Why are the moles and molar concentration in an old peroxide bottle greater than a new one?
Q. I recently did an experiment. The hypothesis is hydrogen peroxide decomposes in sunlight. So I titrated 50 ml of potassium parmengate into 10 ml of new hydrogen peroxide and 2 ml of sulfuric acid. I repeated this procedure using old hydrogen peroxide instead. After my calculations I found the moles and molar concentration of the old bottle to be greater than the new. Is this correct, I may have miscalculated. Explain why it is greater?
Asked by Teddiboy09 - Tue Nov 3 23:20:13 2009 - - 1 Answers - 0 Comments
A. it seems right to me...i would conclude that in an old bottle of H2O2 would have a slightly higher concentration because some of the water has had time to evaporate out of the solution raising the concentration
Answered by Erick M - Tue Nov 3 23:29:15 2009
Q. I recently did an experiment. The hypothesis is hydrogen peroxide decomposes in sunlight. So I titrated 50 ml of potassium parmengate into 10 ml of new hydrogen peroxide and 2 ml of sulfuric acid. I repeated this procedure using old hydrogen peroxide instead. After my calculations I found the moles and molar concentration of the old bottle to be greater than the new. Is this correct, I may have miscalculated. Explain why it is greater?
Asked by Teddiboy09 - Tue Nov 3 23:20:13 2009 - - 1 Answers - 0 Comments
A. it seems right to me...i would conclude that in an old bottle of H2O2 would have a slightly higher concentration because some of the water has had time to evaporate out of the solution raising the concentration
Answered by Erick M - Tue Nov 3 23:29:15 2009
How would i calculate the molar concentration of a base?
Q. 0.3727g sample of KHC8H4O4 required 18.53mL of NaOH solution to reach the equivalence point. What is the molar concentration of the base?
Asked by Fgfg D - Wed Nov 5 06:15:38 2008 - - 1 Answers - 0 Comments
A. first write an equation for the reaction find the molar mass of KHC8H4O4 divide 0.3737 by the molar mass to find the moles of KHC8H4O4 use the stoichiometric ratio from the equation to find out the moles of NaOH
Answered by suddsmcduff92 - Wed Nov 5 06:25:08 2008
Q. 0.3727g sample of KHC8H4O4 required 18.53mL of NaOH solution to reach the equivalence point. What is the molar concentration of the base?
Asked by Fgfg D - Wed Nov 5 06:15:38 2008 - - 1 Answers - 0 Comments
A. first write an equation for the reaction find the molar mass of KHC8H4O4 divide 0.3737 by the molar mass to find the moles of KHC8H4O4 use the stoichiometric ratio from the equation to find out the moles of NaOH
Answered by suddsmcduff92 - Wed Nov 5 06:25:08 2008
what was the molar concentration of acetic acid in the solution?
Q. If 25.0 mL of a solution of acetic acid requires 31.2 mL of a 0.0724 M solution of sodium hydroxide to reach the endpoint, what was the molar concentration of acetic acid in the solution?
Asked by Nawimkidding.or.am.i - Thu Oct 1 01:03:15 2009 - - 2 Answers - 0 Comments
A. moles NaOH = 0.0312 L x 0.0724 M=0.00226 CH3COOH + NaOH = CH3COONa + H2O the ratio between CH3COOH and NaOH is 1 : 1 moles acetic acid = 0.00226 Molarity acetic acid = 0.00226 mol/ 0.0250 L=0.0904 M
Answered by Dr.A - Sun Oct 4 09:02:30 2009
Q. If 25.0 mL of a solution of acetic acid requires 31.2 mL of a 0.0724 M solution of sodium hydroxide to reach the endpoint, what was the molar concentration of acetic acid in the solution?
