molar concentration?
Q. A solution was made by dissolving 0.514 g Ba(OH)2 in 320 mL final volume. What is the molar concentration of OH- in the solution? What is the pOH?What is the pH?
Asked by wonderer - Tue Apr 24 17:42:12 2007 - - 1 Answers - 0 Comments
A. Ba(OH)2 dissociates in solution: Ba(OH)2 --> Ba2+ (aq) + 2OH- (aq) 1 mole of Ba(OH)2 will form 2 moles of OH- but how many moles of Ba(OH)2 are in 0.514 grams? To find that out, divide the mass by the molar mass, which is 171.32 grams per mole, and you get 0.003 moles. So 0.006 moles of OH- are produced. Molarity is moles divided by volume. Convert 320 mL into Liters: 0.006 moles / 0.320 L = 0.019 M pOH = -log [OH-] pOH = -log(0.019) pOH = 1.72 pH + pOH = 14 pH = 14 - pOH pH = 14 - 1.72 pH = 12.28
Answered by coconutty beanz xD - Tue Apr 24 17:50:20 2007
Q. A solution was made by dissolving 0.514 g Ba(OH)2 in 320 mL final volume. What is the molar concentration of OH- in the solution? What is the pOH?What is the pH?
Asked by wonderer - Tue Apr 24 17:42:12 2007 - - 1 Answers - 0 Comments
A. Ba(OH)2 dissociates in solution: Ba(OH)2 --> Ba2+ (aq) + 2OH- (aq) 1 mole of Ba(OH)2 will form 2 moles of OH- but how many moles of Ba(OH)2 are in 0.514 grams? To find that out, divide the mass by the molar mass, which is 171.32 grams per mole, and you get 0.003 moles. So 0.006 moles of OH- are produced. Molarity is moles divided by volume. Convert 320 mL into Liters: 0.006 moles / 0.320 L = 0.019 M pOH = -log [OH-] pOH = -log(0.019) pOH = 1.72 pH + pOH = 14 pH = 14 - pOH pH = 14 - 1.72 pH = 12.28
Answered by coconutty beanz xD - Tue Apr 24 17:50:20 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 a 1 Liter solution of HCl that has 65 grams of HCl in it?
Q. What is the molar concentration of a 1 Liter solution of HCl that has 65 grams of HCl in it?
Asked by x3_crazii_babii_x3 - Thu Sep 10 13:21:29 2009 - - 1 Answers - 0 Comments
A. You have a 1 liter solution. It has 65 g HCl; the molecular weight of HCl is 36.5 g / mole therefore you have 65 g HCl/ (36.5 g HCl/ mole HCl) = 65/36.5 moles of HCl. This means you have 65/36.3 moles HCl/ Liter of solution. Molarity is moles per liter so you have your answer. You can do the calculation.
Answered by GTB - Thu Sep 10 13:30:24 2009
Q. What is the molar concentration of a 1 Liter solution of HCl that has 65 grams of HCl in it?
Asked by x3_crazii_babii_x3 - Thu Sep 10 13:21:29 2009 - - 1 Answers - 0 Comments
A. You have a 1 liter solution. It has 65 g HCl; the molecular weight of HCl is 36.5 g / mole therefore you have 65 g HCl/ (36.5 g HCl/ mole HCl) = 65/36.5 moles of HCl. This means you have 65/36.3 moles HCl/ Liter of solution. Molarity is moles per liter so you have your answer. You can do the calculation.
Answered by GTB - Thu Sep 10 13:30:24 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 total molar concentration of ions in each of the following solutions?
