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April 16, 2014

Search: saturated solution of Mg(OH)2 is prepared having a large excess of Mg(OH)2. Sn(NO3)2 is added to the solution

Number of results: 54,473

Chemistry
A saturated solution of Mg(OH)2 is prepared having a large excess of Mg(OH)2. Sn(NO3)2 is added to the solution. Ksp = 1.9 x 10^-11 for Mg(OH)2 and Ksp = 6.0x10^-26 for Sn(OH)2. What [Sn2+] is required so that the [Mg2+] in solution will be 0.15 M?
Saturday, March 26, 2011 at 6:16pm by Nikki

chemistry
A saturated solution of Mg(OH)2 is prepared having a large excess of Mg(OH)2. Sn(NO3)2 is added to the solution. Ksp = 1.9 10-11 for Mg(OH)2 and Ksp = 6.0 10-26 for Sn(OH)2.
Tuesday, April 27, 2010 at 4:47pm by Anonymous

Chemistry
A saturated solution of Mg(OH)2 is prepared having a large excess of Mg(OH)2. Sn(NO3)2 is added to the solution. Ksp = 1.8 10-11 for Mg(OH)2 and Ksp = 5.1 10-26 for Sn(OH)2. (a) What [Sn2+] is required to start the precipitation of Sn(OH)2? (b) What [Sn2+] is required so that ...
Thursday, March 14, 2013 at 10:19pm by Gregory

chemistry
Mg(NO3)2 + 2NaOH ==> Mg(OH)2 + 2NaNO3 mols Mg(OH)2 formed = 2.97/molar mass Mg(OH)2. 1 mol Mg(OH)2 was formed from 1 molo Mg(NO3)2. M Mg(NO3)2 = mols Mg(NO3)2/L soln Note: 50 mL each soln = 100 mL total or 0.1 L. This calculation is based upon Mg(NO3)2 and NaOH being in ...
Tuesday, September 18, 2012 at 10:39pm by DrBob222

Chemistry
First determine the OH^- already in the solution from Mg(OH)2. .......Mg(OH)2 ==> Mg2+ + 2OH^- I.......solid.......0......0 C.......solid.......x......2x E.......solid.......x......2x Ksp = (Mg^2+)(OH^-)^2 Solve for x = Mg and OH = 2x. Then go through the Sn(OH)2 the same ...
Thursday, March 14, 2013 at 10:19pm by DrBob222

Chemistry
First I want to make it very clear that Mg(NO3)2 and Li2SO4 will NOT react at all and it is folly to try to calculate the M of the Mg(NO3)2 this way. However, the calculation can be done (although it doesn't man anything)so in the spirit of chemistry I will continue. Mg(NO3)2...
Tuesday, February 21, 2012 at 8:09pm by DrBob222

JHU
When excess solid Mg(OH)2 is shaken with 1.00 L of 1.2 M NH4Cl solution, the resulting saturated solution has pH = 9.30. Calculate the Ksp of Mg(OH)2
Friday, November 30, 2012 at 5:39pm by Anzeeel

Chemistry
When excess solid Mg(OH)2 is shaken with 1.00 L of 1.2 M NH4Cl solution, the resulting saturated solution has pH = 9.30. Calculate the Ksp of Mg(OH)2
Saturday, December 1, 2012 at 10:15pm by Anzeel

Chemistry
What minimum number of moles of NH4Cl must be added to 1.0 liter of solution that is 0.10 M in Mg(NO3)2 and 1.0 M in NH3 to prevent precipitation of Mg(No3)2?
Sunday, October 24, 2010 at 5:21pm by Ana

chemistry
When excess solid Mg(OH)2 is shaken with 1.00 L of 1.2 M NH4Cl solution, the resulting saturated solution has pH = 9.30. Calculate the Ksp of Mg(OH)2 I am not sure where to even begin on this problem.
Sunday, March 21, 2010 at 2:56pm by Raj

chemistry
1) List a series of tests that would determine the order of activity (least active to most active) for Zn, Mn, and Ag. 2) What would be the reaction for the addition of excess OH- ions to Mg(NO3)2 and Cu(NO3)2? This is a complex ion forming reaction. Would the complete ionic ...
Sunday, March 2, 2014 at 12:21am by Sandy

