35.0 µg of pesticide is present in a 200.0 mL aqueous solution. Express the pesticide's concentration in parts per million and parts per billion.
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![1. 35.0 ug of pesticide is present in a 200.0 mL aqueous solution. Express the pesticide's
concentration in parts per million and parts per billion.
2. Calculate the molar analytical concentrations and pK of K,Fe(CN), (329.24 g/mol) that
contains 48.0 ppm.
3. What is the molar concentration of nitric acid (63.0 g/mol) in a solution that is 60.5% HNO,
(w/w)? The specific gravity of the solution is 1.39. (.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F225480a0-4880-4d19-97af-f9a18d637cec%2Feafc6e1c-acb0-445a-8bdf-6ef1bfa9579f%2F6uzw26j_processed.jpeg&w=3840&q=75)
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- Calculate the concentration, in mol/L, of a saturated aqueous solution of Ag3P04 (Ksp = 1.80×10¯18). 1.61×10 mol/L You are correct. Calculate the solubility, in g/100mL, of A93PO4. 6.73x104 g/100mL You are correct. Calculate the mass of Pb3(PO4)2 (Ksp = 1.00x10-54) which will dissolve in 100 ml of water. Submit Answer Tries 0/5 Rank the following five salts in order of decreasing solubility, in terms of mass per unit volume. (The most soluble gets rank 1, the least soluble gets rank 5.) v Cas(PO4)3F (Ksp = 1.00x10-60) (Ksp = 1.50x10-9) (Ksp = 1.20x10-5) (Ksp = 1.00x10-54) (Ksp = 1.80x10-18) v BaSO4 Ag2SO4 Pb3(PO4)2 v A93PO4A 2.187 g sample of a solid mixture containing only potassium carbonate (MM = 138.2058 g/mol) and potassium bicarbonate ( MM 100.1154 g/mol) is dissolved in distilled water. A volume of 33.47 mL of a 0.749 M HCI standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture. K₂CO₂: KHCO,: wt% wt%3.A sample is known to contain NaOH, NA2CO3 NaHCO3 or compatible mixture of these together with inert matter. With methyl orange, a 1.100 g sample requires 31.40 mL of HCI ( 1.00 mL is equivalent to 0.0140g CaO). With phenolphthalein indicator, the same weight of sample requires 13.30mL of the acid. What is the percent composition of the sample?
- The apparent solubility products of AgCN and PbF2 at 25°C are 6.0x10-1/ and 3.3×10¬8, respectively. Calculate the solubility (g/100. g of solution) of these compounds. (Assume each solution has a density of 0.99705 g·cm-3.) 4.0 solubility of A9CN g/100. g of solution solubility of PBF2 4.0 g/100. g of solutionThe solubility-product constants, Ksp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10 x 10-11 CdCO3 1.80 × 10-14 Part A A solution of Na2CO3 is added dropwise to a solution that contains 1.02x10-2 MFe²+ and 1.48x10-2 M Cd²+. What concentration of CO3²- is need to initiate precipitation? Neglect any volume changes during the addition. Express your answer with the appropriate units. ► View Available Hint(s) [CO3²- ] = Submit μA Value Part B Complete previous part(s) Part C Complete previous part(s) Units ?The apparent solubility products of AgCN and PBF2 at 25°C are 6.0x10¬1/ and 3.3x10-8, respectively. Calculate the solubility (g/100. g of solution) of these compounds. (Assume each solution has a density of 0.99705 g·cm-3.) solubility of AgCN 4.0 g/100. g of solution solubility of PbF2 4.0 g/100. g of solution
- A 5.0 g sample containing a pesticide with molecular formula [C14H9Cl5], was decomposed with metallic sodium in alcohol, and the liberated chloride ion was precipitated as AgCl. (i) Express the results of this analysis in terms of percent based on the recovery of 0.1606 g of AgCl. (ii) Convert your answer (g/g) to ppm.What weight of sample in gram containing 8.00 % Fe3O4 (MW= 231.53 g/mole) must be taken to obtain a precipitate of Fe (OH)3 (MW= 106.867 g/mol) that, when ignited to Fe2O3 (MW = 159.69 g/mole), weighs 150.0 mgFormulate a hypothesis regarding the solubility of aspirin at different pH.The experimentA) Three teaspoons of water (approx. 15 ml) were added to one tablet said to contain 300 mg of aspirin. Fizzingwas observed. Most of the tablet dissolved, but there were some solid particles. By heating the mug in amicrowave for 10 second increments until the water came to the boil (approx. 3x), all of the solid particlesdissolved. The solution was left to cool to room temperature and then placed in a fridge and NOTHINGHAPPENED. Try this yourself if you can spare two aspirin tablets, your results might look different.• Questions to ask:1. What might the fizzing bubbles be?2. Can you give a chemical explanation?3. Can you write a chemical reaction equation with aspirin reacting with something to give a gas and aspirinin another form?4. What might be the formulation (what the manufacturer mixes with aspirin in making the tablet) “trick”for aspirin to improve solubility?5. How does this compare with…
- (a) If the molar solubility of Cd3(AsO4)2 at 25 oC is 1.15e-07 mol/L, what is the Ksp at this temperature?Ksp = __________(b) It is found that 8.90e-06 g of Y2(CO3)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Y2(CO3)3.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3? solubility = ________mol/LA 0.5123g sample (molar mass 204.23g/mol) of KHP was dissolved in about 25 mL of distilled water and titrated to the phenolphthalein end point with 28.75 mL of a sodium hydroxide solution. Calculate the molar concentration of the hydroxide solution.A 0.8729 g sample containing an unknown amount of Pb was dissolved in concentrated HNO3 and diluted to 250 mL in a volumetric flask. Excess KIO3 was added to a 50.00 mL aliquot to precipitate the Pb (MM = 207.2 g/mol) as Pb(IO3)2 (MM = 557.0 g/mol). Calculate the %Pb in the original sample if the precipitate had a mass of 0.1278 g.