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Consider the titration of a 26.1 mL sample of 0.115 M RbOH with 0.110 M HCl. Determine each of the following.
.The initial pH.the volume of added acid required to reach the equivalence point.the pH at 4.7 mL of added acid.the pH of the quivilant point.the pH after adding 4.7 mL of acid beyond the equivalence point
Calculate the energy needed to raise the temperature of 180.0 g of water from 10.0 degrees Celsius to 40.0 degree Celsius. The molar heat capacity for water is 75.3 J/K mol.
A solution of ethanol (C2H5OH) in water is prepared by dissolving 10.0mL ethanol (density is 0.79g/cc) in enough water to make 250.0mL of solution. What is the molarity of the ethanol solution?
Using calorimetry experiment, how many grams of CaCl are required to cause a burn at 60 degrees celsius in 1000mL of water?
if 100% of the NaCl molecules dissociated, the van't Hoff factor i=2 calculate the experimental van't Hoff factor of NaCl from your data. I dissolved 30 g of salt into 100ml of water
What is the free energy change, ?G°, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453°C? Kc = 0.020
the uncatalyzed decomposition of hydrogen peroxoide is first order with an activation energy of 75.3 kj/mol and a half life of 6 hrs at 40 degrees celcius.
Describe how you will prepare a H2PO4-/HPO42- buffer using solid sodium dihydrogen phosphate and sodium hydrogen phosphate (pH 7.4, 500 mL 0.40M each). How much solid is needed to prepare each solution? How much volume of each of the solutions sho..
what is the balanced chemical reaction describing the decomposition of ammonium nitrate, and calculate the standard heat of reaction using the appropriate enthalpies of formation
the elemental mass percent composition of ascorbic acid (vitamin C) is 40.92% C, 4.58% H, and 54.50% O. Determine the empirical formula
It is desired to inflate a baggie with a volume of 869 milliliters by filling it with hydrogen gas at a pressure of 0.847 atm and a temperature of 296 K. How many grams of H2 gas are needed? answer in g please
At constant volume, the heat of combustion of a particular compound is -3698.0 KJ/mol. When 1.895 g of this compound (molar mass=181.06 g/mol) was burned in a bomb calorimeter
Equilibrium constant for the cell reaction is (A)100 .32/0.0591 (B)100.32/0.0295 (C) 100.26/0.0295 (D) e0.32/0.295
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