Wednesday
April 23, 2014

# Search: CaSO4

Number of results: 251

Chemistry
CaSO4.2H2O ==> CaSO4 + 2H2O moles CaSO4.2H2O = 15.00 g x (1 mole CaSO4.2H2O/172.172) = 0.08712 moles. moles CaSO4 = same. grams CaSO4 = moles CaSO4 x molar mass CaSO4 = ?? Wait,.. how do I know the moles CaSO4? do I do .08712* CaSO4's gfm?
Monday, November 9, 2009 at 12:09am by c

chemistry
Do you really believe you can start with 15.00 g CaSO4.2H2O, lose the water, and end up with more than 15.00 g? Not likely. It MUST be less than 15.00 grams CaSO4. CaSO4.2H2O ==> CaSO4 + 2H2O moles CaSO4.2H2O = 15.00 g x (1 mole CaSO4.2H2O/172.172) = 0.08712 moles. moles ...
Sunday, November 8, 2009 at 9:56pm by DrBob222

chemistry - Can you please check
I believe you are missing something here. You want mols S = 0.200L x 2M = 0.4 mol S. 0.4mol S x (1 mol CaSO4/1 mol S) = 0.4 mol CaSO4 0.4 mol CaSO4 x molar mass CaSO4 = g CaSO4.
Wednesday, January 23, 2013 at 7:14pm by DrBob222

Chemistry
I recognize this from my post last night. Since you have 0.08712 mole of CaSO4.2H2O AND there is 1 mole CaSO4 per 1 mole CaSO4.2H2O (from the equation), then you must have 0.08712 mole CaSO4. Then moles CaSO4 x molar mass CaSO4 = grams CaSO4. It's approximately 12 grams.
Monday, November 9, 2009 at 12:09am by DrBob222

College Chemistry
Consider the reaction: CaSO4*(1/2H2O) -> CaSO4 + 1/2H2O 1/2 mole of H2O will be released per mole of CaSO4*(1/2H2O) Start by calculating how many moles of CaSO4*(1/2H2O) you start with. The molar mass of CaSO4*(1/2H2O) is 40 + 32 + 64 + 9 = 145 g/mol You start out with 0....
Saturday, October 8, 2011 at 1:13am by drwls

Chemistry 12
The molar solubility of calcium sulphate CaSo4 is 8.43 x 10-3(10 to the power of negative 3) M. Calculate the mass of solid CaSo4 which can be evaporated from 250.0 mL of a saturated solution of CaSO4.
Tuesday, October 8, 2013 at 1:12am by Riann

chemistry
Consider the following reaction CaCl2(aq) + 2Ag2SO4(aq) ! CaSO4(?) + 2AgCl(?) .Which of the following statements is true? 1. Both CaSO4 and AgCl will precipitate from solution. 2. Neither CaSO4 nor AgCl will precipitate from solution. 3. CaSO4 will precipitate from solution, ...
Wednesday, September 19, 2012 at 5:11pm by cheri

chemistry
7.8% CaSO4 by mass means 7.8 g CaSO4/100 g solution. So in 24 g of the solution, there must be 7.8 x (24/100) = ?? g CaSO4 24.0 g solution - g CaSO4 = grams solvent.
Thursday, December 9, 2010 at 4:55pm by DrBob222

chemistry
Calculate the xolubility of calcium sulfate in 0.010 mol/L calcium nitrate at SATP CaSO4 ==> Ca^+2 + SO4^= Ca(NO2)2 ==> Ca^+2 + 2NO3^- = 0.01 M Ksp CaSO4 = (Ca^+2)(SO4^=) = ??. Look up Ksp for CaSO4. Subsitute 0.01 for Ca^+2 and x for SO4^= and solve for solubility CaSO4...
Tuesday, April 8, 2008 at 4:22pm by Dustin

chemistry
CaSO4.XH2O find the mole ratio of water to CaSO4. moleswater=.523/18 molesCaSO4=(2.5-.523)/molmassCaSO4 divide moles water by the moles CaSO4, that is X
Friday, February 19, 2010 at 2:20pm by bobpursley

chemistry
CaSO4 ==> Ca^+2 + SO4^= Ca(NO2)2 ==> Ca^+2 + 2NO3^- = 0.01 M Ksp CaSO4 = (Ca^+2)(SO4^=) = ??. Look up Ksp for CaSO4. Subsitute 0.01 for Ca^+2 and x for SO4^= and solve for solubility CaSO4. Post your work if you get stuck.
Monday, April 7, 2008 at 8:02pm by DrBob222

AP Chemistry
Consider the following reaction. CaSO4(s) Ca2+(aq) + SO42-(aq) At 25°C the equilibrium constant is Kc = 2.4 10-5 for this reaction. (a) If excess CaSO4(s) is mixed with water at 25°C to produce a saturated solution of CaSO4, what are the equilibrium concentrations of Ca2+ and ...
Saturday, October 20, 2012 at 2:02pm by Olivia

Chemistry
I was wondering if you could help me with this problem. If the reaction proceeds with a 96.8% yield, how many kilograms of CaSO4 are formed when 5.34 kg SO2 reacts with an exfess of CaCO3 and O2? Thanks for your help. Write the equation for the reaction and balance it. CaCO3...
Monday, July 9, 2007 at 10:21pm by Ally

Chemistry
..........M2SO4 + CaCl2 --> CaSO4 + 2MCl initial....1.42g....0........0........0 add................xs.......... change.......................1.36 equil......0..................1.36 moles CaSO4 = 136/molar mass CaSO4. moles M2SO4 = moles CaSO4 (1 mole CaSO4 came from 1 mole...
Tuesday, December 13, 2011 at 7:43pm by DrBob222

chemistry
This is a solubility product problem with a common ion. The common ion is sulfate (SO4 in CaSO4 and SO4 in Na2SO4).l let x = solubility in mols/L. .........CaSO4 ==> Ca^2+ + SO4^2- .........solid......x........x Ksp = 4.93E-5 = (Ca^2+) (SO4^2-) For Na2SO4 ==> 2Na^+ + SO4...
Friday, February 15, 2013 at 7:23pm by DrBob222

Chemistry
Solubility CaSO4 = grams/molar mass = mols in 100 mL. Convert mols CaSO4 to g. g = mols x molar mass CaSO4. a. Total grams - grams dissolved = ? b. mols CaSO4 in 100 mL x (1000/100) = mols CaSO4 in 1 L and M = mols/L.
Thursday, October 25, 2012 at 11:40pm by DrBob222

Chemistry
Consider the reaction CaSO4(s)rightleftharpoons Ca^2+(aq)+ SO_4^2-(aq) At 25 C the equilibrium constant is Kc = 2.4 \times 10^-5 for this reaction. If excess CaSO4(s) is mixed with water at 25C to produce a saturated solution of CaSO4, what are the equilibrium concentration of...
Tuesday, November 6, 2012 at 1:24am by Josh G.

A reaction requires pure anhydrous calcium Sulfate CaSO4 only unidentified hydrate of calcium Sulfate CaSO4.xH2O is available 1-we heat 67.59 g of unknown hydrate until all the water has been driven off. The resulting mass of pure CaSO4 is 53.4g what is the formula of the ...
Monday, May 3, 2010 at 4:12am by Anonymous

Chemistry
The Ksp of CaSO4 is 4.93× 10–5. Calculate the solubility (in g/L) of CaSO4(s) in 0.300 M Na2SO4(aq) at 25 °C
Tuesday, November 12, 2013 at 3:19pm by Katherine

chemistry
calcium nitrate + sulfuric acid =caso4+? write a balanced chemical equation for this reaction including states. Ca(NO3)2 + H2SO4 ==> CaSO4 + 2HNO3 You don't have enough information to provide states. CaSO4 will be a solid so you write CaSO4(s). H2SO4 will be (l) if it is ...
Monday, July 30, 2007 at 3:14am by walter

chemistry
do not understand this problem The Ksp of CaSO4 is 4.93× 10–5. Calculate the solubility (in g/L) of CaSO4(s) in 0.500 M Na2SO4(aq) at 25 °C.
Friday, February 15, 2013 at 7:23pm by Mohsain

Chem
You made up a saturated solution of calcium sulfate (CaSO4). The temp is 25 degrees Celsius. You then add 5.00*10^-3 of sodium sulfate (NaSO4). What are the concentrations of calcium and sulfate after equilibrium is reached? The pKs of CaSO4 is 4.58. I know the Ks of CaSO4 to ...
Sunday, June 5, 2011 at 8:33am by Mig

chemistry
calculate the # of oxygen atoms in 30 grams of CaSO4 #O atoms= 4 times the moles of CaSO4 * avagradoo's number. How many moles of CaSO4 is in 30 g? there is 0.22 mol in 30 grams of CaS)4
Thursday, June 22, 2006 at 1:37pm by Hawk

Chemistry
The solubility of CaSO4 is 0.209 g/100 mL of water at 30 degrees celsius. if 0.500 g CaSO4 is stirred overnight at 30 Degrees Celsius with 100.0 mL of water, a. How many grams of CaSO4 remain undissolved? b. Calculate the molarity of CaSO44 in solution
Thursday, October 25, 2012 at 11:40pm by Anne

Chemistry
eqn 1 CaF2 ==> Ca^2+ + 2F^- eqn 2 Ca^2+ + SO4^2- ==> CaSO4 ------------------------------- sum 1+2 CaF2 + SO4^2- ==> (F^-)^2 + CaSO4 since CaF2 and CaSO4 are solids we can cancel them since they are not involved in the Keq. You note that eqn 1 is Ksp for CaF2 and eqn ...
Tuesday, April 8, 2014 at 11:59am by DrBob222

college chemistry
If 100.0 mL of 0.0025 M Na2SO4 (aq)is saturated with CaSO4 how many grams of CaSO4 would be present in the solution? [Hint: Does the usual simplifying assumption hold?]
Thursday, December 12, 2013 at 5:38pm by sarah

Chemistry
........CaSO4 ==> Ca^2+ + SO4^2- I........solid.....0........0 C........solid.....x........x E........solid.....x........x For Na2SO4(aq) ==> 2Na^+ + SO4^2- I.....0.300M........0........0 C......-0.300......0.300*2...0.300 E........0.........0.600....0.300 Ksp CaSO4 = (...
Tuesday, November 12, 2013 at 3:19pm by DrBob222

chemistry
CaSO4.(1/2)H2O 0.5 mole = how many grams. (g = moles x molar mass) What percentage water is in CaSO4.(1/2)H2O
Tuesday, March 22, 2011 at 6:06pm by DrBob222

chem
a 2.50g sample of hydrate of calcium sulfate losses 0.523g of water when heated. what is the mass percent of water in the hydrate and the formula for the hydrate difference of the two masses divided by the initial mass. I believe Adam should reconsider his answer. mass percent...
Tuesday, June 19, 2007 at 10:29am by mocha81

chemistry
Just make it a regular stoichiometry problem. CaSO4*2H2O ==> CaSO4 + 2H2O
Sunday, November 8, 2009 at 9:56pm by DrBob222

chemistry
You say calcium carbonate and write calcium sulfate. The formula mass of CaSO4 is 136.1 on my table; for CaCO3 it is 100. I agree with B for CaSO4.
Saturday, November 10, 2012 at 8:57pm by DrBob222

