Friday
April 18, 2014

Search: AgNO3+ CaCl2

Number of results: 1,586

SI Chemistry
Add a common ion that is not the ion of the desired product; e.g., for chloride analysis one uses AgNO3 to ppt the Cl as AgCl. So you add an excess of AgNO3 (Ag is the common ion).
Friday, November 11, 2011 at 1:03pm by DrBob222

Chemistry
mols CaCl2 = grams/molar mass Substitute and solve for mols. molality = mols/kg solvent Substitute and solve for m. Then delta T = i*Kb*m i = 3 for CaCl2.
Thursday, March 7, 2013 at 1:54pm by DrBob222

AP Chemistry
We add excess Na2CrO4 solution to 68.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.270 grams. What is the molarity of the AgNO3 solution? Answer in units of M
Wednesday, September 11, 2013 at 6:15pm by Gabriella

chem 101
We add excess Na2CrO4 solution to 42.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.590 grams. What is the molarity of the AgNO3 solution? Answer in units of M
Friday, October 18, 2013 at 7:07pm by maria

chemistry 101
We add excess Na2CrO4 solution to 42.0 mL of a solution of silver nitrate (AgNO3) to form insoluble solid Ag2CrO4. When it has been dried and weighed, the mass of Ag2CrO4 is found to be 0.590 grams. What is the molarity of the AgNO3 solution? Answer in units of M
Friday, October 18, 2013 at 7:13pm by maria

AP Chemistry
I don't know how you came up with that answer. Here is how you do it to determine if CaSO4 will ppt. CaCl2 + K2SO4 ==> CaSO4 + 2KCl Both CaCl2 and K2SO4 are diluted by a factor of two since the final volume is 200 mL and each is just 100 mL. (CaCl2) = 0.05 x (100/200) = 0....
Wednesday, April 21, 2010 at 9:32pm by DrBob222

Shawn
How many milliliters of 0.355 M NaF solution are needed to react completely with 24.6 mL of 0.216 M CaCl2 solution? How many grams of CaF2 will be formed? The reaction is CaCl2(aq) + 2NaF(aq) → CaF2(s) + 2NaCl(aq)
Friday, July 8, 2011 at 3:06pm by Chemistry

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

AP Chemistry
3.50% AgNO3 means 3.50g AgNO3/100 g soln. You want 400 g; therefore, you will need 3.50g x (400/100) = ?? g AgNO3. For your second post, this link will work all of your stoichiometry problems. Remember M x L = moles. http://www.jiskha.com/science/chemistry/stoichiometry.html
Monday, October 3, 2011 at 9:19pm by DrBob222

chemistry
From the information available how are you supposed to know if these are in solution or not? KCl(aq) + AgNO3(aq) ==> AgCl(s) + KNO3(aq) OR KCl(s) + AgNO3(s) ==> no reaction
Saturday, February 25, 2012 at 3:51am by DrBob222

Chemistry
AgCl--->Ag^(+)+Cl^(-) AgNO3= 2E^-4L*0.15mol/L AgNO3/(.01L)=mol/L AgNO3=mol/L Ag^(+)=.003M Find Ksp(AgCl) in solubility constant table Ksp(AgCl)=1.77E-10 1.77E-10=[.oo3M Ag(+)][Cl^(-)] solve for Cl^(-) Cl^(-)=5.9E-8M 5.9E-8mol/L*.01L in tank * mm 35.453 g/mol=2*10^-8 g
Saturday, November 20, 2010 at 10:44am by Donna

chemistry
predict the identity of the precipitate that forms. calcium nitrate, Ca(NO3)2, and sodium chloride , NaCl why does the answer come out as no reaction? couldnt it form to be CaCl2 or NaNO3 i thought it had something to do with the fact that Na and NO3 are both soluble so they ...
Tuesday, January 13, 2009 at 8:10pm by lyne

Chemistry
A .972g sample of a Cacl2 2H2O/K2C2O4 H2O solid salt mixture is dissolved in 150 ml of deionized water, previously adjusted to a pH that is basic . The precipitate after having been filtered and air dried has a mass of .375g. what is the percent by mass of CaCl2 2H2O
Tuesday, March 23, 2010 at 8:52pm by Ann

chem
0.1802 g sample of a chlorocarbon compound was analyzed by burning in oxygen and collecting the evolved gases in a solution of sodium hydroxide. After neutralizing, the sample was treated with 39.50 mL of a 0.025 M AgNO3. This precipitated the Cl- as AgCl and left an excess of...
Wednesday, April 11, 2012 at 4:19pm by lara

