Search: A 500 mL saturated solution of calcium fluoride at 25C is evaporated to dryness, yielding 8.00 x 10-3 grams of solid CaF2. What is the Ksp of CaF2 at 25C?

Number of results: 35,238

CHEMISTRY
A FALSK CONTAINS 49.8 mL OF 0.150 CALCIUM HYDROXIDE. HOW MANY MILLILITERS OF 0.500 SODIUM CARBONATE ARE REQUIRED TO REACT COMPLETELY WITH THE CALCIUM HYDROXIDE IN THE FOLLOWING REACTION? Na2CO3(aq)+ Ca(OH)2(aq)¨CaCO3(s)+2NaOH(aq)
Tuesday, October 23, 2012 at 5:34pm by HAMZA

pharmacy math
if 500 ml of a 15% solution is diluted to 1500 ml, how would you label the final strength of the solution?
Friday, December 7, 2012 at 1:37pm by cleondra

chemistry
A solution is saturated with Ag2CrO4. a) Calculate [CrO4^2-] in this saturated solution. b) What mass of AgNO3 must be added to 0.635 L of the solution to reduce [CrO4^2-] to 1.0* 10^-8M?
Monday, March 19, 2012 at 11:24am by Justin

Chemistry
What are the units for crying out loud? Are all of them 100 mL. I will assume that is what you meant except for the dilution which I assume is 0.500 L or 500 mL. 14 g/100 = 0.14 g/mL You took 55 mL of that so you have in the aliquot of 55 mL exactly 0.14 g/mL x 55 mL = 7.70 g...
Monday, February 8, 2010 at 10:54pm by DrBob222

Chemistry
c1v1 = c2v2 50*?mL = 0.5 x 500 mL Solve for ?mL. Add ?ml stock to a 500 mL volumetric flask and make to the mark.
Friday, October 12, 2012 at 5:15pm by DrBob222

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

Chm
What is the molarity of a saturated solution of potassium sulfate if the solubility is 13 g per 100 g H2O at 25°C? The density of the solution is 1.1 g/mL
Thursday, January 17, 2013 at 6:04pm by Chris

Chemistry
Use the dilution relationship (Mi x Vi = Mf x Vf) to calculate the volume of 0.500 M NaOH needed to prepare 500 mL of .250 M NaOH. This is my work ? L Solution = 500mL x (1L/1000mL) = .500L ? mol NaOH = .500 L Solution x (0.250 M NaOH/1 L Solution) = .125 mol NaOH ? L solution...
Saturday, February 28, 2009 at 9:35pm by Bob

CHEMISTRY
A 2.800-g mineral sample was analyzed for its calcium carbonate, CaCO3, content by titrating it with hydrochloric acid (the reaction products are calcium chloride, carbon dioxide, and water). The sample required 28.48 mL of a 0.1505 M HCl solution to react completely. ...
Sunday, November 28, 2010 at 7:45pm by Anonymous

chem
15% w/w means 15 g H2SO4/100 g solution. That's 15 g H2SO4/(15 g H2SO4 + 85 g H2O) BUT that doesn't tell us the volume of that 100 grams of solution. I don't know how much solute is in 500 mL because I don't know what 500 mL weighs. You need the density of the ...
Thursday, November 29, 2012 at 10:51am by DrBob222

College Chemistry
48.70 mL of an HCl stock solution was transferred into a 500 mL volumetric flask and filled to the mark. 47.67 mL of the diluted solution was titrated with 0.179 M NaOH and found to have the concentration of 0.885 M. What is the concentration of the stock solution?
Saturday, December 11, 2010 at 5:28pm by Mark

Buffer
You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 M sodium acetate (CH3COONa). What will the pH of this solution be after the addition of 93 mL of 1.00 M NaOH solution?
Monday, April 11, 2011 at 4:54pm by Nicole

AP Chem
A 3.50 g sample of KCl is dissolved in 10.0 mL of water. The resulting solution is then added to 60.0 mL of a 0.500 M CaCl2(aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution. *confused*
Monday, November 3, 2008 at 7:37pm by Anna

CHEMISTRY
I didn't answer your original question because it makes no sense. There is no such thing as preparing a molarity solution. You can prepare a MOLAR solution or a TWO MOLAR solution but you can't prepare a molarity solution. You CAN add an maount of material to a certain...
Monday, March 16, 2009 at 9:00pm by DrBob222

Chemistry
17.0 g in 100 mL. 55 mL taken diluted to 500 mL. So the glucose placed in the 500 mL flask is 17.0 x (55/100) = ?? Therefore, the concn (grams/mL) in the 500 mL flask is ??/500 mL. Multiply by 100 if you want the grams/100 mL.
Wednesday, July 7, 2010 at 8:31pm by DrBob222

Chemistry
Calculate the mass of calcium phosphate that forms when 5.50 x 10 -2 mol of solid calcium chlorate is dissolved in 600.0 mL of 1.00 x 10 -2 M lithium phosphate solution.
Tuesday, February 21, 2012 at 8:27pm by Bella

Chemistry
A solution is prepared by mixing 100 mL of 0.500 M NH3 and 100 mL of 0.500 M HCl. Assuming that the volumes are additive, what is the pH of the resulting mixture? kb for ammonia is 1.8x10-5
Thursday, May 2, 2013 at 5:46pm by Chris

Chemistry
12.0 g/100 mL 0riginal. Take a 50.0 mL aliquot so now you have 6.0 g in the 50.0 mL. That is diluted to 500 mL so now you have 6.0 g in 500 mL. If you take 100 mL of that solution you will have 1/5 of 6.0 = ??
Wednesday, September 29, 2010 at 2:54am by DrBob222

Chemistry
I'm trying to find the solubility of Ca(OH)2 in .0125 mol/L aqueous NaOH. Here is my data: Vol of solution used per titration: 20mL Conc of HCl: .1201 mol/L Average Titre: 4.71 I need to calculte: 1. the TOTAL [OH-] in the saturated solution of Ca(OH)2 in NaOH 2. the [OH...
Wednesday, April 14, 2010 at 1:49pm by Kristin

Organic Chemistry
What are proper techniques to induce crystallization from a saturated solution? (Select all correct answers.) Allowing the solution to cool down. Scratching the outside of the container with a glass rod. Seeding the solution. Adding a solvent that lowers the solubility of the...
Thursday, April 29, 2010 at 1:42pm by Joanna

Science
10.0 g of KCl and 18.5 g of CaCl2 were dissolved in 500 mL of water. How many mL of 1.57 M AgNO3 solution would be required to precipitate all Cl- from the solution?
Friday, October 19, 2012 at 2:31pm by Jared

Science
Calculate the molarity of the following solution: 7.48g of calcium chloride (CaCl2) in 215 mL of aquous solution.
Friday, October 19, 2012 at 2:30pm by Emily

Chemistry
see same question how many grams nitric acid HNO3 must be dissolved in 350 ml water to make a solution with pH of 4.5"? or "how many ml of a 4.2M nitric acid solution are required to make 500 ml of solution with pH of 2.9
Sunday, May 12, 2013 at 11:29am by kriti

Chemistry
A buffer is prepared by mixng 150.0 mL of 0.500 M ammonia, 250.0 mL of 0.200 M ammonium chloride and 600.0 mL of water. To this solution is added 50.0 mL of 0400 M hydrochloric acid. What is the final pH?
Wednesday, December 9, 2009 at 9:37pm by Cathy

Chemistry
I know not how a student would do it but I would use c1v1 = c2v2 0.08500M*500 mL = 0.3180M*v2 v2 = 133.6 mL The way you do this is to pipet or measure accurately 133.6 mL of the stock solution and transfer quantitatively to a 500 mL volumetric flask. Then add distilled water ...
Wednesday, November 21, 2012 at 6:17pm by DrBob222

Chemistry
What volume of a 0.332 M hydrobromic acid solution is required to neutralize 29.6 mL of a 0.155 M calcium hydroxide solution ?
Monday, October 22, 2012 at 2:32pm by Kaitlin

College Chemistry
The concn of the titrated solution is 0.885M. It came from the 500 mL flask; therefore, it must be 0.885M also. How many moles HCl are in the 500 mL flask? That will be 0.885 x 0.500L = 0.4425 moles. All of those moles came from the 48.70 mL stock solution; thus, the M of the ...
Saturday, December 11, 2010 at 5:28pm by DrBob222

see this too---chemistry
If you substitute 500 g and 0.500 L the density will be in units of g/L. If you want g/mL or g/cc, you need to substitute 500 g/500 mL = ? g/mL.
Thursday, September 6, 2012 at 7:57am by DrBob222

chemistry
Your question isn't stated very well. Do you mean something like this? Prepare 100 mL of a 500 mM HCl solution using HCl with a purity of 37% HCl and a density of 1.18 g/mL. If so, the first thing to do is to calculate the molarity of the 37% HCl solution. That will be ...
Wednesday, March 30, 2011 at 11:26pm by DrBob222

chemistry
280 ppm = 280 g/10^6 g solution. If we call the density of the solution 1.00 g/mL and we ignore the contribution of the mass of the salt to the solution (usually ok since the amount of salt is so small), then 280 ppm = 280 g/10^6 mL which is the same as 0.280 g/10^3 mL = 0.280...
Wednesday, April 21, 2010 at 10:21pm by DrBob222

chemistry
#1, calculate the M of the commercial solution. 1000 mL x 1.20 g/mL x 0.37 = grams HCl/1L grams/molar mass HCl = ?M since that will be moles/L. Then Mconcd x ?mL concd = 0.500M x 2,500 mL Solve for ?mL.
Sunday, November 6, 2011 at 1:16am by DrBob222

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
3.21 g of calcium carbonate is dissolved into 250.0 mL of water to make a homogenous solution. What is the concentration os this solution?
Tuesday, August 28, 2012 at 10:17pm by Meeeee

chemistry
3.21 g of calcium carbonate is dissolved into 250.0 mL of water to make a homogenous solution. What is the concentration os this solution?
Tuesday, August 28, 2012 at 8:56pm by Meeeee

Chemistry
A student dissolves 18.9 grams of Zn(NO3)2 [molar mass = 189] in enough water to make 500.0 of solution. A 100.0 ml portion of this solution is diluted to 1000.0 ml.What is the [NO3¯ ] in the second solution? A) 0.0100M B) 0.0200M C) 0.0300M D) 0.0400M E) 0.0500M
Wednesday, February 9, 2011 at 9:26am by Paul

Chemistry
A student must make 500 mL of a 1.5 M HCl solution. The student has plenty of water and a stock solution of 6.0 M HCl to use. What volume of the 6.0 M HCl solution must be added to what volume of water to make the desired 500 mL of 1.5 M solution? I don't really know how ...
Sunday, March 8, 2009 at 3:27pm by Katie

chemistry (buffer)
If 5.00 mL of 1.60 nitric acid is added to a solution of 2.00 mmol thiocyanic acid (HSCN pKa=4.00) and 4.500 mmol calcium thiocyanide, assume a soluble salt- what is teh pOG of the resultant complex solution (of total volume .350L). I worked the problem out and ended up ...
Thursday, May 2, 2013 at 6:50pm by rani

Chemistry
Hi, my question is: "Classify each of the following as saturated, supersaturated, or unsaturated: KNO3 90g/100g at 82*C NaCl 36g/100g at 23*C KCl 35g/100g at 18*C NaNO3 90g/100g at 28*C How do I determine if they are saturated, supersaturated, or unsaturated? Since the ...
Sunday, June 11, 2006 at 1:51pm by Waleed

chemistry
A 0.500 L solution of 7.50 M hydrochloric acid is used to neutralize a 250.0 g sample of calcium hydroxide. Calcium chloride – a chemical used to control highway dust, strengthen concrete mixes, and add flavor to foods – is produced by the reaction. 2 HCl + Ca(OH)2 &...
Monday, March 1, 2010 at 4:34pm by BT

chemistry
An ethylene glycol solution is mad using 58.5g of (C2H6O2) and diluting to a total volume of 500.0 mL. Calculate the freezing and boiling point. Assume a density of 1.09 g/ml for the solution
Saturday, November 5, 2011 at 9:49am by Monique

Chemistry
A solution is made by mixing exactly 500 mL of 0.178 M NaOH with exactly 500 mL of 0.100 M CH3COOH. Calculate the equilibrium concentrations of H+, CH3COOH, CH3COO-, OH-, and Na+.
Monday, May 2, 2011 at 3:20pm by Martina

Chemistry
The 1.97 grams is extraneous information. You don't need it (as long as the problem says the solution is saturated AND there is a small amount of solid in the container). The (Pb^+2) IS 1/2 the (OH^-); i.e., 1/2*(OH^-)=(Pb^+2) So you know (OH^-) and you know (Pb^+2); (Pb^+...
Monday, May 11, 2009 at 9:11pm by DrBob 222

Ap chem
If 200 ml of .300 molarity of silver nitrate are mixed with 350 ml of .500 molarity calcium chloride ions how many grams of percipitate are formed? How many moles of each ions are present?
Tuesday, November 6, 2012 at 8:57pm by Eman

chemistry
Consider a solution made by mixing 500.0 mL of 0.04182 M Na2HAsO4 with 500.0 mL of 0.03645 M NaOH. Complete the mass balance expressions below for Na and arsenate species in the final solution. There are 4 arsenate species, but I only got three of them. I am unsure of what the...
Saturday, March 23, 2013 at 12:34am by Jackie

Chemistry
How many grams of formaldehyde, H2CO, are in 500 ml of a 40% solution of formaldehyde in water? (Assume for this problem that the density of the formalin solution is 0.98 g/ml)
Monday, September 19, 2011 at 5:40pm by Kelsey

chemistry
If 0.694 grams of pure KHP are needed to exactly neutralize 30.5 mL of a calcium hydroxide solution, what is the concentration (in molarity) of the base solution?
Thursday, September 15, 2011 at 11:02am by andrea

Chemistry
What is the molarity of a solution of Mg(OH)2 if the solution contains 1.35 g in exactly 100 mL of solution??? A 15.0 mL solution of H2SO3 is neutralized by 12.0 mL of a standradized 1.00M NaOH solution. What is the concentration of the H2SO3 solution?????? What volume of a 1....
Wednesday, December 12, 2012 at 12:24am by Tasha

Chemistry
How much of a 500 ml bottle of 1.00 molar KCI solution should be diluted with deionized water to give 200.0 ml of a 0.100 molar solution
Monday, February 14, 2011 at 6:44pm by Jane

quantitative chemistry
Consider a solution made by mixing 500.0 mL of 0.04182 M Na2HAsO4 with 500.0 mL of 0.03645 M NaOH. Complete the mass balance expressions below for Na and arsenate species in the final solution. There are 4 arsenate species, but I only got three of them. I am unsure of what the...
Friday, March 22, 2013 at 2:23pm by Jackie

Chemistry
aqueous sulfurous acid H2SO3 was made by dissolving 0.200 L of sulfur dioxide gas at 19 C and 745 mm Hg in water to yield 500.0 ml of solution. the acid solution required 12.9 ml of sodium hydroxide solution to reach the titration end point. what was the molarity of the sodium...
Sunday, February 20, 2011 at 8:20pm by Sierra

Chemistry
You are a lab technician and must create 250 ml of a 17% salt solution. You have available three stock solutions. You have a one liter container of a 5% salt, a 500 ml container of a 28% salt solution, and a 400 ml container of a 40% salt solution. Discuss and explain the ...
Monday, March 5, 2012 at 11:35am by Fatih

Chemistry
Technically, you can't make a solution with a known normality unless you know the reaction in which the H3PO4 will be used. Using the simple case, normality = number equivalents/liter solution. Therefore, one dissolves 1 equivalent (molar mass/3) grams in some water, add ...
Wednesday, February 17, 2010 at 1:11pm by DrBob222

chem
I don't think your question is worded properly. I think you have 12 M HCl and want to prepare 500 mL of 0.4M. c1v1 = c2v2 12*mL = 0.4*500 Solve for mL of the 12 M material. Place that in the 500 mL volumetric flask and make to the mark. Shake thoroughly.
Tuesday, October 16, 2012 at 5:21pm by DrBob222