Chemistry
From the solubility product constants for CaF2 (fluorite) and CaSO4 (anhydrite) determine the equilibrium constant for the reaction CaF2 + SO4 2- --> CaSO4 + 2F-
Tuesday, April 8, 2014 at 11:59am by Me

chemistry/ quantitative analysis
Look up the Ksp for CaSO4, set up an ICE chart, and solve for solubility (in moles/L) of CaSO4, then convert to grams and multiply by 6.
Sunday, May 22, 2011 at 9:52pm 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
Below are the formulas of some hydrates. what is the mole ratio of salt to water? Hydrate Na2SO4.10H2O Co(NO3)2.6H2O Mo(NO3)2.5H2O CaSO4.2H2O (CaSO4)2.H2) Thankk you
Thursday, July 22, 2010 at 4:10pm by Rose

Chemistry
I think you have answered the first question and second question correctly. For the third question, here is what should have happened Notice the equation is Na2SO4(aq) + CaCl2(aq) == CaSO4(s) + 2NaCl(aq) So 1 mole Na2SO4 reacts with 1 mole CaCl2 to produce 1 mole of the solid...
Thursday, November 25, 2010 at 5:43pm by DrBob222

sci/chemistry
when 1.87 g of gypsum(hydrated calcium sulfate) was heated to constant mass, it lost 0.39 g of water. What is the formula of gypsum? YOu know it is of the form: CaSO4.XH2O the idea here is to find x. calculate the number of moles of water in .39g. Calculate the number of moles...
Thursday, March 22, 2007 at 3:35am by jas

chemistry
Using data in table below and S °(CaSO4·H2O(s))= 194.0 J·mol-1·K-1, calculate Delta fS° for CaSO4·H2O(s) in J·mol-1·K-1.
Thursday, May 13, 2010 at 8:05am by write2khin

chemistry quick help!
6CaCl2 + 2Al2(SO4)3 = 6CaSO4 + 4AlCl3 So, now you know that each mole of CaCl2 produces one mole of CaSO4 How many moles in 4.19g of CaCl2? How many g in that much CaSO4?
Friday, January 25, 2013 at 2:03pm by Steve

chemistry
percent water = (mass H2O/mass sample)*100= (0.523/2.50)*100 = 20.92 which I would round to 20.9%. To find the formula, take a 100 gram sample which provides 20.9 g H2O 100-20.9 = 79.1 g CaSO4 moles water = 20.9/18 = 1.16 moles CaSO4 = 79.1/136 = 0.582 Now find the ratio of ...
Friday, February 19, 2010 at 2:20pm by DrBob222

Chemistry
I looked up the Ksp values. It would have helped if you had since my values in the book I used for Ksp values probably will not agreed with the values in your text. My book is old. Ag2SO4 ==> 2Ag^+ + SO4^2- Ksp = (Ag^+)^2(SO4^2-) Plug in Ag^+ and solve for SO4. I obtained ...
Tuesday, February 4, 2014 at 12:13am by DrBob222

chemistry
Using data in table below and S °(CaSO4·H2O(s))= 194.0 J·mol-1·K-1, calculate ÄfS° for CaSO4·H2O(s) in J·mol-1·K-1.
Wednesday, May 12, 2010 at 9:21pm by write2khin

chemistry
Write and balance the equation. Convert g CaCl2 to mols Convert g Na2SO4 to mols. Use the coefficients in the balanced equation to convert mols CaCl2 to mols CaSO4. Do the same for mols Na2SO4 to mols CaSO4. The SMALLER value is the correct value to choose for the mols CaSO4 ...
Saturday, October 19, 2013 at 11:51pm by DrBob222

Chemistry- HELP
Can someone please help me? Are these questions correct...if not any suggestions would be greatly appreciated! 1. What salt forms as the result of a mixture of calcium hydroxide and hydrochloric acid? a. CaCl b. CaHCl c. CaCl2 d. CaOH e. Cl(OH)2 I believe this is C- CaCl2, is ...
Wednesday, October 7, 2009 at 3:25pm by Adam

Chemistry
If you had shown your work I could have found the error by now and both of us could move on. CaSO4 ==> Ca^+2 + SO4^-2 Ksp = (Ca^+2)(SO2^-2) I looked up the molar mass of CaSO4 and found 136.142 BUT you need to confirm that using values from your text/notes. 0.209 g CaSO4/...
Tuesday, November 30, 2010 at 10:17pm by DrBob222