Chem 22
molecular equation, and net ionic equation of K2SO4 + MgCl2 NiCl2 + NaOH MgCl2 + NaOH K2SO4 + NaOH Ba(OH)2 + NiCl2 Ba(OH)2 + MgCl2 Ba(OH)2 + K2SO4 Ba(OH)2 + NaOH Na2CrO4 + Sr(NO3)2 Na2CrO4 + Al2(SO4)3 K2CrO4 + Sr(NO3)2 K2CrO4 + Al2(SO4)3 AgNO3 + BaCl2 AgNO3 + Na2CrO4 AgNO3 + ...
Friday, December 3, 2010 at 1:35am by Anonymous

Chemistry
If you were to prepare a 1.00 molal solution of CaCl2 beginning with water at 27.0 C, what would the final temperature of the solution be (in C)? Assume that the specific heats of both pure H2O and the solution are the same, 4.18 J/K*g. The dissolution of CaCl2 in water is ...
Monday, April 18, 2011 at 4:20pm by Bob

Chemistry
How many grams of Ag2S can be generated from a mixture of 2.48 g Na2S and 3.41 g of AgNO3 given the following unbalanced reaction: Na2S(aq) + AgNO3(aq) → Ag2S(aq) + NaNO3(aq)
Wednesday, February 8, 2012 at 11:07pm by Jacob

Chemistry
2AgNO3 + K2Cr2O7 ==> 2KNO3 + Ag2CrO4 moles AgNO3 = M x L = ?? moles K2Cr2O7 = 1/2 x moles AgNO3 M K2Cr2O7 = moles/L solve for L and convert to mL.
Saturday, February 19, 2011 at 5:43pm 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

chem
Can someone help me please? 1)Calcium chloride is found in salt mixtures that are used to melt ice on the roads in winter. The dissolving of CaCl2 is exothermic. Provide two reasons why CaCl2 is a good choice for this application as compared to a salt such as NaCl or a salt ...
Thursday, April 19, 2007 at 5:01pm by Mary

Chemistry Balancing
Mary, The point is that you need the parentheses to show that it is two OH- ions in Ca(OH)2 like OH Ca OH not H Ca OH Maybe it would be easier if you wrote it as two separate reactions Ca++ + 2 Cl- ---> CaCl2 2 H+ + 2 (OH)- ---> 2 H2O ------------------------- add those ...
Tuesday, December 25, 2007 at 6:27am by Damon

Chemistry
CaCO3 + 2HCl ==> CaCl2 + H2O + CO2 Convert 29.0g CaCO3 to mols. mol = grams/molar mass. Convert 13.0g HCl to mols. Using the coefficients in the balanced equation, convert mols CaCO3 to mols CaCl2. Do the same for mols HCl to mols CaCl2. It is likely that the two values ...
Sunday, September 22, 2013 at 7:09pm by DrBob222

chem 103
No. The dilution formula is c1v1 = c2v2 where c = concn v = volume 8*v1 = 0.750*175 Solve for v1 = approximately 16 mL. 3CaCl2 + 2Na3PO4 ==> Ca3(PO4)2 + 6NaCl mols CaCl2 = grams/molar mass = estimated 0.002 mols Na3PO4 = M x L = estimated 0.0012. Now convert mols Na3PO4 and...
Sunday, July 14, 2013 at 1:35pm by DrBob222

Chemistry
I thought I worked this for you a couple of nights ago. moles Cacl2 in 10 g CaCl2 = 10/111 = 0.090 moles CaCl2 moles Cl in that is 0.090 x 2 = 0.180 moles Cl. moles NaCl in 10 g NaCl = 10/58.44 = 0.171 moles total moles Cl = 0.171 + 0.180 = 0.351 M = moles/L = 0.351 moles Cl/0...
Monday, July 12, 2010 at 9:33am by DrBob222

chemistry
This is a limiting reagent problem. Write and balance the equation. NaCl + AgNO3 ==> AgCl + NaNO3 moles NaCl = M x L = ? moles AgNO3 = M x L = ? Use the coefficients in the balanced equation to convert mol NaCl to mol AgCl. Do the same for AgNO3. You get two answers; only ...
Sunday, February 26, 2012 at 5:50pm by DrBob222

chem
Initially, you have 1.00g of BaCl2 (mm= 208.23) and 1.00g of AgNo3 (MM=169.88). How many moles of AgNO3 do you have initially in the mixture?
Thursday, March 24, 2011 at 7:00pm by cendy

