Question

In: Chemistry

analysis of mercury (200.59 g/mol) in the sample of mercuric ointment described here. A 4.026 g...

analysis of mercury (200.59 g/mol) in the sample of mercuric ointment described here. A 4.026 g sample of a mercuric ointment is digested in nitric acid. After dilution, the Hg2+ is titrated with 23.05 mL of a 0.1124 M solution of NH4SCN. The titration involves the formation of a stable, neutral complex: Hg2+ (aq) + 2 SCN- (aq) = Hg(SCN)2 (aq)

How many mmoles of mercury are in the sample?

How many mg's of mercury are in the sample?

What is the percent mercury (w/w) in the ointment?

Solutions

Expert Solution

Hg2+ (aq) + 2 SCN- (aq) ----------------> Hg(SCN)2 (aq)

number of mmoles of SCN- = 23.05 x 0.1124

                                          = 2.591

number of mmoles of Hg+2 = 2.591 / 2

                                          = 1.296

number of mmoles of Hg+2 = 1.296

mass of Hg+2 = mmoles x molar mass of Hg

                        = 1.296 x 200.59

mass of Hg+2 = 259.96 mg

mass of sample = 4.026 g

percent mercury (w/w) = (mass of Hg+2 / mass of sample ) x 100

                                     = (259.96 x 10^-3 / 4.026 ) x 100

                                     = 6.46 %

percent mercury (w/w) = 6.46 %

molar mass =


Related Solutions

A sample of gas contains 0.1600 mol of CH4(g) and 0.1600 mol of H2O(g) and occupies...
A sample of gas contains 0.1600 mol of CH4(g) and 0.1600 mol of H2O(g) and occupies a volume of 12.1 L. The following reaction takes place: CH4(g) + H2O(g)-----3H2(g) + CO(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. ____(?)Liters
A sample of gas contains 0.1000 mol of HCl(g) and 5.000×10-2 mol of Br2(g) and occupies...
A sample of gas contains 0.1000 mol of HCl(g) and 5.000×10-2 mol of Br2(g) and occupies a volume of 4.79 L. The following reaction takes place: 2HCl(g) + Br2(g)2HBr(g) + Cl2(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. A sample of gas contains 0.1800 mol of HCl(g) and 9.000×10-2 mol of Br2(g) and occupies a volume of 9.74 L. The following reaction takes place: 2HCl(g) + Br2(g)2HBr(g)...
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...
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.
1. A 5.75 mL sample of mercury has a measured mass of 77.05 g. The density...
1. A 5.75 mL sample of mercury has a measured mass of 77.05 g. The density is ___________ 2. Mercury’s accepted density is 13.53 g·mL-1. The % error in your measurement is: ____________ 3. Is this person accurate? ____                        Is the person precise? ___ Defend your answer! 4. This molecule contains ____ elements and ____ atoms. Carbon=black    Oxygen=Red     White=Hydrogen The molecular formula for this substance is: ___________ 5. Calculate the number of seconds in 5.25 years using unit analysis:...
A 0.5065 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and...
A 0.5065 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and Ce(NO3)3 (molar mass = 326.13 g/mol) was dissolved in water. The solution was titrated with KIO3, producing the precipitates La(IO3)3(s) and Ce(IO3)3(s). For the complete titration of both La3 and Ce3 , 44.81 mL of 0.1252 M KIO3 was required. Calculate the mass fraction of La and Ce in the sample.
A 0.1276−g sample of a monoprotic acid (molar mass = 1.10 × 102 g/mol) was dissolved...
A 0.1276−g sample of a monoprotic acid (molar mass = 1.10 × 102 g/mol) was dissolved in 25.0 mL of water and titrated with 0.0633 M NaOH. After 10.0 mL of base had been added, the pH was determined to be 4.87. What is the Ka for the acid? Answer in scientific notation.
A 0.5072 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and...
A 0.5072 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and Ce(NO3)3 (molar mass = 326.13 g/mol) was dissolved in water. The solution was titrated with KIO3, producing the precipitates La(IO3)3(s) and Ce(IO3)3(s). For the complete titration of both La3 and Ce3 , 44.01 mL of 0.1289 M KIO3 was required. Calculate the mass fraction of La and Ce in the sample.
A 21.8 g sample of ethanol (C2H5OH, 46.07 g/mol) is burned in a bomb calorimeter, according...
A 21.8 g sample of ethanol (C2H5OH, 46.07 g/mol) is burned in a bomb calorimeter, according to the following reaction equation. If the temperature of the rises from 13.0 °C to 79.3 °C, what is the heat capacity of the calorimeter? C2H5OH(l) + 3 O2(g) →2 CO2(g) + 3 H2O(g)    ΔH°rxn = –1235 kJ   
A 0.5070 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and...
A 0.5070 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and Ce(NO3)3 (molar mass = 326.13 g/mol) was dissolved in water. The solution was titrated with KIO3, producing the precipitates La(IO3)3 and Ce(IO3)3. For the complete titration of both La3+ and Ce3+, 42.10 mL of 0.1204 M KIO3 was required. Calculate the mass fraction of La and Ce in the sample. mass fraction La: g Lag sample mass fraction Ce: g Ceg sample
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT