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April 21, 2014

Search: Al2(SO4)3

Number of results: 991

chemistry
0.575 moles of Al2(SO4)3 has -------moles of Al3+ ions
Thursday, October 28, 2010 at 11:21pm by Anonymous

Chemistry
Is this question trying to ask, "Will or will not a reaction occur?" There is no reaction between Na^+ and Al2(SO4)3.
Wednesday, May 5, 2010 at 2:19pm by DrBob222

Chemistry
How many moles of sulfur are present in 2.6 moles of Al2(SO4)3?
Monday, March 10, 2014 at 10:29pm by Anthony

Chemistry
3H2SO4+2Al>>Al2(SO4)3 + 6H2 how many moles of sulfuric acid is in 16.01 grams?
Wednesday, July 13, 2011 at 1:41am by bobpursley

Chemistry
Minimum elevation in boiling point is given by a solution of 1. 0.1M Urea 2. 0.1 NaCL 3. 0.1 Mgcl2 4. 0.1M AL2(So4)3
Thursday, April 10, 2014 at 2:18pm by Raghavendra

Chemistry
2Al + 3CuSO4 --> + 3Cu + Al2(SO4)3 * copper(II) sulphate is a hydrate 1.2g of CuSo4 50mL of water 1.0 g of aluminum foil What is the limiting reactant?
Tuesday, February 15, 2011 at 10:04pm by Sylvia

chemisrty
what volume of hydrogen gas at STP can be produced by reacting 15.0 grams of uluminum with sulfuric acid? the equation is: 2Al+ 3H2SO4---> Al2(SO4)3+ 3H2
Thursday, March 29, 2012 at 6:49am by kim

Chemistry
It isn't. NaOH + Al2(SO4)3 forms Al(OH)3 easily. Heating will delay the pptn of Al(OH)3 since it is more soluble at elevated temperatures.
Monday, March 22, 2010 at 5:56pm by DrBob222

Science
3 CaSO4 + 2 AlCl3 Al2(SO4)3 + 3 CaCl2 How many moles of aluminum chloride are required to produce 97.0 g of calcuim chloride in the above reaction?
Thursday, December 16, 2010 at 7:06pm by Catherine

Chemistry
Balance these reactions. A)h2o2-h2o+so2. B)al+cuso4-al2(so4)3+cu. C) mno2+hcl-mncl2+h2o+cl
Sunday, September 25, 2011 at 8:03pm by dineo

chemistry
Suggest chemical reactions that could be used to identify the contents of four unlabeled bottles containing solutions of the following substances: CuSO4, Al2(SO4)3, Pb(NO3)2, and FeSO4.
Sunday, July 3, 2011 at 1:33pm by ABCD

chemistry
For the reaction 2Al+3CuSO4->Al2(SO4)3+3Cu a maximum of ? moles of CO2 could be formed from 6.5 mol of C6H6 and 4.56 mol of O2.
Tuesday, August 30, 2011 at 8:34pm by Yep

Chemistry
For the given reaction, how many moles of water will be formed starting with 45.0 moles of aluminum hydroxide: 2AL(OH)3(s) + 3 H2SO4 > Al2(SO4)3 + 6H2O
Sunday, April 3, 2011 at 7:37pm by Elaine

Chemistry
What is the molarity of a solution made by dissolving 32.654 g of aluminum sulfate, Al2(SO4)3, in water and diluting with water to 125.0 mL total?
Saturday, June 9, 2012 at 1:41pm by Jamie

chemistry
Copper container can be used to store (A) Al2(SO4)3 solution (B) ZnSO4 solution (C) FeSO4 solution (D) All of these
Thursday, March 21, 2013 at 7:43am by PARUSH

CHEM Help!
how to balance these equations S8+Fe- Fe2S3 C6H14+O2- CO2+H2O Al(No3)3+H2SO4 -Al2(SO4)3+HNO3 Bi@S3+HCl-BiCl3+H2S
Tuesday, March 11, 2008 at 4:40pm by Anonymous

