A 0.7257 g mixture of KCN (MW = 65.116 g/mol) and NaCN (MW =
49.005 g/mol) was dissolved in water. AgNO3 was added to the
solution, precipitating all the CN– in solution as AgCN (MW =
133.886 g/mol). The dried precipitate weighed 1.650 g. Calculate
the weight percent of KCN and NaCN in the original sample.
MW (g/mol) / MP ( oC) / Solubility in cold H2O (g / 100 mL) /
Solubility in boiling H2O (g / 100 mL)
Acetanilide 135.2 / 114 / 0.54 / 5.0
Phenacetin 179.2 / 135 / 0.076 / 1.22
Using solubility data in the table of reagents, calculate the
minimum amount water needed to recrystallize:
i. 1.5 g of phenacetin.
ii. 1.5 g of acetanilide.
b. If the minimum amount of water needed is used, how many grams
of...
Calculate the freezing point of a solution of 40.0 g methyl
salicylate, (MW: 152.15 g/mol), dissolved in 800. g of benzene,
C6H6. Kf of benzene is 5.10 C/m and the freezing point is 5.50°C
for benzene.
Calculate the vapor pressure of a 20 % by mass sucrose (MW=
342.30 g/mol) solution. The vapor pressure of pure water is 23.8
torr.
A) 23.50 torr B) 1.40 torr C) 23.8 torr D) 0.987 torr E) 4.44
torr
3. Calculate the pH of a buffer solution made by adding 25.5 g
of NaCH3CO2 (MW:82.034g/mol), and 0.550M HCH3CO2 (Ka=1.8x10-5) to
make 500 mL of the buffer. a. Identify the acid and the base (write
the formula and the ID next to it) b. Will Na+ affect the pH of the
solution? Why? c. What is your prediction for the calculated pH
compared to the pKa of the sample? Why? d. What is the pH of the
solution? Was your...
A sample containing a mixture of SrCl2·6H2O (MW = 266.62 g/mol)
and CsCl (MW = 168.36 g/mol) originally weighs 1.7215 g. Upon
heating the sample to 320 °C, the waters of hydration are driven
off SrCl2·6H2O, leaving the anhydrous SrCl2. After cooling the
sample in a desiccator, it has a mass of 1.2521 g. Calculate the
weight percent of Sr, Cs, and Cl in the original sample.
If you are given the following
solids:
Na3PO4 MW
= 163.94 g/mol
K3PO4
MW = 212.26 g/mol
NaH2PO4
MW = 119.98 g/mol
K2HPO4
MW = 174.17 g/mol
Na2HPO4
MW = 141.96 g/mol
KH2PO4
MW = 136.08 g/mol
Which compounds would you use to
prepare your stock solutions? Why?
I picked KH2PO4 and K2HPO4 because potassium salts dissolve more
readily in H2O which would make the lab go more smoothly. I would
like to know if I'm missing any...
Calculate the freezing point of a solution containing 1.25 g of
benzene (78 g/mol) in 100 g of chloroform.
∆T =
Km
Kfp chloroform = 4.68
oC/m
Freezing point chloroform = -63.5
oC