Asked by Nawimkidding.or.am.i - Thu Oct 1 01:03:15 2009 - - 2 Answers - 0 Comments
A. moles NaOH = 0.0312 L x 0.0724 M=0.00226 CH3COOH + NaOH = CH3COONa + H2O the ratio between CH3COOH and NaOH is 1 : 1 moles acetic acid = 0.00226 Molarity acetic acid = 0.00226 mol/ 0.0250 L=0.0904 M
Answered by Dr.A - Sun Oct 4 09:02:30 2009
What is the logarithm of the molar concentration of this salt?
Q. Consider a salt of the composition, A2B3. For this salt, pKsp = 68.288. What is the logarithm of the molar concentration of this salt?
Asked by Sammie L - Fri Feb 29 10:21:50 2008 - - 1 Answers - 0 Comments
A. Ksp = 10^-68.288 = 5.15 x 10^-69 = ( 2x)^2 ( 3x)^3 = 108 x^5 x = molar concentration = 8.62 x 10^-15 log 8.62 x 10^-15 = 14.1
Answered by Dr.A - Fri Feb 29 11:07:26 2008
Q. Consider a salt of the composition, A2B3. For this salt, pKsp = 68.288. What is the logarithm of the molar concentration of this salt?
Asked by Sammie L - Fri Feb 29 10:21:50 2008 - - 1 Answers - 0 Comments
A. Ksp = 10^-68.288 = 5.15 x 10^-69 = ( 2x)^2 ( 3x)^3 = 108 x^5 x = molar concentration = 8.62 x 10^-15 log 8.62 x 10^-15 = 14.1
Answered by Dr.A - Fri Feb 29 11:07:26 2008
What is the osmotic pressure and molar concentration?
Q. A)Isotonic saline solution, which has the same osomotic pressure as blood, can be prepared by dissolving 0.923g of NaCl in enough water to produce 100mL of solution. What is the osmotic pressure of this solution at 25C ? B)Osmosis is the process responsible for carrying nutrients and water from groundwater supplies to the upper parts of trees. The osmotic pressures required for this process can be as high as 18.1atm . What would the molar concentration of the tree sap have to be to achieve this pressure on a day when the temperature is 25C?
Asked by Melanie - Wed Jul 11 18:48:33 2007 - - 1 Answers - 0 Comments
A. Use this equation, osmotic pressure = CRT, where C is the concentration in molarity, R is the gas constant, and T is the temperature in Kelvin. So, the answers to your problems are: A) osmotic pressure = CRT to get C, get the number of moles of NaCl then divide it with volume of the solution mole NaCl = 0.923g / 58.442 g/mol mole NaCl = 0.0158 mol C = 0.0158 mol / 0.1L C = 0.158 mol/L So, osmotic pressure = 0.158 mol/L*(0.082058 L-atm/mol-K)*(25+273K) osmotic pressure = 3.86 atm B) C = osmotic pressure / RT C = 18.1 atm / (0.082058 L-atm/mol-K * 298K) C = 0.740 mol/L
Answered by titanium007 - Thu Jul 12 09:54:36 2007
Q. A)Isotonic saline solution, which has the same osomotic pressure as blood, can be prepared by dissolving 0.923g of NaCl in enough water to produce 100mL of solution. What is the osmotic pressure of this solution at 25C ? B)Osmosis is the process responsible for carrying nutrients and water from groundwater supplies to the upper parts of trees. The osmotic pressures required for this process can be as high as 18.1atm . What would the molar concentration of the tree sap have to be to achieve this pressure on a day when the temperature is 25C?
Asked by Melanie - Wed Jul 11 18:48:33 2007 - - 1 Answers - 0 Comments
A. Use this equation, osmotic pressure = CRT, where C is the concentration in molarity, R is the gas constant, and T is the temperature in Kelvin. So, the answers to your problems are: A) osmotic pressure = CRT to get C, get the number of moles of NaCl then divide it with volume of the solution mole NaCl = 0.923g / 58.442 g/mol mole NaCl = 0.0158 mol C = 0.0158 mol / 0.1L C = 0.158 mol/L So, osmotic pressure = 0.158 mol/L*(0.082058 L-atm/mol-K)*(25+273K) osmotic pressure = 3.86 atm B) C = osmotic pressure / RT C = 18.1 atm / (0.082058 L-atm/mol-K * 298K) C = 0.740 mol/L
Answered by titanium007 - Thu Jul 12 09:54:36 2007
What is the molar concentration of the ammonia with following info:?