Chemistry
What minimum volume of 3.0 M H2SO4 is required to produced 13 L of H2 at STP? Reaction formula: 2Al(s) + 3H2SO4(aq) --> Al2(SO4)3(aq) + 3H2 (g)
Sunday, December 4, 2011 at 8:52pm by Diva

Chemistry
thank you so much! It makes more sense now!! I was clearly on the right path but scared I was making a mistake. For the g of SO4 is it mols Fe x mw of SO4^2-? not mols of SO4^2- x mw of SO4^2-?
Sunday, July 15, 2012 at 4:39pm by ALex

Chemistry PLEASE HELP!
I wonder what is going on here? this is incredibly easy Moles sulfate ions in Al2(SO4)3 Molarity= molessulfateions/liters of solution = 3*.042/.763 moles/liter
Monday, October 11, 2010 at 4:09pm by bobpursley

STOICHIOMETRY
2Al + 3CuSO4 ! Al2(SO4)3 + 3Cu What is the maximum amount of Cu (63.5 g/mol) that could be produced by reacting 20.0 grams of Al (27.0 g/mol) with excess CuSO4?
Thursday, November 4, 2010 at 8:30pm by MAGGIE

chem101
Which of the following solutes in aqueous solution would be expected to exhibit the LARGEST freezing-point lowering (assuming ideal behavior)? A. 0.1 m NaCl B. 0.2 m CH3COOH C. 0.1 m MgCl2 D. 0.05 m Al2(SO4)3 E. 0.25 m NH3
Sunday, June 20, 2010 at 3:47am by joan

chemistry
calculate the necessary amounts of solutes and solvent to make a 4l bottle of antifreeze that will have a 35 degree change in the freezing point of water. soultes are: Al2(SO4), KBr) and Mg(NO3)2.
Sunday, February 13, 2011 at 5:53pm by redgy

chemistry 110
what combinations of Zn, Al, ZnSO4 and Al2(SO4)3 would you make to illustrate that Zn is less active than Al?
Thursday, October 28, 2010 at 9:04pm by shannon

Chemistry 111
Calculate the number of moles of alumunium sulfer, oxygen atoms in 9.00 moles of Alumunium sulfate, Al2(SO4)3?
Thursday, July 14, 2011 at 5:06pm by kee

Chemistry
What is the minimum amount of 5.0M H2So4 necessary to produce 24.1g of H2(g) according to the following reaction? 2Al(s) +3H2So4(aq) produces Al2(So4)3(aq) + 3H2(g)
Saturday, October 2, 2010 at 10:41pm by Anonymous

chemistry
Consider the reaction 2Al + 3CuSO4 = Al2(SO4)3 + 3Cu What is the maximum amount of Cu (63.5 g/mol) that could be produced by reacting 20.0 grams of Al (27.0 g/mol) with excess How do i do this?
Wednesday, November 17, 2010 at 9:40pm by lance

Chemistry
Which of the following pairs of compounds will give a precipitate in a diluted solution? Question 4 options: A) Cu(NO3)2 and Na2CO3 B) KNO3 and NaCl C) MgCl2 and Ba(NO3)2 D) NH4Cl and Al2(SO4)3
Thursday, May 10, 2012 at 11:35pm by Katie

Chemistry
What is the minimum amount of 5.9M H2SO4 necessary to produce 27.7g of H2 (g) according to the following reaction? 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g)
Wednesday, March 5, 2014 at 10:36pm by Jill

science
The molecule Al2(SO4)3 has dissolved in water. What ions are formed and how many ions are formed of each type?
Thursday, March 25, 2010 at 4:55pm by Taylor

Chemistry
In what reaction? This one? Al(OH)3+ 3H2SO4 >>Al2(SO4)3 + 3H2O you need 1/3 the moles, or 2.75/3 moles of aluminum hydroxide.
Wednesday, February 13, 2013 at 10:46am by bobpursley

chemistry
convert grams to moles Each mole of Al2(SO4)3 requires 6 moles of KOH and produces 2 moles of Al(OH)3 Now just plug in your numbers and chug out the answers.
Monday, April 29, 2013 at 2:30pm by Steve

science
I need help to find the answer to this problem: The formula for aluminum sulfate is Al2(SO4)3. Figure the molar mass of aluminum sulfate to the nearest gram?
Tuesday, December 16, 2008 at 7:54am by wizzkid01

chem
Aluminum hydroxide and sulfuric acid neutralize to make water and aluminum sulfate. the first step i have done: Al(OH)3 + H2SO4 -> H2O + Al2(SO4)3 i find this one confusing XD
Monday, November 22, 2010 at 3:58pm by hannah

chemistry
calculate the necessary amounts of solutes and solvent to make a 4 liter bottle of antifreeze that will have a 35 degree change in freezing point of water. solutes are Al2(SO4)3, KBr, Mg(NO3)2
Tuesday, February 8, 2011 at 9:37am by shaknocka lewis

chemistry
calculate the necessary amounts of solutes and solvent to make a 4 liter bottle of antifreeze that will have a 35 degree change in freezing point of water. solutes are Al2(SO4)3, KBr, Mg(NO3)2
Tuesday, February 8, 2011 at 9:37am by shaknocka lewis

Chemistry
"A 25.0% solution of Al2(SO4)3 has a density of 1.75 g/ml. What is the mass of dissolved solute in 40.0 ml of solution?" How would one set this problem up?
Wednesday, December 8, 2010 at 11:30pm by Kathryn

chemistry
I need help finding the net and total ionic for this reation. i know the steps but i keep getting the wrong answer. Al2(SO4)3 (aq) + 6 NaOH (aq) ----> 2 Al(OH)3 (s) +3 Na2SO4 (aq) Category
Wednesday, January 20, 2010 at 11:55pm by jake

AP Chemistry
If you were to draw diagrams (such as that shown on the right) representing aqueous solutions of each of the following ionic compounds, how many anions would you show if the diagram contained six cations? (a) NiSO4, (b) Ca(NO3)2, (c) Na3PO4, (d) Al2(SO4)3
Friday, July 27, 2012 at 11:13am by Anonymous

chemistry lab
calculate the necessary amounts of solutes and solvent to make a 4 liter bottle of antifreeze that will have a 35 degree change in freezing point of water. solutes are Al2(SO4)3, KBr, Mg(NO3)2
Monday, February 7, 2011 at 11:53am by shaknocka

chemistry hw help please ASAP
if 25.2 g of aluminum (AW=27.0) are mixed with 125 g of sulfuric acid(MM=98.1)then how many grams of aluminum sulfate will be produced? 2Al+ 3 H2SO4 --> 3H2 + Al2(SO4)3
Tuesday, November 29, 2011 at 9:31pm by ally

URGENT CHEMISTRY
Which of the following pairs of compounds will give a precipitate in a diluted solution? Question 4 options: A) Cu(NO3)2 and Na2CO3 B) KNO3 and NaCl C) MgCl2 and Ba(NO3)2 D) NH4Cl and Al2(SO4)3 ALL OF THEM ARE SOLUBLE? WHAT DO I DO?
Wednesday, May 15, 2013 at 7:37pm by scilover

Chemisry
What is the minimum amount of 5.2M H2SO4 necessary to produce 22.8g of H2 (g) according to the following reaction? 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) (Please be precise and clear)
Tuesday, February 11, 2014 at 1:12pm by Tyler Jones

Chemistry
An unlabeled bottle containing a solution was found in the lab. It contains one of the following: AgNo3, CaCl2, or Al2(SO4)3. Describe how you would test the solution to determine which solution it is. Include equations in your answer.
Tuesday, December 7, 2010 at 9:11pm by Abigal

Chemistry
What is the percent yield if 4.65g of copper is produced when 1.87g of aluminum reacts with an excess of copper(II) sulfate? 2Al(s)+3CuSO4(aq)==>Al2(SO4)3(aq)+3Cu(s)
Saturday, March 27, 2010 at 7:28pm by Keith

Chem 22
balance molecular formula, total ionic formula and net ionic formula of Sr(NO3)2 + Al2(SO4)3. Thank you
Thursday, December 2, 2010 at 6:57pm by Ivy

Chem 22
balance molecular formula, total ionic formula and net ionic formula of Sr(NO3)2 + Al2(SO4)3. Thank you
Thursday, December 2, 2010 at 6:59pm by Ivy

Chem 101
Your question is a little confusing because of lack of information. If you are trying to make Al2(SO4)3 you must use H2SO4. HCl would produce the chloride and HNO3 would produce he nitrate.
Sunday, July 21, 2013 at 7:58am by DrBob222

medicinal chemistry
PbSO4==> Pb^2+ + SO4^2- ...x.......x......x Ksp = 1.6E-8 = (Pb^2+)(SO4^2-) How advanced is this class? This is quite a difficult problem. The solubility is increased due to the presence of H^+ that reacts with the SO4^2- to produce HSO4^-. To counter that, the SO4^2- from ...
Monday, May 28, 2012 at 1:08pm by DrBob222

Chemistry
In the following equations determine which reactant is the limiting and which reaactant is in excess. 1. KCL + HNO3--->KNO3 + HCL 22.0g 18.3g 2. 2Al(OH)3 + 3H2SO4---> Al2(SO4)3 + 6H2O where there is 25 g of Al(OH)3 and 25g H2SO4.
Monday, August 3, 2009 at 12:29pm by Ashley

chemistry
What is the minimum amount of 5.0M H2SO4 necessary to produce 24.1g of H2(g) according to the following reaction? 2Al(s) + 3H2SO4(aq) produces Al2(SO4)3(aq)+3H2(g). Express your answer using two significant figures.
Saturday, October 2, 2010 at 6:40pm by Anonymous

chemistry
balance the equation FIRST 2Al+ 3H2SO4>>Al2(SO4)3 + 3H2 so, for each mole of acid, you get 1/3 mole of aluminum sulfate. How many moles of sulfuric acid is 250grams?
Monday, November 30, 2009 at 7:31pm by bobpursley

Chemistry Stoichiometry
3H2SO4+ 2Al >> 3H2 + Al2(SO4)3 moles H2=3/2 moles Al=3/2 *massAl/atomicmassAl grams H2=molesH2*2g/mole
Saturday, October 27, 2012 at 4:46am by bobpursley

chemistry urgent
given the reaction: 2 Al + 3 H2SO4 -> Al2(SO4)3 + 3 H2 what volume of H2 gas measured at STP will be produced from 5.4 grams of AL reacting with an excess of H2SO4?
Tuesday, November 30, 2010 at 4:17pm by lianne

Chemistry
If 20.0 grams of Al is placed into a solution containing 115 grams of H2SO4, how many grams of hydrogen gas could be produced? 1. Write the balanced equation. 2Al + 3H2SO4 ==> Al2(SO4)3 + 3H2 2. Convert 20.0 g Al to mols. Remember mols = g/atomic mass 3. Using the ...
Sunday, March 18, 2007 at 8:28pm by Britney

Chemistry
delta T (increase in b.p.) = i*Kb*m All are the same m so that is a constant. kb is a constant. Threfore, it all depends upon i, the van't Hoff factor. i = 1 for urea i = 2 for NaCl i = 3 for MgCl2 i = 5 for Al2(SO4)3. So which will cause the SMALLEST CHANGE?
Thursday, April 10, 2014 at 2:18pm by DrBob222

General Chemistry
Ag2SO4 will begin to ppt when Ksp = (Ag^+)^2(SO4^2-) is exceeded. (SO4^2-) = Ksp/(Ag^+)^2 (SO4^2-) = Ksp/(0.290)^2 Solve for SO4^2- and substitute into Ksp for CaSO4. Solve for Ca^2+
Tuesday, March 18, 2014 at 10:07pm by DrBob222

chemistry
(2xmolarmass SO4/molar mass AlK(SO4)2.H2O)*100. Let me point out that alum is AlK(SO4)2.12H2O. I don't know if your problem is real or a typo. Just look at it to see.
Monday, October 11, 2010 at 4:14pm by DrBob222

chemistry
If 0.755 g of Al3+ dissolved in 960 mL of water reacts stoichiometrically according to the balanced equation, what volume (mL) of 0.0875 M aqueous Cl- is required? Al2(SO4)3(aq) + 3 BaCl2(aq) → 2 AlCl3(aq) + 3 BaSO4(s)
Saturday, April 3, 2010 at 1:01am by eng

