A 0.9140 g sample of a mixture of NaCl and KCl is
dissolved in water, and the solution is then treated with an excess
of AgNO3 to yield 1.943 g of AgCl.
Calculate the percent by mass of each compound in the
mixture.
A 0.9000 g sample of a mixture of NaCl and KCl is dissolved in
water, and the solution is then treated with an excess of
AgNO3 to yield 1.923 g of AgCl. Calculate the percent by
mass of each compound in the mixture.
____% mass of NaCl
____% mass of KCl
1.8 grams of ammonia, NH3 (M=18 g/mol), is dissolved in 10L of
water. Which best approximates the pH of the solution? Please
explain/show work.
The answer is 7-11.9, but I got 12 and was wondering why it's
less than that.
When a 7.00-g sample of RbBr is dissolved in water in a
calorimeter that has a total heat capacity of 1.931 kJ·K–1, the
temperature decreases by 0.480 K. Calculate the molar heat of
solution of RbBr.
Quantitative Analysis a. A 1.861g sample of a certain monoprotic
acid was dissolved in water and titrated with a 0.1984 M sodium
hydroxide solution. The titration endpoint was reached after 45.9
mL of the titrant was added. What is the molar mass of the
acid?
b. Combustion analysis of a hydrocarbon released 321 mg carbon
dioxide and 164 mg water. What is the empirical formula of the
compound?
A mixture contains only and . A 4.51-g sample of the mixture is
dissolved in water and an excess of is added, producing a
precipitate of . The precipitate is filtered, dried, and weighed.
The mass of the precipitate is 1.06 g. What is the mass percent of
in the sample?
%
A 1.23 gram sample of an unknown monoprotic
acid is dissolved in 25.0mL of water and titrated
with a a 0.227 M aqueous barium
hydroxidesolution. It is observed that after
12.1 milliliters of barium
hydroxide have been added, the pH is
3.653 and that an additional 6.30
mL of the barium hydroxide solution is required to
reach the equivalence point.
(1) What is the molecular weight of the
acid? g/mol
(2) What is the value of Ka for the acid?
A 29.0-g sample of NaOH is dissolved in water, and the solution
is diluted to give a final volume of 1.60 L. The molarity of the
final solution isA) 18.1 M B) 0.453 M C) 0.725 M D) 0.0552 M E)
0.862 M
A 0.15 g sample of a purified protein is dissolved in water to
2.0ml of solution. The osmotic pressure is found to be 18.6 torr.
Calculate the molar mass of the protein.