Q. Ammonia has the formula NH3. Household ammonia is a dilute aqueous solution of NH3. Aqueous ammonia is a base that can neutralize acids. If 18.0 mL of 0.800 M HCl solution are needed to neutralize 5.00 mL of a household ammonia solution, what is the molar concentration of the ammonia?
Asked by Loopti - Tue Jun 9 22:18:18 2009 - - 1 Answers - 0 Comments
A. Write a balanced equation HCl + NH3 ---> NH4Cl(aq) 1 mole of HCl is required to neutralise 1 mole of NH3 So the nuber of moles of HCl in 18.0 ml of 0.800 M HCl = moles of NH3 in 5.00 ml ammonia solution Molarity = moles / L Therefore moles = Molarity x L moles HCl = 0.800 M x 0.0180 L moles HCl = 0.0144 moles Therefore there are 0.0144 moles of NH3 in the 5.00 ml of solution Molarity = moles / L = 0.0144 moles / 0.00500 L = 2.88 M NH3
Answered by Lexi R - Wed Jun 10 02:32:35 2009
Q. Ammonia has the formula NH3. Household ammonia is a dilute aqueous solution of NH3. Aqueous ammonia is a base that can neutralize acids. If 18.0 mL of 0.800 M HCl solution are needed to neutralize 5.00 mL of a household ammonia solution, what is the molar concentration of the ammonia?
Asked by Loopti - Tue Jun 9 22:18:18 2009 - - 1 Answers - 0 Comments
A. Write a balanced equation HCl + NH3 ---> NH4Cl(aq) 1 mole of HCl is required to neutralise 1 mole of NH3 So the nuber of moles of HCl in 18.0 ml of 0.800 M HCl = moles of NH3 in 5.00 ml ammonia solution Molarity = moles / L Therefore moles = Molarity x L moles HCl = 0.800 M x 0.0180 L moles HCl = 0.0144 moles Therefore there are 0.0144 moles of NH3 in the 5.00 ml of solution Molarity = moles / L = 0.0144 moles / 0.00500 L = 2.88 M NH3
Answered by Lexi R - Wed Jun 10 02:32:35 2009
What is the molar concentration of NaCl in the resulting solution? Look for details?
Q. We have dissolved 0.909 lbs of NaCl in 1.56 gallons of water. What is the molar concentration of NaCl in the resulting solution?
Asked by sh4olinh - Tue Feb 6 00:19:10 2007 - - 3 Answers - 0 Comments
A. 1.2 molar good luck
Answered by bige1236 - Tue Feb 6 00:31:04 2007
Q. We have dissolved 0.909 lbs of NaCl in 1.56 gallons of water. What is the molar concentration of NaCl in the resulting solution?
Asked by sh4olinh - Tue Feb 6 00:19:10 2007 - - 3 Answers - 0 Comments
A. 1.2 molar good luck
Answered by bige1236 - Tue Feb 6 00:31:04 2007
How do you calculate the molar concentration of a solution?
Q. I'm taking a correspondence course for chemistry, and I can't figure out these two questions: a) 12.9 g of potassium hydroxide, KOH, dissolved in water to make 2.5 L of solution. b) 0.08 g ethanol, C2H6O(l), in 100 mL of blood (the legal limit of blood alcohol concentration in Canada when driving a car) Can anyone explain how to calculate the molar concentration to these two questions, which are aqueous solutions? please? Thanks!