Chemistry
Use Ksp to find the concentration of an ion in a saturated solution. Consider a 2.50E-3 M solution of Al2(SO4)3. (a) What [OH^-] is required to initiate precipitation of Al^3+ from the solution? (b) What [OH^-] is required to lower the [Al^3+] to 2.00E-7 M ?
Saturday, July 28, 2012 at 12:04am by Jo

chemistry
Use the same system used for the KBr, Al2(SO4)3. Mg(NO3)2 problem EXCEPT use Kb for the boiling point constant instead of Kf (the freezing point constant). i = 4 for AlCl3 i = 2 for NaCl i = 1 for ethanol i = 3 for MgCl2
Tuesday, February 8, 2011 at 9:36am by DrBob222

Chemistry
How many moles of Sulfur are in 1 mole of Al2(SO4)3 and If the densitry of a noble gas is 1.783 g/L at STP, that gas is.... My guess: Argon? Then theres a question that says "Which as the greater mole.... and it lists things like: 1 mole Of Ar 1 Mole of O How would you figure ...
Friday, February 15, 2013 at 2:36pm by Bryce

Chemistry
Ksp = 2E-8 = (Pb^2+)(SO4^2-) (SO4^2-) = 2E-8/0.02 = 1E=6M Ksp = 1.2E-5 = (Ag^+)^2(SO4^2-) (SO4^2-) = 1.2E-5/(0.045)^2 = 5.9E-3 When Na2SO4 is added incrementally, the first Ksp exceeded will begin to ppt. Ksp for PbSO4 is smaller; therefore, it will be the first ppt. It will ...
Thursday, March 14, 2013 at 11:57pm by DrBob222

chem121
Use the coefficients in the balanced equation to convert moles Al(OH)3 to moles H2SO4. Al(OH)3 + H2SO4 ==> Al2(SO4)3 + H2O You will need to balance the equation.
Monday, June 28, 2010 at 10:35pm by DrBob222

Chemistry
How many atoms of carbon are contained in 47.6 g of Al2(CO3)3? The molar mass of Al2(CO3)3 is 233.99 g/mol.
Thursday, December 6, 2012 at 11:17pm by Emma

CHEMISTRY
Hi!! pls i need help! 1) Mg + Al2(So4)3 2)Fe + CuSO4 3)Mg + CuSO4 4)Zn + CuSO4 5)Mg + FeSO4 FOR ALL 5: a)balanced eq b)ionic equation c) net ionic
Tuesday, February 18, 2014 at 6:57am by Deepa

CHEMISTRY
Here's one last equation I can't balance: Al{subscript 2}(SO{subscript 4}){subscript 3} + ZnCl{subscript 2} -> AlCl{subscript 3} + ZnSO{subscript 4} Please help, and thanks again. Response Al2(SO4)3 + 3ZnCl2 ---> 2AlCl3 + ?___ZnSO4 Why do you have "?____" before the ZnSO4?
Monday, October 13, 2008 at 7:50pm by Anonymous

Chemistry
It makes no difference since mols Fe = mols SO4. g Fe = mols Fe x atomic mass Fe. g SO4 = mols SO4 x molar mass SO4 OR g SO4 = mols Fe x molar mass SO4. You can do it another way, also. g SO4 = g Fe x (molar mass SO4/atomic mass Fe) = ?
Sunday, July 15, 2012 at 4:39pm by DrBob222

Chem
CaSO4 ==> Ca^2+ + SO4^2- Ksp = (Ca^2+)(SO4^2-) = 2.63E-5 From CaSO4 alone; (Ca^2+) = x (SO4^2-) = x Na2SO4 ==> 2Na^+ + SO4^2- You added 5.00E-3 WHAT? Is that molar? If so, then Na^2+ = 2*5.00E-3M and (SO4^2-) = 0.005M Plug all of this into Ksp for CaSO4. Ksp = (x)(x+0....
Sunday, June 5, 2011 at 8:33am by DrBob222

