Question

Show the calculation for determing mass % of P25O5 in your fertilizer sample (starting from the...

Show the calculation for determing mass % of P25O5 in your fertilizer sample (starting from the MgNH4PO6​​ ​​* 6H2O product mass you will measure = 3 g).

Homework Answers

Answer #1

1 mole of P2O5 whose molar mass is 141.95 g/mol, with its 2 P's produces 2 molar masses of MgNH4PO4*6H2O , whose molar mass is 245.40 g/mol

therefore 2 x 245.40 g of MgNH4PO4*6H2O is produced from 141.95 g of P2O5

hence 3 g of MgNH4PO4*6H2O is produced from 141.95 x 3/ (2 x 245.40) g of P2O5 = 0.868 g of P2O5

Therefore % of P2O5 in fertilizer sample = (0.868/ wt. of fertilizer taken) x 100

[wt. of fertilizer taken is not given, so the final result could not be calculated]

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Mass of small beaker                        112.64 g Mass of Fertilizer and Beaker         &nbs
Mass of small beaker                        112.64 g Mass of Fertilizer and Beaker                         123.03 g Mass of fertilizer sample                          10.39 g   Mass of filter paper                             0.44 g      Mass of filter paper and dry MgNH4PO4*6H2O precipitate                             0.96 g Mass of dry MgNH4PO4*6H2O precipitate                              0.52 g Moles of MgNH4PO4*6H2O                           0.0021 mol Moles of Phosphorous                            0.0021 mol Mass of Phosphorous                             0.0065 g % P in fertilizer sample                                  .62 %                  Moles of P2O5                                   mol Mass...
A student uses 3.00g of a fertilizer with an NPK ratio of 15-15-10, how much MgNH4PO4*6H2O...
A student uses 3.00g of a fertilizer with an NPK ratio of 15-15-10, how much MgNH4PO4*6H2O (MM =245.1 g/mol) should the student produced? Hint*: first determine the amount of phosphorous in the fertilizer sample and use stochiometry to convert to mass of product.
A student uses 3.00g of a fertilizer with an NPK ratio of 15-15-10, how much MgNH4PO4*6H2O...
A student uses 3.00g of a fertilizer with an NPK ratio of 15-15-10, how much MgNH4PO4*6H2O (MM =245.1 g/mol) should the student produced? Hint*: first determine the amount of phosphorous in the fertilizer sample and use stochiometry to convert to mass of product. Answer should be in decimal form to two decimal places.
1. Show the calculation of the mass of Ca3(PO4)2 needed to make 200 ml of a...
1. Show the calculation of the mass of Ca3(PO4)2 needed to make 200 ml of a 0.128 M solution. 2. Show the calculation of the volume of 0.987 M solution which can be prepared using 24.6 grams of NaNO3. 3. Show the calculation of the volume of 0.238 M solution which can be prepared using 13.4 grams of Ca3(PO4)2.
Show each step of your calculation.
Show each step of your calculation.
Show a sample calculation for the concentration of borax using 2.25 mL of 0.225 M HCl...
Show a sample calculation for the concentration of borax using 2.25 mL of 0.225 M HCl and 5.0 mL of borax solution. Make sure to include the units on all numbers and variables. You may find Equation 23.7 (B4O5(OH)4 (aq) + 2H(aq) --> 4B(OH)3(aq)) helpful in this set up. You must show all of your work for this question to receive full credit.
Calculate percent yield of 1.4736g K(Fe(C2O4)2)·4H2O OBTAINED FROM starting compound 1.2770g (NH4)2Fe(SO4)2·6H2O again 1.2770g = starting...
Calculate percent yield of 1.4736g K(Fe(C2O4)2)·4H2O OBTAINED FROM starting compound 1.2770g (NH4)2Fe(SO4)2·6H2O again 1.2770g = starting material 1.4736g = product
1- A 0.0456 g sample of an unknown sample was titrated using the EDTA titrant from...
1- A 0.0456 g sample of an unknown sample was titrated using the EDTA titrant from question 1 and the procedure below. The starting burette volume was 0.05 mL. The ending burette volume was 42.35 mL. Calculate the % calcium oxide (CaO; 56.0774 g/mol) by mass in the sample. Show all work. 2-  100.0 mL of an unknown water sample was titrated using the EDTA from question 1 and the procedure below. The starting volume was 0.25 mL and the ending...
starting materials experimental mass (g) experimental mmol vanillin 3.01 sodium borohydride 0.41 product experimental mass (g)...
starting materials experimental mass (g) experimental mmol vanillin 3.01 sodium borohydride 0.41 product experimental mass (g) experimental mmol theoretical mass (g) % yield vanillyl alcohol 3.017
Show how to find the deltaHf° for 1 mol of cyclohexane starting from graphite and H2(g)....
Show how to find the deltaHf° for 1 mol of cyclohexane starting from graphite and H2(g). Cite where you get any values you use in all calculations.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT