molar mass of H3PO4 IS 97.99g/mol. Mass Na3PO4 formed = 0.833 mol X 163.9 g/mol = 137 g Na3PO4 Can someone give me a step by step to the solution? H3PO4 is a colorless viscous liquid at room temperature. d. How many H atoms are there in 2.5 mol H3PO4.2.5pt - 13159451 ams) has entries 4.9, 14.7. moles of H3PO4 = 25.4 g x a million mol/ninety 8 g = 0.259 mol H3PO4 Kg of solvent = (100g - 25.4 g) = seventy 4.6 g = 0.0746 kg Molality = moles of solute/kg of solvent = 0.259 mol/0.0746 kg solvent Molality = 3.47m To do this work out how much H3PO4 you would get if all of each reagent individually were to fully react. The molar mass of H3PO4 (phosphoric acid) is: 97.993 grams/mol. Calculations: Formula: H3PO4 Molar Mass: 97.9937 g/mol 1g=1.02047376515021E-02 mol Percent composition (by mass): Element Count Atom Mass %(by mass) The one that produces the least H3PO4 is the limiting reagent. Solution The molar mass of H3PO4 is 97.99 g. The percent by mass of each of the elements in H3PO4 is calculated as follows: %H=(3(1.008 g) H/ 97.99 g H3PO4)*100%= 3.086% Calculate the formula and molar mass. From its MSDS sheet it is 1.680g/mL. Start with a liter of solution which is 1000 mLx 1.680 g/mL gives a mass of 1680 g. mass H3PO4 = 1680 g solution x 85 parts H3PO4/100 parts solution = 1430 g H3PO4. 1. Molar Mass: 97.9952. The third column labeled Mass of Washers m subscript w (kilograms) has entries 0.0049, empty. Now there is 15 moles of H3PO4 in the initial liter so it is 15M H3PO4! Mass H3PO4 remaining = 18.3 g H3PO4 remaining. work out the limiting reagent. Example Reactions: • PH3 + 2 O2 = H3PO4 • 3 KOH + H3PO4 = K3PO4 + 3 H2O • H3PO4 + 5 HCl = PCl5 + 4 H2O • H3PO4 + 3 NH3 = (NH4)3PO4 • H3PO4 + NaOH = NaH2PO4 + H2O Mass H3PO4 consumed = 2.50 mol NaOH X (1 mol H3PO4 / 3 mol NaOH) X 97.99 g/mol = 81.7 g H3PO4 consumed. I don't know what to do with this, I tried: (.005 L)(x M) = (.055 L)(0.258 M) And I got 2.838 mol/L But the answer is wrong apparently. moles P4O10 = mass / molar mass = 10.00 g / 283.88 g/mol = 0.035226 mol. See also our theoretical yield calculator for chemical reactions (probably your next stop to finish the problem set). A 5.00 mL sample of an aqueous solution of H3PO4 requires 55.0 mL of 0.258 M NaOH to convert all of the H3PO4 to Na2HPO4. The other product of the reaction is water. Complete the following calculations for H3PO4.4 pts (1pt each) a. How many oxygen atoms are in one unit of H3PO4? P4O10 + 6H2O ----> 4 H3PO4. Molar mass of *2H3PO4 is 195.9904 g/mol Convert between *2H3PO4 weight and moles b. What is the molar mass of H3PO4? c. How many moles of PO43-ions are present in 2.5 moles of phosphoric acid, H3PO4? mole H3PO4 = 1430 g H3PO4 x 1 mole H3PO4/98 g H3PO4 = 15 moles. moles H2O = 12.0 g / 18.016 g/mol = 0.66607 mol. What am I doing wrong? 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