Question
In: Chemistry
1) If a solution is prepared by mixing 15.7 mL of CH3CH2OH (d = 0.792 g/mL)...
1)
If a solution is prepared by mixing 15.7 mL of CH3CH2OH (d = 0.792
g/mL) and 457 mL of CH3CH2CH2OH (d = 0.911 g/mL) what is the
concentration in molality m?
2) What would be the vapor pressure if 55.6 g of a sugar
(C6H12O6) is dissolved in 440.0 mL of water (d = 1.00 g/mL). The
vapor pressure of water at this temperature is 23.9 torr.
3) 13.2 mg of an unknown non-volatile compound is dissolved in
403 mL of water at 25C. If the solution has an osmotic pressure of
10.44 torr, what is the molar mass of the compound?
Solutions
queen_honey_blossom answered 3 years agoRelated Solutions
Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d...
Calculate the molality of a solution that is prepared by mixing
25.5 mL of CH3OH (d = 0.792 g/mL) and 387 mL of CH3CH2CH2OH (d =
0.811 g/mL). I get 2.01m, but I am not sure if I am doing this
right.
a solution is prepared by mixing equal masses of methanol, ch3oh, and ethanol, ch3ch2oh what is...
a solution is prepared by mixing equal masses of methanol,
ch3oh, and ethanol, ch3ch2oh what is the mole fraction of each
component in the mixture
1. A solution was prepared by mixing 6.00 mL of 1.00M NaOH with 40.00 mL of...
1. A solution was prepared by mixing 6.00 mL of 1.00M NaOH with
40.00 mL of 0.800M weak acid and diluting to a total volume of
100.0 mL. The pH value of this solution was measured to be 3.12.
Calculate the equilibrium hydrogen ion concentration of this
solution using the pH value.
2. For the solution from question 1, calculate the number of
moles of weak acid and calculate the number of moles of hydroxide
ion that were originally present....
1. Determine the pH of the buffer solution that is prepared by mixing 259 mL of...
1. Determine the pH of the buffer solution that is prepared by
mixing 259 mL of 0.0983 M BIS−TRIS propane−H (C11H27N2O6+ ) to 855
mL of 0.0729 M BIS-TRIS_propane (C11H26N2O6) ). Assume the 5%
approximation is valid. Report your answer to 2 decimal places. The
pKa of BIS−TRIS propane−H is 9.10. Submit Answer Tries 0/3 2.
Determine the pH of the BIS−TRIS propane−H/BIS−TRIS propane buffer
solution after the addition of 25.2 mL of 0.643 M solution of
rubidium hydroxide to...
A solution is prepared by mixing 50 mL of 1 M Pb(NO3)2 and 75 mL of...
A solution is prepared by mixing 50 mL of 1 M Pb(NO3)2 and 75 mL
of .5 M NaF. Calculate the concentration of F- ions present at
equilibrium. (Hint: First, write and balance the double
displacement reaction taking place between Pb(NO3)2 and NaF to form
PbF2(s). Perform the necessary stoichiometry (including finding
which reactant is limiting) to calculate how much of each reactant
remains after the reaction goes to completion. Remember that
stoichiometry has to be done in moles. Once...
1) A 150.0 mL solution was prepared by mixing 100.0 mL of 1.00 M HONO (Ka...
1) A 150.0 mL solution was prepared by mixing 100.0 mL of 1.00 M
HONO (Ka = 4.5 x 10–4 ) with 50.0 mL of 1.00 M NaNO2 . Calculate
the pH, [HONO], and [NO2–], once equilibrium has been
established.
2). What is the pH, [OH–], [HF], [F–], and
the percent ionization of a solution prepared as 0.50 M HF ? (HF:
Ka = 7.2 x 10-4)
50 M HF ? (HF: Ka = 7.2 x 10-4)
3. Consider the...
a) What is the pH of a buffer solution prepared by mixing 120 mL of a...
a) What is the pH of a buffer solution prepared by mixing 120 mL
of a 0.435 M CH3CO2H with 50 mL of a .286 M
CH3CO2Na solution?
CH3CO2H Ka = 1.75 x
10-5
b) What is the resulting pH if we add 10.2 mL of a .513 M HCl
solution to this buffer? Does the pH make sense? Why/why not?
c) What is the resulting pH if we add 3.56 mL of a 0.420 M NaOH
solution to the...
A solution is prepared by mixing 150.0 mL of 0.200 M Mg2+ and 250.0 mL of...
A solution is prepared by mixing 150.0 mL of 0.200 M Mg2+ and
250.0 mL of 0.100 M F-. A precipitate forms. Calculate the
concentrations of Mg2+ and F- at equilibrium. Ksp = 6.4 × 10-9
A buffer solution was prepared by mixing 300.0 mL of a 0.200 M solution of hydroxylamine...
A buffer solution was prepared by mixing 300.0 mL of a 0.200 M
solution of hydroxylamine (OHNH2, Kb = 1.1 × 10-8) and 250.0 mL of
a 0.300 M solution of its hydrochloride salt (OHNH3+ Cl- ).
Calculate the pH of the solution after the addition of 1.08 g of
solid NaOH (molar mass = 40.00 g/mol). Assume that there is no
volume change upon the addition of solid.
A buffer solution was prepared by mixing 300.0 mL of a 0.200 M solution of hydroxylamine...
A buffer solution was prepared by mixing 300.0 mL of a 0.200 M
solution of hydroxylamine (OHNH2, Kb = 1.1 ×
10-8) and 250.0 mL of a 0.300 M solution of its
hydrochloride salt (OHNH3+ Cl- ).
Calculate the pH of the solution after the addition of 1.08 g of
solid NaOH (molar mass = 40.00 g/mol). Assume that there is no
volume change upon the addition of solid.
A.
8.22
B.
5.55
C.
6.30
D.
5.78
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