What is the mass of sodium phosphate (163.94 g/mol) that yields 1.00 g of calcium phosphate (310.18 g/mol) precipitate? __CaCl2(s) + __Na3PO4(aq) → __Ca3(PO4)2(s) + __NaCl(aq)

Md Ariful Islam

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Md Ariful Islam

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m 1.00 3 CaCl2(aq) + 2 Na3PO4(aq) --gt; Ca3(PO4)2(s) + 6 NaCl(aq) 2*163.94 310.18 m=2*163.94*1.00/310.18=1.057g
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An aqueous solution of sodium phosphate is a 0.142 M Na3PO4(aq) has a density of 1.02 g/ml What is the percent by mass of sodium phosphate ? What is the mole fraction of sodium phosphate

The percent mass of Na3PO4 in this solution we can determine, using following equation:w = C×M(Na3PO4) / (10×p), where C is molar concentration; M is molar mass of sodium phosphate;...

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I am currently attempting to make a Chemical Equation Model. This is my equation: Phosphoric Acid plus Calcium hydroxide yields Calcium Phosphate plus Water How do i make a 3D model of this?

You must use some programs like ChemOffice,or you can show it schematically in PowerPoint

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What is the mass of iron(III) bromide (295.55 g/mol) that yields 0.188 g of silver bromide (187.77 g/mol) precipitate? __FeBr3(s) + __AgNO3(aq) → __AgBr(s) + __Fe(NO3)3(aq)

m 0.188 FeBr3(s) + 3AgNO3(aq) = 3AgBr(s) + Fe(NO3)3(aq) 295.55 3*187.77 m = 295.55*0.188/(3*187.77) = 0.986 g

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Calculate the number of mass of phosphoric acid that is produced when 1.45 x1024 molecules of sulfuric acid react with calcium phosphate. Ca3(PO4)2 + 3H2SO4 à 3CaSO4 + 2H3PO4

1 mole of matter contains 6.02214076×10²³ particles.Given number of molecules represents: 1.45 x1024 / 6.02214076×10²³ = 2.4 molesn (H3PO4) = 2/3 n (H2SO4) = 2/3 x 2.4 = 1.6 molesn...

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Calcium hydroxide and phosphoric acid react to form calcium phosphate and water. Find the moles of water, if you have 6.50 moles of calcium hydroxide.

Solution:The balanced chemical equation:3Ca(OH)2 + 2H3PO4 → Ca3(PO4)2 + 6H2OAccording to the equation above: Moles of Ca(OH)2 / 3 = Moles of H2O / 6Moles of Ca(OH)2 = Moles of...

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If a manufacturing company reacts 25 kilograms of 52.5% calcium nitrate ore with excess ammonium phosphate, how many grams of calcium phosphate are produced?

3Ca(NO3)2->Ca3(PO4)2 m(CaNO3)=25*1000*0.525=13125 g N(Ca(NO3)2)=80 moles N(Ca3(PO4)2)= 80/3 = 26.67 moles; m(Ca3(PO4)2) = 8270 g

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What is the maximum number of grams of silver phosphate that can be produced from the reaction of 287 g of silver chlorate with 52.8 g of sodium phosphate? 3 Ag(ClO3) + Na3(PO4)

3AgClO3 + Na3PO4 → Ag3PO4 + 3NaClO3M(AgClO3) = 191.32 g/mol;M(Na3PO4) = 163.94 g/mol;M(Ag3PO4) = 418.58 g/mol;n=m/M;n(AgClO3) = 287 g / (191.32 g/mol) = 1.5 moles;n(Na3PO4) = 52.8/ (163.94 g/mol) =...

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If 50.0 mL of 0.125 mol/L sodium phosphate solution is reacted with 50.0 mL of 0.125 mol/L magnesium nitrate solution, what is the predicted mass of precipitate in g?

  Solution. 0.00625               0,00625                           y2Na3PO4 + 3Mg(NO3)2 → Mg3(PO4)2↓ + 6NaNO3      2                               3                               1V(Na3PO4) = 50,0 mL = 0,05 L;  V(Mg(NO3)2) = 50,0 mL = 0,05 L;n(Na3PO4) = c*V = 0,125*0,05 = 0,00625 mol;n(Mg(NO3)2) = c*V = 0,125*0,05 = 0,00625 mol;Let n(Mg(NO3)2)...

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CaCl2 (aq) + Na3PO4 (aq) —> Ca3(PO4)2 (s) + NaCl (aq) unbalanced How many moles of sodium phosphate need to react with the calcium chloride to make 1.98 moles of calcium phosphate?

3CaCl2 (aq) + 2Na3PO4 (aq) —> Ca3(PO4)2 (s) + 6NaCl (aq) 1.98 x 2/1 = 3.96 moles of sodium phosphate.

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Calculate the molar concentration of calcium, Ca2+ , if 1.2g of calcium phosphate, Ca3(PO4)2 (s), is dissolved in 135mL of solution

Mr=310 g/mol.n= m/Mr = 1.2/310 = 0,00387096774 moles.Cm=n/V = 0,00387096774/0.135 = 0,0286738351 M.

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