Q. What is the total molar concentration of ions in each of the following solutions 1- 1.185 M solution of CH3OH 2- 0.200 M solution of HClO4
Asked by BEST GUY :) - Sun Nov 8 11:39:45 2009 - - 1 Answers - 0 Comments
A. 1- The pKa of methanol is >15; the pkA of water is 14. Methanol doesn't dissociate into aqueous ions; only water contributes ions. [ions] = 2x10^-7 M 2- Perchloric acid is a strong acid. [ions] = 0.4M
Answered by im - Sun Nov 8 11:50:54 2009
Q. What is the total molar concentration of ions in each of the following solutions 1- 1.185 M solution of CH3OH 2- 0.200 M solution of HClO4
Asked by BEST GUY :) - Sun Nov 8 11:39:45 2009 - - 1 Answers - 0 Comments
A. 1- The pKa of methanol is >15; the pkA of water is 14. Methanol doesn't dissociate into aqueous ions; only water contributes ions. [ions] = 2x10^-7 M 2- Perchloric acid is a strong acid. [ions] = 0.4M
Answered by im - Sun Nov 8 11:50:54 2009
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
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 this solution?
Q. Hydrogen peroxide, H2O2. The label claims this solution is 3.0%; that is there are 3.0 grams of H2O2 in every 100 grams of solution. What is the molar concentration of this solution? (Assume a density of 1.00 g/mL)
Asked by Alfaba Fett - Wed Oct 14 12:06:54 2009 - - 1 Answers - 0 Comments
A. volume solution = 100 g / 1.00 g/mL = 100 mL = 0.100 L moles H2O2 = 3.0 g/34.014 g/mol=0.0882 M = 0.0882 / 0.100 L= 0.882
Answered by Dr.A - Wed Oct 14 12:45:26 2009
Q. Hydrogen peroxide, H2O2. The label claims this solution is 3.0%; that is there are 3.0 grams of H2O2 in every 100 grams of solution. What is the molar concentration of this solution? (Assume a density of 1.00 g/mL)
Asked by Alfaba Fett - Wed Oct 14 12:06:54 2009 - - 1 Answers - 0 Comments
A. volume solution = 100 g / 1.00 g/mL = 100 mL = 0.100 L moles H2O2 = 3.0 g/34.014 g/mol=0.0882 M = 0.0882 / 0.100 L= 0.882
Answered by Dr.A - Wed Oct 14 12:45:26 2009
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
What is the total molar concentration of ions?
Q. What is the total molar concentration of ionsin each of the following solutions? 1)A 1.400 M solution of CH3OH 2)A 0.235 M solution of HClO4
Asked by m6 - Sun Nov 2 16:44:45 2008 - - 1 Answers - 0 Comments
A. 1)A 1.400 M solution of CH3OH essentially zero, 2)A 0.235 M solution of HClO4 0.235 M H+ ions & 0.235M ClO4- ions
Answered by Steve O - Sun Nov 2 17:24:14 2008
Q. What is the total molar concentration of ionsin each of the following solutions? 1)A 1.400 M solution of CH3OH 2)A 0.235 M solution of HClO4
Asked by m6 - Sun Nov 2 16:44:45 2008 - - 1 Answers - 0 Comments
A. 1)A 1.400 M solution of CH3OH essentially zero, 2)A 0.235 M solution of HClO4 0.235 M H+ ions & 0.235M ClO4- ions
Answered by Steve O - Sun Nov 2 17:24:14 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 do you calculate molar concentration?
Q. how to calculate the molar concentration of Al2(SO4)3 in 25.00mL solution
Asked by jasmine - Thu Sep 25 15:33:38 2008 - - 1 Answers - 0 Comments
A. Mass of Al2(SO4)3 is needed
Answered by Dr.A - Thu Sep 25 15:39:53 2008
Q. how to calculate the molar concentration of Al2(SO4)3 in 25.00mL solution
Asked by jasmine - Thu Sep 25 15:33:38 2008 - - 1 Answers - 0 Comments
A. Mass of Al2(SO4)3 is needed
Answered by Dr.A - Thu Sep 25 15:39:53 2008
How do i calculate the molar concentration of Ag+ ions in this problem?