Chemistry
If 10.0g of CaCl2 and 10.0g of NaCl are dissolved in 100.0mL of solution, what is the concentration of chloride ions? (the molar mass of CaCl2 is 111.0g/mol; the molar mass of NaCl is 58.44g/mol. I found individual molar mass of: Ca-40.08 Cl-35.45 Na-22.99 So I divided 10g ...
Sunday, July 11, 2010 at 12:57pm by Casey

Chemistry
2-bromo-2-methybutane reacts with AgNO3 to form AgBr precipitate. If NaI is present, it also reacts reacts with AgNO3 to form AgI precipitate. When you observe the precipitate, how would you know what caused it?
Sunday, November 16, 2008 at 1:30pm by GK

chemistry
In the following experiment, a coffee-cup calorimeter containing 100mL of H2 is used. The initial temperature of the calorimeter is 23.0 C . If 3.40g CaCl2 of is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of ...
Thursday, November 24, 2011 at 11:44pm by Yuli

Chemistry
This is a Lab Report on Stoichiometry and Gravimetric Analysis. I have a balance equation for the reaction. Na2Co3+ CaCl2--> CaCo3+ 2NaCl. (CHALK) I think I know the Precipitate: Na2Co3 and CaCl2 - Calulate the dry precipitate and the mole of the precipitate produced in the...
Sunday, October 28, 2007 at 5:56pm by Monte;

chemistry
1.30 M means 1.30 moles / liter of solution 1 mole CaCl2 = 111.0 g (How do you get that?) 1.30 mol x 111 g = 144.3 g CaCl2 1.00 L = 1000 mLs volume x density = mass: 1000 mLs x 1.1 g/mL = 1100 grams solution (total) 1100 g - 144.3g = 955.7 g H2O ---> 0.9553 kg H2O molality...
Tuesday, June 16, 2009 at 4:56pm by GK

Chemistry
Which two solutions, when mixed together, will undergo a double replacement reaction and form a white, solid substance? 1. NaCl(aq) and LiNO3(aq) 2. KCl(aq) and AgNO3(aq) 3. KCl(aq) and LiCL(aq) 4. NaNO3(aq) and AgNO3(aq) I know the answers 2 but I have no idea why.. thanks.
Wednesday, January 23, 2008 at 12:52pm by TJ

chemistry
In the following experiment, a coffee-cup calorimeter containing 100ml of H2O is used. The initial temperature of the calorimeter is 23 degrees celcius. If 7.20g of CaCl2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The ...
Friday, October 3, 2008 at 11:23pm by kayla

Chemistry
1. Convert 20.8 g CaCl2 to moles (Diveide by the formula mass of CaCl2). 2. The heat given off is: ∆H(sln) = (1258 J/C)(37.1C - 25.0C) 3. Divide the answer in step #2 by the answer in #1 to get the joules/mole. This value is negative since the heat is given off.
Saturday, October 18, 2008 at 10:37pm by GK

Chemistry
What do you mean by neutral? For example, CaCl2 has as many + charges on the Ca ion as - charges on the Cl ion. The same is true for B, C, D, E, Or could you mean neutral acid/base. The only one is CaCl2. Or some other meaning for neutral?
Thursday, October 24, 2013 at 1:04am by DrBob222

Chemistry
Hi I hope you can understand this...the Na ion is attached to the oxygen using ionic bonding. The \/ are meant to symbolize the hydrocarbon chain. The || is a double bond that bonds oxgen to carbon. O || Na O/\/\/\/\/\/ + CaCl2 -> ? + NaCl To give you some background, it ...
Thursday, January 20, 2011 at 5:36pm by Me

chemistry
How do the boiling points of 3.0 m C6H12O6 and 3.0 m CaCl2 compare? A. The boiling point of 3.0 m C6H12O6 is higher. B. The boiling point of 3.0 m CaCl2 is higher. C. They are the same. D. The difference cannot be determined from the information given. I think the answer is D...
Thursday, September 15, 2011 at 2:18pm by jasmine

chemistry
Calculate mols and concns and determine if Ksp is exceeded. mols CaCl2 = M x L = 0.24 M x 0.025 L = 0.006 and there are two Cl^- ions so that is 0.012 mols Cl^-. mols AgNO3 = 1.5 M x 0.045 L = 0.0675 mols Ag^+. (Ag^+) = mols/L = 0.0675/0.070 L = 0.964 M Cl^-) = 0.012/0.070 = 0...
Thursday, April 3, 2008 at 10:48pm by DrBob222