Chemsitry
At 25 °C, only 1.9 g CaSO4 (MM = 136 g/mol) will dissolve in 2.00 L of water. Write the equilibrium expression and calculate the equilibrium constant for the reaction below. CaSO4 (s) ⇋ Ca2+ (aq) + SO42- (aq)
Sunday, June 13, 2010 at 2:17pm by Michelle

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
If the reaction below proceeds with a 96.8% yield, how many kilograms of CaSO4 are formed when 5.97 kg SO2 reacts with an excess of CaCO3 and O2? 2 CaCO3(s) + 2 SO2(g) + O2(g) 2 CaSO4(g) + 2 CO2(g)
Thursday, April 7, 2011 at 3:18pm by za

chemistry
you made up a standard solution of calcium sulfate (CaSO4). the temperature is 25C. you then add 5.00*10^-3 odium sulfate (Na2SO4). Calculate the concentrations of calcium and sulfate after equilibrium is reached? The pKs of CaSO4 is 4.58.
Saturday, January 15, 2011 at 6:44pm by Maria

If the reaction below proceeds with a 96.8% yield, how many kilograms of CaSO4 are formed when 5.27 kg SO2 reacts with an excess of CaCO3 and O2? 2 CaCO3(s) + 2 SO2(g) + O2(g) 2 CaSO4(g) + 2 CO2(g)
Thursday, January 27, 2011 at 10:34pm by Matt

Chemistry
I'll do the CaSO4 (btw, you help clutter the problem with the explanation of subscripts etc. It would be nice if html was convenient for subscripts but it isn't. Most of us here recognize that number appearing BEFORE the formula means it is a coefficient and numbers AFTER a ...
Saturday, January 19, 2013 at 11:51am by DrBob222

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

chemistry
Using data in table below and S °(CaSO4·H2O(s))= 194.0 J·mol-1·K-1, calculate ÄfS° for CaSO4·H2O(s) in J·mol-1·K-1. Compound S °, J·mol-1·K-1 C(s) 5.69 H2(g) 130.6 N2(g) 191.5 O2(g) 205.0 Na(s) 51.0 Cl2(g) 223.0 Ca(s) 154.8 S(s) 31.8 Anyone help me please
Wednesday, May 12, 2010 at 9:48pm by write2khin

chemistry
Using data in table below and S °(CaSO4·H2O(s))= 194.0 J·mol-1·K-1, calculate Delta fS° for CaSO4·H2O(s) in J·mol-1·K-1. CompoundS °, J·mol-1·K-1 C(s) 5.69 H2(g) 130.6 N2(g) 191.5 O2(g) 205.0 Na(s) 51.0 Cl2(g) 223.0 Ca(s) 154.8 S(s) 31.8
Thursday, May 13, 2010 at 5:28pm by zacky

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

SCIENCE/CHEM
Al2(SO4)3 + Ca(OH)2-->Al(OH)3 + CaSO4 No. You need the practice. Here is how you start. Right off the bat I see 3 SO4 on the left so we stick a 3 for CaSO4. That takes care of a chunk. I would balance Al next, then count up H and balance them.
Wednesday, May 12, 2010 at 9:11pm by DrBob222

chemistry
Do you mean calcium sulfite (CaSO3) or calcium sulfate(CaSO4)? Your question states calcium sulfate but you have written calcium sulfite for the formula. I suspect that is a typo and you intend for it to be CaSO4.
Tuesday, July 1, 2008 at 1:29am by DrBob222

chemistry
Given the following reaction: Pd(NO3)2+CaSO4-->PdSO4+Ca(NO3)2 If you started with 225.6ml of 6.32M CaSO4 and the percent yield of this reaction was ol 78.2%, what is the actual yield of grams mod of PdSO4?
Saturday, December 4, 2010 at 11:23pm by regina

