What Is the Molarity of 85% Phosphoric Acid Answers
Concentration Problems!?
Q. If you could please try and help. Show working please (: 1.) How many grams of sulfuric acid are present in .500L of a .150M solution? 2.) What volume of a .500M solution of HBr is needed for a reaction that requires 32.5g of HBr? 3.) To produce 40.0g of silver chromate, Ag2Cr O4, you will need at least 23.4g of potassium chromate, K2Cr O4, in solution. All you have on hand in the stock room is 6.0M K2Cr O4 solution. What volume of the solution is needed to give you the 23.4g of potassium chromate needed for this reaction? 4.) What is the molarity of a solution composed of 13.0g of Na Cl dissolved in 500.g of water? 5.) A commercially available solution of Phosphoric Acid, H3PO4, in water is labeled 85.0% Phosphoric Acid with a stated… [cont.]
Asked by StingRay - Sun Apr 17 09:20:16 2011 - Chemistry - 2 Answers - Comments
A. Wassup Taism-er ;)
Answered by - Mon Apr 18 14:27:46 2011
Q. If you could please try and help. Show working please (: 1.) How many grams of sulfuric acid are present in .500L of a .150M solution? 2.) What volume of a .500M solution of HBr is needed for a reaction that requires 32.5g of HBr? 3.) To produce 40.0g of silver chromate, Ag2Cr O4, you will need at least 23.4g of potassium chromate, K2Cr O4, in solution. All you have on hand in the stock room is 6.0M K2Cr O4 solution. What volume of the solution is needed to give you the 23.4g of potassium chromate needed for this reaction? 4.) What is the molarity of a solution composed of 13.0g of Na Cl dissolved in 500.g of water? 5.) A commercially available solution of Phosphoric Acid, H3PO4, in water is labeled 85.0% Phosphoric Acid with a stated… [cont.]
Asked by StingRay - Sun Apr 17 09:20:16 2011 - Chemistry - 2 Answers - Comments
A. Wassup Taism-er ;)
Answered by - Mon Apr 18 14:27:46 2011
How do you calculate Molarity and Normality?
Q. What are the molarity and normality of the following concentrated acids? a) acetic acid b) 85% phosphoric acid c) sulfuric acid d) nitric acid e) HCl if someone could just show me an example of how to do one or two parts, that would be really helpful. Thanks :)
Asked by ChEMIsTrY ChICkiE - Sat Sep 12 12:15:30 2009 - Chemistry - 1 Answers - Comments
A. I must know the density and the % by mass I'm sorry
Answered by Dr.A - Wed Sep 16 11:57:37 2009
Q. What are the molarity and normality of the following concentrated acids? a) acetic acid b) 85% phosphoric acid c) sulfuric acid d) nitric acid e) HCl if someone could just show me an example of how to do one or two parts, that would be really helpful. Thanks :)
Asked by ChEMIsTrY ChICkiE - Sat Sep 12 12:15:30 2009 - Chemistry - 1 Answers - Comments
A. I must know the density and the % by mass I'm sorry
Answered by Dr.A - Wed Sep 16 11:57:37 2009
Density of concentrated phosphoric acid?
Q. concentrated phosphoric acid is 85% by mass H3PO4 assume the rest is water molarity of H3PO4 is 14.5M what is the density of the SOLUTION?
Asked by - Wed Feb 2 20:11:33 2011 - Chemistry - 2 Answers - Comments
A. To make life easy, assume that you have 1.000 L of the solution. In the liter you will have 14.5 moles of H3PO4 (molar mass = 98.0 g/mol) The mass of H3PO4 will be 14.5 mol x 98.0 g/mol = 1421 g You know that the solution is 85 % H3PO4, so you can find the total mass of the solution by writing .85 x = 1421 x = 1671 g Density = mass / volume Density = 1671 g / 1.000 L Density = 1671 g/L or 1.67 g/m L (to 3 sig. fig.)
Answered by - Wed Feb 2 20:30:01 2011
Q. concentrated phosphoric acid is 85% by mass H3PO4 assume the rest is water molarity of H3PO4 is 14.5M what is the density of the SOLUTION?
Asked by - Wed Feb 2 20:11:33 2011 - Chemistry - 2 Answers - Comments
A. To make life easy, assume that you have 1.000 L of the solution. In the liter you will have 14.5 moles of H3PO4 (molar mass = 98.0 g/mol) The mass of H3PO4 will be 14.5 mol x 98.0 g/mol = 1421 g You know that the solution is 85 % H3PO4, so you can find the total mass of the solution by writing .85 x = 1421 x = 1671 g Density = mass / volume Density = 1671 g / 1.000 L Density = 1671 g/L or 1.67 g/m L (to 3 sig. fig.)
Answered by - Wed Feb 2 20:30:01 2011
AP Chemistry Help please!!?
Q. Ok so I have to conduct a lab for AP Chemistry and I need phosphoric acid with a certain molarity. The only phosphoric acid in our chemical storage only says 85% and gives no molarity as far as I can tell. So what is the molarity of the 85% phosphoric acid?
Asked by goheels550 - Tue Jan 15 17:14:34 2008 - Chemistry - 3 Answers - 2 Comments
A. In these settings, an 85% solution usually means 85g of phosphoric acid per 100 m L water. You can convert it to molarity by doing some simple calculations: (85 g phosphoric acid / 100 m L water) * (1 mol phosphoric acid / 98.0 g phosphoric acid) = (0.867 mol phosphoric acid / 100 m L water) (0.867 mol phosphoric acid / 100 m L water) * (1000 m L / L) = (8.67 mol phosphoric acid / L water) So, you have 8.67 moles of phosphoric acid in a liter of water. Your molar concentration is 8.67 M.
