Question
In: Chemistry
The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl,
The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HCl is then neutralized with with NaOH. The reaction of HCI with Zn is shown.
Zn(s)+2 HCl(aq) → ZnCl2 (aq) +H2 (g)
The ore was dissolved in 150 mL of 0.600 M HCI, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.22 mL of 0.539 M NaOH to neutralize the excess HCI. What is the mass percentage (%w/w) of Zn in the ore sample?
The amount of I (aq) in a solution can be determined by titration with a solution containing a known concentration of S2O32- (aq) (thiosulfate ion). The determination is based on the net ionic equation
2S2O32- (aq)+I3-(aq) -> S4O62-(aq) +3I- (aq)
Given that it requires 35.2 mL of 0.240 M Na2S2O3(aq) to titrate a 15.0 mL sample of I3- (aq), calculate the molarity of I3- (aq) in the solution.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
The zinc content of a 1.64 g ore sample was determined by dissolving the ore in...
The zinc content of a 1.64 g ore sample was determined by
dissolving the ore in HCl, which reacts with the zinc, and then
neutralizing excess HCl with NaOH. The reaction of HCl with Zn is
shown below.
The ore was dissolved in 150 mL of 0.600 M HCl, and the
resulting solution was diluted to a total volume of 300 mL. A 20.0
mL aliquot of the final solution required 8.71 mL of 0.510 M NaOH
for the HCl...
The zinc content of a 1.64 g ore sample was determined by dissolving the ore in...
The zinc content of a 1.64 g ore sample was determined by
dissolving the ore in HCl, which reacts with the zinc, and then
neutralizing excess HCl with NaOH.
The ore was dissolved in 150 mL of 0.600 M HCl, and the
resulting solution was diluted to a total volume of 300 mL. A 20.0
mL aliquot of the final solution required 8.71 mL of 0.510 M NaOH
for the HCl present to be neutralized. What is the mass percentage...
The zinc content of a 1.40 g ore sample was determined by dissolving the ore in...
The zinc content of a 1.40 g ore sample was determined by
dissolving the ore in HCl, which reacts with the zinc, and then
neutralizing excess HCl with NaOH. The reaction of HCl with Zn is
shown below.
Zn (s) + 2HCl (aq) --> ZnCl2 (aq) + H2 (g)
The ore was dissolved in 150 mL of 0.600 M HCl, and the
resulting solution was diluted to a total volume of 300 mL. A 20.0
mL aliquot of the final...
The zinc content of a 1.17 g ore sample was determined by dissolving the ore in...
The zinc content of a 1.17 g ore sample was determined by
dissolving the ore in HCl, which reacts with the zinc, and then
neutralizing excess HCl with NaOH. The reaction of HCl with Zn is
shown below.
Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(g)
The ore was dissolved in 150 mL of 0.600 M HCl, and the
resulting solution was diluted to a total volume of 300 mL. A 20.0
mL aliquot of the final solution required 8.50 mL...
After dissolving in 50.0 mL of good water, the zinc in a 0.422 g sample of...
After dissolving in 50.0 mL of good water, the zinc in a 0.422 g
sample of foot powder was titrated at a pH=12.0 with 26.67 mL of a
0.01222 M EDTA solution. Calculate the % Zn in this sample and the
ppm of Zn in the original foot powder sample.
a) A standard ZnCl2 solution is prepared by dissolving 0.6328 g of Zn in an HCl...
a) A standard ZnCl2 solution is prepared by dissolving 0.6328 g
of Zn in an HCl solution and diluting to volume in a 1.00 L
volumetric flask. An EDTA solution is standardized by titrating a
10.00 mL aliquot of the ZnCl2 solution, which requires 10.84 mL of
EDTA solution to reach the end point. Determine the concentration
of the EDTA solution.
b) A 1.4927 g sample of powdered milk is dissolved and the
solution titrated with the EDTA solution prepared...
-- A 1.0000 g sample of zinc metal is added to a solution containing 1.2500 g of...
-- A 1.0000 g sample of zinc metal is added to a
solution containing 1.2500 g of an unknown compound of bismuth and
chlorine. The reaction results in the formation of zinc chloride
and metallic bismuth. When the reaction is complete, unreacted zinc
remains, and this unreacted zinc is consumed by reaction with HCl.
After washing and drying, the mass of bismuth metal recovered is
0.6763g.
Q. Write a balanced chemical equation for the reaction of zinc
with the original unknown...
A sample of a copper ore with a mass of 0.4225 g was dissolved in acid....
A sample of a copper ore with a mass of 0.4225 g was dissolved
in acid. A solution of potassium iodide was added, which caused the
reaction:
2Cu2+(aq) + 5I
Q.-- A 1.0000 g sample of zinc metal is added to a solution containing 1.2500 g...
Q.-- A 1.0000 g sample of zinc metal is added to a solution
containing 1.2500 g of an unknown compound of bismuth and chlorine.
The reaction results in the formation of zinc chloride and metallic
bismuth. When the reaction is complete, unreacted zinc remains, and
this unreacted zinc is consumed by reaction with HCl. After washing
and drying, the mass of bismuth metal recovered is 0.6763g
-- Calculate the experimental % of bismuth in the original
unknown compound
-- If...
A 2.47×10-1 g sample of HCl and a 8.82 g sample of O2 react in a...
A 2.47×10-1 g sample of HCl and a 8.82 g sample of
O2 react in a closed 2.25 L container at 487 K,
according to the following balanced chemical equation:
4HCl(g) +
O2(g) →
2H2O(l) +
2Cl2(g)
Calculate the
PCl2 (in atm) in the container after the reaction has
gone to completion.
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