70.5 mg of K3PO4 (F.W.: 212.27 g/mol) is added to 15.0 mL of 0.0500 M AgNO3 yielding 0.0980 g of precipitate Ag3PO4 (F.W.: 418.58 g/mol)
What is the % yield?
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70.5 mg of K3PO4 (F.W.: 212.27 g/mol) is added to 15.0 mL of 0.0500 M AgNO3...
If 30.0 mL of 0.150 M CaCl2 is added to 31.0 mL of 0.100 M AgNO3, what is the mass of the AgCl precipitate? ?g
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Suppose that 51.0 mL of 0.11 M AgNO3 is added to 50.0 mL of 0.048 M NaCl solution. (a) What mass of AgCl will form? g AgCl the tolerance is +/-2% (b) Calculate the final concentrations of all of the ions in the solution that is in contact with the precipitate. [Ag+] = × 10 M [NO3−] = × 10 M [Na+] = × 10 M [Cl−] = × 10 M (c) What percentage of the Ag+ ions have precipitated?...
4) When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.500 M NH4CI, how many grams of AgCl are formed? (MM AgCI =143.32 g/mol) AgNO3(ag)+ NH4C| (aq) AgCl(s)+ NH4NO3(aq)
A 20.0 mL of 0.100 M AgNO3 is titrated with 0.0500 M MgCl2. Write net ionic equation. What is the volume of MgCl2 to complete the reaction?
Determine the volume of solution that contains 15.0 g of AgNO3 if the solution is 0.375 M 235 mL 31.5 mL 247 ml 33.1 mL
Part 1.) Consider the titration of 50.0 mL of 0.0500 M C2H5NH2 (a weak base; Kb = 0.000640) with 0.100 M HBrO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (b) 6.3 mL pH = (c) 12.5 mL pH = (d) 18.8 mL pH = (e) 25.0 mL pH = (f) 42.5 mL pH = Part 2.) A solution of Na3PO4 is added dropwise to a solution that is 0.0613 M...
Consider the mixing of 2.65 mL of 0.255 M Mg(NO3)2 and 1.00 L of 0.195 M K3PO4. (a)Write a balanced chemical equation that describes the double displacement reaction between these solutions. (Include states-of-matter under the given conditions in your answer.) (b)Calculate how many grams of the precipitate will form. ___?__ g
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