Asked by Em - Tue Mar 25 17:35:26 2008 - - 3 Answers - 0 Comments
A. Well, Im taking Chemistry as well here is how u do it: a) Molarity = moles/Liters therefore convert 12.9grams to moles by taking (12.9) and dividing it by (the mass of KOH,just go to a periodic table and add their molar masses). Once you have that number, divide it by 2.5 liters and there u have the molarity. If you think about it, your answer should be very small since your mixing only 12grams in a whole 2.5 LITERS of solution so it wont be very concentrated at all. b)the same as above, take (.08g) and divide it by the mass of (C2H6O) to solve for moles. Then you divide the moles by Liters. BUT WAIT!!! It is given in (mL) so u must convert to (L). To do that you divide the amount of mililiters u have by 1000. Once you have the amount… [cont.]
Answered by Issam H - Tue Mar 25 17:51:49 2008
Q. I'm taking a correspondence course for chemistry, and I can't figure out these two questions: a) 12.9 g of potassium hydroxide, KOH, dissolved in water to make 2.5 L of solution. b) 0.08 g ethanol, C2H6O(l), in 100 mL of blood (the legal limit of blood alcohol concentration in Canada when driving a car) Can anyone explain how to calculate the molar concentration to these two questions, which are aqueous solutions? please? Thanks!
Asked by Em - Tue Mar 25 17:35:26 2008 - - 3 Answers - 0 Comments
A. Well, Im taking Chemistry as well here is how u do it: a) Molarity = moles/Liters therefore convert 12.9grams to moles by taking (12.9) and dividing it by (the mass of KOH,just go to a periodic table and add their molar masses). Once you have that number, divide it by 2.5 liters and there u have the molarity. If you think about it, your answer should be very small since your mixing only 12grams in a whole 2.5 LITERS of solution so it wont be very concentrated at all. b)the same as above, take (.08g) and divide it by the mass of (C2H6O) to solve for moles. Then you divide the moles by Liters. BUT WAIT!!! It is given in (mL) so u must convert to (L). To do that you divide the amount of mililiters u have by 1000. Once you have the amount… [cont.]
Answered by Issam H - Tue Mar 25 17:51:49 2008
Chemistry what is the molar concentration of the solution?
Q. A 500.0 mL sodium iodide (Nal) solution contains 24.7 g of Nal. What is the molar concentration of the solution?
Asked by Keith - Sun May 17 12:00:24 2009 - - 1 Answers - 0 Comments
Q. A 500.0 mL sodium iodide (Nal) solution contains 24.7 g of Nal. What is the molar concentration of the solution?
Asked by Keith - Sun May 17 12:00:24 2009 - - 1 Answers - 0 Comments
what is the molar concentration of the solution?
Q. When 0.084 mol of aluminum sulfate are dis- solved in enough water to make 711 milliliters of solution, what is the molar concentration of aluminum ions? Answer in units of M.
Asked by myspanishprojectiscolorful - Wed Mar 25 19:05:59 2009 - - 2 Answers - 0 Comments
Q. When 0.084 mol of aluminum sulfate are dis- solved in enough water to make 711 milliliters of solution, what is the molar concentration of aluminum ions? Answer in units of M.
Asked by myspanishprojectiscolorful - Wed Mar 25 19:05:59 2009 - - 2 Answers - 0 Comments
Can someone explain the answer to this molar concentration question?
Q. What is the molar concentration of 2000mL of aqueous solution containing 135 grams of glucose, C6H12O6? A. 12.15M B. 0.750M C. 67.5 M D. 0.667 M E. 0.375 M I am a little confuse on how to get this answer, if you could explain the formula to me for the answer I would really appreciate it. Thank you.
Asked by Lonnie - Mon Mar 30 11:02:42 2009 - - 1 Answers - 0 Comments
A. the molecular weight of glucose is 180: 6x12 (carbon) + 12x1 (hydrogen) and 6x 16 (oxygen) You have 135 grammes in solution, molarity = actual mass/ molecular weight: 135/ 180 = 0.75
Answered by norm c - Mon Mar 30 11:12:58 2009
Q. What is the molar concentration of 2000mL of aqueous solution containing 135 grams of glucose, C6H12O6? A. 12.15M B. 0.750M C. 67.5 M D. 0.667 M E. 0.375 M I am a little confuse on how to get this answer, if you could explain the formula to me for the answer I would really appreciate it. Thank you.
Asked by Lonnie - Mon Mar 30 11:02:42 2009 - - 1 Answers - 0 Comments
A. the molecular weight of glucose is 180: 6x12 (carbon) + 12x1 (hydrogen) and 6x 16 (oxygen) You have 135 grammes in solution, molarity = actual mass/ molecular weight: 135/ 180 = 0.75
Answered by norm c - Mon Mar 30 11:12:58 2009
How do I find the molar concentration?
Q. Calculate the molar concentration of 13.17% (w/w) Na2CO3 solution at 20 C given that its density is 1.267 g mL-1. I made the equation part over whole and then manipulated the numbers to get the answer 1.5, but its wrong.
Asked by sn1per0nther00f - Mon Sep 1 21:02:38 2008 - - 1 Answers - 0 Comments
A. % w/w means % of solute by mass in total mass of solution so, in 100 g of solution you have 13.17 g of Na2CO3 Density = g / ml or weight in gram of 1 ml solution Therefore volume of 100 g of solution can be worked out from density density = 1.267 g / ml 100 g / y ml = 1.267 g / 1 ml therefore y ml = 100 / (1.267 / 1) = 78.93 ml So 100 g of solution, which contains 13.17 g of solute has a volume of 78.93 ml Molarity = moles / litres moles = mass / molar mass molar mass Na2CO3 = (22.99 x 2) + 12.01 + (3 x 16.00) = 105.99 g/mol therefore moles = mass / molar mass = 13.17 g / 105.98 g/mol = 0.1243 moles of Na2CO3 and M = moles / L = 0.1243 mol / 0.07893 L = 1.574 M (4 sig fig)
Answered by Lexi R - Tue Sep 2 02:58:58 2008
Q. Calculate the molar concentration of 13.17% (w/w) Na2CO3 solution at 20 C given that its density is 1.267 g mL-1. I made the equation part over whole and then manipulated the numbers to get the answer 1.5, but its wrong.
Asked by sn1per0nther00f - Mon Sep 1 21:02:38 2008 - - 1 Answers - 0 Comments
A. % w/w means % of solute by mass in total mass of solution so, in 100 g of solution you have 13.17 g of Na2CO3 Density = g / ml or weight in gram of 1 ml solution Therefore volume of 100 g of solution can be worked out from density density = 1.267 g / ml 100 g / y ml = 1.267 g / 1 ml therefore y ml = 100 / (1.267 / 1) = 78.93 ml So 100 g of solution, which contains 13.17 g of solute has a volume of 78.93 ml Molarity = moles / litres moles = mass / molar mass molar mass Na2CO3 = (22.99 x 2) + 12.01 + (3 x 16.00) = 105.99 g/mol therefore moles = mass / molar mass = 13.17 g / 105.98 g/mol = 0.1243 moles of Na2CO3 and M = moles / L = 0.1243 mol / 0.07893 L = 1.574 M (4 sig fig)
Answered by Lexi R - Tue Sep 2 02:58:58 2008
Molar Concentration of Chloride ions in a new solution?
Q. Need help solving this chemistry problem. I don't know how to start or what formula to use to discover the answer. Would be nice if you could show me that as you go, thanks. A solution is made by mixing 40.0ml of 0.750m (molarity) AlCl3 with 50.0ml of 0.400m (molarity) NaCl. What is the molar concentration of the chloride ions in the new solution?