Chemistry
A small correction. CaCl2 added to CuSO4 will form CaSO4 which is a white ppt and relatively insoluble in water.It is listed in most tables as being slightly soluble. Cu(NO3)2 and CaCl2 don't produce CaSO4 and Ca(NO3)2 is quite soluble. I'll be happy to look over your ...
Wednesday, October 8, 2008 at 10:48pm by DrBob222

chemistry
2AgNO3 + Na2CO3 ==> Ag2CO3 + 2NaNO3 mols AgNO3 = M x L = ? Convert mols AgNO3 to mols Ag2CO3. g Ag2CO3 = mols Ag2CO3 x molar mass.
Saturday, March 23, 2013 at 7:12pm by DrBob222

Chemistry
mols AgNO3 = M x L = ? Using the coefficients in the balanced equation, convert mols AgNO3 to mols NaCl. Now convert mols NaCl to grams. g = mols x molar mass.
Friday, February 21, 2014 at 12:10am by DrBob222

chemistry urgent!!!
Step 1. Write a balanced equation. Mg + 2AgNO3 ==> 2Ag + Mg(NO3)2 Step 2. Convert what you have (61.9 g AgNO3) to mols. # mols = grams/molar mass 61.9/170 = 0.36 Step 3. Using the coefficients in the balanced equation, convert mols of what you have (mols AgNO3) to mols of ...
Friday, February 29, 2008 at 7:21am by DrBob222

Gen chem 1
According to the following reaction, what volume of 0.25 M CaCl2 solution is required to react exactly with 50.0 mL of 0.20 M Pb(NO3)2 solution? CaCl2(aq) + Pb(NO3) (aq)- PbCl2(s) + 2 KNO3(aq).
Monday, March 11, 2013 at 9:36am by jenni

Chemistry
How many milliliters of 0.277 M AgNO3 solution are needed to react completely with 47.1 mL of 0.278 M NaCl solution? How many grams of AgCl will be formed? The reaction is NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)
Tuesday, November 1, 2011 at 10:31am by Lynn

chemistry
In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial temperature of the calorimeter is 23 degrees Celsius. If 4.00 g of CaCl2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The ...
Monday, October 19, 2009 at 4:50pm by Katherine

SCIENCE/CHEM
HCl + Ca(OH)2 ==> CaCl2 + H2O I start by seeing 2 Cl on the right. I fix that with a 2HCl 2HCl + Ca(OH)2 --> CaCl2 + H2O So Ca and Cl now balance. That leaves only H and O. I usually count what I have on the left (since the 2 for HCl and 1 for Ca(OH)2 seem to be ok.) I ...
Wednesday, May 12, 2010 at 10:34pm by DrBob222

chemistry
How much heat must be added to the water to move the T from Iinitial = 10 C to Tfinal = 16.4 C. That will be q = massH2O x specific heat water x (Tfinal-Tinitial) = ?? Knowing that 1 mol CaCl2 dissolving in water will produce 82.8 kJ, how many mols CaCl2 are required. Then ...
Monday, November 17, 2008 at 7:29pm by DrBob222

chemistry
If 19.7 g of CaCl2 are present in 200 mL of aqueous solution, what is the concentration in terms of the following? a. molarity 100 M CaCl2 b. weight/volume percent 0.1 % (w/v) c. parts per thousand 100 ppt d. parts per million 10E4 ppm e. parts per billion 10E7 ppb
Wednesday, February 22, 2012 at 6:30pm by krystal

Chemistry
37.5ml 1L .152 mol NaCr 1 mol AgNO3 -------|-------|-------------|-------- 10^3ml 1L 1 mol Na2cr 1 L 25ml -------------|-------- 1 mole AgNo3 10^3ml
Thursday, November 15, 2012 at 4:55pm by Chels