Chemistry
Chalk is a soft, white, porous sedimentary rock, a form of limestone composed of the mineral calcite. Calcite is calcium carbonate, CaCO3. It forms under relatively deep marine conditions from the gradual accumulation of minute calcite plates (coccoliths) shed from micro-...
Thursday, May 19, 2011 at 12:33am by Shell

chem
A solution contains 32 g of KNO3 per 100g of water at 25 degree C. Is the solution unsaturated, saturated, or supersaturated? I think its saturated Look at your saturation chart. I will be happy to critique your thinking. is there one online?
Thursday, April 5, 2007 at 11:38am by jake

chemistry
What volume of water would be required to dilute a 10.0 mL 0.650 M solution of calcium sulfate to create 0.25 M solution, what would the volume of the new solution be?
Thursday, February 10, 2011 at 10:11pm by Elaine

Chemistry
If 31.00 mL of a dilute solution of lime water (calcium hydroxide) required 10.10 mL of 0.246 M hydrochloric acid solution for neutralization to a methyl red end point, calculate the molarity of the lime water. Can you please explain how to do it? Do I use M1V1=M2V2?
Saturday, April 2, 2011 at 3:22pm by Lara

science
how would you make 500.0mL of a 0.200M NaOH solution from a 15.0 M stock NaOH solution?? I assume that you want the volumes rather than the mechanics of carrying it out? a) How many moles do you need in the 500 ml to have 0.200 M? b) What volume of 15.0 M would contain the ...
Thursday, April 5, 2007 at 11:43am by Mel

Chemistry
A 1.00-L solution saturated at 25°C with calcium oxalate (CaC2O4) contains 0.0061 g of CaC2O4. The solubility constant (Ksp) for this salt is [CaC2O4=128.09 g/mol]
Monday, April 16, 2012 at 9:55pm by Anne

Chemistry
In an acid-base neutralization reaction 28.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution? Please help with this question, thank you.
Sunday, September 19, 2010 at 8:48pm by Trever

chemistry
If you add 50 g of sylvite in 100 ml of water at 60 ° C, the resulting solution will she unsaturated, saturated or supersaturated? You prepare a solution and you add 50 g of potassium nitrate to 100 ml of water at 50 ° C. What type of solution are you prepared? Ammonia...
Tuesday, February 8, 2011 at 3:57pm by Kay

Chemistry
You didn't follow the instructions and I don't see that you used MxV= MxV ?? mL x 0.500 M = 500 mL x 0.250 M ?? mL = 500 x 0.250/0.500 = 250 mL.
Saturday, February 28, 2009 at 9:35pm by DrBob222

chemistry
I have no idea how to solve this problem, please help me out.... thanks a) A liter of a solution saturated at 25degree with calcium oxalate, CaC2O4, is evaporated to dryness, giving a 0.0061gm residue of CaC2O4. calculate the concentrations of the ions, and molar solubility ...
Friday, April 6, 2007 at 10:19pm by wendy

College Chemistry
A 1.00-L solution saturated at 25°C with calcium oxalate (CaC2O4) contains 0.0061 g of CaC2O4. The solubility constant (Ksp) for this salt is [CaC2O4=128.09 g/mol]
Monday, December 6, 2010 at 12:23pm by Patrice

chemistry
If you have all of the information posted, then 500 mL of the saturated solution of Ca(OH)2 must have used 0.10 x 0.050 L = 0.005 mols HCl. The reaction is Ca(OH)2 + 2HCl ==> CaCl2 + 2H2O. Therefore, mols Ca(OH)2 must be 1/2 of the HCl mols or 0.005/2 = 0.0025. From ...
Tuesday, April 1, 2008 at 3:23pm by DrBob222

Chemistry
A student mixes 100.0 mL of 0.300 mol/L silver nitrate solution with 100.0 mL of 0.300 mol/L calcium chloride solution. a) Determine the theoretical yield of the precipitate. b) If the actual mass of precipitate is 4.00g, calculate the percent error of this experiment.
Saturday, January 8, 2011 at 2:44pm by Rebekah

chemistry
Bill prepared 5.00-mL of borax solution at 59.2degrees C. He diluted the solution in an Erlenmeyer flask and titrated it to an endpoint with 27.05 mL of 0.500 M HCl. What is the saturation concentration of borate ions? I don't know what to do here. Does it involve a Ksp? ...
Monday, April 9, 2012 at 10:19pm by jason

chemistry
50.00 mL of OOH was diluted to 250.0 mL with deionized water. In the determination of the total cation concentration, 25.00 mL aliquots of the dilute OOH were passed through a cation exchange column and the eluent titrated with an average 27.42 mL of 0.1134 M NaOH. In the ...
Thursday, January 26, 2012 at 10:17pm by Annabelle