Asked by kaijura - Fri Mar 20 20:39:32 2009 - - 1 Answers - 0 Comments
A. Firstly, you should always show Molarity as M m is the symbol for molality ( moles solute / kg solvent) and can be quite a different value. You need to work out how many total moles of Cl- you have in the new solution, so you need to work out the moles of Cl- in each solution added. Molarity = moles / litres Therefore moles = molarity x L - moles in 40.0 ml (0.0400 L) of 0.750 M AlCl3 moles AlCl3 = 0.750 M x 0.0400 L moles AlCl3 = 0.0300 moles Each AlCl3 has 3 Cl- Therefore moles Cl- = 3 x moles AlCl3 Cl- = 3 x 0.0300 mol = 0.0900 moles Cl- moles Cl- in 50.0 ml (0.0500 L) 0.400 M NaCl moles NaCl = M x L moles NaCl = 0.400 M x 0.0500 L = 0.0200 moles NaCl Each NaCl has 1 Cl- Therefore moles Cl- = 0.0200 moles Total moles Cl- = 0.0900 [cont.]
Answered by Lexi R - Sat Mar 21 10:11:39 2009
Q. Need help solving this chemistry problem. I don't know how to start or what formula to use to discover the answer. Would be nice if you could show me that as you go, thanks. A solution is made by mixing 40.0ml of 0.750m (molarity) AlCl3 with 50.0ml of 0.400m (molarity) NaCl. What is the molar concentration of the chloride ions in the new solution?
Asked by kaijura - Fri Mar 20 20:39:32 2009 - - 1 Answers - 0 Comments
A. Firstly, you should always show Molarity as M m is the symbol for molality ( moles solute / kg solvent) and can be quite a different value. You need to work out how many total moles of Cl- you have in the new solution, so you need to work out the moles of Cl- in each solution added. Molarity = moles / litres Therefore moles = molarity x L - moles in 40.0 ml (0.0400 L) of 0.750 M AlCl3 moles AlCl3 = 0.750 M x 0.0400 L moles AlCl3 = 0.0300 moles Each AlCl3 has 3 Cl- Therefore moles Cl- = 3 x moles AlCl3 Cl- = 3 x 0.0300 mol = 0.0900 moles Cl- moles Cl- in 50.0 ml (0.0500 L) 0.400 M NaCl moles NaCl = M x L moles NaCl = 0.400 M x 0.0500 L = 0.0200 moles NaCl Each NaCl has 1 Cl- Therefore moles Cl- = 0.0200 moles Total moles Cl- = 0.0900 [cont.]
Answered by Lexi R - Sat Mar 21 10:11:39 2009
How can you find the molar concentration of a neutral compounds?
Q. Molar Concentration of a neutral compound
Asked by hotmose3 - Thu Dec 27 17:56:09 2007 - - 4 Answers - 0 Comments
A. Yellow pages?
Answered by GaBoy - Thu Dec 27 17:59:11 2007
Q. Molar Concentration of a neutral compound
Asked by hotmose3 - Thu Dec 27 17:56:09 2007 - - 4 Answers - 0 Comments
A. Yellow pages?
Answered by GaBoy - Thu Dec 27 17:59:11 2007
What is the molar concentration of sodium hypochlorite (Bleach)?
Q. The active ingredient in bleach, NaOCl, is present at 6.00%. That substance has a mass of 74.44 g/mole and the solution has a density of 1.10 g/mL. How do I find its molar concentration?
Asked by Matt - Sun Apr 27 20:00:58 2008 - - 1 Answers - 0 Comments
A. Calculate the mass of 1 liter- 1000 mL x 1.10 g/mL = 1100 grams Calulate the mass of NaOCl- 1100 grams x 0.0600 = 66.0 grams Calculate the moles of NaOCl- 66.0 g / 74.44 g/mole = 0.887 moles Molarity = 0.887 moles/liter
Answered by skipper - Sun Apr 27 20:13:50 2008
Q. The active ingredient in bleach, NaOCl, is present at 6.00%. That substance has a mass of 74.44 g/mole and the solution has a density of 1.10 g/mL. How do I find its molar concentration?
