In Part A a stock solution will be prepared by mixing solutions containing the colorless thiocyanate ion. In preparing the stock solution, we will make the iron (III) ion conce the thiocyanate ion concentration. This causes the equilibrium above to shift far to the essentially all of the SCN into FeSCN²+. We will then assume that the equilibrium equals the original concentration of the SCN-. 30 mL of a stock FeSCN2+ solution will be prepared by mixing the following in a sn measure volumes: 3.0 mL of 0.00200 M KSCN solution 10.0 mL of 0.200 M Fe(NO3)3 solution 17.0 mL of 0.5 M HNO3 solution 1. What is the concentration of the FeSCN²+ in the stock solution? Concentration of FeSCN2+ in Stock Solution (M) Stock Solution Stock

Q: Which of the following react with ammonia to form a black precipitate?     AgCl     PbCl2…

A: Here the following is Hg2Cl2 which will give black precipitate with ammonia.

Q: What is the molarity of the FAS titrant solution given the following: Vol of K2Cr2O7: 100 mL Vol of…

A: Vol of K2Cr2O7: 100 mLVol of FAS titrant: 15.2 mLMolar mass of FAS: 284.1 g/molMass of FAS: 24.135 g

Q: What is the concentration of Cl in the solution 0.25 M CuCl2

A: Since in each molecule of CuCl2 we have 2 Cl Hence the moles of Cl = moles of CuCl2 X 2

Q: You analyze the Free SO2 level for the red wine using the Aeration Oxidation or Aspiration Method.…

A: The question is based on the titration.  We are titrating SO2 with a strong base. We need to…

Q: What is the pH of a buffer solution that contains 0.30 M H2PO4–1  and 0.60 M HPO4–2  ? Given: pKa…

A:

Q: pka of 4.9 what is the weak acid and conjugate base pH of buffer solution is 5.90

A: The pKa value of 4.9 indicates the acidity of a weak acid. To determine the weak acid and its…

Q: Iodine can be in the form of I3 and I-2.  Why are these forms used in the titration of vitamin C?

A: Please find your solution below : Vitamin C also known as ascorbic acid is a water soluble vitamin.…

Q: Which of the following do not dissolve in hot water?      AgCl     PbCl2     Hg2Cl2     both…

A: The ability of a substance to get dissolve in particular amount of solvent is termed as solubility.

Q: Adding OH–(aq) to Co(H2O)62+(aq) changes the solution color from ___ to ___. Co(H2O)62+(aq) +…

A: When a solution of Co(H2O)6^2+(aq) reacts with NaOH(aq), the hydroxide ions (OH-) from the NaOH…

Q: A buffer solution made from HNO, and NaNO2 has a pH of 3.01. If p Ka for HNO2 is 335 , what is the…

A: Given buffer is  HNO2 + NaNO2 pH of buffer = 3.01 pKa of HNO2 = 3.35 [NO2-]/[HNO2] in buffer = ?

Q: 2) Acetic acid has a Ka of 1.80x10-5. What is the pH of a buffer solution made from 0.150 M HC₂H30₂…

A:

Q: What is the equivalence point pH of a 0.1M solution of phenylalanine that is fully titrated with…

A:

Q: Differentiate between diphenylamine redox indicator and the following redox indicators  a) Starch-…

A: Interpretation: To differentiate between diphenylamine and starch-iodine indicators. Also, to…

Q: Which of the below statements is false? O Phosphate is an important intracellular buffer. Le…

A: A buffer solution is a solution that has the ability to resist changes in pH when small amounts of…

Q: Which one is not required for the titration of ascorbic acid with I2 ? indicator mortar and pestle…

A: Titration of ascorbic acid with iodine requirements. 1. indicator :  in this titration we use strach…

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

A:

Q: addition of a small amount of HNO3 to a solution containing CN- ions and HCN?

A: We will explain change in solution upon addition of HNO3

Q: Questions 6 through 9 refer to the following situation: A solid sample containing some Fe2+ ion…

A:

Q: MW (g/mol)-137.99 Buffer 1: 1 M NaH₂PO V 100 mL m(g) Buffer 2: 1 M Na2HPO4 V-100 mL MW (g/mol) 142…

A: The objective of the question is to calculate the-Mass of Monosodium phosphateMass of Disodium…

Q: A buffer with a pH of 11.2 contains CH3NH2 and CH3NH3C1 in water. You may want to reference (Page)…

A: Given: pH of buffer = 11.2 pKb of CH3NH2 = 3.36 And the buffer solution is of CH3NH2 and CH3NH3Cl.

Q: Calculate the K for this reaction: 2Fe*3 + Pd 22FE*2(ag) + Pd*2 (aq) (aq) (aq) + Pd+2

A: For a reaction at equilibrium- K = [Product][Reactant]

Q: The Ksp of PbCl2 is 6.65 10-10 M. Calculate the solubility of each ion in a saturated solution: M…

A:

Q: 6) The Ksp of Cd(OH)2 is 1.2 x 10-14. What is the pH of a saturated solution of Cd(OH)2? 9.5 9.7 9.2…

A: The Ksp of Cd(OH)2 = 1.2 × 10-14  Ksp of a substance shows how much a solid dissociates into ions in…

Q: 0 mL of a H₂SO4 solution with an unknown concentration was titrated to a phenolphthalein endpoint…

A: Molarity is defined as number of mole of solute divide by volume of solution in liter

Q: ow to write a balanced chemical equation for the dissolution of each of the following compounds :…

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Q: Hypothetical [Zn *2] [Cu *2] e transferred Ecell # 1 0.1 M 0.1 M 0.1 M # 2 1 x 10 -3 M # 3 0.1 M 1 x…

A: We have to fill the given table

Q: What is the molar solubility of Ag2SO4 in the presence of 1.52 M aqueous solution of AgNO3?…

A: Given : [AgNO3] = 1.52M  Ksp = 1.5 x 10-5

Q: What is the solubility of PbCO3(s) in 0.5M Na2CO3?

A: The solubility of a salt decreases in the solution due to common ion effect. The solubility of a…

Q: Another buffer found in blood is based on the equilibrium between dihydrogen phosphate and…

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Q: The pH of normal urine is 6.30, and the total phosphate concentration ([PO43−] + [HPO4 2−] + [H2 PO4…

A:

Q: What color will you solution turn today when FeCl3 is added to hydrolyzed ASA?

A: A question based on color change, which is to be accomplished.

Q: In a titration 36.7 mL of HBr solution is put In a flask with a few drops of phenolphthalein and…

A: Given: The volume of HBr is 36.7 mL. The volume of Sr(OH)2 is 51.4 mL. The molarity of Sr(OH)2 is…

Q: Fe3+(aq)+ SCN–(aq) ⇄FeSCN2+(aq) What two precipitaes will form when silver nitrate is added to it?

A:

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.