Chemistry
50.00 mL of OOH was diluted to 250.0 mL with deionized water. In the determination of the total cation concentration, 25.00 mL aliquots of the dilute OOH were passed through a cation exchange column and the eluent titrated with an average 27.42 mL of 0.1134 M NaOH. In the ...
Thursday, January 26, 2012 at 5:51am by Georgia

chemistry
It's tough to read questions posted in CAPS. The hot coffee dissolved all of the sugar and the solution was not saturated. On cooling, the solubility of the sugar decreases, the solution was saturated, and the excess amount present crystallized.
Thursday, February 24, 2011 at 11:02pm by DrBob222

chemistry
When performing a titration, 23.65 mL of 1.25 M calcium carbonste was used to neutralize 9.68 mL of HCl. What is the concentration of the HCl solution? (Create a balanced equation first)
Friday, June 3, 2011 at 9:03am by lexi

chemestry
A student weighs out a 14.0 g sample of Fe(NO3)2, transfers it to a 500 mL volumetric flask, adds enough water to dissolve it and then adds water to the 500 mL tic mark. What is the molarity of iron(II) nitrate in the resulting solution?
Wednesday, November 17, 2010 at 1:26am by cristy

chemistry
A saturated solution is prepared by dissolving 3.2 g of a salt in 9.10 g of water to yield a saturated solution. What is the solubility of the salt (in g salt/100g of H2O)?
Sunday, March 18, 2012 at 5:06pm by Riley

Chemistry
500 mL x 0.1M = ?mL x 2.0M Solve for mL, measure that quantity of 2.0M NaOH and make up to 500 mL with DI water.
Wednesday, March 28, 2012 at 1:39pm by DrBob222

Chemistry
One of the main components of hard water is CaCO3. When hard water evaporates, some of the CaCO3 is left behind as a white mineral deposit. If hard water solution is saturated with calcium carbonate, what volume of the solution has to evaporate to deposite 1.00x10^2 mg of CaCO3
Sunday, April 24, 2011 at 9:12pm by Trista Nigh

analytical chemisty
Consider the standardization of a solution of K2Cr2O7 with iron metal according to the following: Reaction: Fe + Cr2O7-2 → Fe +3 + Cr+3a. How many grams of K2Cr2O7 are required to prepare 500 ml of a 0.13 N solution? What is the exact normality of the solution ...
Saturday, February 2, 2013 at 7:39pm by Anonymous

Chemistry
(a) Grams of solute in 185.8 mL of 0.267 M calcium acetate Moles solute = M x L. Then moles x molar mass = grams. (b) Molarity of 500. mL of solution containing 21.1g of potassium iodine M = moles/L. 21.1/molar mass KI = mols KI and divide by 0.5L. (c) Moles of solute in 145.6...
Monday, September 28, 2009 at 12:28am by DrBob222

Chemistry
Aqueous ammonia is typically sold by chemical supply houses as the saturated solution, which has a concentration of 14.5mol/L. What volume of NH3 at STP is required to prepare 100. mL of concentrated ammonia solution?
Wednesday, May 1, 2013 at 7:43pm by Shashi

chemistry
Calculate the solubility (in g of compound per 100 g of water) of a compound for which 0.74 g form a saturated solution in 2 mL of water. Density of water: 1.00 g/mL
Monday, September 26, 2011 at 12:01pm by Anonymous

chemistry
Write the correct equation for the formation of a white precipitate on mixing together 10 mL each of 1 M calcium chloride, 1 M calcium bromide, 1 M calcium nitrate, 1 M sodium carbonate, 1 M potassium carbonate, and 1 M rubidium carbonate.
Tuesday, March 27, 2012 at 4:59pm by liz

chemistry
a solution (S) is prepared by dissolving 50.0 g calcium chloride in 250 ml volumetric flask wich is then filled with distilled water up to the line mark. calculate the molar concentration of solution (S)
Sunday, March 10, 2013 at 9:11am by alia