Q. 121 mL of 1.54M AgNO3 is mixed with 45 mL of 1.17mL of K2SO4. calc the molar concentration of Ag+ ions in the final solution im getting .463 M but its telling me im wrong... what am i doing wrong? i mean .464... rounded
Asked by Mike - Thu Mar 19 02:25:59 2009 - - 2 Answers - 0 Comments
A. find the no. of moles of AgNO3. since 1 mole of AgNO3 gives 1 mole of Ag+, this figure will also be the no. of moles of Ag+. find the no. of moles of K2SO4. 1 mole of it gives 1 mole of SO42- so this fig will be e no of moles of SO42-. 2Ag+ + SO42- -> Ag2SO4 each mole of SO42- requires 2 moles of Ag+, so multiply no. of moles of SO42- by 2 and minus this from the no. of moles of Ag+. then divide this figure by the total vol of liquid (121x10^-3 +45x10^-3) to get the molar conc of Ag+.
Answered by charlotte - Thu Mar 19 02:40:56 2009
Q. 121 mL of 1.54M AgNO3 is mixed with 45 mL of 1.17mL of K2SO4. calc the molar concentration of Ag+ ions in the final solution im getting .463 M but its telling me im wrong... what am i doing wrong? i mean .464... rounded
Asked by Mike - Thu Mar 19 02:25:59 2009 - - 2 Answers - 0 Comments
A. find the no. of moles of AgNO3. since 1 mole of AgNO3 gives 1 mole of Ag+, this figure will also be the no. of moles of Ag+. find the no. of moles of K2SO4. 1 mole of it gives 1 mole of SO42- so this fig will be e no of moles of SO42-. 2Ag+ + SO42- -> Ag2SO4 each mole of SO42- requires 2 moles of Ag+, so multiply no. of moles of SO42- by 2 and minus this from the no. of moles of Ag+. then divide this figure by the total vol of liquid (121x10^-3 +45x10^-3) to get the molar conc of Ag+.
Answered by charlotte - Thu Mar 19 02:40:56 2009
What is the molar concentration of the Fe3+?
Q. A solution contains Fe2(SO4)3 as the only solute. The sulfate ion concentration in the solution is 0.501 M. What is the molar concentration of the Fe3+?
Asked by Pat M - Tue Mar 6 23:41:55 2007 - - 1 Answers - 0 Comments
A. When you break down the solution, you get Fe+3 and So-2 4. The sulphate ion have parts in the solution compared to Fe. 4 parts= 0.501, 1 part= 0.12525 So, the molar concentration of Fe+3 is 0.12125M I hope this helps. :)
Answered by Juni Mccoy - Tue Mar 6 23:47:44 2007
Q. A solution contains Fe2(SO4)3 as the only solute. The sulfate ion concentration in the solution is 0.501 M. What is the molar concentration of the Fe3+?
Asked by Pat M - Tue Mar 6 23:41:55 2007 - - 1 Answers - 0 Comments
A. When you break down the solution, you get Fe+3 and So-2 4. The sulphate ion have parts in the solution compared to Fe. 4 parts= 0.501, 1 part= 0.12525 So, the molar concentration of Fe+3 is 0.12125M I hope this helps. :)
Answered by Juni Mccoy - Tue Mar 6 23:47:44 2007
Calculate the molar concentration of hydroxyl ions in a 0.511 M solution of sodium hypobromite ion, NaBrO?
Q. Calculate the molar concentration of hydroxyl ions in a 0.511 M solution of sodium hypobromite ion, NaBrO (Kb = 4.0 10-6). What is the pH of this solution?
Asked by Ashley G - Wed Mar 5 13:20:20 2008 - - 1 Answers - 0 Comments
A. BrO- + H2O <---> HBrO + OH- 4.0 x 10^-6 = x^2 / 0.511-x x = [OH-] =0.00143 M pOH = - log 0.00143 =2.85 pH = 14 - 2.85 =11.15
Answered by Dr.A - Wed Mar 5 14:32:39 2008
Q. Calculate the molar concentration of hydroxyl ions in a 0.511 M solution of sodium hypobromite ion, NaBrO (Kb = 4.0 10-6). What is the pH of this solution?