chemistry
Using data in table below and S °(CaSO4·H2O(s))= 194.0 J·mol-1·K-1, calculate ÄfS° for CaSO4·H2O(s) in J·mol-1·K-1. CompoundS °, J·mol-1·K-1 C(s) 5.69 H2(g) 130.6 N2(g) 191.5 O2(g) 205.0 Na(s) 51.0 Cl2(g) 223.0 Ca(s) 154.8 S(s) 31.8 somebody help me please i cant ork it out
Thursday, May 13, 2010 at 8:05am by write2khin

chemistry - Can you please check
I believe #3 is wrong. Let me show you how I would do it. Either I showed you something wrong earlier or you misunderstood somewhere along the line. At any rate, here is how to do these. You want mols S = M x L = 2 x 0.200 = 0.400 mol S. 0.400 mol S x (1 mol CaSO4/1 mol S) = ...
Wednesday, January 23, 2013 at 7:14pm 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
Na2SO4 + Ca(NO3)2 ==> CaSO4(s) +2NaNO3 millimols Na2SO4 = mL x M = 1.125 millimols Ca(NO3)2 = 0.945. I don't know what % Ca undissolved means? and % of what? It will form 0.000945 mols CaSO4 solid
Thursday, March 8, 2012 at 3:10pm by DrBob222

chemistry - Can you please check
I'm confused again. Can you show me how to get the CaSO4 so I can do the other two? What did I do wrong? I showed you my work. I thought I followed your instructions from Saturday. You said I needed a number near 13. I got the 12.8264. If you could please do the CaSO4, I could...
Wednesday, January 23, 2013 at 7:14pm by Sejul

science(chemistry) -Q for Dr.Bob
Drierite is not CoCl2. I believe it is anhydrous CaSO4. INDICATING drierite has CoCl2 added to it; the CoCl2 is the indicator of water. Blue when no water, pink with water. CaSO4 without the CoCl2 would be my first choice as a drying agent if you need one.
Monday, April 20, 2009 at 11:56pm by DrBob222

chemistry
Ksp Ag2SO4 = 1.2E-5 = (Ag^+)^2(SO4^2-) Ksp CaSO4 = 4.93E-5 = (Ca^2+)(SO4^2-) So CaSO4 ppts first. How do you know that. Calculate the (SO4^2-) when each bgins to ppt. Ag2SO4. (SO4^2-) = Ksp/(Ag^+)^2 (SO4^2-) = you do it. I get approx 2.7E-2M CaSO4. (SO4^2-) = Ksp/(Ca^2+) = you...
Thursday, April 10, 2014 at 11:21pm by DrBob222

chemistry
I have tried virtually everything, i can't fogure out this problem. I have 2K^+ + SO4^2- + Ca^2+ + 2I^- --> CaSO4(s) + 2K^+ + 2I^-. but it is incorrect and i dnt see how, can u help me? Write balanced complete ionic equation for K2SO4 (aq) + CaI2 (aq)CaSO4 (s) + KI(aq)?
Monday, October 4, 2010 at 11:24pm by Amy

chemistry
A 1.994 g sample of gypsum, a hydrated salt of calcium sulfate, CaSO4, is heated at a temp. above 170 C in a crucible until a constant mass is reached. The mass of anhydrous CaSO4 is 1.577g. what is percent by mas of water in the hydrated calcium sulfate salt
Tuesday, February 9, 2010 at 10:08am by neha

chemistry
CaSO4 --> Ca^+2 + SO4^= Ksp = (Ca^+2)(SO4^=) Substitute 0.02M for (Ca^+2) and calculate (SO4^=) needed to cause ppt of CaSO4. That will be in M; therefore, for 1 L of solution that will be the moles. Then grams Na2SO4 = moles x molar mass Na2SO4.
Tuesday, July 27, 2010 at 10:32pm 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

