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An unsuspecting individual had 4.40 mL of 1.000 M HCl injected into their bloodstream. Assuming that the person has 1 gallon of blood circulating, and that the buffering capacity is controlled by phosphate buffer present at a formal concentration of 0.0250 moles L?1 and pH of 7.35, what is the global pH change incurred after injection of the HCl? What would the pH change be if this same amount of 1.000 M HCl were put into a gallon of pure water?
What is the expected molar solubility of silver phosphate, Ag3PO4 in water? B) What is the expected molar solubility, in ppt (parts per thousand), of lead(II) iodide, PbI2 in water
What is the molality of a solution prepared by dissolving 10.0 grams of methylamine, CH3NH2, in 50.0 mL of ethanol, C2H5OH?
What is the Volume of 1.05mol of Benzene (C6H6) at 20.7 degrees C. The density of Benzene is 0.879 g/mL
Calculate the molar mass of the uknown compound. The boiling point elevation constant for water is0.52°C/m
Determine How many moles each are in 1.30L of the saline solution if a physiological saline solution contains 174mEq/L each of Na+ and Cl - .
In the reaction 4 P4 + 5 S8 -> 4 P4S10 600 g of P4 is mixed with 1300 g of S8.
What is the molar mass of the unknown compound if the solution has a freezing point of -5 oC?
Calcium phosphate, silicon dioxide, and coke may be heated together in an electric furnace to produce phosphorus, as shown in the following equation: 2Ca3(Po4)2+6SiO2+10C=6CaSiO3+10CO +P4
With respect to the corrosion of steel in concrete, explain the significance of the following terms: carbonation of concrete, passivity of steel, electrical resistivity of concrete, state of oxidation of iron.
If a 2.1 L reaction vessel initially contains 723 torr of cyclopropane at 485 degrees C , how long will it take for the partial pressure of cylclopropane to drop to below 105 torr ?
What is the temperature at which the solution of KI will freeze if the solution contains 52.43 grams of KI dissolved in 479.1 grams of water.
What is the pH of the solution at the equivalence point for the titration of 100 mL of a .786 M HCO2H solution with a .786 M Solution of sodium Hydroxide? Formic acid has a Ka=1.80*10^-4
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