Answered by Shan - Tue Jan 15 17:29:08 2008
Q. Ok so I have to conduct a lab for AP Chemistry and I need phosphoric acid with a certain molarity. The only phosphoric acid in our chemical storage only says 85% and gives no molarity as far as I can tell. So what is the molarity of the 85% phosphoric acid?
Asked by goheels550 - Tue Jan 15 17:14:34 2008 - Chemistry - 3 Answers - 2 Comments
A. In these settings, an 85% solution usually means 85g of phosphoric acid per 100 m L water. You can convert it to molarity by doing some simple calculations: (85 g phosphoric acid / 100 m L water) * (1 mol phosphoric acid / 98.0 g phosphoric acid) = (0.867 mol phosphoric acid / 100 m L water) (0.867 mol phosphoric acid / 100 m L water) * (1000 m L / L) = (8.67 mol phosphoric acid / L water) So, you have 8.67 moles of phosphoric acid in a liter of water. Your molar concentration is 8.67 M.
Answered by Shan - Tue Jan 15 17:29:08 2008
How do you calculate Molarity and Normality?
Q. What are the molarity and normality of the following concentrated acids? a) acetic acid b) 85% phosphoric acid c) sulfuric acid d) nitric acid e) HCl if someone could just show me an example of how to do one or two parts, that would be really helpful. Thanks :)
Asked by ChEMIsTrY ChICkiE - Sat Sep 12 12:15:30 2009 - Chemistry - 1 Answers - Comments
A. Molarity= No. of Moles/ Volume of solution Now here's the Hint- Normality= Molarity * Z [valency factor] Z is always known to us Thus by knowing molarity, normality can be calculated
Answered by - Sat Sep 12 12:37:07 2009
Q. What are the molarity and normality of the following concentrated acids? a) acetic acid b) 85% phosphoric acid c) sulfuric acid d) nitric acid e) HCl if someone could just show me an example of how to do one or two parts, that would be really helpful. Thanks :)
Asked by ChEMIsTrY ChICkiE - Sat Sep 12 12:15:30 2009 - Chemistry - 1 Answers - Comments
A. Molarity= No. of Moles/ Volume of solution Now here's the Hint- Normality= Molarity * Z [valency factor] Z is always known to us Thus by knowing molarity, normality can be calculated
Answered by - Sat Sep 12 12:37:07 2009
chemistry density problem?
Q. I have no idea how to do this chemistry density problem please help me if you can and explain how you got the answer Concentrated phosphoric acid si 85.0% by mass H3PO4. If the molarity of concentrated H3PO4 is 14.5 M, what is the density? a 1.95 g/m L b not enough information to solve c 1.87 g/m L d 1.32 g/m L e 1.67 g/m L
Asked by - Sat Dec 17 15:09:51 2011 - Chemistry - 1 Answers - Comments
A. in 1.000 L (1000 m L) there are 14.5 moles of H3PO4. (14.5 mol H3PO4) x (97.9953 g H3PO4/mol) = 1420.9 g H3PO4 (1420.9 g) / (0.850) = 1671.6 g total weight density = (1671.6 g) / (1000 m L) = 1.67 g/m L So answer e.
Answered by Roger the Mole - Sat Dec 17 18:24:36 2011
Q. I have no idea how to do this chemistry density problem please help me if you can and explain how you got the answer Concentrated phosphoric acid si 85.0% by mass H3PO4. If the molarity of concentrated H3PO4 is 14.5 M, what is the density? a 1.95 g/m L b not enough information to solve c 1.87 g/m L d 1.32 g/m L e 1.67 g/m L
Asked by - Sat Dec 17 15:09:51 2011 - Chemistry - 1 Answers - Comments
A. in 1.000 L (1000 m L) there are 14.5 moles of H3PO4. (14.5 mol H3PO4) x (97.9953 g H3PO4/mol) = 1420.9 g H3PO4 (1420.9 g) / (0.850) = 1671.6 g total weight density = (1671.6 g) / (1000 m L) = 1.67 g/m L So answer e.
Answered by Roger the Mole - Sat Dec 17 18:24:36 2011
How do you do this problem?
Q. Stock phosphoric acid solution is 85.0% H3PO4 and has a specific gravity of 1.70. What is the molarity of the solution?
Asked by o-O - Wed Aug 20 14:32:59 2008 - Chemistry - 2 Answers - Comments
A. 1700 g/L x 85.0 / 100 =1445 g/L of H3PO4 in the solution 1445 g/L / 98.0 g/mol =14.7 mol/L => 14.7 M
Answered by Dr.A - Wed Aug 20 14:51:49 2008
Q. Stock phosphoric acid solution is 85.0% H3PO4 and has a specific gravity of 1.70. What is the molarity of the solution?
Asked by o-O - Wed Aug 20 14:32:59 2008 - Chemistry - 2 Answers - Comments
A. 1700 g/L x 85.0 / 100 =1445 g/L of H3PO4 in the solution 1445 g/L / 98.0 g/mol =14.7 mol/L => 14.7 M
Answered by Dr.A - Wed Aug 20 14:51:49 2008
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