Chemistry
2.20 x 10^-3g *(1mole/148.3 g of Mg(NO3)2)= moles of Mg(NO3)2 moles of Mg(NO3)2 *(2 moles of NO3/1 mole of Mg(NO3)2))= moles of NO3 moles of NO3/7.35L=molarity
Thursday, March 14, 2013 at 1:45pm by Devron

GCC
In the activity series, Na is more reactive than Mg, thus it can displace Mg: Mg(NO3)2 + Na -> NaNO3 + Mg Balancing the reaction, Mg(NO3)2 + 2Na -> 2NaNO3 + Mg Hope this helps :)
Tuesday, October 29, 2013 at 2:08am by Jai

science
Nitrate concentrations exceeding 44.3 mg NO3-/L are a concern in drinking water due to the infant disease, methemoglobinemia. Nitrate concentrations near three rural wells were reported as 0.01 mg NO3- N/L, 1.3 mg NO3- N/L, and 20.0 mg NO3- N/L. Do any of these three wells ...
Saturday, August 24, 2013 at 9:02am by cucu

Chem
Determine the number of moles of N atoms in 43.5 g of Mg(NO3)2. Textbook answer: 1.43 mol N My answer: 43.5 g Mg(NO3)x x (1 mol Mg(NO3)2/148.313 g Mg(NO3)2) x (2 mol N/1 mol Mg(NO3)2) = .293 Can tell me where i went wrong?
Sunday, March 8, 2009 at 11:01pm by Bob

chemistry
mols Mg(NO3)2 = M x L = ? mols Mg = same as mols Mg(NO3)2. moles NO3^- = 2x mols Mg(NO3)2 total mol = mols Mg^2+ + mols NO3^-
Tuesday, April 24, 2012 at 10:59pm by DrBob222

chemistry
Frankly, I don't think the problem is worded very well. This is an example of a problem in which the unknown amount of Mg(OH)2 is treated with a known amount of HNO3, which happens to be an excess. Then we determine the excess, subtract from the initial amount HNO3 there, and ...
Wednesday, November 17, 2010 at 4:06pm by DrBob222

Chemistry
Mg(NO3)2 ==> Mg^2+ + 2NO3^- Look at the equation. The equation tells you that you get 1 mol Mg^2+ and 2 mols NO3^- for every 1 mol Mg(NO3)2 that dissolves.
Wednesday, July 31, 2013 at 11:14pm by DrBob222

Chemistry
Mg + 2HNO3 ==> Mg(NO3)2 + H2 mols Mg = grams/molar mass mols Mg(NO3)2 = mols Mg (look at the mole ratio) which is 1 mol Mg to 1 mol Mg(NO3)2. Then grams Mg(NO3)2 = mols x molar mass. For HNO3 needed, convert mols Mg to mols HNO3 and convert mol HNO3 to grams as in the above.
Monday, February 17, 2014 at 6:48pm by DrBob222

Chemistry
What volume of a 0.33 M Mg(NO3)2 solution contains 96 g of Mg(NO3)2?
Tuesday, November 30, 2010 at 7:10pm by Kelsey G

Chemistry
0.161 M Mg(NO3)2. There are two nitrate ions in one molecule of Mg(NO3)2; therefore, the nitrate is twice the concn of Mg(NO3)2.
Monday, October 22, 2012 at 3:36pm by DrBob222

chemistry
Write a balanced equation for the dissociation of Mg(NO3)2. I wrote Mg(NO3)^2(s)==>Mg^2+(aq)+NO3^3-(aq) That isn't the answer in the book. Can someone explain to me how dissociation works?
Friday, November 1, 2013 at 11:23pm by rose

chemistry
Determine the concentration of a solution of Mg(NO3)2 given the precipitate formed is 2.97 g and there are 50mL of Mg(NO3)2 and 50 mL of NaOH. Please show all work for each step clearly
Tuesday, September 18, 2012 at 10:39pm by LARA

chemistry
What is the molar mass of Mg(NO3)2? How many mols of Mg(NO3)2 are there in 42.5 g? How many mols N are in 1 mol Mg(NO3)2?
Friday, September 19, 2008 at 4:15pm by DrBob222