Chemistry
AgNO3+FeCl3 --> AgCl+Fe(NO3)3 In an experiment, it was planned to mix a solution containing 25 g of AgNO3 with another solution containing 45 g of FeCl3. a) What is the maximum number of moles of AgCl that could be obtained? I already found the limiting reagent, I just need...
Friday, March 9, 2012 at 1:53am by Jamie

chimistry
3.24 moles of Cl2 will, in the right kind of reaction, produce the equivalent of 3.24 moles of CaCl2. 1 mole of CaCl2 has a mass of ?? grams (look up the molar mass). Therefore, 3.24 moles should be ?? grams.
Thursday, February 18, 2010 at 10:10pm by DrBob222

Chemistry
Note the reaction produces 81.5 kJ energy per 1 mol CaCL2. Convert that to kJ/1 g CaCl2. q = mass x speific heat water x (Tf-Ti). mass = 14.0 sp.h. water is in the problem. Tf is final T Ti is initial T.
Saturday, November 10, 2007 at 10:08am by DrBob222

AP Chemistry
Setting up an ICE chart is a great move; however, I don't get the answers you have (perhaps I just can't red the spacing since the board doesn't recognize anything over one space). At any rate, the equation is right but the Ksp is wrong. CaCl2 + K2SO4 ==> CaSO4 Since I can'...
Wednesday, April 21, 2010 at 10:06pm by DrBob222

Chemistry
A solution is prepared by placing 27.8 g of KCl in a 0.700 L volumetric flask and adding water to dissolve the solid, then filling the flask to the mark. What is the molarity of an AgNO3 solution if 22.1 mL of the KCl solution react exactly with 43.0 mL of the AgNO3 solution?
Sunday, March 2, 2014 at 10:21pm by Ali

Science
CaCl2 is three particles per molecule. deltaTemp=1.3=.52*molality solve for molality, then molality= moles/1000 solve for moles, then finally,grams of CaCl2 from moles, then divide by 1000 to get kg
Wednesday, January 25, 2012 at 8:52pm by bobpursley

Chemistry
Draw a line, something like this, at the bottom of the equation connecting Ag and AgNO3. |_______________|. Write zero under Ag and +1 under Ag of AgNO3. Now draw another line upside down from the one above and place it above the equation connecting N of HNO3 and N of NO2...
Saturday, May 28, 2011 at 10:30pm by DrBob222

AP Chemistry
I decided to set up an ICE chart but I am a little confused. This is what I did: CaCl2 + K2SO4 = CaSO4 + 2 KCl I 0.020M 0.20M 0 0 C -X -X +X +2X E 0.020-x 0.20-x 0+x 0+2x Am I right in saying this? Additional information: Ksp= (CaSO4)(KCl)^2 / (CaCl2)(K2SO4) Ksp= 2.4 x 10^ -5
Wednesday, April 21, 2010 at 10:06pm by Bob

Gen chem 1
50.0 mL of 0.20 M Pb(NO3)2 contains .05*.02 = .01 moles according to the equation, each mole of PbNO3 requires one mole of CaCl2. so, since 1L of .25M CaCl2 contains .25 moles, you want .01/.25 = .04L = 40mL
Monday, March 11, 2013 at 9:36am by Steve

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 101
I had a snag from a question I asked yesterday, here is the thread. (My snag being the final post) I am trying to find the theoretical yield for this lab I am working on. The steps to finidng it would be great. In my lab I took 40mls of H2O + 4g of AgNO3+ 8g of NaCL then I ...
Monday, June 8, 2009 at 12:18pm by Gweedo8

Chemistry
Consider the following chemical reaction 2HCL+ Ca(OH)2 CaCl2+2H2O You have mixed 30.00ml of 0.150 M HCl solution with 20.00ml of 0.100m Ca(OH)2 solution what is the molarity of the HCl, Ca( OH)2 and CaCl2 after the reaction has stopped
Tuesday, December 3, 2013 at 8:37pm by Ruffles

Chemistry
a)HCl + NaHCO3 -> NaCl + H2O + CO2 b)2HCl + CaCO3 -> CaCl2 + H2CO3 -> CaCl2 + H2O + CO2 c) Al2O3 + HCl -> AlCl3 + H2O + O2 hmmm a) 1mole b) 2moles 3) 1 ??
Thursday, December 9, 2010 at 9:04am by prince