chem
How do you balance this equation?: (NH4)2SO4+Ca(OH)2==>CaSO4+NH3+H20 Thanks! 2 NH3 2H2O Others are ones. (NH)2SO4 + Ca(OH)2 --> CaSO4+2NH3+2H2O Thanks!
Thursday, March 22, 2007 at 5:18pm by Fidelia

chemistry
It lost 0.532 g H2O out of a 2.500 g sample. %H2O = (mass water lost/mass sample) x 100 = approximately 22 but you need to go through it to do it more exacting than that. Now take 100 g sample. That will give you 22% H2O (or the value you recalculate) 78% CaSO4 (found by 100...
Saturday, February 27, 2010 at 10:14pm by DrBob222

Chemistry
A 2.914 gram sample of gypsum, a hydrated salt of calcium sulfat, CaSO4, is heated at a temperature greater than 170 degrees Celcius in a crucible until a constant mass is reached. The mass of the anhydrous CaSO4 salt is 2.304 grams. Calculate the percent by mass of water in ...
Monday, September 24, 2012 at 10:47pm by Sara

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
That's all you need. g H2O = 2 moles H2O = 2*molarmass H2O. Then %H2O = (2*molar mass H2O/molar mass CaSO4.2H2O)*100 = ?? This looks simple enough; however, I don't believe CaSO4.2H2O has a molar mass even close to 4905 g/mol.
Sunday, November 28, 2010 at 8:42pm by DrBob222

chem help
first write just the compounds. K2CO3 + MgCl = KCl + MgCO3 Note you have 2K on the left, but just one on the right. Fix that: K2CO3 + MgCl2 = 2KCl + MgCO3 Now things match on both sides Similarly, you can work your way to H2SO4 + CaCO3 = CaSO4 + CO2 + H2O Na2SO4 + Ca(NO3)2 = ...
Tuesday, January 15, 2013 at 1:49pm by Steve

college chemistry
I think the idea here is to be able to recognize which of the ions in the set will react. In the first set. Hg2Cl2 is an insoluble compound (a precipitate). Hg2^+2(aq) + 2Cl^-(aq) ==> Hg2Cl2(s) In the second set, CaSO4 is insoluble. Ca^+2(aq) + SO4^-2(aq) ==> CaSO4(s)
Saturday, November 20, 2010 at 12:28pm by DrBob222

chemistry
Your next to last line doesn't make sense but I assume you want to know how many gram PdSO4 you have at the end of the reaction. moles CaSO4 = M x L Using the coefficients in the balanced equation, convert moles CaSO4 to moles PdSO4. Now convert moles PdSO4 to grams. g = moles...
Saturday, December 4, 2010 at 11:23pm by DrBob222

Chemistry
No although you got part way home with that answer. I do the following. Ksp CaSO4 = (Ca^2+)(SO4^2-) = 4.93E-5 What must SO4 be to ppt CaSO4? (SO4^2-) = (4.93E-5/0.05) = 9.86E-4M. Ksp Ag2SO4 = (Ag^+)^2(SO4^2-) = 1.2E-5 What must SO4 be to ppt Ag2SO4. That's (SO4^2-) = [1.2E-5/(...
Sunday, March 17, 2013 at 10:49pm by DrBob222

Chemistry
This is a limiting reagent problem. 1. You have the equation. 2a. Convert 1 kg calcium phosphate to moles. moles = grams/molar mass. 2b. Convert 1 kg H2SO4 to moles. Same process BUT you are starting with 1,000 x 0.98 grams and not 1 kg. 3a. Using the coefficients in the ...
Monday, August 16, 2010 at 10:26pm by DrBob222

Chemistry
OK. But great, I think I've interpreted my entire experiment incorrectly. So the magnesium and sulfuric acid combination is soluble, and no precipitate forms. Now let's say I added sulfuric acid to calcium sulfate. Would this be soluble with no precipitate forming? A little ...
Wednesday, December 3, 2008 at 3:31pm by DrBob222

chemistry - Can you please check
Calculate the amount (g) of each of the following salts that need to be added to a 200 mL volumetric flask to produce a 2 M solution of S. CaSO4 (NH4)2SO4 Fe2(SO4)3 Dr. BOB222, Could you please check the following? Thank you. CaSO4: moles x atomic mass = .0400 x 32.066 amu = ...
Wednesday, January 23, 2013 at 7:14pm by Sejul