Chem.
1 mg/mL of Fe x 1000 mL = 1,000 mg in the L container. 1000 mg Fe^+3 = ? mg Fe(NO3)3*6H2O. Just convert 1000 mg Fe^+3 to the hexahydrate. That will be 1000 mg Fe^+3 x (1 mol Fe(NO3)3*6H2O/1 mol Fe^+3) x (349.95 g Fe(NO3)3*6H2O/1 mol Fe(NO3)3*6H2O) x (1 mol Fe^+3/55.85) = ?? ...
Wednesday, February 17, 2010 at 11:05am by DrBob222

chemistry
AgOH ==> Ag^+ + OH^- Mg(OH)2 ==> Mg^2+ + 2OH^- Ksp Mg(OH)2 = (Mg^2+)(OH^-)^2 Ksp AgOH = (Ag^+)(OH^-) Calculate (OH^-) in a saturated solution of Mg(OH)2. That is .........Mg(OHO2 ==> Mg^2+ + 2OH^- I........solid........0.......0 C........solid........x.......2x E...
Sunday, February 9, 2014 at 6:38pm by DrBob222

chemistry
Pb(NO3)2 (aq) + MgCl2 (aq) ----> PbCl2 (s) + Mg(NO3)2 (aq) Pb++ + 2NO3- + Mg++ + 2Cl- ---> PbCl2 + Mg++ + 2 NO3- Mg and NO3 the same both sides, ions so net: Pb++ + 2 Cl- ---> PbCl2 solid
Monday, March 3, 2014 at 3:30pm by Damon

CHEMISTRY
Step 1 is to calculate the concn of the stock solution so you will know what you're starting with. mols Sn(NO3)4 = grams/molar mass Step 2. The M of the stock soln is mols/L soln or mol/0.250. Let's call this y molar. Then dilutions are handled with the dilution formula which ...
Thursday, October 17, 2013 at 9:41pm by DrBob222

Chemistry
Hg2+ + 2Cl- → HgCl Mercuric nitrate was standardized by titrating a solution containing 147.6 mg of NaCl(FM 58.44), which required 28.06 ml of Hg(No3)2 solution. Part a: Find the molarity of Hg(No3)2. I already calculated the molarity to be 0.04500 M Part b: When the ...
Sunday, October 16, 2011 at 11:48pm by Asuna

chemistry
Determine the molarity of nitrate ions in a solution prepared by mixing 25.0 mL of 0.50 M Fe(NO3)3 and 35.0 mL of 1.00 M Mg(NO3)2 Please explain fully do not know where to start?
Monday, December 13, 2010 at 3:32pm by Lisa

Chemistry
Mg ==> Mg^+2 + 2e Eo = 2.37 = E1 Sn^+2 + 2e ==> Sn Eo = -0.14 = E2 ------------------------------- Mg + Sn^+2 ==> Mg^+2 + Sn Eo = E1+E2 = 2.23 v. Note that you should look up these values. My tables are 20 years old. Ecell = Eocell - (0.0592/n)*log Q. Q is where you ...
Tuesday, May 11, 2010 at 2:32pm by DrBob222

Chemistry
A reference solution is to be prepared with 5 PPM parabenzopyrene (molecular weight = 252). The quantity of parabenzopyrene required for preparing one litre 5 PPM solution is (A) 252 mg (B) 25.2 mg (C) 5 mg (D) 252 g
Tuesday, June 25, 2013 at 6:27am by rohit

chemistry
You are tasked with preparing a 500mL nutrient solution containing 5mg/L of phosphorous (P), 3mg/L nitrate (NO3 -) and 100 mg/L chloride (Cl-). To make this solution, you have powdered sodium chloride, a 100 mg/L solution of phosphorus, a 1000 mg/L of sodium nitrate (NaNO3) ...
Monday, January 13, 2014 at 4:57pm by Bruce

Chemistry
Do you know how to tell? Look up the activity series. You will find a long list of metals there. If Zn is ABOVE any ion, Zn will replace (displace) the ion from solution. Zn will not displace any ion ABOVE it in the activity series. For example, Mg will replace Ag^+ from ...
Sunday, March 7, 2010 at 5:58pm by DrBob222