Chemistry
CaCO3 + 2HCl ==> CaCl2 + H2O + CO2 Convert 27.0 g CaCO3 to mols. Convert 14.0 g HCl to mols. Use the coefficients to convert mols CaCO3 to mols CaCl2. Do the same for HCl. It is likely that the two values will not be the same (mols CaCl2 that is) and one of them must be ...
Wednesday, October 3, 2012 at 12:39am by DrBob222

college chemistry
When solutions of AgNO3 and NaOH react, the balanced molecular equation is 2AgNO3(aq) + 2NaOH(aq) Ag2O(s) + 2NaNO3(aq) + H2O(l) How much Ag2O is produced when 0.200 g of AgNO3 and 0.200 g of NaOH react?
Saturday, August 7, 2010 at 8:07pm by michelle

Chemistry
Can someone please check to see if I am doing this correctly. Thank you :) Q) Calculate the new molarity of a 35mL sample of 0.450 M CaCl2 solution that is diluted with enough water to make 250 mL of solution. A) 0.450 m CaCl2 x 35mL/250mL = 0.063 mL diluted solution
Monday, April 1, 2013 at 5:21pm by Kishwa

chemistry
It looks right to me. The problem gives us 2M and 4M CaCl2 and wants 6L of 2.5M CaCl2. If you mix 1.5L of the 4M and 4.5L of the 2M that will give you 6L of 2.5M. 4.5L + 1.5L = 6L so that's ok. 4.5L x 2M = 9 moles + 1.5L x 4M = 6 moles; the total is 15 moles CaCl2 and since M...
Wednesday, May 11, 2011 at 6:13pm by DrBob222

chemistry ><
Heat energy is released when anhydrous calcium chloride is dissolved in water. CaCl2 (s) CaCl2 (aq) + 83 kJ Calculate the final temperature when 0.01 mol of calcium chloride is dissolved into 100 mL of water initially at a temperature of 18.0 degree celsius.
Thursday, September 8, 2011 at 5:52am by Samantha

chemistry
AgNO3(aq) + KCl(aq) ==> AgCl(s) + KNO3(aq) mols AgNO3 = M x L = ? mols KCl = the same (Look at the coefficients in the balanced equation.) g KCl = mols KCl x molar mass KCl.
Sunday, September 29, 2013 at 4:28pm by DrBob222

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
moles = g/molar mass moles AgNO3 = 3.41/approx 170 = approx 0.02 moles Na2S = 2.48/about 78 = about 0.032 .........2AgNO3 + Na2S ==>Ag2S + 2NaNO3 initial...0.02....0.032......0.....0 Now we take them one at a time. First, 0.02 mol AgNO3 will produce how much Ag2S if we had ...
Wednesday, February 8, 2012 at 11:07pm by DrBob222

Chemistry
The first part is right. The second is not. Yes, M x L = mols = 3.5 x 2L = 7 mols Then mol = g/molar mass 7 = grams/molar mass CaCl2. grams = 7*molar mass CaCl2 = estimated 7*111 = about 777 grams.
Saturday, August 17, 2013 at 5:03pm by DrBob222

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

science
The molecular weight of AgNO3 is 108 +14 +48 = 170 g/mole. 5.00 grams is 5/170 = 0.0294 moles of AgNO3. How many liters of solution do you need if there are 1.25 moles of solute per liter? V = 0.0294 moles/1.25 mole/l = ___ l Convert to milliters of you wish
Thursday, November 11, 2010 at 10:11pm by drwls

Chemistry
0.315*254.6g= Mass of CaCl2 254.6g-Mass of CaCl2=Mass of H2O
Wednesday, January 23, 2013 at 8:37pm by Devron

Chemistry
CaCl2(s) Ca2+(aq) + 2 Cl-(aq) H = -81.5 kJ A 14.0 g sample of CaCl2 is dissolved in 130. g of water, with both substances at 25.0C. Calculate the final temperature of the solution assuming no heat lost to the surroundings and assuming the solution has a specific heat capacity...
Saturday, November 10, 2007 at 10:08am by Joe

Chemistry
1. AgNO3 Soluble, rule 3 2. Ag2SO4 Insoluble, rule 4slightly soluble 3. HgCl2 soluble. Hg2Cl2 is insol. Insoluble, rule 2 4. BaSO4 Insoluble, rule 4 5. CaCl2 Soluble, rule 2 6. NH4OHThis is NH3 + H2O and technically there is no NH4OH ? 7. PbCl4PbCl2 is the common chloride. ...
Monday, April 23, 2012 at 4:25pm by DrBob222