Asked by Matt - Sun Apr 27 20:00:58 2008 - - 1 Answers - 0 Comments
A. Calculate the mass of 1 liter- 1000 mL x 1.10 g/mL = 1100 grams Calulate the mass of NaOCl- 1100 grams x 0.0600 = 66.0 grams Calculate the moles of NaOCl- 66.0 g / 74.44 g/mole = 0.887 moles Molarity = 0.887 moles/liter
Answered by skipper - Sun Apr 27 20:13:50 2008
Intro to Chemistry question: Molar and Molal concentration of ions?
Q. The question is: What is the molar concentration of ions in a 1.5 M KNO3 solution? What is the Molal Concentration of ions in a 1.5 m KNO3 solution? (please provide all the work and steps, it will help A LOT!!! Thanks!
Asked by danie - Tue Jul 8 23:48:18 2008 - - 1 Answers - 0 Comments
A. A solution of KNO3 completely dissociates into K+1 ions and NO3 -1 ions. So...if you start with a 1.5M solution you get 1.5M K+1 and 1.5M NO3 -1 (1:1:1 ratio) If you want the TOTAL molar concentraion of ions it would be 3.0M Same reasoning for the molal solution: 1:1:1 ratio
Answered by The Old Professor - Tue Jul 8 23:55:20 2008
Q. The question is: What is the molar concentration of ions in a 1.5 M KNO3 solution? What is the Molal Concentration of ions in a 1.5 m KNO3 solution? (please provide all the work and steps, it will help A LOT!!! Thanks!
Asked by danie - Tue Jul 8 23:48:18 2008 - - 1 Answers - 0 Comments
A. A solution of KNO3 completely dissociates into K+1 ions and NO3 -1 ions. So...if you start with a 1.5M solution you get 1.5M K+1 and 1.5M NO3 -1 (1:1:1 ratio) If you want the TOTAL molar concentraion of ions it would be 3.0M Same reasoning for the molal solution: 1:1:1 ratio
Answered by The Old Professor - Tue Jul 8 23:55:20 2008
Question on calculating molar concentration of the solution.?
Q. A 4000 ml solution of AgNO3 contains 17.00 g of solute in water. Calculate the molar concentration of the solution.
Asked by Mimi - Fri Jul 24 12:33:07 2009 - - 1 Answers - 0 Comments
A. Molar Concentration = No of moles/ volume in litres = 17.00g/170gper molex4L = 0.025 mole/litre (Answer)
Answered by vij - Fri Jul 24 12:41:42 2009
Q. A 4000 ml solution of AgNO3 contains 17.00 g of solute in water. Calculate the molar concentration of the solution.
Asked by Mimi - Fri Jul 24 12:33:07 2009 - - 1 Answers - 0 Comments
A. Molar Concentration = No of moles/ volume in litres = 17.00g/170gper molex4L = 0.025 mole/litre (Answer)
Answered by vij - Fri Jul 24 12:41:42 2009
Convert the following value to a molar concentration.?
Q. If the maximum allowable concentration of lead in water is 0.01 mg/L convert this value to a molar concentration. What are the steps to complete this problem?
Asked by Jada - Sun Jan 6 19:55:14 2008 - - 1 Answers - 0 Comments
A. 0.01 mg = 0.0001 gram 0.0001 g per L / 207.2 g per mol = 4.8 x 10^-8 mol per liter 4.8x10^-8 Molar
Answered by skipper - Sun Jan 6 20:03:59 2008
Q. If the maximum allowable concentration of lead in water is 0.01 mg/L convert this value to a molar concentration. What are the steps to complete this problem?
Asked by Jada - Sun Jan 6 19:55:14 2008 - - 1 Answers - 0 Comments
A. 0.01 mg = 0.0001 gram 0.0001 g per L / 207.2 g per mol = 4.8 x 10^-8 mol per liter 4.8x10^-8 Molar
Answered by skipper - Sun Jan 6 20:03:59 2008
How can I calculate the molar concentration of ca ^2+ in the unknown solution in mol/L?
