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During the distillation of a mixture of two miscible liquids with very different boiling points, the temperature rises to a constant reading and then drops off before returning to a higher reading. Explain the likely cause of this fluctuation in temperature readings.
hydroxylamine is titrated to the equivalence point with 35.8 m of .15 M HCl. What is the pH at the equivalence point?
Calculate a change in pH when 10 mL of 0.2 M LiOH is added to the buffer made by mixing 50mL of 0.1 M hydrobromous acid (HOBr) and 40 mL of 0.2 M of sodium hydrobromide
For the equilibrium H2(g)+ CO2 (g) H20 (g) + CO(g) Kc = 3.18 at 1106K. If each of the four species was initially present at a concentration of 3.000M, calculate the equilibrium concentration of the CO(g) at this temperature
What is the pH of this buffer after 0.45 mL of 10.0 M hydrochloric acid are added to it? The Ka for HF is 6.8 x 10-4.
Since the freezing point of a solution depends on the number of particles, what would you expect the freezing point of 0.1 m solutions of aqueous NaCL and BaCl2?
Karel added 45.5 mL of 1.1 M HCl to his; and Caleb added 50.0 mL of 1.0 M HCl. Two of these students will report, within experimental error, the same increase in solution temperature for the neutralization. Which are the two students? Explain.
suppose you want to find out how many milliliters of 1.0 M AgNO3 are needed to provide 169.9g of pure AgNO3.
Predict the outcome of the following reactions represented by the following equations by using the activity series, and balance the equations.
What ions and/or molecules are present in relatively large proportions in a solution of a weak base NH4OH (aq)?
what percentage of HSO4- is dissociated in 2M solution? Why does molarity approximate molality at low concentrations?
A 100.0 mL sample of .20 M HF is titrated with .10 M KOH. Determine the pH of the solution after the addition of 100.0 mL of KOH. The Ka of HF is 3.5*10^-4
the heat of combustion of c10h18 is -6286 kj/mol. the heat of combustion for c10h8 is -5157kj/mol.
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