-14°C 5) Design: The iron(II) solution is titrated to iron (III) with a standard cerium (IV) ion solution which is reduced to cerium (III). The indicator shows, as the endpoint, a sharp colour change from red to pale blue. Evidence: Titration of 25.0 mL of Fe²+ (aq) with 0.125 mol/L Ce+ (aq). Trial Final burette reading (mL) Initial burette reading (mL) Volume of Ce4+ = 1 15.7 0.6 2 30.7 15.7 3 45.6 30.7 4 40.2 25.3 (Answer: 14.975) Problem: What is the amount concentration of iron (II) ionis in a solution obtained in an iron ore analysis? (Answer: 7.49 x 10¹² M) ENG £ 1 0 + O E 5:42 PM

-14°C 5) Design: The iron(II) solution is titrated to iron (III) with a standard cerium (IV) ion solution which is reduced to cerium (III). The indicator shows, as the endpoint, a sharp colour change from red to pale blue. Evidence: Titration of 25.0 mL of Fe²+ (aq) with 0.125 mol/L Ce+ (aq). Trial Final burette reading (mL) Initial burette reading (mL) Volume of Ce4+ = 1 15.7 0.6 2 30.7 15.7 3 45.6 30.7 4 40.2 25.3 (Answer: 14.975) Problem: What is the amount concentration of iron (II) ionis in a solution obtained in an iron ore analysis? (Answer: 7.49 x 10¹² M) ENG £ 1 0 + O E 5:42 PM

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

Related questions

Q: To study the effects of a weakly acidic medium on the rate of corrosion of a metal alloy, a student…

Q: During a titration, the pH of an analyte solution containing HA(aq) is 5.56 and the ratio of (A…

A: Given pH of solution is 5.56 ratio of [A-]/[HA] is .842 we have to determine Ka

Q: For the following reaction, determine the equilibrium concentrations of all species present if the…

A: In a reversible reaction, the reaction takes place in both forward and reverse reaction. However, it…

Q: A base is added to a 0.050 M solution of MnClz, raising the pH gradually. Calculate the pH of the…

A: Answer: Manganese will precipitate in form Mn(OH)2 when its ionic product will become greater than…

Q: Part A - Reactions of Carbon Dioxide Gas Part B - Carbonate Equilibrium 1. Place a small lump of dry…

A: Reaction of gaseous carbon dioxide with water is a chemical reaction which leads to the four…

Q: Calculate the molar concentration of zinc ions in a solution containing 0.200 M [Zn(NH3)4]2+ (Kf =…

Q: a. A 0.3108-g sample of primary-standard-grade Na2 C2O4 was dissolved in H2SO4 and titrated with…

Q: A 1.963-g sample of an alloy is dissolved in HNO3 and diluted to volume in a 100-mL volumetric…

A: Answer: This question is based on stoichiometric calculation where moles of SCN- needs to be…

Q: Calculate AG° and K at 25°C for the reactions. a. 7H20 + 2 Cr3++3Cl, — Сr20,2- + 6 CI + 14H* €— 0.03…

Q: help please answer in text form with proper workings and explanation for each and every part and…

A: Step 1: Identify the given data:Volume of KMnO4 solution used, V = 37.4 mL = 0.0374 L (since 1 mL =…

Q: Write a balanced net ionic equation to show why the solubility of PbCO3(s) increases in the presence…

A: We have to write a balanced net ionic equation to show why the Solubility of Pb(CO3) increases in…

Q: Calculate the concentration of Fe2O3 in a mineral sample after solubilization of 0.4891g and…

A: from the reaction, 6 mole Fe2+ react with 1 mole K2Cr2O7. mole = mass molar mass

Q: The permanganate ion (MnO4- ) is often used in redox titrations. The strongly colored (violet) the…

A: The balanced equation for the reaction between permanganate and oxalate in an acidic solution is:…

Q: A buffer solution consists of 0.15M C6H5COOH and 0.50M C6H5COONA. The pH of the solution is 5.0. The…

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: In a redox titration, 20ml of completely oxidised by 12.5ml of 0.02mol/L acidified Fe(II)SO4 was

A: 1) In acidic medium K2Cr2O7 is OA (reduced) and converts into Cr+3 ions FeSO4 is RA (oxidized)…

Q: 1. What is the equilibrium constant for the following reaction at 25 "C? Ni (s) + Cd²+ (aq) Ni²+…

A: Since you have asked multiple questions, we will answer the first question for you. If you want any…

Q: To analyze the amount of iron (Fe; Mw = 55.85 g/mol) contained in an ore sample, the sample was…

A: Given in the question, Volume of EDTA = 25 ml Molarity of EDTA = 0.2922 M Total moles of EDTA =…

Q: A 3.25 g sample of an iron-containing mineral was dissolved in an acid medium and calibrated to 500…

A: This problem is based on analytical chemistry. Here we shall find the amount of Fe3+ in the sample.…

Q: A titration of 50.0 mL of 0.10 M Sn2+ with 0.2 M Fe3+ in 1 M HCl to give Fe2+ and Sn4+ using Pt and…

A: To Calculate Cell potential a) 25 mL Fe3+ b) 50 mL Fe3+ b) 70 mL Fe3+

Q: A 50.00 mL sample of ascorbic acid (H2C6H606) is titrated with 0.1200 M KOH. The second…

A: Here is your answer...... This curve is just for illustration of how titration takes place of the…

Q: g+ + Sn2+ oxide reduction equilibria

Q: Write the balanced dissociation equation for nickel(II) iodide in aqueous solution. If it does not…

A: In the aqueous solution, Nickel(II) iodide dissociates into nickel (Ni2+) and Iodide (I-) ions.