Asked by Ashley G - Wed Mar 5 13:20:20 2008 - - 1 Answers - 0 Comments
A. BrO- + H2O <---> HBrO + OH- 4.0 x 10^-6 = x^2 / 0.511-x x = [OH-] =0.00143 M pOH = - log 0.00143 =2.85 pH = 14 - 2.85 =11.15
Answered by Dr.A - Wed Mar 5 14:32:39 2008
I dont know how to determine molar concentration please help?
Q. I need to calculate the molar concentration of H3O+ in a 0.40 M HF (aq) solution
Asked by Kaia - Thu Jan 1 17:11:30 2009 - - 1 Answers - 0 Comments
A. I don't know the level of chemistry that you are at so; The very basic answer HF + H2O = H3O+ + F- As 1 mole of HF produces 1 mole of H3O+ the concentration of H3O+ will be 0.40M. This answer assumes that the entire Hf will dissociate. Full answer; if you have studied equilibrium constants (ie pKa or Ka) pKa for HF is 3.17 As pKa = -logKa The Ka = 6.76*10-4 From the above equation Ka = product/reactants = [H3O+][F-]/[HF] As one mole of HF will dissociate to form 1 mole of H3O= and 1 mole of F- then [H3O+] = [F-] Substitute this into the equation Ka = [H3O+][H3O+]/[HF] rearrange to solve for [H3O+] [H3O+] = (Ka * [HF])^0.5 = 0.016M
Answered by ktrna69 - Thu Jan 1 17:27:24 2009
Q. I need to calculate the molar concentration of H3O+ in a 0.40 M HF (aq) solution
Asked by Kaia - Thu Jan 1 17:11:30 2009 - - 1 Answers - 0 Comments
A. I don't know the level of chemistry that you are at so; The very basic answer HF + H2O = H3O+ + F- As 1 mole of HF produces 1 mole of H3O+ the concentration of H3O+ will be 0.40M. This answer assumes that the entire Hf will dissociate. Full answer; if you have studied equilibrium constants (ie pKa or Ka) pKa for HF is 3.17 As pKa = -logKa The Ka = 6.76*10-4 From the above equation Ka = product/reactants = [H3O+][F-]/[HF] As one mole of HF will dissociate to form 1 mole of H3O= and 1 mole of F- then [H3O+] = [F-] Substitute this into the equation Ka = [H3O+][H3O+]/[HF] rearrange to solve for [H3O+] [H3O+] = (Ka * [HF])^0.5 = 0.016M
Answered by ktrna69 - Thu Jan 1 17:27:24 2009
How do I calculate the equilibrium molar concentration ??
Q. How do i do this consider 1.30 mol of carbon monoxide and 2.40 mol of chlorine sealed in a 7.00 L container at 476 oC. The equilibrium constant, Kc, is 2.50 (in M-1) for CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium molar concentration of CO.
Asked by BumbleBee - Tue Feb 16 20:12:34 2010 - - 1 Answers - 0 Comments
Q. How do i do this consider 1.30 mol of carbon monoxide and 2.40 mol of chlorine sealed in a 7.00 L container at 476 oC. The equilibrium constant, Kc, is 2.50 (in M-1) for CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium molar concentration of CO.
Asked by BumbleBee - Tue Feb 16 20:12:34 2010 - - 1 Answers - 0 Comments
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Moran Wang
Fri, 02 May 2008 01:23:02 GM
The other parameters are c d =0.1 for the microstructure generation process, the bulk . molar concentration. c =10 -4 M, and = -50 mV. The electroosmotic permeability increases with the porosity monotonically. ...
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