Question

In: Chemistry

The active ingredient in a zinc nutritional supplement is ZnSO4⋅7H2O (molar mass = 287.58 g/mol). Ten...

The active ingredient in a zinc nutritional supplement is ZnSO4⋅7H2O (molar mass = 287.58 g/mol). Ten zinc tablets containing a mix of the active ingredient and an inactive filler were ground and mixed together thoroughly. The total mass of these 10 tablets was 10.005 g. A 2.494 g sample of the finely ground tablets was dissolved in an acidic solution. The solution was neutralized with ammonia and subsequently warmed in a water bath. Addition of (NH4)3PO4 to the solution resulted in the precipitation of ZnNH4PO4. The precipitate was filtered and dried, then ignited to produce 0.272 g of Zn2P2O7 (molar mass = 304.76 g/mol). What is the mass percent of ZnSO4⋅7H2O in each tablet? What is the average mass of the active ingredient ZnSO4⋅7H2O and inactive filler in each tablet?

Solutions

Expert Solution


Related Solutions

The active ingredient in a zinc nutritional supplement is ZnSO4·7H2O (molar mass = 287.58 g/mol). Ten...
The active ingredient in a zinc nutritional supplement is ZnSO4·7H2O (molar mass = 287.58 g/mol). Ten zinc tablets containing a mix of the active ingredient and an inactive filler were ground and mixed together thoroughly. The total mass of these ten tablets was 10.165 g. A 1.830 g sample of the finely ground tablets was dissolved in an acidic solution. The solution was neutralized with ammonia and subsequently warmed in a water bath. Addition of (NH4)3PO4 to the solution resulted...
The active ingredient in a zinc nutritional supplement is ZnSO4·7H2O (molar mass = 287.58 g/mol). Ten...
The active ingredient in a zinc nutritional supplement is ZnSO4·7H2O (molar mass = 287.58 g/mol). Ten zinc tablets containing a mix of the active ingredient and an inactive filler were ground and mixed together thoroughly. The total mass of these ten tablets was 11.890 g. A 2.242 g sample of the finely ground tablets was dissolved in an acidic solution. The solution was neutralized with ammonia and subsequently warmed in a water bath. Addition of (NH4)3PO4 to the solution resulted...
Chem Question - Gases Molar Mass N = 14.01 g/mol Molar Mass H2O = 18.016 g/mol...
Chem Question - Gases Molar Mass N = 14.01 g/mol Molar Mass H2O = 18.016 g/mol Vapor Pressure of Water at 25 C is 23.76 torr Vapor Pressure of Water at 65 C is 187.54 torr (Show all work and calculations, include units in answer. If calculations must be used in several parts, rounding should be made to 6 decimal points to ensure accuracy. Final Answers can be rounded to 3 decimal points.) A syringe filled with air can be...
Ethanol, C2H5OH (molar mass = 46 g/mol) is mixed with methanol, CH3OH (molar mass = 32...
Ethanol, C2H5OH (molar mass = 46 g/mol) is mixed with methanol, CH3OH (molar mass = 32 g/mol) to make an ideal solution at a given temperature. If 5.00 g of ethanol and methanol are mixed, what is the resulting vapor pressure of the solution? (the vapor pressure at the same temperature for pure ethanol is 44.5 mm Hg and pure methanol is 88.7 mm Hg)
What mass of a weak acid with a molar mass of 100 g/mol is necessary to...
What mass of a weak acid with a molar mass of 100 g/mol is necessary to neutralize 25 ml of 0.10 M NaOH solution? What is the pH of 0.15 g of sodium acetate NaC2H3O2 in 100 ml water H2O?
A compound has a molar mass of 100 g/mol and the percent composition (by mass) of...
A compound has a molar mass of 100 g/mol and the percent composition (by mass) of 65.45% C, 5.45% H, and 29.09% O. Determine the empirical formula and the molecular formula.
A 0.520 g sample of a diprotic acid with a molar mass of 255.8 g/mol is...
A 0.520 g sample of a diprotic acid with a molar mass of 255.8 g/mol is dissolved in water to a total volume of 23.0 mL . The solution is then titrated with a saturated calcium hydroxide solution. a. Assuming that the pKa values for each ionization step are sufficiently different to see two equivalence points, determine the volume of added base for the first and second equivalence points. b. The pH after adding 23.0 mL of the base was...
1)A typical commercial antacid tablet contains 0.350 g of CaCO3 [MW=100.09 g/mol] as an active ingredient....
1)A typical commercial antacid tablet contains 0.350 g of CaCO3 [MW=100.09 g/mol] as an active ingredient. How many moles of HCl could this tablet neutralize? 2)A student was analyzing an antacid tablet with a mass of 2.745 g. The student found that a 1.872 g sample of the tablet would neutralize 67.35 mL of stomach acid. Calculate how much stomach acid would be neutralized by the entire tablet. 3)A student determined that 29.43 mL of 0.132 M NaOH reacts with...
What mass (in g) of iron (Fe, molar mass = 55.85 g∙mol–1) is needed to experimentally...
What mass (in g) of iron (Fe, molar mass = 55.85 g∙mol–1) is needed to experimentally produce 50.0 g of iron(III) oxide (Fe2O3, molar mass = 159.70 g∙mol–1) in excess oxygen if the percent yield is 78.7%? 4Fe(s) + 3O2(g)2Fe2O3(s) A. 22.2 g B. 27.5 g C. 35.0 g D. 44.4 g
A .435 g sample of a nonvolatile, nonionizable solute with a molar mass of 67.4 g/mol...
A .435 g sample of a nonvolatile, nonionizable solute with a molar mass of 67.4 g/mol is dissolved in 15.1 g of cyclohexane. Calculate the molar concentration of solute in the solution. Calculate the boiling point of the solution described. Calculate the freezing point of the solution described.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT