is it possible to remove silver nitrate stains from skin?
Q. I used a hospital-grade silver nitrate swab to stop bleeding on a dog yesterday and got the silver nitrate on my hands. Now the stains are darkening and I'm wondering if it is possible to remove the stains with anything such as oxalic acid or tarnish remover. I know that the stains wear off, but I am scheduled to be in a wedding on Saturday. Call me vain, but I'm looking for a quicker solution. What about iodine or sodium thiosulfate? I'm not worried about it hurting.
Asked by texastailfeathers - Wed Dec 13 10:46:56 2006 - - 3 Answers - 0 Comments

A. The stains can be removed. But it will be very painful. Don't worry they will wear off. Eventually.
Answered by namsaev - Wed Dec 13 10:49:42 2006

How many moles of silver nitrate are needed to react?
Q. Silver nitrate and sodium chloride react to form insoluble silver chloride. How many moles of silver nitrate are needed to exactly react with 0.327 moles of sodium chloride. (Silver, Ag, forms Ag* ion)
Asked by mitchel c - Mon Nov 9 15:50:46 2009 - - 0 Answers - 0 Comments

What happen after adding iodine and silver nitrate to the tube?
Q. Silver nitrate and Iodine Activity.
Asked by Karlene W - Wed Oct 8 14:30:20 2008 - - 1 Answers - 0 Comments

A. Not sure exactly what you are looking for, but if they are solutions, the silver and iodine will combine to form an insoluble precipitate silver chloride AgCl. Hope that's what you're looking for
Answered by sfgrc - Thu Oct 9 15:22:01 2008

Why is the silver nitrate test considered to be the specific test for the halogens?
Q. Can I add this up please?? Thanks!! What is the equations involved in the silver nitrate (AgNO3) test? Thanks a LoT!!! :)
Asked by MiG - Wed Nov 15 06:33:00 2006 - - 3 Answers - 0 Comments

A. This is because a compound of silver with any halogen is definitely insoluble in water. This is the ONLY compound of silver that gives such a result, and it can be immediately concluded that halogen(s) are present in the unknown reactant. Also, the other product of the reaction is a nitrate, which is soluble in water and will not affect the results. This is why it is the specific test for the halogens. FYI, silver chloride gives white, silver bromide gives yellow-white, and silver iodide gives yellow. The colour intensity increases down the group. Taking Y to be a halide and X to be a positive ion, AgNO3 (aq) + XY (aq) --> AgY (s) + XNO3 (aq) Thus it can be seen very clearly that the precipitate formed contains a halogen.
Answered by donteatflowers - Wed Nov 15 07:42:11 2006

What quantity of silver nitrate is needed to react with 0,035 g of sodium chloride?
Q. Silver nitrate is used in labs to determine the quantity of sodium chloride present in food products. Silver nitrate reacts with sodium chloride in a 1:1 ratio, shown in the following equation: AgNO3 + NaCl --> AgCl + NaNO3.
Asked by Christine - Fri Aug 28 15:56:16 2009 - - 3 Answers - 0 Comments

A. Take .035 g NaCl and divide it by the molar mass of NaCl which is 58.43 1.) You can calculate the molar mass by looking at the periodic table of elements and adding the number at the bottom of Na and Cl 2.) .035 g NaCl * (1 Mol NaCl / 58.43 g) = 5.99 * 10 ^-4 3.) You have a 1:1 ratio of AgNO3 and NaCl. You also know this because of the balanced equation: AgNO3 + NaCl --> AgCl + NaNO3 to determine what the ratio is, look at the coefficients in front of each compound, in this case there is no so the coefficient is 1 4.) Take 5.99 * 10 ^ -4 Moles of NaCl and multiply it by the molar mass of AgNO3 *you get the molar mass of AgNO3 the same was as you got the molar mass for NaCl (look at the periodic table of elements and add (Ag + N + 3 *… [cont.]
Answered by Wilson B - Fri Aug 28 16:44:04 2009

What is the enthalpy of solvation for silver nitrate?
Q. When 5.00 grams of AgNO3(s) is dissolved in 75.00 grams of H2O(l), the temperature of the solution drops by 2.0 C. What is the enthalpy of solvation for silver nitrate? (The enthalpy of solvation for a compound is defined as the enthalpy of reaction when the solid compound is dissolved in water.) Take the specific heat of the solution as 4.2 J/g C.
Asked by HowDoUGetOut - Mon Mar 26 17:13:44 2007 - - 1 Answers - 0 Comments

A. go find someone that knows physical chemistry these people on yahoo are idiots
Answered by killswitcheng4ge - Mon Mar 26 17:18:20 2007

Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium?
Q. Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.50 of sodium carbonate is mixed with one containing 5.00 of silver nitrate. How many grams of sodium carbonate are present after the reaction is complete? How many grams of silver nitrate are present after the reaction is complete? How many grams of silver carbonate are present after the reaction is complete? How many grams of sodium nitrate are present after the reaction is complete?
Asked by gabem480 - Wed Sep 24 00:29:24 2008 - - 1 Answers - 0 Comments

A. I'll do one to show you how and will assume you mean 3.50g and 5.00g; you should ALWAYs specify UNITs. Let UNITs guide you; always use them in your calculation to prevent errors eqn: Na2CO3 + 2AgNO3 ---> 2NaNO3 + Ag2CO3 (# moles that react and are produced) moles init of Na2CO3 = 3.50g / MW Na2CO3 g/mole = ?? 0.0330 moles init of AgNO3 = 5.00g / MW AgNO3 g/mole = ?? 0.0294 mole Na2CO3 left = moles init of Na2CO3 - [(mole Na2CO3 / 2 moles AgNO3) * moles init of AgNO3] = ?? g Na2CO3 left = mole Na2CO3 left * MW Na2CO3 g/mole = ?? moles AgNO3 left = moles init of AgNO3 - [(2 mole AgNO3 / moles Na2CO3) * moles init of Na2CO3] = ?? none left plug and SOLVE Basic mathematics is a prerequisite to chemistry I just try to help… [cont.]
Answered by SciMann - Wed Sep 24 12:04:45 2008

If a coil of copper is placed in a solution of silver nitrate, what colour will it be?
Q. If a coil of copper is placed in a solution of silver nitrate, the copper gradually dissolves. What colour will the solution become?
Asked by salomikuddy - Wed Jun 11 16:18:07 2008 - - 4 Answers - 0 Comments

A. Blue you have 2AgNO3 + Cu == Cu(NO3)2 + 2Ag Cu(NO3)2 is blue in color
Answered by Abu Hafsah - Wed Jun 11 16:26:48 2008

how can i remove a silver nitrate spot from my shoes?
Q. During an chemistry experiment at school I accidentally spelled some silver nitrate on my shoes. now all i have is a pair of shoes with a big brown spot. thank you these are sport shoes, and the spot is on the white front linen
Asked by romanu13 - Mon Nov 20 02:48:09 2006 - - 4 Answers - 0 Comments

A. depends on the colour??? black?? brown??? just polish it ..any other colour!! and ther is not a heck of alot you can do
Answered by Button Face - Mon Nov 20 03:13:45 2006

How do I remove acetic acid from a solution of silver nitrate?
Q. I have mixed a solution containing: water... 2000ml Silver Nitrate ...140g Glacial Acetic Acid ...140ml Silver Iodide... trace I would like to reclaim the silver nitrate from the solution. How would this be possible?
Asked by richard_cynan - Tue Jul 14 18:35:42 2009 - - 3 Answers - 0 Comments

A. Rotary evaporator, add fresh water until all acetic is distilled. Add an antisolvent to precipitate the nitrate. (consider the compatibility of the antisolvent and strong oxidising agent).
Answered by fred k - Wed Jul 15 04:49:01 2009

When copper and silver nitrate are mixed?
Q. Why do crystals form around copper when it is put into silver nitrate solution? Can anyone state a hypothesis for it?
Asked by - a n g e l z - - Tue Feb 17 03:46:28 2009 - - 1 Answers - 0 Comments

A. When copper and silver nitrate solution is mixed, silver is formed coz each silver ion gains an electron from the metallic bond of copper. In the copper's metallic bond, there are 2 electrons for each copper atom. When the copper atoms lose their electrons, they become part of an aqueous solution in copper II nitrate. When the copper forms copper II nitrate, the solution turns a light blue color. This color indicates the presence of the copper II ions. Cu + AgNO3 gives Cu(NO3)2 + Ag
Answered by sUpEr StArrr - Tue Feb 17 04:03:01 2009

what is the minimum mass of copper should you add to 500 mL of a 2.00 mol/L solution of silver nitrate?
Q. copper metal can be added to a solution of silver nitrate to produce copper(II) nitrate and solid silver. what is the minimum mass of copper should you add to 500 mL of a 2.00 mol/L solution of silver nitrate, so that all of the silver ions will precipitate?
Asked by miss_independent3065 - Sat May 3 06:40:52 2008 - - 1 Answers - 0 Comments

A. (0.500 L)(2.00 mol/L)(63.55 g/mol) = 63.55 g
Answered by Helmut - Sat May 3 22:27:42 2008

If a dog's toenail is bleeding, is a silver nitrate stick, Clotisol liquid, or styptic power better?
Q. We accidentally quicked our Weim's toenail last night, and it gushed blood everywhere (the vet was closed). Finally this morning I went to the vet and she let me have a few silver nitrate sticks to bring home to cauterize the nail. It worked like a charm. I decided to order them online to have on hand, and I learned about two other remedies also: Clotisol liquid and styptic power. Does anyone have experience with these? I don't know which to get of the three remedies. The nitrate sticks certainly did work. Home remedies such as flour and cornstarch did nothing, because he is a big dog with big nails. After this incident, we will use a Dremmel on his nails, not clippers! My thanks to anyone who can offer some info. Thanks for… [cont.]
Asked by Vix - Tue Sep 11 16:42:52 2007 - - 12 Answers - 0 Comments

A. I've used all three of these products and they all have their good points. The powder works well but can be messy. Sometimes it takes quite a bit to get the bleeding stopped as well. But it does work well. The liquid also works OK but again, very messy! I'd take the liquid as a last resort. Now the sticks are what I like! They work great, but sometimes they can sting a bit. Also, don't let the tip of the sticks rub your own skin - this is because as soon as your skin is exposed to light it will blacken where the sticks rubbed and it's next to impossible to get off. It doesn't hurt anything, but it just looks bad. Of these three, I like the sticks the best. They work quickly and are less messy than the other two.
Answered by FaithE - Tue Sep 11 16:56:03 2007

How many grams of aluminum must react to displace all the silver from 30.8 g of silver nitrate? The reaction o?
Q. How many grams of aluminum must react to displace all the silver from 30.8 g of silver nitrate? The reaction occurs in aqueous solution. how is this problem done?!
Asked by emmie - Mon Oct 12 23:40:50 2009 - - 1 Answers - 0 Comments

A. i take a guess first write the balance equation. grams of Al= molar mass*moles aluminum/ moles of silver nitrate* grams of silver nitrate to find moles you need a balance equation. Al+ 3AgNO3---> 3Ag+ + Al(NO3)3 i hope this is right i am not too sure
Answered by K.S - Mon Oct 12 23:52:57 2009

What is the solubility of Silver Nitrate?
Q. So I know that according to the solubility rules, nitrates are soluble, and salts of silver are insoluble.. But what if I have AgNO3? Would it be soluble or insoluble, and in cases like this, which component should I look at first to determine this?
Asked by Cathy - Fri Oct 17 01:34:02 2008 - - 4 Answers - 0 Comments

A. Nitrates (NO3) are alllwaysss soluble!! regardless of what the other element/CATION IS!!! the following are the alllwayyss solubles: 1) aLkali metals (GROUP 1A) 2)AMOMONIA (NH4) 3)NITRATE(NO3) 4)ACETIC (C2H3O2) these are soluble with exceptions 1)CL, BR, I ---Are soluble except if the other element is...SILVER,MRECURY,OR LEAD. 2)F ---Are soluble except if the other element is...MAGNESIUM,STRONTIUM, BARIUM, CALCIUM,OR LEAD. 3)SO4---Are soluble except if the other element is...STRONTIUM,BARIUM,CAL CIUM, or lead the non- solubles are with the exceptions: 1)CO3---ARE NON-Soluble except if the other element is...One of the alllwaayyyss soluble substance 2)PO4---ARE NON-Soluble except if the other element is...One of the… [cont.]
Answered by yishunshin - Fri Oct 17 02:11:39 2008

Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate?
Q. Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 5.00 g of sodium carbonate is mixed with one containing 5.00 g of silver nitrate. After the reaction is complete, the solutions are evaporated to dryness, leaving a mixture of salts. How many grams of sodium carbonate, silver nitrate, silver carbonate, and sodium nitrate are present after the reaction is complete?
Asked by little chicken - Sun Aug 2 16:46:04 2009 - - 1 Answers - 0 Comments

A. Na2CO3 + 2 AgNO3 = Ag2CO3 + 2 NaNO3 moles Na2CO3 = 5.00 g/105.9884 g/mol=0.0472 moles AgNO3 = 5.00 g/ 169.87 g/mol= 0.0294 (limiting reactant) moles Ag2CO3 = 0.0294/2=0.0147 mass Ag2CO3 = 0.0147 mol x 275.75 g/mol=4.06 g moles NaNO3 = 0.0294 mass NaNO3 = 0.0294 x 84.9935 g/mol= 2.50 g moles Na2CO3 needed = 0.0294/2=0.0147 moles Na2CO3 in exess = 0.0472 - 0.0147 =0.0325 mass Na2CO3 in excess = 0.0325 x 106.9884 =3.48 g silver nitrate =0 check : mass products = 5.00 + 5.00 = 10.00 mass products = 2.50 + 4.06 =6.56 g mass reactant in excess = 3.48 3.48 + 6.56 = 10 g
Answered by Dr.A - Mon Aug 3 13:04:33 2009

Calculate what mass silver would would be produced when 2 moles of Fe reacts with silver nitrate?
Q. Two moles of iron and a beaker full of silver nitrate: (assume Fe is the Limiting reactant)
Asked by lexi l - Mon Jan 5 08:25:41 2009 - - 4 Answers - 0 Comments