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Problem- What is the freezing point of a solution that contains 28.3g of urea, CO(NH2)2, in 275mL water, H2O? Assume a density of water of 1.00 g/mL.
Using textbook reference solve the reactions given in above problem
There is an inherent flaw in the drying procedure for the gravimetric determination that causes the measured mass of BaSO4 to be erroneously high
The pH at the ¼ neutralized point in the titration of a weak acid is 3.958. What is the pKa of this acid
Suppose that 0.570 mol of methane is reacted with 0.720 mol of fluorine forming CF4(g) and HF(g) as sole products. Assuming that the reaction occurs at constant pressure, how much heat is released?
silver has only two naturally occurring isotopes 107ag with a mass of 106.90509amu and an abundance of 51.84% and 109ag with a mass of 108.9047 amu calculate the atomic mass of silver.
How much heat energy is required to raise the temperature of 0.367 kg of copper from 23.0 degrees C to 60.0 degrees C? The specific heat of copper is 0.0920 cal/(g*C)
2.51 moles of a gas occupies 50.88 liters, and its density is 1.43 g/L at a particular temperature and pressure. Calculate the molar mass of the gas.
Calculate the PH of the cathode compartment solution if the cell emf at 298K is measured to be 0.660V when (Zn^2+)=0.22 M and(P_H2)= 0.87atm
Magnesium Hydroxide is a slightly soluble substance. If the pH of a saturated solution of Mg(OH)2 is 10.49 at 25 degrees celcius, calculate Ksp for Mg(OH)2.
The equilibrium constant Kc for this reaction is 1.2 102 at 150°C. What is the direction (forward or reverse) needed to attain equilibrium at 150°C
A solution is 0.0100 M in Pb2+ ions. If 0.103 mol of solid NaI is added to 1.00L of this solution (with negligible volume change), what percent of the Pb2+ ions remain in solution?
Show your calculations for the pH when 0.00 mL, 4.00 mL, 6.00 mL, 12.00 mL (equivalence point), and 16.00 mL of 0.10 M HCl have been aded to an initial
How many grams of potassium nitrate are required to prepare 0.250 L of a 0.700 M solution?
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