Chemistry
Q1: You wish to prepare a buffer solution with pH = 11.10. What volume of 6.0 M HCl would you add to 500 mL of 0.10 M (C2H5)2NH to prepare the buffer? You may assume that the solution’s volume remains constant. Q2: What is the resulting pH when 20 mL of 0.20 M NaOH is ...
Sunday, February 24, 2013 at 2:16pm by Anonymous

chemistry
Hey, I am having a real hard time getting the answers to the problems. Any help would be greatly aprreciated! 1. When 11 mL of a solution containing 2.9 M AlBr3 is diluted to 33 mL, a dilute solution is formed. What is the Br- concentration in 25 mL of the dilute solution? 2. ...
Wednesday, November 7, 2007 at 5:35pm by chelsea

chemistry
Let me repost the important information only: Purpose: The purpose of this experiment is to determine the Ksp for calcium hydroxide. Materials are: *50.0 mL of 0.10 M HCl(aq) *bromophenol blue indicator *50.0 mLsaturated calcium hydroxide *50.0 mL buret *125 mL Erlynmyer Flask...
Tuesday, April 1, 2008 at 11:53pm by Jessica

chemistry
Purpose: The purpose of this experiment is to determine the Ksp for calcium hydroxide. Materials are: *50.0 mL of 0.10 M HCl(aq) *bromophenol blue indicator *50.0 mLsaturated calcium hydroxide *50.0 mL buret *125 mL Erlynmyer Flask *50.0 mL of distilled water *10.0 mL pipet ...
Friday, April 4, 2008 at 3:39pm by Tim's Titration Lab

chemistry
please help solve this problem now. I really need an answer. thank you When one mole of KOH is neutralized by sulfuric acid, q=-56kJ. At 22.8 C , 25.0 mL of 0.500 M H2SO4 is neutralized by 50.0 mL of 0.500 M KOH in a coffee-cup calorimeter. What is the final temperature of the...
Saturday, March 3, 2012 at 7:08am by ogi

Chem
In a titration process it takes 22.00 mL of nitric acid to neutralize 16.70 mL of 0.200 M calcium hydroxide solution. what is the balanced equation and what is the molarity of the acid. please explain
Wednesday, June 13, 2012 at 11:29pm by Piper

Chem
The molecular weight of CaCl2 is 110.98 g/mol. In order to make up 500.0 ml of a 0.500 M solution, you need how many g?
Thursday, July 26, 2012 at 9:52am by Danny

Chemistry
I have no idea what I'm doing wrong here... Question: A solution is 0.3% by mass calcium chloride. Therefore, 145 g of the solution contains how many grams of calcium chloride? My solution: 145g x (0.3g / 100g) = 0.435g or 0.44g CaCl2 What am I doing wrong? Thank you!
Sunday, May 9, 2010 at 9:42pm by Jake

Chem
How do I do this problem Assume you dissolve 2.56 g of malic acid, C4H6O5, in half a liter of water (500.0 g). Calculate the molarity, molality, mole fraction, and weight percent of acid in the solution. (Assume the final volume of the solution is 500. mL)
Sunday, July 24, 2011 at 10:29pm by Ann

CHM 152
1.06 g/mL x 1000 = 1060g is mass 1000 mL soln. This 1000 mL soln consists of 500 mL ethylene glycol and 500 mL H2O(equal volumes of ethylene glycol and H2O). The mass of 500 mL ethylene glycol is 500 x 1.114 g/mL = 557 grams or 557/62.07 = 8.97 moles ethylene glycol per 1000 ...
Tuesday, June 8, 2010 at 12:06am by DrBob222

Chemistry
A 500.0-mL sodium iodide (NaI) solution was prepared by dissolving 37.7g of solid NaI in water. Chlorine gas was bubbled through a 100.0-mL sample of this solution until the reaction was complete. How many grams of molecular iodine were produced?
Friday, November 6, 2009 at 1:18pm by L

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