Q. Hello~ I did Gravimetric Determinarion of Calcium experimnet and I got 0.2191g CaC204 H20 (hydrate calcium oxlate) so, how can I calculate the molar concentration of ca ^2+ in the unknown solution in mol/L?? plz help me Thank you!
Asked by qufkrl - Tue Nov 3 22:43:02 2009 - - 1 Answers - 0 Comments
A. use the molar mass of calcium oxalate to find moles: 0.2191g CaC204 H20 @ 146.112 g/mol = 0.001499 mol CaC204 H20 since 1 mole of calcium oxalate has 1 mole of calcium, 0.001499 mol CaC204 H20 = 0.0014995 mol Ca to find Molarity of Ca+2, divide the moles of Ca by the sample size: if a 25.00 ml sample, gave the 0.2191g CaC204 H20, ... then: 0.0014995 mol Ca / 0.02500 litres = 0.05998 Molar Ca+2 if a 100.0 ml sample gave the 0.2191g CaC204 H20...then: 0.0014995 mol Ca / 0.1000 litres = 0.01500 Molar Ca+2
Answered by Steve O - Wed Nov 4 00:32:00 2009
Q. Hello~ I did Gravimetric Determinarion of Calcium experimnet and I got 0.2191g CaC204 H20 (hydrate calcium oxlate) so, how can I calculate the molar concentration of ca ^2+ in the unknown solution in mol/L?? plz help me Thank you!
Asked by qufkrl - Tue Nov 3 22:43:02 2009 - - 1 Answers - 0 Comments
A. use the molar mass of calcium oxalate to find moles: 0.2191g CaC204 H20 @ 146.112 g/mol = 0.001499 mol CaC204 H20 since 1 mole of calcium oxalate has 1 mole of calcium, 0.001499 mol CaC204 H20 = 0.0014995 mol Ca to find Molarity of Ca+2, divide the moles of Ca by the sample size: if a 25.00 ml sample, gave the 0.2191g CaC204 H20, ... then: 0.0014995 mol Ca / 0.02500 litres = 0.05998 Molar Ca+2 if a 100.0 ml sample gave the 0.2191g CaC204 H20...then: 0.0014995 mol Ca / 0.1000 litres = 0.01500 Molar Ca+2
Answered by Steve O - Wed Nov 4 00:32:00 2009
College Chemistry Question: Can you answer this molar concentration question?
Q. A lab technician dilutes a 45.5 mL of a 1.50 mol/L solution to a final volume of 200.0 mL. What is the concentration of the diluted solution?
Asked by Chelsea L - Mon Jun 8 17:00:41 2009 - - 1 Answers - 0 Comments
A. 0.0455L * 1.50 mol/L = 0.06825 mol Concentration = 0.06825 mol / 0.2L Concentration = 0.34125 mol/L
Answered by Fanservice - Mon Jun 8 17:54:38 2009
Q. A lab technician dilutes a 45.5 mL of a 1.50 mol/L solution to a final volume of 200.0 mL. What is the concentration of the diluted solution?
Asked by Chelsea L - Mon Jun 8 17:00:41 2009 - - 1 Answers - 0 Comments
A. 0.0455L * 1.50 mol/L = 0.06825 mol Concentration = 0.06825 mol / 0.2L Concentration = 0.34125 mol/L
Answered by Fanservice - Mon Jun 8 17:54:38 2009
From Yahoo Answer Search: 'molar concentration'
Wed Nov 18 00:16:38 2009 [ refresh local cache ]
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Wed, 07 Jan 2009 00:00:37 GM
(lower case letters represent . molar. ratios; upper case letters represent actual compounds, but in the equation, . molar concentration. of the compounds). stoichiometry molarity=moles/liters of solution. here we have this sort of induction ...
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