A Fe2 + solution is titrated with a K,Cr, O, solution according to the unbalanced reaction below.Cr,0; (aq) + Fe? + (aq) ·Cr * (aq) + Fe +(aq)Select net ionic equation that shows the above reaction balanced in acidic solution.Cr, 0; (aq) + 6 Fe² + (aq) + 14 H* (aq)* (aq)→ 2 Cr+ (aq) + 6 Fe³+(aq) + 7 H,0(1)2 Cr, 0; (aq) + Fe²+Cr, 0; (aq) + Fe? * (aq) + 14 H*(aq) -O Cr,0; (aq) + 6 Fe² + (aq) + 7 H,O(1)→ 4 Cr³ + (aq) + Fe³+(aq) + 7O,(g)2 Cr³ + (aq) + Fe³+(aq) + 7 H,O(1)> 2 Cr³+ (aq) + 6 Fe³ +(aq) + 14 OH¯(aq)22.50 mL of the Fe?+ solution required 12.50 mL of 0.255 M K, Cr, O, to reach the end point.Calculate the concentration of the Fe2 + solution.[Fe? +] =M* TOOLSx10

Answered: Image /qna-images/answer/5d679952-03e1-4d1e-b57c-69a239a8210f.jpg

A Fe2 + solution is titrated with a K, Cr, O, solution according to the unbalanced reaction below. Cr, 0; (aq) + Fe²* (aq) Cr +(aq) + Fe³ +(aq) Select net ionic equation that shows the above reaction balanced in acidic solution. Cr,0; (aq) + 6 Fe? + (aq) + 14 H* (aq) 2 Cr + (aq) + 6 Fe³* (aq) + 7 H,O(1) 2 Cr,0; (aq) + Fe²+ (aq) 4 Cr + (aq) + Fe³ +(aq) + 7 O,(g) Cr, 0; (aq) + Fe² + (aq) + 14 H*(aq) → 2 Cr3 + (aq) + Fe³+ 3+(aq) + 7 H,O(1) O Cr, 0; (aq) + 6 Fe² * (aq) + 7 H, O(1) → 2 Cr³+ (aq) + 6 Fe³ + (aq) + 14 OH¯(aq)

A Fe2 + solution is titrated with a K, Cr, O, solution according to the unbalanced reaction below. Cr, 0; (aq) + Fe²* (aq) Cr +(aq) + Fe³ +(aq) Select net ionic equation that shows the above reaction balanced in acidic solution. Cr,0; (aq) + 6 Fe? + (aq) + 14 H* (aq) 2 Cr + (aq) + 6 Fe³* (aq) + 7 H,O(1) 2 Cr,0; (aq) + Fe²+ (aq) 4 Cr + (aq) + Fe³ +(aq) + 7 O,(g) Cr, 0; (aq) + Fe² + (aq) + 14 H(aq) → 2 Cr3 + (aq) + Fe³+ 3+(aq) + 7 H,O(1) O Cr, 0; (aq) + 6 Fe² (aq) + 7 H, O(1) → 2 Cr³+ (aq) + 6 Fe³ + (aq) + 14 OH¯(aq)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 37QAP: An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is...

See similar textbooks

Similar questions

An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
A student is given 0.930 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.615 M NaOH. The equivalence point is reached when 33.6 mL are added. What is the unknown acid?
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
The concentration of a hydrogen peroxide solution is determined by titrating it with a 0.1878 M solution of Ce. The balanced net ionic equation for the reaction is shown below. 4+ 2 Ce (aq) + H202(aq)+2 H20(1)–2 Ce"(aq) + 02(g)+2 H30 (aq) In one experiment, 16.94 mL of the 0.1878 M Ce solution is required to react completely with 40.00 mL of the hydrogen peroxide solution. Calculate the concentration of the hydrogen peroxide solution. 4+
Ag+ (aq) + NH3(aq) Ag(NH3)*(aq) Ag(NH3)* (aq) + NH3(aq) → Ag(NH3)2* (aq) Equal volumes of 0.1 MAgNO3(aq) and 2.0 MNH3(aq) are mixed and the reactions represented above occur. Which Ag species will have the highest concentration in the equilibrium system shown below, and why? Ag+ (aq) + 2 NH3(aq) ⇒ Ag(NH3)2* (aq) Keqs =? (A) (B) C (D) Ag+ (aq), because Keq3 = 4 Ag+ (aq), because Keq1 < Keq2 Ag(NH3)2(aq), because Keq3 = 1.7 x 107 Keq, = 2.1 × 10³ = 8.2 x 10³ Keq2 Ag(NH3)2(aq), because Keq1 < Keq2
Complete the following reaction and balance it. Fe(OH)3(aq) + HCl(aq) → a) FeCl3(aq)+ 3 H2O(l) b) FeCl(aq) + H2O(l) c) Fe(aq) + HOCl(aq) d) FeCl(aq) + 3 OH–(aq) e) H2O(l) + FeCl2(aq)
A reaction is initiated by preparing an aqueous solution with 0.421 M silver ion, Ag+ (aq), and 0.778 M ammonia, NH3 (aq). The following reaction proceeds until equilibrium is achieved. Ag+ (aq) + 2 NH3 (aq) = [Ag(NH3)2]+(aq) At equilibrium, it is determined that the solution contains 0.292 M [Ag(NH3)2]+ (aq). The value of K is Write your answer to 3 sig figs (ie. 1.23E1)
If 17.0 g of NaOH is added to 0.600 L of 1.00 M Mn(NO 3 ) 21 , how many grams of Mn(OH) 2 will be formed in the following precipitation reaction ? 2NaOH(aq)+Mn(NO 3 ) 2 (aq) Mn(OH) 2; (s) + 2NaN * O_{3} * (aq)
You prepare a standard NaOH solution for the laboratory, using potassium hydrogen phthalate (KHC,H,O,, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC̟H,O, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 19.14 mL of the NaOH to titrate (react exactly with) the ascorbic acid found in one 500.0 mg tablet. What is the percent vitamin C by mass in the tablet?
The concentration of a H3AsO3 solution is determined by titrating it with a 0.1956 M solution of Ce4+. The balanced net ionic equation for the reaction is shown below. 2 Ce4+(aq) + H3AsO3(aq)+5 H2O(l)2 Ce3+(aq) + H3AsO4(aq)+2 H3O+(aq) In one experiment, 21.72 mL of the 0.1956 M Ce4+ solution is required to react completely with 30.00 mL of the H3AsO3 solution. Calculate the concentration of the H3AsO3 solution.
A buffer solution made from hydrocyanic acid and potassium cyanide titrated with hydrochloric acid. What is the net ionic equation for the reaction ? a) H 3 O^ + (aq)+HCN(aq)=>H 2 O(l)+H 2 CN(aq) b) HCl(aq)+CN-(aq)=>HCN(aq)+C(-(aq); c) HCl(aq)+OH^ - (aq)=>H 2 O(l)+Cl^ - (aq) d)No answer text provided e) . H 3 O^ + (aq)+CN^ - (aq)=>HCN(aq)+H 2 O(l)
Which of the following is a balanced molecular equation describing the titration of a weak acid with a strong base? O HF(aq) + NACH(ag) = H20(1) + NaF(aq) O HI(aq) + NH4OH(aq) = H2O(1) + NH4|(aq) O HF(aq) + OH (aq) = H2O() + F'(aqg) O HI(aq) + NaOH(aq) = H2O() + Nal(aq) O H;O'(aq) + NH,OH(aq) = H2O(1) + NH, (ag) O H;O"(aq) + OH (ag) = 2 H2O()