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
When 20.8 g of calcium chloride, CaCl2, was dissolved in water in a calorimeter, the temperature rose from 25.0C to 37.1C. If the heat capacity of the solution and the calorimeter is 1258 J/C, what is the enthalpy change when 1 mol of calcium chloride dissolves in water? ...
Saturday, October 18, 2008 at 10:37pm by Glenna

Chemistry
Please help me with this question: Calculate the theoretical yield amount of CaCl2 that would be required to change the temp of 50ml of water from room temp 20degree to 45 degrees. Heat Capacity H20 is 4.184 Jg^-1deg^-1 and density is 1g/mL. I've already calculated: Q=mc delta...
Monday, March 7, 2011 at 8:47am by Selena

Chem hwk
3CaCl2 + Al2(SO4)3 ==> 3CaSO4 + 2AlCl3 mols CaCl2 = grams/molar mass Convert mols CaCl2 to mols CaSO4 using the coefficients in the balanced equation. Convert mols CaSO4 to g. g = mols x molar mass.
Monday, January 28, 2013 at 2:58pm by DrBob222

Chemistry
I was asked to consider the solubility for hydrated calcium sulfate in HCl. The principal acid my proffesor had posted for the solution was [ CaSO4(hyrdrated) + HCl <--> H30^+ + Ca^2+ + SO4^2- ]. I guess what I'm asking is what happened to the Cl^- and why isn't it ...
Sunday, June 17, 2007 at 8:39pm by john peterson

Chemistry
mols Na ions from NaCl = M x L = ? mols Cl^- from NaCl = M x L = ? mols Ca^2+ = M x L = ? moles Cl^- from CaCl2 = 2 x mols CaCl2. M = moles/L. For Na it is 0.125 x 1.10 = 0.1375 and total volume is 125 mL + 105 mL = 230 mL = 0.230L (Na^+) = 0.597 M Ca^2+ is done the same way. ...
Thursday, June 14, 2012 at 3:25pm by DrBob222

Chemistry/maths
Using the following stock solutions: NaCl, 100mmol KCl, 200mmol CaCl2, 160mmol Glucose, 5mmol Calculate the volumes of each stock solution and the volume of water needed to prepare 100ml of a single solution containing NaCl at 5.0mmol KCl at 2.5mmol CaCl2 at 40mmol Glucose at ...
Thursday, October 22, 2009 at 8:35am by jess

Chemistry
Don't we need to know how much solution we are to prepare? I'll assume we are to use 1 kg water. 1.00 m CaCl2 = 110.983 g CaCl2/kg water. What's the density of the solution. I will assume 1.00 g/mL which probably is not a valid assumption. 81,300 J = 1,000g x 4.184 J/C*g x (...
Monday, April 18, 2011 at 4:20pm by DrBob222

CHEMISTRY
3 moles CaSO4 react with 2 moles AlCl3 (notice it isn't ALCL3) yielding 3 moles CaCl2 (not CaCL2) and 2 moles Al2(SO4)3 [not AL2(SO4)3]
Sunday, June 13, 2010 at 12:05am by DrBob222

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

chem hwk help!
cmon, we just did one of these. convert grams to moles, then use the reaction to figure the relative amounts needed/produced. moles of input = 1.837/111 = .01655 moles CaCl2 Each 3 CaCl2 requires 2 H3PO4 so, 2/3 * .01655 = .011 moles H3PO4 .011 moles H3PO4 = .011 * 98 = 1.081g
Friday, January 25, 2013 at 3:06pm by Steve

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

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
Please help me with this question: Calculate the theoretical yield amount of CaCl2 that would be required to change the temp of 50ml of water from room temp 20degree to 45 degrees. Heat Capacity H20 is 4.184 Jg^-1deg^-1 and density is 1g/mL. I've already calculated: Q=mc delta...
Monday, March 7, 2011 at 2:28am by Selena

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

Chemistry
CaCO3 ==> CaCl2.6H2O 1 mol CaCO3 will produce 1 mol CaCl2.6H2O so 4.0 mols CaCO3 will produce......
Tuesday, April 3, 2012 at 3:23am by DrBob222

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

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

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