20.00 cm3 of a 0.1500 mol.dm–3 iron(II) sulphate solution is titrated with a 0.02345 mol.dm–3
sodium dichromate solution in a sulphuric acid medium. What will the titration value be?
20.00 cm3 of a 0.1500 mol.dm–3 iron(II) sulphate solution is titrated with a 0.02345 mol.dm–3 sodium dichromate soluti...
2) ( ) An acidic potassium dichromate can be used to titrate a solution of iron(II) ions since it reacts according to the following equation: Cr2O72 (aq) +6 Fe* (aq) +14 H30' (aq) - 2 Cr* (aq) + 6 Fe" (aq) + 21 H20 (1) a. What is the oxidizing agent in the above reaction? b. A dichromate stock solution is made by dissolving 2.567 g of K Cr2O, (294.2 g/mol) in a total of 50.0 ml. What is the...
A 20.00-mL solution of 0.120 M nitrous acid (Ka = 4.0 × 10–4) is titrated with a 0.215 M solution of sodium hydroxide as the titrant. What is the pH of the acid solution at the equivalence point of titration? (if needed: Kw = 1.00 × 10–14)
1. During a titration experiment, a student titrated 25.00 mL of a 0.100 M sodium hydroxide solution with 5.10 mL of a 0.250 M sulphuric acid solution. What is the pH of the resulting solution? [8]
A 20.00-mL aqueous solution containing tin(II) ions with a concentration of 0.0850 M is titrated with a standard aqueous solution of cerium(IV) ions having a concentration of 0.1100 M. Write a balanced chemical equation for the titration reaction and then find the volume, in mL, of the titrant that is required to reach the stoichiometric point of the titration. b. If the titration were followed potentiometrically using a platinum electrode and a saturated Ag/AgCl electrode, find the following voltages in...
A 20.00 mL wine sample is titrated with a 1.04×10-1M solution of sodium hydroxide. The equivalence point is determined to be 25.926 mL. What is the acidity of the wine expressed as (g tartaric acid / L; MW tartaric acid = 150.085 g/mole)?
The reaction between iron(II) ( Fe2+ ) and dichromate ( Cr2O2−7 ) in the presence of a strong acid ( H+ ) is shown. Cr2O2−7+6Fe2++14H+⟶2Cr3++6Fe3++7H2O Determine the volume, in milliliters, of a 0.180 M solution of Mohr's salt ( (NH4)2Fe(SO4)2⋅6H2O ) needed to completely react with 0.0500 L of 0.180 M potassium dichromate ( K2Cr2O7 ). volume? ... mL What volume, in milliliters, of 0.180 M K2Cr2O7 is required to completely react with 0.0500 L of a 0.180 M solution...
Part A When titrated with a 0.1198 M solution of sodium hydroxide, a 58.00 mL solution of an unknown polyprotic acid required 20.15 mL to reach the first equivalence point. Calculate the molar concentration of the unknown acid. O A¢ * R O ? Submit Request Answer Part B The titration curve was found to have three equivalence points. What volume of the sodium hydroxide solution was necessary to fully titrate the unknown acid solution? IVO ADD A O O...
The reaction between iron(II) (Fe2+) and dichromate (Cr, O) in the presence of a strong acid (Ht) is shown. Cr,O +6 Fe2+ + 14H 2 Cr +6 Fe +7 H,O Determine the volume, in milliliters, of a 0.250 M solution of Mohr's salt ((NH,), Fe(So react with 0.0500 L of 0.250 M potassium dichromate (K,Cr,O,) 6H,O) needed to completely volume: mL What volume, in milliliters, of 0.250 M K,Cr, O, is required to completely react with 0.0500 L of a...
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...
When a 29,8 mL sample of a 0.322 M aqueous acetic acid solution is titrated with a 0,434 M aqueous sodium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 33.2 mL of sodium hydroxide have been added?