AP CHEM
19. Burning coal and oil in a power plant produces pollutants such as sulfur dioxide, SO2. The sulfur-containing compound can be removed from other waste gases, however, by the following reaction: 2 SO2(g) + 2 CaCO3(s) + O2(g)  2 CaSO4(s) + 2 CO2(g) [Molar masses: 64....
Thursday, October 7, 2010 at 9:23pm by Megan

A 1.994 g sample of gypsum, a hydrated salt of calcium sulfate, CaSO4, is heated at a temp. above 170 C in a crucible until a constant mass is reached. The mass of anhydrous CaSO4 salt is 1.577 g. Calculate the percent by mass of water in the hydrated calcium sulfate salt. ...
Friday, November 21, 2008 at 3:41pm by Sarah

chemistry
the Ksp of CaSO4 is
Friday, March 29, 2013 at 2:37am by Anonymous

Chem
What is molar mass of CaSO4?
Tuesday, November 13, 2007 at 5:29am by Ryan

chemistry
A white ppt of CaSO4.
Tuesday, March 1, 2011 at 5:04pm by DrBob222

College Chemistry
You can do this the long way or a short way or one that's in between. The short way isn't taught anymore I don't think. The long way is to write an equation, balance it, and solve as if it were a stoichiometry problem. Here is a worked example that will solve all of your ...
Saturday, October 8, 2011 at 9:01am by DrBob222

chemistry
first convert the kg of SO2 to grams of SO2 then convert to moles by dividing by its molar mass secondly convert between moles of 2SO2 and 2CaSO4 which is a 2/2 ration so no change in moles then multiply your moles by CaSO4's molar mass to get grams, then multiply that amount ...
Thursday, April 7, 2011 at 3:18pm by Chris

chemistry
How many moles are in 52.3 grams of CaSO4?
Friday, February 19, 2010 at 12:01am by Jessica

chemistry
mole ratio of (CaSO4)2.H2O
Thursday, July 22, 2010 at 3:29pm by Rose

chemistry
mole ratio of CaSO4.2H2O
Thursday, July 22, 2010 at 3:29pm by Rose

Chemistry
Please help me....are these questions right or no? If not can you help me...any suggestions please? 7.(14). Which of the following is a salt? a. HNO3 b. H2SO4 c. CaSO4 d. NaOH e. NH3 I put down C- CaSO4, is that right or am I way off track? 8.(15). Which of the following is a ...
Tuesday, October 6, 2009 at 1:57pm by Taylor

chem
Na2SO4 + Ca(OH)2 ==> 2NaOH + CaSO4
Friday, February 29, 2008 at 11:52am by DrBob222

chemistry
Ca + H2SO4 ==> CaSO4 + H2
Tuesday, May 13, 2008 at 10:11pm by DrBob222

Chemistry
See the procedure for CaSO4 and H3PO4 above.
Monday, August 16, 2010 at 10:17pm by DrBob222

Chemistry
See the H3PO4 and CaSO4 problem above.
Monday, August 16, 2010 at 10:14pm by DrBob222

Chemistry
what is the gram formula mass of CaSO4*2H20?
Sunday, January 2, 2011 at 10:05pm by Penny

Chemistry
calculate the percent water in CaSO4*2H20 20.9%?
Sunday, November 8, 2009 at 9:45pm by c

Chemistry
Wouldn't it be 2 moles water per 1 mole CaSO4?
Sunday, November 8, 2009 at 9:43pm by DrBob222

chemistry
so then would i find the gfm of the CaSO4? and get 136.2 as my answer?
Sunday, November 8, 2009 at 9:56pm by c

Pages: 1

Search
Members