Potenciometric titration
Why the solution turns green as the titration proceeds? Explain what is causing this phenomenon. 6Fe +2 + Cr2O7-2 + 14H+ ⇌ 6Fe+3 + 2Cr+3 + 7H2O.
Potenciometric titration Why the solution turns green as the titration proceeds? Explain what is causing this...
Write balanced half-reactions for the following redox reaction: Cr2O7^2-(aq)+14H^+(aq)+6Fe^+2(aq)? 2Cr^+3(aq)+7H2O(l)+6Fe^+3(aq) Reduction: Oxidation:
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...
Using the molar ratio of the redox reaction between chromium as potassium dichromate and Fe2+ as ferrous ammonium sulfate, how can we determine how much of the ferrous ammonium sulfate (solid) should be added to a 20mL sample of wastewater containing 600mg/L of chromium (from potassium dichromate) in order to reduce the hexavalent chromium to trivalent chromium? Based on 6Fe2 + Cr2O7 2- + 14H+ - - > 2Cr 3+ + 7H2O + 6Fe 3+
Redox titration between Sn2 + 0.2 M 20 ml and Cr2O7 ^ -2 0.0006 M in 1 M H2So4 solution at all times Sn4+ + 2e >> Sn2+ E (v) = 0.154 Cr2O7^-2 + 14H + 6e>> 2Cr3 + 7H2O E (v) = 1.33 1.initial point 2.Before equivalence point 100 ml and 200 ml 3. Equivalent point 4.After equivalent point
A solution of iron (II) sulfate was prepared by dissolving 10.00g of FeSO4-7H20 (FW= 277.9) in water and diluting up to a total volume of 250 ml. The solution was left to stand, exposed to air, and some of the iron (II) ions became oxidized to Iron (III) ions. a 25.0 ml sample of this partially oxidized solution required 23.70 ml of 0.0100M potassium dichromate K2Cr2O7 solution for complete reaction in the presence of dilute sulfuric acid. Calculate the percentage...
explain why it is important to rinse the buret with KMnO4 solution twice before titration? And why you should rinse buret with water thoroughly before you leave?
10. Explain why the pH titration curve shown below for the titration of an unknown weak acid with a strong base has two inflection points or "bumps". List the species present in solution at each of the equivalence points. 6 2 8 Volume of Strong Base Added (mL) 11. What are the points A, B and C on the pH titration curve shown in question 10 called? Fill in the blanks in the sentences below for each of the points...
what is the main reason behind titration and why solution turn pink in acid base titration when o.1 % thymol blue.?
4. Explain why the solution being titrated first turns pink then goes colorless before the endpoint is reached. 5. A student gets a dark pink color for trial 2 but uses that data to calculate the mass percent of acetic acid. Would the mass percent be too high or too low? Explain and be specific Experiment 10 Determination of the Molar Gas Constant, R
What color, and why, appears brighter in the darkness? Red or green? Explain. What color, and why, appears brighter in the darkness? Red or yellow? Explain.