Chemistry
I have to point out, in an aqueous solution, if the Mg is in excess, you have this reaction: Mg(s)+ H2O(l)>>Mg(OH)2(s) + H2 Magnesium hydroxide precipates, as it has very low solubility in water.
Thursday, October 7, 2010 at 8:07pm by bobpursley

Chem 12
Okay, this is a two-part question and the unit is acids and bases. Ka for NH4 is 5.6 x 10^ -10 Kb for NH3 is 1.8 x 10^ -5 1. Determine the pH of a solution prepared by adding 0.0500 mole of solid ammonium chloride to 100mL of a 0.150 molar solution of ammonia. 2. If 0.0800 ...
Tuesday, March 27, 2007 at 12:21am by Kevin

Chemistry
What is the molarity of nitrate ions in a solution containing 2.20 mg of Mg(NO3)2 dissolved in 7.35 L of water?
Thursday, March 14, 2013 at 1:45pm by Maddie

chemistry
225 mg sample of diprotic acid is dissolved in enough water to make 250mL solution.the pH of this solution is 2.06. a saturated solution of calcium hydroxide Ksp=1.6E-6 Then the saturated solution of calcium hydroxide is prepared by adding excess calcium hydroxide to pure ...
Sunday, March 2, 2008 at 2:09pm by timmathy

chemistry
For a,how much NaCl is needed? 100 mg/L is what you want, and you want 500 mL; therefore, you need 100 mg/L x 0.500 L = ? mg. For b, You want 500 mL of 5 mg/L; therefore, you need 5 mg/L x 0.5L = 2.5 mg P. You have 100 mg/L solution, how much of that do you need? 100 mg/L x ?L...
Monday, January 13, 2014 at 4:57pm by DrBob222

chem
The solubility product of Mg(OH)2 is 1.2 x 10^-11. What minimum OH- concentration must be attained (for example, by adding NaOH) to decrease the Mg concentration in a solution of Mg(NO3)2 to less than 1.0 x 10^-10 M (molar)?
Saturday, November 1, 2008 at 3:14pm by Mischa

chemistry
a 205 mg sample of diprotic acid is dissolved in enough water to make 250 ml of solution. The pH of this solution is 2.15. A saturated solution of calcium hyrdoxide (Ksp=1.3*10^-6) is prepared by adding excess calcium hydroxide to water and then removing the undissovled solid ...
Sunday, March 4, 2012 at 8:09pm by cat

chemistry
And you are correct. When calculating molar mass Fe(NO3)3 it is atomic mass Fe + 3*mass NO3^-. And for Mg(NO3)2 it is atomic mass Mg + 2*mass NO3^-. I don't see that we used the molar mass of either of these substances in this problem. The problem asks for molarity of the ...
Tuesday, December 14, 2010 at 4:16pm by DrBob222

Algebra
An asthma medicine is to be prepared from an elixir with a drug concentration of 5 mg/mL and a cherry flavored syrup that is to be added to hide the taste of the drug. How much of each must be used to prepare 100 mL of solution with a drug concentration of 2 mg/mL?
Monday, September 16, 2013 at 6:09pm by Serena

Algebra
An asthma medicine is to be prepared from an elixir with a drug concentration of 5 mg/mL and a cherry flavored syrup that is to be added to hide the taste of the drug. How much of each must be used to prepare 100 mL of solution with a drug concentration of 2 mg/mL?
Monday, September 16, 2013 at 8:19pm by Serena

Gr.11 Chemistry
Is this right? Balanced: 3 Mg(s) + 2 Al(NO3)3(aq) = 2 Al(s) + 3 Mg(NO3)2(aq) Total Ionic Equation: 3 Mg(s) + 2 Al +3 (aq) + 6NO3 -1 (aq) = 2 Al(s) + 3 Mg+2 (aq) + 6NO3 -1 (aq) Net Equation : 3 Mg(s) + 2 Al +3 (aq) = 2 Al(s) + 3 Mg+2 (aq)
Thursday, March 17, 2011 at 7:55pm by Kwan

Chemistry
A 205 mg sample of a diprotic acid is dissolved in enough water to make 250.0 ml of solution. The pH of this solution is 2.15. A saturated solution of calcium hydroxide (Ksp= 1.3 x 10-6) is prepared by adding excess calcium hydroxide to water and then removing the undissolved ...
Monday, February 25, 2013 at 6:27pm by Summer