Q: Calculate AG° and K at 25°C for the reactions. 7H2O + 2 Cr³+ + 3 Cl2 = Cr2 0,² + 6 Cl¯ + 14H+ = 0.03…

Q: 4. A chromate in a water solution exists in equilibrium with the corresponding dichrarhate ion…

A: Le Chatelier's principle :- It states that, when stress is applied to a system at equilibrium by…

Q: Knowing that the concentration of silver ions, Agt, in a solution of silver chromate, Ag₂ CrO4, is…

A: [Ag+] = 2s = 1.510-4 M = s = ?

Q: Fe3+ + OH- FEOH²+ + OH- Fe(OH)2* + OH- Fe(OH)3(ferihydrite) + OH- Fe(OH)4

A: pH is the negative logarithm of the hydrogen ion concentration. It is a measure of acidity or…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

100%

A W
5 Hour Timer - YouTub X
-14°C
Cloudy
Copy of Copy of Lesso X
Redox Titration Practic X
https://classroom.google.com/c/NTQ1NDc3NTQ2OTc1/m/NTU4NjA2OTk2MjYz/details
OVO *
Electrochemistry Unit X MInbox - hadia.ali@prs X
1
15.7
0.6
2
30.7
5) Design: The iron(II) solution is titrated to iron (III) with a standard cerium (IV) ion solution
which is reduced to cerium (III). The indicator shows, as the endpoint, a sharp colour change
from red to pale blue.
Evidence: Titration of 25.0 mL of Fe²+ (aq) with 0.125 mol/L Ce+ (aq).
15.7
Tum Kon Piya FULL OS X
Trial
Final burette
reading (mL)
Initial burette
reading (mL)
Volume of Ce** =
(Answer: 14.975)
Problem: What is the amount concentration of iron (II) ionis in a solution obtained in an iron ore
analysis?
(Answer: 7.49 x 10.² M)
3
45.6
W
30.7
b Success Confirmation X
+
4
40.2
25.3
用
ENG
US
X
⠀
Other favorites
♂
·
14
-
a
+
→→
5:42 PM
2022-11-06

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Part 1

VIEW

Part 2

VIEW

Step by step

Solved in 3 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Write the balance equation of aqueous Pb(ClO3)2 with NaI. Include phases.
Consider the series of equilibrium reactions below. In which way would you expect the reaction to “tend” at high pH? What about low pH? Why? Circle the Fe(III) species that you’d expect to be least soluble. Fe3+ + OH- <---> FeOH2+ + OH- <---> Fe(OH)2+ + OH- <---->Fe(OH)3(ferrihydrite) + OH- <--->Fe(OH)4-
The calcium content of a milk sample was to be determined by EDTA titration. A sample weighing 0.206 g was mixed with an aqueous buffer at pH 11.5. A few drops of EBT indicator were added and the solution required 24.25 mL of 1.538 x 10-2 M EDTA to reach the endpoint. Calculate the weight percent of calcium (FW =40) in the milk.
Hh.88.
Please don't provide handwritten solution ....
16,17, & 18
calculationS H= 1 Fe = 55.8; S = 32; O= 16; 10 10g of an impure iron(11) salt were dissolved in water and made un to 200 cm of solution. 20cm of this solution, acidified with dilute sulphuric acid, required 25 cm3 of 0.04 M KMNO4(aq) before a faint pink colour appeared. (a) Write a balanced ionic equation (or half-equations) for the reaction of acidified manganate(vII) (permanganate) ions with iron(11) ions. (b) How many moles of iron(1) ions react with one mole of MnO4 ions? (c) How many moles of Fe2 react with 25 cm' of 0.04 M KMNO4(aq)? (d) How many grams of Fe2 are there in the 200 cm' of original solution? (Fe 56) (e) Calculate the % by mass of iron in the impure iron(11) salt.
22. The following problem pertains to AgBr(s), Ksp = 5.0 x 10-13, Hg,Br2(s), Ksp = 1.3 x 10-22, and [Ag(S2O3)2]³-, Kf= 2.9 x 1013. A. (i) Include state symbols. Write the reaction for dissolving (dissolution) of AgBr(s) into its aqueous ions. Write the reaction for dissolving (dissolution) of Hg2Br2(s) into its aqueous ions. (ii) Include state symbols. Hint: recall mercury forms a Hg22* ion. (iii) Write the formation constant expression (Kr) for the complex ion [Ag(S2O3)2]3-
Write a balanced net ionic equation to show why the solubility of AgCN(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Be sure to specify states such as (aq) or (s). K= + + +
Calculate AG° and K at 25°C for the reactions. 7H2O + 2 Cr+ + 3 Cl2 = Cr2 07²- + 6 Cl¯ + 14H = 0.03 V cel a. AG° = kJ K = Cu²+ (aq) + Ba(s) = Ba2+ (aq) + Cu(s) e° = 3.24 V b. AG° : kJ K = Cl2 (g) + 2 Br (aq) = Br2 (g) + 2 Cl¯ (ag) e° = 0.27 V C. AG° = kJ K = 3H2 O(1) + 5 IO4 (ag) + 2 Mn²+ (aq) = 5 IO3 (aq) + 2 MnO4¯(ag) + 6H† (ag) d. 0.09 V ´cell AG° = kJ K =