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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?
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- 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…
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