Chemistry 114
Write the balanced ionic equations for the following precipitations and complex forming reactions: a) AgNO3 solution + copper sulphate solution b) copper sulphate solution + lead nitrate solution c)CoCl2 solution + conc. HCl d) Zinc chloride solution + NaOH solution, added ...
Monday, April 12, 2010 at 6:01am by Chenny

CHEMISTRY!
Specifications for lactated Ringer's solution, which is used for intravenous (IV) injections, are as follows for each 100mL of solution: 285-315 mg NA+ 14.1 - 17.3 mg K+ 4.9 - 6.0 mg Ca2+ 368 - 408 mg Cl 231 - 261 mg lactate, C3H5O3 How would you make this solution if you have...
Tuesday, August 30, 2011 at 2:44am by Kevin

Chemistry
I have a certain concentration of NaCl (in mg/L). I have to convert it to ppm Na+. I read some of the previous posts, and I understand that if I don't know the density, I should assume that 1ppm = 1mg/L. Does this also apply to ppm Na+ since there is 1 Na+ ion for each ...
Tuesday, February 20, 2007 at 1:23pm by Maggie

Physical Science
The molecular equation is 2HNO3 + Mg(OH)2 ==> Mg(NO3)2 + 2H2O. If these are in solution (the problem doesn't say that but the implication is that they are, then 2HNO3(aq) + Mg(OH)2(aq) ==> Mg(NO3)2(aq) + 2H2O(l) Net ionic equation is 2H^+ + 2OH^- ==> 2H2O and if you ...
Monday, February 20, 2012 at 9:38pm by DrBob222

Chemistry
I would do this. (Mg^+2)(OH^-)^2 = 1.9E-11 Plug in 0.15 for Mg and solve for (OH^-)^2. Then (Sn^+2)(OH^-)^2 = 6.0E-26 Plug in (OH^-)^2 from above and solve for (Sn^+2)
Saturday, March 26, 2011 at 6:16pm by DrBob222

College Chemistry
Suppose you take 2 mL of boiling A. X = 2 mL x 200 mg/mL = 400 mg so all of X will dissolve. Y = 2 mL x 200 mg/mL = 400 mg so all of Y will dissolve. Now cool the solution to room temperature. How much X and Y will recrystallize? 2 mL x 20 mg/mL = 40 mg X will stay in solution...
Monday, January 21, 2013 at 11:49pm by DrBob222

Chemistry
How many Mg WHAT? g Mg = 32*0.0045 = ? mols Mg = ?g Mg/atomic mass Mg = y #atoms Mg = y mols Mg*6.02E23 = ??
Wednesday, October 9, 2013 at 4:14pm by DrBob222

chemistry
Mg(OH)2 + 2HCl ==> MgCl2 + 2H2O mols HCl = M x L = ? mols Mg(OH)2 = 1/2 that (use the coefficients in the balanced equation.) M Mg(OH)2 = mols Mg(OH)2/L Mg(OH)2. Then M OH^-) = twice M Mg(OH)2 because there are two OH^- ions/Mg(OH)2.
Thursday, October 3, 2013 at 7:13pm by DrBob222

Chemistry
Which of the following substances will oxidize Sn(s) to Sn^2+? a) Cu(s) b) Cl2(g) c)Cl-(g) d) Mg(s) e) Cu^2+(aq) f) Mg^2+(aq)
Monday, April 4, 2011 at 6:15pm by Lauren

Chemistry
Nope, you can't directly convert the 1.27 g sample to moles of Mg because it is impure or not 100% Mg. Since there is some HCl left after the reaction, the impure Mg is the limiting reactant and HCl is in excess. Note that the Mg used was impure. To get the number of moles, we...
Sunday, September 22, 2013 at 10:28pm by Jai

Chemistry
No. Mg + Ca(NO3)2>>Mg(NO3)2 + Ca is the likely answer as Mg is more active than Ca and will replace it. This is a "book" problem, as the reaction is not likely to occur in nature.
Sunday, May 31, 2009 at 7:59pm by bobpursley

