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A 67.0-g piece of gold at 725K is dropped into 165 g of H2O(l) at 298K in an insulated container at 1 bar pressure. Calculate the temperature of the system once equilibrium has been reached. Assume that Cp,m for Au and H2O is constant at its value for 298K throughout the temperature range of interest.
The Henderson-Hasselbalch equation is used to calculate the pH of a weak base, but not the pH of a weak acid.
An aqueous solution of unoxygenated hemoglobin containing 5 g of protein (M= 64000 g/mol) in the 100cm3 of solution is placed in an insulated vessel.
What is the concentration of the HNO3 solution? (b) How many moles of NaOH were in excess after the first addition?
A saturated solution (aqueous) of the acid contains 11 g/L and has a pH = 2.94. What is the value of the acid dissociation constant?
What volume in mL of concentrated nitric acid (72.0% HNO3 (w/w), sp. gr. 1.42) is required to prepare exactly 2.00 L of 0.200 M HNO3?
How many stereoisomers are possible for CH2Cl2 provided that the central carbon has a square planar geometry
Using the data in your textbook, calculate the concentrations of the molecular and ionic species and the pH in aqueous solution that has a formal composition of 0.0700 M KH2PO4 + 0.5500 M K2HPO4.
why is the identity of an element determined by the number of protons in its nucleus? why cant the identity be
If 56.4 mL of BaCl2 solution is needed to precipitate all the sulfate ion in a 748 mg sample of Na2SO4, what is the molarity of the solution?
Equilibrium is established for the reaction 2X(s) + Y(g) ? 2Z(g) at 500K, Kc = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K. A) 3.2 M B) 3.5 M C) 4.5 M D) 7.1 M E) None of these.
A mixture of 7.50 g He and 29.5 g Ne has a pressure of 750. mm Hg. What is the partial pressure of each of the gases?
What is the equilibrium concentration of Cl at 1000 ? What is the equilibrium concentration of COCl2 at 1000 ?
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