The reaction between iron(II) (Fe²+) and dichromate (Cr, 0;) in the presence of a strong acid (H*) is shown. Cr,0+6 Fe2+ + 14H* 2 Cr+ + 6 Fe* +7H,0 Determine the volume, in milliliters, of a 0.240 M solution of Mohr's salt ((NH,),Fe(SO,), 6 H,0) needed to completely react with 0.0800 L of 0.240 M potassium dichromate (K, Cr, O,). volume: mL What volume, in milliliters, of 0:240 M K,Cr, O, is required to completely react with 0.0800 L of a 0.240 M solution of Mohr's salt? volume: mL

The reaction between iron(II) (Fe²+) and dichromate (Cr, 0;) in the presence of a strong acid (H) is shown. Cr,0+6 Fe2+ + 14H 2 Cr+ + 6 Fe* +7H,0 Determine the volume, in milliliters, of a 0.240 M solution of Mohr's salt ((NH,),Fe(SO,), 6 H,0) needed to completely react with 0.0800 L of 0.240 M potassium dichromate (K, Cr, O,). volume: mL What volume, in milliliters, of 0:240 M K,Cr, O, is required to completely react with 0.0800 L of a 0.240 M solution of Mohr's salt? volume: mL

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A chemist mixes 1.63 L each of 0.195 M Na2CO3 and 0.390 M CaCl2 in a beaker. What is the concentration of carbonate ion, CO32−, in the final solution?
Silver chromate is sparingly soluble in aqueous solutions. The ?sp of Ag2CrO4 is 1.12×10−12 M^3 What is the solubility (in moles per liter) of silver chromate in a 1.10 M silver nitrate aqueous solution? M=
Describe (in detail) the preparation of 800 mL of 50 parts per thousand of Cl- from 0.02 M Lead(II) chloride
The iron content of iron ore can be determined by titration with K₂Cr₂O₇ according to the equation 14H⁺(aq) + Cr₂O₇²⁻(aq) + 6Fe²⁺(aq) → 6Fe³⁺(aq) + 2Cr³⁺(aq) + 7H₂O(l) Diphenyl amine is used as an indicator as it changes color from green to purple when the endpoint is reached. A sample of iron ore with a mass of 3.255 g was dissolved with HCl and then treated with a reducing agent to convert any Fe³⁺ in the ore to Fe²⁺. Titration with 0.0645 M K₂Cr₂O₇ solution required 45.65 mL of the solution to reach the endpoint. The molar mass of Fe is 55.85 g/mol. Calculate the mass percent iron in the ore.
What is the concentration of Co(OH)₂ (aq) in a solution in which the concentrations of Co²+ and OH are fixed at 2.9 x 10-5 M? The cumulative formation constant (B₂) for Co(OH)₂ (aq) in water is 1.6 × 10⁹. [Co(OH)₂] = M
A sample consisting of Na2CO3, NaHCO3 and inert matter weighs 1.179 grams. It is titrated with 0.1 N HCl with phenolphthalein as the indicator, and the solution became colorless after the addition of 24.00 mL. Another duplicate sample was titrated with HCl using methyl orange as indicator. It required 50.25 mL of the acid for the color change from yellow to red. What are the percentage of Na2CO3 and NaHCO3 in the sample? Note [EXAMPLE IN THE IMAGE]
What will be the solubility product constant, Qsp, for the reaction of 64.5 mL of 0.045 M Ni(NO3)2 and 85.5 mL of 0.025 M Li2CO3? Ni(NO3)2 (aq) + Li2CO3 (aq) →
Nitesh
What quantity in moles of precipitate will be formed when 60.5mL of 0.350M AgNO3 is reacted with excess Mgl2 in the following reaction? 2 AgNO3(aq)+Mgl2(aq)= 2Agl(s)+Mg(NO3)2(aq)
(a) For lead(II) bromate, Pb(BrO3)2, at 25°C, a team of student researchers finds that 0.290 g is the maximum amount of the solid that dissolves in water to give 50.0 mL of solution. Based on these results, what is the molar solubility of lead(II) bromate? (b) Using your result from part a, find the molar solubility of lead(II) bromate in 0.150 M NaBrO3.
2Fe(s) + 3Cu2+(aq) 2Fe3+(aq) + 3Cu(s) a)Calculate the minimum volume of 1.16M CuSO4 solution that is required to ensure complete reaction of 1.04g of Fe.Since you do not know which reaction will be the one to occur, you must base the calculation on whichever of the equations requires more CuSO4 solution. b)To ensure that sufficient CuSO4 is used, it is common practice to add an excess.Calculate the volume of 1.16M CuSO4 needed to provide a 20% excess in this case.
A 750. mL sample of 0.13 M K₂CO3(aq) is combined with 250. mL of 0.13 M CUNO3(aq). The Ksp for Cu₂CO3 = 1.4 x 10-10 and the Ksp for KNO3 = 1.4 x 10¹0. Which of the following statements is true? Both Cu₂CO3 and KNO3 will precipitate. KNO3 will precipitate. No precipitate forms. There is not enough information to make any of the above predictions. Cu₂CO3 will precipitate.