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Suppose that a student is determining the total base content of an antacid tablet by performing a back titration. He/she weighs out a .3012g portion of a tablet whose total weight is 1.5312g, dissolves this in exactly 40.00mL of DI water, and then adds exactly 30.00mL of 0.1000M HCl in order to bring the pH down to 1.9. This solution is then carefully back-titrated with .2000MNaOH with 12.5mL required to reach the equivalence point. Calculate the total base content (The total # of mmoles of base contained) of the antacid tablet.
Describe the Bohr effect in oxygen binding by hemoglobin, including all structural
Calculate the pH of the 0.20 M NH3/0.24 M NH4Cl buffer. B)What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 55.0 mL of the buffer?
The four major attractive forces between particles are ionic bonds, dipole-dipole attractions, hydrogen bonds, and dispersion forces. Consider the compounds below
How many grams of dry NH4Cl need to be added to 2.00 L of a 0.600 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.89. Kb for ammonia is 1.8 X10^-5.
Explain the solubility of oxygen in water is 14.74mg/L at 0 Celsius and 7.03mg/L at 35 Celsius. Estimate the solubility at 50 Celsius.
A star can be considered a black body. Find the surface temperature of a star where ?max = 609 nm
Assuming that the temperature remains constant, to what volume of helium will the balloon expand when it rises to an altitude where the pressure is only 50.0 kPa.
Consider a mixture of potassium chloride and potassium nitrate that is 43.2% potassium by mass. What is the percent KCL by mass of the original mixture?
plasma is the fluid portionof blood. the concentraton of acetylsalicylic acid aspirinc9h8o4 molar mass180 gmol in your
the oxidizing power of household bleach solutions can be lost when they are exposed to heat or sunlight or due to
calculate the molar concentration of OH- ions in an 0.85M solution of hypobromite ion, BrO- (Kb = 4.0x10^-6). what is the pH of this solution?
Calculate the mass of methane that must be burned to provide enough heat to convert 151.0 g of water at 43.0°C
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