Question

a 2.50 gram sample of an unknown silver salt (possibly AgClO3, AgClO4, AgNO3, or AgF) is dissolved in water. An excess of HCl solution is added and 1.88 g of AgCl is collected. Determine the identity of the silver salt.

Answer #1

a 12.42g sample of a mixture of NaCl and CaCl was dissolved in
water. Excess AgNO3 was added and all of the chloride was
precipitated as AgCl. 31.70g of AgCl was collected. Calculate the
w/w% of NaCl in the orginal mixture.

A 2.960 gram sample containing an unknown amount of arsenic
trichloride and the rest inerts was dissolved into a NaHCO3 and HCl
aqueous solution. To this solution was added 1.520 grams of KI and
50.00 mL of a 0.00820 M KIO3 solution. The excess I3– was titrated
with 50.00 mL of a 0.02000 M Na2S2O3 solution. What was the mass
percent of arsenic trichloride in the original sample?

A 1.199 gram sample containing an unknown amount of arsenic
trichloride and the rest inerts was dissolved into a NaHCO3 and HCl
aqueous solution. To this solution was added 1.810 grams of KI and
50.00 mL of a 0.00834 M KIO3 solution. The excess I3– was titrated
with 50.00 mL of a 0.02000 M Na2S2O3 solution. What was the mass
percent of arsenic trichloride in the original sample?

A 1.26 gram sample of an unknown monoprotic
acid is dissolved in 50.0 mL of water and titrated
with a a 0.306 M aqueous potassium
hydroxide solution. It is observed that after
12.7 milliliters of potassium
hydroxide have been added, the pH is
3.193 and that an additional 19.3
mL of the potassium 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...

A 0.872 gram sample of an unknown monoprotic acid is dissolved
in 50.0 mL of water and titrated with a a 0.424 M aqueous sodium
hydroxide solution. It is observed that after 9.40 milliliters of
sodium hydroxide have been added, the pH is 3.350 and that an
additional 5.50 mL of the sodium 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...

A 1.54 gram sample of an unknown monoprotic
acid is dissolved in 30.0 mL of water and titrated
with a a 0.225 M aqueous potassium
hydroxide solution. It is observed that after
19.3 milliliters of potassium
hydroxide have been added, the pH is
7.171 and that an additional 34.5
mL of the potassium 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...

A 1.22 gram sample of an unknown monoprotic acid is dissolved in
25.0 mL of water and titrated with a a 0.299 M aqueous potassium
hydroxide solution. It is observed that after 10.4 milliliters of
potassium hydroxide have been added, the pH is 3.039 and that an
additional 19.4 mL of the potassium 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...

A sample of 1.699g of an unknown compound container silver is
dissolved in water and treated with an ecesss of sodium chloride in
acidic condition. F the mass of the silver chloride precipitate
formed is 1.434g, what is the percent by mass of silver in our
original unknown compound

When 2.50 g of an unknown weak acid (HA) with a molar mass of
85.0 g/mol is dissolved in 250.0 g of water, the freezing point of
the resulting solution is -0.259 ∘C.
Calculate Ka for the unknown weak acid.

20.0 L of an aqueous solution of silver nitrate (AgNO3). 10.0 L of a 0.0500 mol / L solution of calcium iodide (CaI2) is added thereto. At the end, all the Ag + ions precipitated and the molar concentration of the I ions is 0.0100 mol / L.
a) What was the initial molar concentration of AgNO3?
b) What mass of silver iodide has precipitated?
c) What is the melting point of the final water (suppose 1 liter of solution...

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