Physics
A pendulum is composed of a mass m suspended from the ceiling by a massless string of length L. If the mass is pulled back so that it is raised an amount L/4 and then released, what is the tension on the string at the bottom of the swing? A.3 mg B.4 mg C.2 mg D.5/2 mg E.3/2 mg...
Friday, May 4, 2012 at 6:20pm by Chris

chemistry
Assume that 50ml of 0.01M edta solution were added to 25ml of co solution and the excess edta required 20ml of 0.005M mg solution. Calculate ppm co+ present. The answer 942ppm Bob helps me
Saturday, March 2, 2013 at 11:46am by Fai

chemistry
How many moles of Mg do you have? (25/23.5 ?) how many moles of H do you have? (.075*2) The reaction: Mg+2HNO3>>H2+Mg(NO3)2 so is the nitric acid moles twice the Mg? If moles Nitric acid is >2*moles Mg, then Mg is limiting.
Wednesday, February 17, 2010 at 8:11pm by bobpursley

Chem
You've just prepared a solution by transferring 20.0 g of glucose into a 1.0 - L volumetric flask, and adding water to the mark. Calculate the concentration of the glucose solution in terms of millimoles/Liter, mg/mL, and % (m/v). Ok, I think i'm overwhelmed by the wordinng of...
Monday, September 7, 2009 at 10:53pm by Britt

Chemistry
you add excess sodium sulfate to a solution of a soluble barium compound in order to precipitate all of the barium ion as barium sulfate, BaSO4. Suppose a 458 mg sample of the barium compound is dissolved to create the solution. Then when the sodium is added, 513 mg of barium ...
Monday, March 12, 2012 at 6:04pm by India

Chemistry
you add excess sodium sulfate to a solution of a soluble barium compound in order to precipitate all of the barium ion as barium sulfate, BaSO4. Suppose a 458 mg sample of the barium compound is dissolved to create the solution. Then when the sodium is added, 513 mg of barium ...
Monday, March 12, 2012 at 6:41pm by India

Chemistry
Will Zinc react with Zn(NO3)2, Cu(NO3)2,Pb(NO3)2, Mg(NO3)2, AgNO3, Al(NO3)3, or Fe(NO3)3
Thursday, January 27, 2011 at 1:41am by Jenn

Chemistry
Consider the following equilibrium: Mg(OH)2 (s) <--> Mg 2+ (aq) + 2OH-(aq) What happens to the amount of solid Mg(OH)2 when some HCl is added? It decreases because it has least entropy? So in the reaction, both the concentration of Mg(OH)2 and OH- decreases?
Sunday, February 7, 2010 at 10:49pm by sh

Chemistry
In a lab that I am doing I am having difficulty in determining this: What are two indications that suggest a reaction has taken place when HCI was added to Mg? In this lab I am taking 0.1 Mg and adding it to the flask, then recording the temperature of the Mg which is (21 C). ...
Saturday, February 14, 2009 at 6:54pm by Anonomyous

Chemistry
"What is the concn of the resulting solution" is an open ended question. What units? The easy answer is it's 0.1 mg/50 mL but that probably isn't the unit you want. Since you want to prepare a dilute solution in ppm I thin the answer probably should be in ppm 1 ppm = 1 mg/L so...
Thursday, November 8, 2012 at 1:58pm by DrBob222

physics
Lets do this the long way. In the water, the net force=mass*acceleration (neglecting considerable friction). but net force=bouyantforce-mg or bouyant force=mass*g* 1/3 +mg=4/3 mg this bouyant force does not change. So to go now, bouyant force-(m+Masssand)g=-1/4 (M+m) 4/3 mg-mg...
Monday, August 15, 2011 at 1:02pm by bobpursley

Chemistry
I am having a little trouble understanding exactly what you did and exactly what you want to calculate? Generally, these experiment are to determine q/g or q/mol for a substance, in this case q/g for Mg and q/g for MgO. The other thing I'm having trouble with is you had 0.15 g...
Monday, February 13, 2012 at 3:50pm by DrBob222

Chemistry
Specifications for lactated Ringer's solution, which is used for intravenous (IV) injections, are as follows for each 100mL of solution: 285-315 mg NA+ 14.1 - 17.3 mg K+ 4.9 - 6.0 mg Ca2+ 368 - 408 mg Cl 231 - 261 mg lactate, C3H5O3 How would you make this solution if you have...
Tuesday, August 30, 2011 at 12:06am by Kevin

Chemistry
Excess sodium sulfate is added to exactly 50 mL of a solution containing an unknown amount of silver(I) cation. Determine the concentration of the silver ion in this solution if 3.54 mg of a solid is isolated.
Monday, July 11, 2011 at 2:38pm by Anonymous

AP Chem
A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to precipitate all of the barium ion as barium sulfate, BaSO4. How many grams of barium ion are in a 458-mg sample of the barium compound if a solution of the sample gave 513 mg BaSO4 ...
Monday, November 3, 2008 at 11:02pm by Anna

chemistry
the activity series of metals is: Au < Ag < Cu < Sn < Cd < Zn < Al < Mg < Na < Cs which reaction below occutrs spontaneously upong mixing the reageant shown? a) Sn(s) + Al3+ (aq)-> sn2+(aq) + al(s) b) sn(s) + zn 2+ (aq) -> sn 2+ (aq) +zn (s) c...
Sunday, October 23, 2011 at 7:54pm by Dani

chemistry
mols Mg(OH)2 = 1.8 g/molar mass Mg(OH)2 = ?? mols Mg = mols Mg(OH)2 since one Mg atom is in one Mg(OH)2. g Mg = mols Mg x atomic mass Mg = xx %Mg = (mass Mg/mass sample)*100 = (xx g Mg/2.3 g sample)*100 = ?? Post your work if you get stuck.
Monday, October 15, 2007 at 9:03pm by DrBob222

Chemistry
A saturated Ni(OH)_2_ can be prepared by dissolving 0.239 mg of Ni(OH)_2_ in water to make 500.0 mL of solution. What is the Ksp for Ni(OH)_2_?
Thursday, March 15, 2012 at 11:17pm by Shane

Chemistry
Would Mg+Ca(NO3)2 yield Mg(NO3)2)+Ca? Thank you for checking.
Monday, June 1, 2009 at 8:45pm by Narasaq

Math
Rename: 74 mg = ?mg A. 740 mg B. 7400 mg C. 7.4 mg D. 74 000 mg
Wednesday, August 15, 2012 at 6:56pm by Sammyjoo

Chemistry
How can i calculate the concentration of each ions remaining in the solution after precipitation is complete? ok heres the full question:: 2KOH + Mg(NO3)2 -------------> 2KNO3 + Mg(OH)2 a 100.0 mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0mL of 0....
Monday, August 23, 2010 at 9:43pm by Crickett

chemistry
How can i calculate the concentration of each ions remaining in the solution after precipitation is complete? ok heres the full question:: 2KOH + Mg(NO3)2 -------------> 2KNO3 + Mg(OH)2 a 100.0 mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0mL of 0....
Monday, August 23, 2010 at 11:31pm by Crickett

chemistry
How can i calculate the concentration of each ions remaining in the solution after precipitation is complete? ok heres the full question:: 2KOH + Mg(NO3)2 -------------> 2KNO3 + Mg(OH)2 a 100.0 mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0mL of 0....
Tuesday, August 24, 2010 at 12:03am by Crickett

Chemistry
How can i calculate the concentration of each ions remaining in the solution after precipitation is complete? ok heres the full question:: 2KOH + Mg(NO3)2 -------------> 2KNO3 + Mg(OH)2 a 100.0 mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0mL of 0....
Tuesday, August 24, 2010 at 1:09pm by Crickett

chemistry
a saturated solution of milk of magnesia, Mg(OH)2, has a pH of 10.5. What is the hydronium concentration of the solution? is the solution acidic or basic?
Tuesday, July 14, 2009 at 7:10pm by angela

chem
Excess Ag+ is added to 50 mL of NaBr soln and precipitated out 22.8 mg of AgBr. What is the original concentration of Br- ion in the solution in ppm?
Tuesday, October 26, 2010 at 4:22pm by janie

