When measuring the PO43– concentration of a solution using the Volhard method, why is it necessary...
When measuring the PO43– concentration of a solution using the Volhard method, why is it necessary to make the solution acidic using HNO3 during the back titration of the excess Ag with SCN–?
Homework Answers
To prevent hydrolysis of iron(III) to form hydrated oxide. It precipitates in the solution preventing the formaton of complex with SCN- .
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When measuring the PO43– concentration of a solution using the Volhard method, why is it necessary...
It is customary to perform a blank titration with each analysis. Volhard method, an example of...
It is customary to perform a blank titration with each analysis. Volhard method, an example of back titration, does not make use of a blank. Explain why.
In the United States, table salt is “iodized” and contains NaCl and a small amount of...
In the United States, table salt is “iodized” and contains NaCl and a small amount of KI. The iodide was added to help prevent thyroid disorders in the population. The iodide concentration in table salt was measured using the following steps: 1.000 g of table salt was dissolved in 100.0 mL of water. The salt solution was titrated using 4.00 × 10−5 M Ag+ and a Volhard titration (back titration). 15.00 mL of 4.00 × 10−5 M Ag+ solution was...
In the United States, table salt is “iodized” and contains NaCl and a small amount of KI. The iodide was added to help p...
In the United States, table salt is “iodized” and contains NaCl and a small amount of KI. The iodide was added to help prevent thyroid disorders in the population. The iodide concentration in table salt was measured using the following steps: 1.000 g of table salt was dissolved in 100.0 mL of water. The salt solution was titrated using 4.00 × 10−5 M Ag+ and a Volhard titration (back titration). 15.00 mL of 4.00 × 10−5 M Ag+ solution was...
(5 marks) A solution containing chloride ion was analyzed by the mL sample containing chloride ion...
(5 marks) A solution containing chloride ion was analyzed by the mL sample containing chloride ion was treated with 25.00 mL of 0.2500 M silver nitrate. The precipitated AgCl was removed from the solution by filtration, and 1.00 mL of 0.1000 M Fe3 was added to the filtrate in order to titrate excess Ag with SCN. A volume of 10.67 mL of 0.2380 M KSCN was required for solution to turn red colour. What is the concentration of chloride ion...
6. a. In a lab project, a student obtained a highly turbid acidic solution whose concentration...
6. a. In a lab project, a student obtained a highly turbid acidic solution whose concentration has to be determined. Write one method by which he can determine the concentration. Give reason for your answer. (2 marks) b. A chlorophyll sample contains Mg2+ ions. Describe in brief the sequential steps to determine the concentration of the metal ion in the sample using a simple titration. Which medium is suitable for performing the titration, acidic or basic medium and why? (3...
J. Using activity coefficients calculate the molar concentration of SCN- in a solution saturated with AgSCN...
J. Using activity coefficients calculate the molar concentration of SCN- in a solution saturated with AgSCN that also contains 0.050 M KNO3, an inert salt AgSCN (s) -> Ag* + SCN- Ksp= 1.1 X 10-12
Calculate the concentration of the acid (or base) remaining in solution when 6.57 mL of 6.11...
Calculate the concentration of the acid (or base) remaining in solution when 6.57 mL of 6.11 M HNO3 is added to 7.65 mL of 7.95 M NaOH. Note the final volume is the sum of the two added volumes. Which of the following statements is true for the solution after mixing? -NaOH is in excess over HNO3. -HNO3 is in excess over NaOH. -HNO3 and NaOH are exactly balanced. What is the concentration of the excess NaOH (or HNO3) you...
Why is a large excess of Fe3+ added when preparing the standard solution. Why do you...
Why is a large excess of Fe3+ added when preparing the standard solution. Why do you not add a large excess of Fe3+ when preparing the equilibrium solution. Fe^3+ + SCN^- = FeSCN^2+?
When measuring the concentration of the blue dye you get a reading of 3.0 for an...
When measuring the concentration of the blue dye you get a reading of 3.0 for an initial stock solution, and again after it is diluted. Explain why this result could occur
Why is a large excess of Fe3+ added when preparing the standard solution. But you not...
Why is a large excess of Fe3+ added when preparing the standard solution. But you not add a large excess of Fe3+ when preparing the equilibrium solution. Fe^3+ + SCN^- = FeSCN^2+
(5 marks) A solution containing chloride ion was analyzed by the mL sample containing chloride ion was treated with 25.00 mL of 0.2500 M silver nitrate. The precipitated AgCl was removed from the solution by filtration, and 1.00 mL of 0.1000 M Fe3 was added to the filtrate in order to titrate excess Ag with SCN. A volume of 10.67 mL of 0.2380 M KSCN was required for solution to turn red colour. What is the concentration of chloride ion...
6. a. In a lab project, a student obtained a highly turbid acidic solution whose concentration has to be determined. Write one method by which he can determine the concentration. Give reason for your answer. (2 marks) b. A chlorophyll sample contains Mg2+ ions. Describe in brief the sequential steps to determine the concentration of the metal ion in the sample using a simple titration. Which medium is suitable for performing the titration, acidic or basic medium and why? (3...
J. Using activity coefficients calculate the molar concentration of SCN- in a solution saturated with AgSCN that also contains 0.050 M KNO3, an inert salt AgSCN (s) -> Ag* + SCN- Ksp= 1.1 X 10-12
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