4. 62.4 mL of 0.39 M NaCl solution was added to 26.8 mL of 058 M
Pb(NO3)2 solution. a. Write the full balanced reaction, the
molecular ionic equation and the net ionic equation.
b. What is the precipitate? c. How many grams of the precipitate
can be made
If the density of water is 1g/mL and the density of a 0.16 M HCl
solution is 1.023 g/mL, how do I use this information to determine
the mass of both water and HCl in one liter of the solution?
***Cancel this question! I figured it out!
9) An aqueous solution of HCl is 0.500 M. Its density
is 1.20 g/mL. Calculate the molality of HCl in this solution.
a) 0.417 m
b) 0.424 m
c) 0.430 m
d) 0.500 m
e) 0.600 m
10) The normal freezing point of benzene
(C6H6) is 5.48°C. When 2.00 g of an unknown
covalent compound is dissolved in 100.0 g of benzene, the freezing
point of the resulting solution is 5.08°C. What is the molar mass
of the unknown compound?...
The density of a 40 wt% solution of ethanol in water is 0.937
g/mL. The density of n-butanol is 0.810 g/mL. What is the
concentration of n-butanol in ppm if you dissolve 20 μL of this
alcohol in a 40 wt% solution of Ethanol in water. The final volume
of the solution is 25 mL. Assume that the density of the ethanol
solution does not change upon dissolution of the butanol. Use the
correct number of significant figures! Hint: to...
A 0.380 m aqueous solution of NaCl is prepared at 20.0∘C. Assume
that the density of the solution at 20.0∘C is 1.082 g/mL.
Calculate the molarity of the salt solution.
A solution prepared by mixing 22.4 mL of 0.380 M NaCl and 22.4
mL of 0.380 M KI was titrated with 0.190 M AgNO3 in a cell
containing a silver indicator electrode and a saturated calomel
reference electrode.
(a) What is [Ag ] when 21.2 mL of 0.190 M AgNO3 have been added?
Express your answer as x, where [Ag ] is a quotient having the form
Ksp,AgI/x. (b) What is [Ag ] when 67.0 mL of 0.190 M AgNO3...