AP Chemistry
Will a precipitate form when 100.0 mL of a 7.5 10-4 M Mg(NO3)2 is added to 100.0 mL of 5.8 10-4 M NaOH? (Hint: Ksp for Mg(OH)2 = 8.9 10-12) Give the value of Q, to support your answer.
Sunday, December 4, 2011 at 7:43pm by Bill

chemistry half reactions
How do i solve this half reaction with Mg(OH)2(s) --> Mg(s)? Complete and balance the displayed half reaction in basic aqueous solution taking into account the electrons. Mg(OH)2(s) → Mg(s)
Tuesday, November 23, 2010 at 3:25am by Confused

AP Chemistry
Mg(s) + N2(g) + 3O2(g) ==> Mg(NO3)2
Sunday, November 14, 2010 at 7:03pm by DrBob222

chemistry
Mg + 2HNO3 ==> H2 + Mg(NO3)2
Wednesday, January 18, 2012 at 2:19pm by DrBob222

Physics
mg=17.1 N => mg= kx k=mg/x On the moon mg`=kx₁ x₁=mg`/k =m1.6gx /mg=1.6x=1.60.044=0.0704 m
Thursday, January 24, 2013 at 7:44pm by Elena

chemistry
You must mean Mg(OH)2. Mg(OH)2 ==> Mg^+2 + 2OH^- If solubility of Mg(OH)2 is 0.61 g/L, convert that to moles/L. moles = grams/molar mass. Call the solubility in moles/L = S That is Mg(OH)2. Thus (Mg^+2) = S and (OH^-) = 2S. Use that to calculate pOH and pH from that.
Monday, April 19, 2010 at 1:02am by DrBob222

Chemistry
Mg(NO3)2 ==> Mg^+2 + 2NO3^-
Monday, November 8, 2010 at 7:57pm by DrBob222

chemistry
Mg + 2HNO3 = Mg(NO3)2 + H2
Tuesday, April 24, 2012 at 5:04pm by Dev

Chemistry - Solubility
Mg(OH)2 ==> Mg^2+ + 2OH^- Ksp = (Mg^2+)(OH^-)^2 When NH3 is added to the solution of MgCl2 (which is quite soluble) the NH3 reacts with the H2O to form NH4^+ + OH^-. That increases the OH^- enough to form a Mg(OH)2 ppt because Ksp for Mg(OH)2 is exceeded. (SO YOU SHOULD ...
Saturday, March 29, 2014 at 8:40pm by DrBob222

chemistry
identify the reducing and the oxidizing agent for each reaction: a) 2na + br2 = 2nabr b) h2 + cl2 = 2hcl c) 2li + f2 = 2lif d) s + cl2 = scl2 e) n2 + 2o2 = 2no2 f) mg + cu(no3)2 = mg(no3)2 + cu
Tuesday, February 26, 2013 at 8:26pm by mfsl123

Chemistry
I recently performed an experiment in which magnesium oxide formed. I have to find out the simplest whole number ratio of Mg atoms to O atoms. How do I go about doing this? * Chemistry - DrBob222, Tuesday, October 13, 2009 at 11:19pm Mass MgO - mass Mg initially = mass oxygen ...
Wednesday, October 14, 2009 at 3:31pm by Anonymous

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

chemistry
What [Ag1+] is required to start precipitation of AgOH from a saturated solution of Mg(OH)2? Ksp = 2.4 ✕ 10-8 for AgOH and Ksp = 2.6 ✕ 10-11 for Mg(OH)2
Sunday, February 9, 2014 at 6:38pm by Danielle

Chemistry
Write the equation and balance it. Mg + Br2 ==> MgBr2 Convert 3.214 g Mg to moles. moles = grams/molar mass Convert 8.416 g bromine to moles using th same procedure. Since you know bromine is the limiting reagent (since Mg is in excess), work this as in any stoichiometry ...
Friday, January 28, 2011 at 12:25am by DrBob222

Chem II
Just do the ionization. MgSO4 ==> Mg^+2 + SO4^= so i = 2 See the former post for Mg(NO3)2 and NaCl.
Friday, June 6, 2008 at 1:40pm by DrBob222

Chemistry
What is the percentage yield of 10.1g mg reacts with an excess of water and 21.0 g Mg(OH)2 is removed ?
Sunday, January 10, 2010 at 4:25pm by Alondra

Chemistry
What is the percentage yield of 10.1g mg reacts with an excess of water and 21.0 g Mg(OH)2 is removed ?
Sunday, February 5, 2012 at 4:16pm by Alondra

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