In basic solution hydrogen peroxide oxidizes chromite ions, Cr(OH)4- to chromate ions, CrO4^2-. The hydrogen peroxide...

In basic solution hydrogen peroxide oxidizes chromite ions, Cr(OH)4- to chromate ions, CrO4^2-. The hydrogen peroxide is reduced to hydroxide ions. Write and balance the net ionic equation for this reaction. What is the sum of the reactant coefficients?

Expert Solution

queen_honey_blossom answered 1 year ago

Balance the following basic solution H20+CrO4+Cn-->OCN+Cr(OH)3+h20

10 OH- + 2 Cr(OH)3 +3 Br2 --> 2 CrO4 2- +8 H2O + 6 Br-...

10 OH- + 2 Cr(OH)3 +3 Br2 --> 2 CrO4 2- +8 H2O + 6 Br- Identify element oxidized, reduced, and both the oxidixing and reducing agents.

1)What element is being oxidized in the following redox reaction? Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) +...

1)What element is being oxidized in the following redox reaction? Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) + Cl^- 1B) Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in frot of H+ and Fe3+ in the balance reaction? Fe2+ (aq) + MnO4^- (aq) ---> Fe 3+ (aq) +Mn 2+ 1C) determine the cell notation for the redox reaction given below. [hint: remember sometimes inert electrodes are used. 3 Cl2(g) + 2Fe(s) ---> 6Cl- (aq) +2...

1)What element is being oxidized in the following redox reaction? Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) +...

1)What element is being oxidized in the following redox reaction? Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) + Cl^- 1B) Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in frot of H+ and Fe3+ in the balance reaction? Fe2+ (aq) + MnO4^- (aq) ---> Fe 3+ (aq) +Mn 2+ 1C) determine the cell notation for the redox reaction given below. [hint: remember sometimes inert electrodes are used. 3 Cl2(g) + 2Fe(s) ---> 6Cl- (aq) +2...

1. Determine the molar solubility of Cr3+& OH- ions in the compound Cr(OH)3 at 25oC at:...

1. Determine the molar solubility of Cr3+& OH- ions in the compound Cr(OH)3 at 25oC at: a pH of 7.9 b.0.010 M chromium (III) nitrate c.Distilled water The Ksp is 6.30 x 10-31 2.A solution is prepared by mixing 0.050 M Pb(NO3)2 with 0.00350 M KBr. a. Determine where this solution will be unsaturated,saturated or super saturated. b. Write a balanced net ionic equation for this chemical reaction. 3) The Ksp for PbBr2is 6.6 x 10-63.Calculate the solubility Ag2CrO4(s) in...

A dilute solution of hydrogen peroxide is sold in drugstores as a mild antiseptic. A typical...

A dilute solution of hydrogen peroxide is sold in drugstores as a mild antiseptic. A typical solution was analyzed for the percentage of hydrogen peroxide by titrating it with potassium permanganate: 5H2O2(aq) + 2KMnO4(aq) + 6H+(aq). 8H2O(l) + 5O2(g) + 2K+(aq) + 2Mn2+(aq). What is the mass percent of H2O2 in solution if 55.7g of solution required 38.9 ML of 0.534 M KMnO4 for it's titration?

For each of the transition metal complex ions (a) [Ti(NH3)6]2+ (b) [Cr(H2O)4(OH)2]1- (c) trans–[Pt(CN)2(en)2]2+ (i) Draw...

For each of the transition metal complex ions (a) [Ti(NH3)6]2+ (b) [Cr(H2O)4(OH)2]1- (c) trans–[Pt(CN)2(en)2]2+ (i) Draw the structure of the transition metal complex ion. Show the charge on the complex. (ii) Determine the number of d electrons. (iii) Draw the ground state arrangement of the d electrons in the ground state. (iv) Calculate the LFSE (in units of Δo or ΔT) for each complex.

Part A Calculate the molar concentration of OH− ions in a 8.1×10−2 M solution of ethylamine...

Part A Calculate the molar concentration of OH− ions in a 8.1×10−2 M solution of ethylamine (C2H5NH2)(Kb=6.4×10−4). Express your answer using two significant figures. [OH−] = M Part B Calculate the pH of this solution. Express your answer using two decimal places.

Part A Calculate the molar concentration of OH− ions in a 7.4×10−2 M solution of ethylamine...

Part A Calculate the molar concentration of OH− ions in a 7.4×10−2 M solution of ethylamine (C2H5NH2)(Kb=6.4×10−4). Express your answer using two significant figures. [OH−] = M SubmitMy AnswersGive Up Part B Calculate the pH of this solution. Express your answer using two decimal places. pH = SubmitMy AnswersGive Up

A solution is 5 mM in each of the following ions: number ion Ksp of M(OH)2...

A solution is 5 mM in each of the following ions: number ion Ksp of M(OH)2 1 Mg2+ 1.8e-11 2 Cd2+ 2.5e-14 3 Co2+ 1.6e-15 4 Zn2+ 4.4e-17 5 Cu2+ 2.2e-20 Indicate which of the metal ions would precipitate (or start to precipitate) at each of the following pH values. Indicate your answer with the number of the ion. Use 0 to indicate no precipitate. If more than one precipitate is expected, list the numbers in increasing order and separate...

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In basic solution hydrogen peroxide oxidizes chromite ions, Cr(OH)4- to chromate ions, CrO4^2-. The hydrogen peroxide...

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Balance the following basic solution H20+CrO4+Cn-->OCN+Cr(OH)3+h20

10 OH- + 2 Cr(OH)3 +3 Br2 --> 2 CrO4 2- +8 H2O + 6 Br-...

1)What element is being oxidized in the following redox reaction? Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) +...

1)What element is being oxidized in the following redox reaction? Cr(OH)4^-(aq) +ClO^- (aq)----> CrO4^2- (aq) +...

1. Determine the molar solubility of Cr3+& OH- ions in the compound Cr(OH)3 at 25oC at:...

A dilute solution of hydrogen peroxide is sold in drugstores as a mild antiseptic. A typical...

For each of the transition metal complex ions (a) [Ti(NH3)6]2+ (b) [Cr(H2O)4(OH)2]1- (c) trans–[Pt(CN)2(en)2]2+ (i) Draw...

Part A Calculate the molar concentration of OH− ions in a 8.1×10−2 M solution of ethylamine...

Part A Calculate the molar concentration of OH− ions in a 7.4×10−2 M solution of ethylamine...

A solution is 5 mM in each of the following ions: number ion Ksp of M(OH)2...