Chemistry
Why is heating required for this formation: 6NaOH (aq) + Al2(SO4)3 (aq) 2Al(OH)3 (s) + 3Na2SO4 (aq)? Wouldn't freezing favour the formation of Al(OH)3 since freezing lower the KSP and more Al(OH)3 would precipitate?
Monday, March 22, 2010 at 5:56pm by Alan

science
2Al+3H2SO4--> Al2(SO4)3+3H2 a.)determine the oxidation number of each element in both the reaction and products of this oxidation-reduction reaction of aluminum and sulfuric acid. b.) what element is oxidized in this reaction? c.) what element reduces in the reaction?
Tuesday, May 3, 2011 at 2:39am by michael

Chemistry
delta T = i*Kf*m Since Kf is constant we can forget that. dT depends upon i and m so i*m for each. NaCl is 0.1*2 = ? for i = 2 CH3COOH is 0.2*1 for i = 1 Al2(SO4)3 is 0.05*5 for i = 5 MgCl2 i = 3 NH3 i = 1 The greatest i*m causes the greatest dT (or the smallest i*m causes the...
Tuesday, February 19, 2013 at 5:44am by DrBob222

Chemistry
The balanced equation is Al2(CO3)3 ==> Al2O3 + 3CO2 Step 1. Convert 1.45 g Al2(CO3)3 to mols. Step 2. Using the coefficients in the balanced equation, convert mols Al2(CO3)3 to mols CO2. Post your work if you get stuck.
Sunday, February 24, 2008 at 7:50pm by DrBob222

Chem 101
why must we used sulfuric acid H2SO4, in 2KAl(OH)4 + H2SO4->2Al(OH)3(s)+K2SO4 +2H2O and 2Al(OH)(s)+3H2SO4->Al2(SO4)3+6H2O rather than hydrochloric acid,HCl,or nitric acid, HNO3?
Sunday, July 21, 2013 at 7:58am by Nida McLaurin

Chemistry 20
There is no equation to balance. Fe2(SO4)3 ==> 2Fe^+3 + 3SO4^-2 So I look at 0.620 M Fe2(SO4)3. So Fe^+3 must be twice that and SO4^-2 must be three times that. right? Don't make problems any harder than they need to be.;-)
Monday, November 15, 2010 at 9:59pm by DrBob222

Chemistry
Consider the reaction 2Al + 3CuSO4 = Al2(SO4)3 + 3Cu What is the maximum amount of Cu (63.5 g/mol) that could be produced by reacting 20.0 grams of Al (27.0 g/mol) with excess CuSO4? 1. 70.6 g 2. 57.2 g 3. 129 g 4. 31.4 g I dont understand how to set it up nor what I do with ...
Thursday, May 6, 2010 at 4:07pm by Annalie

Chemistry
RMM for Al2(SO4)3 =27*2+(32+4*16)*3 =342 RMM for H2O =2+16 =18 Number of water molecules = n Thus 27*2/(342+18n)=0.082 Solve for n to get 18 (to 2 signinficant digits).
Thursday, August 26, 2010 at 10:36pm by MathMate

chem
Did you mean, SrSO4(s) ==> Sr^+2 + SO4^= and SO4^= + H2O ==> HSO4^- + OH^- Then MB: (Sr^+2) = (SO4^=) + (HSO4^-) CB: 2*(Sr^+2)=2*(SO4^=) + (HSO4^-) + (OH^-)
Thursday, November 13, 2008 at 6:16pm by DrBob222

Chemistry
Hi!! pls i need help! 1) Mg + Al2(So4)3 2)Fe + CuSO4 3)Mg + CuSO4 4)Zn + CuSO4 5)Mg + FeSO4 FOR ALL 5: a)balanced eq b)ionic equation c) net ionic PLEASE HELP ME..THERE ARE SOO MANY MORE QUESTIONS I NEED TO DO!!!:(
Tuesday, February 18, 2014 at 3:47am by Deepa

