A sample of copper ore with a mass of 0.4225 g was dissolved in acid. A...
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A sample of copper ore with a mass of 0.4225 g was dissolved in
acid. A...
A 2.50 g sample of bronze was dissolved in sulfuric acid. The copper in the alloy...
A 2.50 g sample of bronze was dissolved in sulfuric acid. The copper in the alloy reacted with sulfuric acid as follows: Cu(s) + 2H2SO4 (aq) → CuSO4 (aq) + SO2(g) + 2 H20 (1) The CuSO4 formed in the reaction was mixed with Kl to form Cul (copper iodide). 2 CuSO4 (aq) + 51 → 2 Cul (s) + 1; (aq) + 2 So(aq) The formed in that reaction was then titrated with (aq) + 2 5,03 – 31...
A 0.1362g iron ore sample was dissolved in hydrochloric acid and the iron was obtained as...
A
0.1362g iron ore sample was dissolved in hydrochloric acid and the
iron was obtained as Fe^2+(aq). The iron solution was titrated with
Ce4+ solution according to the balanced chemical reaction shown
below. After calculation, it was found that 0.0238g of iron from
the ore reacted with the cerium solution.
Ce^4+(aq) + Fe 2+(aq) -> Ce^3+(aq) + Fe^3+(aq).
Calculate the mass percent of iron in the original ore sample.
Please round your answer to the tenths place.
Question 7 (2...
A 50.0 g sample of ore containing FeBr2 is dissolved in acid and titrated to an...
A 50.0 g sample of ore containing FeBr2 is dissolved in acid and titrated to an end point with 24.80 mL of 0.629 M Cr2O72−. The following redox reaction takes place: Cr2O72− (aq) + Fe2+ (aq) ⟶ Cr3+ (aq) + Fe3+ (aq) a. balance the reaction b. what % of the ore sample if FeBr2 (molar mass = 215.65 g/mol)
The zinc content of a 1.23 g ore sample was determined by dissolving the ore in...
The zinc content of a 1.23 g ore sample was determined by dissolving the ore in HCI, which reacts with the zinc, and then neutralizing excess HCl with NaOH. The reaction of HCI with Zn is shown below. Zn(s)-2HCl(aq) → ZnCl2(aq)-H,(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 9.19 mL of 0.529 M NaOH...
2. A 0.1000 g sample of KBrO3 was dissolved in dilute acid and treated with an...
2. A 0.1000 g sample of KBrO3 was dissolved in dilute acid and treated with an excess of KI. BrO3 +91 +6H+ → Brº+ 313 + 3H20 The generated 13. required 11.92 mL of a Na2S2O3 solution to reduce it to 1. Use the above balanced equation and those found in the introduction to determine the molarity of the Na2S2O3 solution. 3. The following data was obtained for an iodometric titration of an ascorbic acid tablet. Mass of tablet: 1.2191...
A 0.450 g sample of impure CaCO, (s) is dissolved in 50.0 mL of 0.150 M...
A 0.450 g sample of impure CaCO, (s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is CaCO,(s) + 2 HCl(aq) — CaCl, (aq) + H, 0(1) + CO2(g) The excess HCl(aq) is titrated by 4.85 mL of 0.125 M NaOH(aq) Calculate the mass percentage of Caco, (s) in the sample. mass percentage: The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl, which reacts with the...
An iron ore sample weighing 0.5562 g is dissolved HCl (aq), and the iron is obtained...
An iron ore sample weighing 0.5562 g is dissolved HCl (aq), and the iron is obtained as Fe2+ in solution. This solution is then titrated with 28.72 mL of 0.04021 M K2Cr2O7 (aq). What is the percent by mass iron in the ore sample? How do I get to the equation 6Fe^2+ + 14H^+ + Cr2O7^2- ----> 6Fe^3+ + 2Cr^3+ + 7H2O ??? I am just generally confused on how to start this and how to do this step by...
A 0.4598 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid....
A 0.4598 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO2·4H2O and removed by filtration. The resulting filtrate and washings were diluted to a total volume of 250.0 mL. A 20.00 mL aliquot of this solution was buffered, and titration of the lead, copper, and zinc in solution required 34.81 mL of 0.001487 M EDTA. Thiosulfate was used to mask the copper in a second 25.00 mL aliquot. Titration of...
A 0.4505 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid....
A 0.4505 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO2⋅4H2Oand removed by filtration. The resulting filtrate and washings were diluted to a total volume of 250.0 mL. A 15.00 mL aliquot of this solution was buffered, and titration of the lead, copper, and zinc in solution required 35.10 mL of 0.001497 M EDTA. Thiosulfate was used to mask the copper in a second 20.00 mL aliquot. Titration of the...
A 0.4504 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid....
A 0.4504 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO2⋅4H2O and removed by filtration. The resulting filtrate and washings were diluted to a total volume of 250.0 mL. A 15.00 mL aliquot of this solution was buffered, and titration of the lead, copper, and zinc in solution required 35.78 mL of 0.001478 M EDTA. Thiosulfate was used to mask the copper in a second 20.00 mL aliquot. Titration of...
A 2.50 g sample of bronze was dissolved in sulfuric acid. The copper in the alloy reacted with sulfuric acid as follows: Cu(s) + 2H2SO4 (aq) → CuSO4 (aq) + SO2(g) + 2 H20 (1) The CuSO4 formed in the reaction was mixed with Kl to form Cul (copper iodide). 2 CuSO4 (aq) + 51 → 2 Cul (s) + 1; (aq) + 2 So(aq) The formed in that reaction was then titrated with (aq) + 2 5,03 – 31...
A
0.1362g iron ore sample was dissolved in hydrochloric acid and the
iron was obtained as Fe^2+(aq). The iron solution was titrated with
Ce4+ solution according to the balanced chemical reaction shown
below. After calculation, it was found that 0.0238g of iron from
the ore reacted with the cerium solution.
Ce^4+(aq) + Fe 2+(aq) -> Ce^3+(aq) + Fe^3+(aq).
Calculate the mass percent of iron in the original ore sample.
Please round your answer to the tenths place.
Question 7 (2...
The zinc content of a 1.23 g ore sample was determined by dissolving the ore in HCI, which reacts with the zinc, and then neutralizing excess HCl with NaOH. The reaction of HCI with Zn is shown below. Zn(s)-2HCl(aq) → ZnCl2(aq)-H,(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 9.19 mL of 0.529 M NaOH...
2. A 0.1000 g sample of KBrO3 was dissolved in dilute acid and treated with an excess of KI. BrO3 +91 +6H+ → Brº+ 313 + 3H20 The generated 13. required 11.92 mL of a Na2S2O3 solution to reduce it to 1. Use the above balanced equation and those found in the introduction to determine the molarity of the Na2S2O3 solution. 3. The following data was obtained for an iodometric titration of an ascorbic acid tablet. Mass of tablet: 1.2191...
A 0.450 g sample of impure CaCO, (s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is CaCO,(s) + 2 HCl(aq) — CaCl, (aq) + H, 0(1) + CO2(g) The excess HCl(aq) is titrated by 4.85 mL of 0.125 M NaOH(aq) Calculate the mass percentage of Caco, (s) in the sample. mass percentage: The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl, which reacts with the...
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