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At 298K, the osmotic pressure of a glucose solution is 10.50 atm. Calculate the freezing point of the solution if the density is 1.16g/mL
What concentration of aqueous CaCl2 solution freezes at -10.2ºC? The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºC/m.
calculate the temperature change in the water upon complete melting of the ice. hint determine how much heat is
the enthalpy of formation = 0? Something with standard states? But how do I know what the standard states are
Phosphate systems form essential buffers in organisms. Calculate the pH of a buffer made by dissolving 0.80mol of NaOH in 0.50L of 1.0M H3PO4.
A certain anesthetic contains 64.9 percent C, 13.5 percent H, and 21.6 percent O by mass. At 120°C and 750 mmHg, 1.00 L of the gaseous compound weighs 2.30 g. What is the molecular formula of the compound
ethanol c2h5oh melts at -114degc. the enthalpy of fusion is 5.02 kjmol. the specific heats of solid and liquid ethanol
What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl? a: 0.24 b: 13.1 c: 0.076 d: 6.55 e: 14.3
The atomic mass of boron is 10.81 g/mol. The two naturally occuring isotopes are B-10 with a mass of 10.0129 amu and B-11 with a mass of 11.0093 amu. Determine the percent of naturally occuring B-10.
How come when you add an electron to an anion, the ionic radius increases, but as you go right across a periodic table, atomic radius decreases
predict a shape of small organic molecules that could bind tightly with G4. Be sure to explain your reasoning in terms of the measured distances and discuss the likely intermolecular forces involved in the interaction.
Calculate the mass of solid NaCl that must be aded to 1.50 L of a .100 M AgNO3 solution to precipitate all the AG+ ions in the form of AgCl
The dipole moment of a compound depends on the resultant partial charges based on the electronegativities of the individual constituents present in the compound. Based on this definition, write the resulting dipole moment in the following compounds
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