CHEMISTRY
Here's one last equation I can't balance: Al{subscript 2}(SO{subscript 4}){subscript 3} + ZnCl{subscript 2} -> AlCl{subscript 3} + ZnSO{subscript 4} Please help, and thanks again. Responses Al2(SO4)3 + 3ZnCl2 ---> 2AlCl3 + ?___ZnSO4 What is your thinking? What goes in ...
Monday, October 13, 2008 at 8:22pm by Anonymous

chemistry
I should point out that Al2(CO3)3 is not soluble in water. Convert 5.00 g Al2(CO3)2 to mols. mol = grams/molar mass. Convert HBr to mols mols = M x L = ? Use the equation below to determine the limiting reagent and use that information to determine how much of each reagent ...
Monday, April 16, 2012 at 9:20pm by DrBob222

Chemistry
Aluminum reacts with excess copper(II) sulfate according to the unbalanced reaction Al(s) + CuSO4(aq) −→ Al2(SO4)3(aq) + Cu(s) If 2.21 g of Al react and the percent yield of Cu is 40.8%, what mass of Cu is produced? Answer in units of g. I got 7.807423031 g of Cu. ...
Monday, December 3, 2012 at 9:15pm by Anonymous

general chemistry
6.0/molar mass Fe2(SO4)3 = moles Fe2(sO4)3. moles Fe2(SO4)3 x (3 atoms S/1 mole Fe2(SO4)3 = moles S. Then moles S x atomic mass S = grams S.
Wednesday, October 28, 2009 at 12:15pm by DrBob222

chemistry
In aqueous solution Mg consists as an ion +2 . What would the formula of the metal salt magnesium sulfate be?? I think it will be Mg(SO4)2 as Mg is a positive ion +2 and SO4 is negative ion SO4- Can you chceck please?
Saturday, September 1, 2007 at 6:39am by Miki

chemistry
delta T = i*Kf*molality Solve for molality molality = moles/kg solvent solve for moles moles = grams/molar mass Solve for grams. Go through the above for each solute. i for Al2(SO4)3 = 5 i for KBr = 2 i for Mg(NO3)2 = 3
Tuesday, February 8, 2011 at 9:37am by DrBob222

Chemistry
I had a 1.094g of mystery Alum. "AB(SO4)c. dH2O" (I assume that that the Alum is KAl(SO4)2-12H2O but we don't know A B c or d, we do know that mass percent of water is 51.9) After processing the alum (Ba(NO3)2 and HNO3 through a gooch crucible) we end up with 1.739g of BaSO4. ...
Friday, February 1, 2013 at 3:07pm by Graham

chemistry
How many mols Fe2(SO4)3 do you have? That's mols = M x L = ? There are 3 SO4 ions for every 1 mol Fe2(SO4)3.
Tuesday, March 19, 2013 at 9:18am by DrBob222

chemistry
2Al(s) + 3CuSO4(aq) ==>3Cu(s) + Al2(SO4)3 mols Al = 3.86E22/6.022E23 = ?? Using the coefficients in the balanced equation, convert mols Al to moles Cu. Now convert moles Cu to grams. g = moles x molar mass.
Tuesday, November 30, 2010 at 12:50am by DrBob222

gen chem
CaSO4 ==> Ca^+2 + SO4^-2 Ksp = (Ca^+2)(SO4^-2) S = solubility CaSO4; then S = (Ca^+2) S = (SO4^-2) Substitute and solve for S.
Sunday, May 9, 2010 at 5:54pm by DrBob222

chemistry
PV=nRT now to n... 2Al+3H2SO4>> Al2(SO4)3 + 3H2 which would indicate 4.5*3/2 moles H2 But what if the acid were HCl? 2Al+ 6HCl>>2AlCl3 + 3H2 moles of H2: 4*3/2 again.
Sunday, March 14, 2010 at 4:26pm by bobpursley

Chemistry
Which of the following solutes in aqueous solution would be expected to exhibit the smallest freezing-point lowering (assuming ideal behavior? 0.1 m NaCl .2 m CH3COOH .05 m Al2(SO4)3 .1 m MgCl2 .25 m NH3 What would be the steps to picking the right option? Because just picking...
Tuesday, February 19, 2013 at 5:44am by Marcus

Chemistry
An 800-mg sample containing sulfate was treated with slight excess of barium chloride, yielding a precipitate that contained 4.3 mg of co precipitated CaCO3. after ignition and cooling, the precipitate weighed 277.0 mg. Calculate the a.) apparent % SO4 b.) true % SO4 and c.) ...
Sunday, May 12, 2013 at 11:19pm by Jay-jay

chemistry
Aluminum reacts with sulfuric acid, which is the acid in car batteries. If 20.0 grams of Al is placed into a solution contain 115 gram of H2SO4, how many grams of hydrogen ga could be be produced? 2Al + 3H2SO4 ---> Al(SO4)3 + 3H2 20.0g/27 = .741 .741 X 3/2 = 1.11 1.11 X 2...
Tuesday, May 15, 2007 at 4:03pm by mike

chemistry quick help!
In the balanced double replacement reaction of calcium chloride CaCl2 and aluminum sulfate Al2(SO4)3, how many grams of calcium sulfate can be produced if you start the reaction with 4.19 grams of calcium chloride and the reaction goes to completion?
Friday, January 25, 2013 at 2:03pm by thad

Chem hwk
In the balanced double replacement reaction of calcium chloride CaCl2 and aluminum sulfate Al2(SO4)3, how many grams of calcium sulfate can be produced if you start the reaction with 18.97 grams of calcium chloride and the reaction goes to completion?
Monday, January 28, 2013 at 2:58pm by Thad

chemistry
This requires a little imagination. If I call k1 = Ka for HCN it will be HCN ==> H^+ + CN^- k1 = Ka for HCN = (H^+)(CN^-)/(HCN) k2=Ka2 for H2SO4 HSO4^- ==> H^+ + SO4^- k2 = (H+)(SO4^2-)/(HSO4^-) but I want the reverse of this; therefore, 1/k2 = (HSO4^-)/(H^+)(SO4^2-) HCN...
Thursday, March 7, 2013 at 4:57pm by DrBob222

chem
CaSO4(s) ==> Ca^+2 + SO4^= Ksp = (Ca^+2)(SO4^=) I would calculate moles Ca^+2 and moles SO4^=, from an ICE chart you will know which is the limiting reagent and from there which is the common ion (that will be the one in excess). Then calculate the solubility and from there...
Thursday, April 23, 2009 at 5:39pm by DrBob222

Chemistry
This is a nutty question. I suspect the trick is NOT to choose #3. Adding SO4 will increase sulfate. Adding Ba^2+ DECREASES SO4. I can't think of NH containing compound that might do it unless it's a complexing agent. IF it complexed Ba so that Ba^2+ is decreased then SO4 will...
Wednesday, May 29, 2013 at 11:03pm by DrBob222

chemistry
But since Al3+ is only one Al doesn't it equal the moles of the compound, and Al2 would be .24 M? Basically why is Al3+ considered Al2? Isnt Al3 just the ionic version of Al?
Friday, August 26, 2011 at 3:08am by Van M

Chemistry
The problem doesn't ask for you to solve for Ksp. It asks for the solubility of PbSO4 in 1 x 10^-3 M Na2SO4. PbSO4 ==> Pb^+2 + SO4^= Ksp = (Pb^+2)(SO4^=) = 1.8 x 10^-8 If solubility of PbSO4 = S (or x if you wish), then (Pb^+) = S and (SO4^=) = S The Na2SO4 in solution is ...
Monday, April 14, 2008 at 8:06pm by DrBob222

Chemistry: Compound
1) ZnSO4 would it be Zn(SO4) does the polyatomic ion always have to have ( ) ? Parentheses are required ONLY when the subscript for SO4 is not 1. In ZnSO4 the parentheses are not needed. 2) Is Ba(SO4) right? since Ba is 2+ and SO4 is 2- right? Yes, Ba(SO4) is right but the ...
Wednesday, September 8, 2010 at 8:13pm by DrBob222

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