Many fertilizers contain ammonium phosphate as a source of phosphorus and nitrogen. A 8.22 g sample of a fertilizer is dissolved in water and mixed with excess barium chloride solution, and the following reaction occurs: 2 (NH4)3PO4(aq) + 3 BaCl2(aq) → Ba3(PO4)2(s) + 6 NH,CI(aq) The product mixture is found to contain 2.61 g of barium phosphate. Using this information, calculate the percentage by mass of ammonium phosphate in the fertilizer. Type your final answer below and upload your work for this question in question. You will not earn ANY points if you do not upload the solution to this question. Please do not include any units. Report your answer to one decimal place.

For the following molecular equation, write the complete ionic and net ionic equation. Z n ( s ) + P b ( N O 3 ) 2 ( a q ) → Z n ( N O 3 ) 2 ( a q ) + P b ( s )

Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. 0- Ba(CIo), (aq) + H,0(1)

W Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed. O 2 H* (aq) + CO3²-(aq) → H₂CO3(s) 2 Na* (aq) + CO3²- (aq) + 2 H*(aq) + 2 Cï(aq) → H₂CO3(s) + 2 NaCl(aq) O 2 H* (aq) + CO3²-(aq) → H₂O(1) + CO₂(g) 2 Na* (aq) + CO3²- (aq) + 2 H* (aq) + 2 Cl(aq) → H₂CO3(s) + 2 Na*(aq) + 2 Cl(aq) No reaction occurs.

A mixture consisting of only chromium(III) bromide (CrBr3) and aluminum bromide (AlBr3) weighs 1.1218 g. When the mixture is dissolved in water and an excess of silver nitrate is added, all the bromide ions associated with the original mixture are precipitated as insoluble silver bromide (AgBr). The mass of the silver bromide is found to be 2.2708 g. Calculate the mass percentages of chromium(III) bromide and aluminum bromide in the original mixture. Mass percent CrBr3 Mass percent AlBr3 = % %

If 5.15 grams of copper metal react with 14.1 grams of silver nitrate, what is the mass of silver, in grams, that can be theoretically produced? 2 AgNO3 (aq) + Cu (s) → Cu(NO3)2 (aq) + 2 Ag (s)

Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. 0 - H,0(1) NaF (aq) +

For the following reaction, 0.166 moles of perchloric acid (HC104) are mixed with 0.344 moles of tetraphosphorus decaoxide. perchloric acid (HC1O4)(aq) + tetraphosphorus decaoxide(s) → phosphoric acid(aq) + dichlorine heptaoxide(l) What is the formula for the limiting reagent? What is the maximum amount of phosphoric acid that can be produced? moles

How many grams of silver nitrate must react to give 1.00g of Ag? Cu(s)+2AgNO3(aq)-->Cu(NO3)2(aq)+2Ag(s) Express your answer with the appropriate units.

Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.) Note: you are writing the molecular, and not the net ionic equation. → Ba ClO Ba a(CIO) (aq) + H₂O(1) 3)2(aq) ローロ ×