(iii) The pH range of phenolphthalein is 8.2 -10. Give an acid and an alkali for which phenolphthalein is suitable as an indicator during tit ration

Q: Enumerate at least 3 specific medical applications of complexometric titration and discuss each.

A: The ligand is a species that contains an unshared electron pair or a negative charge. This electron…

Q: n determination of mixed alkali, does adding H2O to the analyte can afect the process of titration?

A: Titration is an analytical method to determine the concentration of an analyte.

Q: A solution containing a mixture of metal cations was treated with dilute HCl and a precipitate…

A:

Q: Write two features of Erichrome black- T which makes it a suitable indicator in complexometric…

A: Two features of Eriochrome black- T has to be written The medium it undergoes complex formation has…

Q: Write a molecular, full ion and effective ion equation of the reaction involving aqueous solutions…

A: We need to write balanced molecular, ionic and net ionic equation for Potassium carbonate in aqueous…

Q: A solution was prepared by adding 4.95 g sodium acetate (NaC2H3O2) to 250.0 mL of 0.150 M. acetic…

A:

Q: Ammonium acetate (CH3COONH4) is also a salt of weak acid (CH3COOH) and weak base (NH4OH). The Ka and…

A: Option b is correct. This is because on hydrolysis ammonium acetate produces ammonium hydroxide and…

Q: Show by calculation how could you prepare 250 ml of 0.1N Na,CO; from the solid primar standard of…

A:

Q: Give six differences between tituration and levigation

A: Six differences between trituration and levigation- 1) Triturate is the continual rubbing of a solid…

Q: 665 mL of 0.875 M aqueous aniline solution CC2H5 are boiled gently to reduce the volume to 401 m L…

A: Answer:- This question is answered by using the simple concept of dissociation of a weak base and…

Q: Which of the following statements is TRUE regarding an ideal precipitating reagent? Of unknown…

A: The precipitate is a water insoluble solid product in a chemical reaction.

Q: The dissociation vapor pressure of a salt A2B(s) ⇌ A2(g) + B(g) at 367°C is 208 kPa but at 477°C it…

A:

Q: Determination of sodium carbonate by acidimetric titration involves: Direct titration by acid…

A: Process of determination of sodium carbonate by acidimetric titration: CO32- + H+ → HCO3- HCO3- + H+…

Q: If the test tube used in the determination of the ΔHrxn for nitric acid (neutralization with NaOH)…

A: Given: The test tube used in the determination of the ΔHrxn for nitric acid (neutralization with…

Q: In complexometric titration ‘the reaction with analyte should be rapid and complete’ give reason…

A: Complexometric titrations are those titrations in which chelates or soluble complexes, usually…

Q: Consider the following list of indicators. Indicator pK, Methyl red Chlorophenol red Ethyl orange…

A: When choosing the indicator for the acid base titration choose an indicator whose pH range falls…

Q: 2. The solubility product for the dissolution of calcium carbonate in water (ar pH-7, 20 C) is K4.8…

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

Q: A 250 cm3 volumetric flask contains exactly 200,0 cm3 of a 0,025 mol.dm3 sulphuric acid solution.…

A: GIVEN Volume of sulphuric acid (H2SO4) =200.0 cm3 ( 1 Litre = 1000 cm3) = 0.200 L  Concentration of…

Q: Jon 24 The colour exhibited by Bromo cresol indicator in acidic and basic medium is

A: Indicator have different colour in acidic and basic medium

Q: A solution containing Mg2+ was buffered to pH 9.99 and titrated with EDTA. Eriochrome black T, with…

A: Eriochrome black T is a diprotic acid, represented as H2E.

Q: Explain the difference between 'stoichiometric (equivalence) point' and 'end point' in the context…

A: Titration is used Redox reaction and Acid-Base reaction. There are 2 important stages of the…

Q: 5. Magnesium hydroxide (Mg(OH)2) has a pKsp value of 11.25. In a solution at pH 10, what is the…

A: Given,  pKsp of Mg(OH)2 = 11.25  pH = 10  What is the maximum Mg2+ concentration in µmol/L = ?  What…

Q: What happens when too much NaSCN is prepared in solution of mixtures of standard solutions of…

A: Fe3+ (from Fe(NO3)3 and SCN- ions (from NaSCN) react to form a complex.

Q: Write the relevant chemical reaction and mass-balance expression for 0.1 M NaCl and 0.1 M NaH2PO4.

A: Sodium Dihydrogen Phosphate + Sodium Chloride = Nahpoite + Hydrogen Chloride 0.1 M of aqueous Sodium…

Q: A 110.00 mL solution of 0.00195 M A3B2 is added to a 160.00 mL solution of 0.00155 M C3D4. What is…

A: Given: Volume of A3B2 = 110.0 mL concentration of A3B2 = 0.00195 M Volume of C3D4 = 160.0 mL…

Q: Given the chemical equation for the anthocyanin extract of red cabbage as an indicator. HIn + H20 S…

A: Indicator is a compound that indicates the acidic and basic character of the solution. These are…

Q: Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.393 M HCl.…

A:

Q: A 250 cm volumetric flask contains exactly 200,0 cm3 of a 0,025 mol.dm sulphuric acid solution.…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: Calculate the masses of (a) Ca(NO3)2 and, separately, (b) NaCI to add to a 0.150 mol kg-1 solution…

A:

Q: A solution containing Mg2+ was buffered to pH 9.97 and titrated with EDTA. Eriochrome black T, with…

A: Predominant form of Eriochrome black T in the solution at pH 9.97 = HIn​​​​2- color of the solution…

Q: 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH values are…

A: Given: Volume of weak acid = 50 cm3 Concentration of weak acid = 0.05 M Concentration of NaOH = 0.1…

Q: Condition of permanganatometric titration of sodium oxalate includes: pH = 1 and heating of analyte…

A: Permanganatometric titration is a technique used in chemical quantitative analysis. It is a type of…

Q: Show that the equivalence point N1V1=N2V2 where V1mL of analyte of strength N1 reacts with V2L of o…

A: At the equivalence point, equivalent quantities  of titrant and analyte have chemically reacted with…

Q: 3. This produces the observable physical change upon reaching the enc point of a titration indicator…

A: A point marking the completion of a reaction called end point

Q: Different masses of aspirin (e.g 10mg, 100mg, 1000mg) used in an acid base titration. what could be…

A: Since we are not providing the handwritten notes and according to our guidelines, we are providing…

Q: The dissociation vapor pressure of a salt A2B(s) A2ig) + B(g) at 367°C is 208 kPa but at 477°C it…

A:

Q: What is the mole ratio of sodium acetate to acetic acid (Ka=1.8 x 10^-5) in a buffer with the pH of…

A: Given- Ka=1.8×10-5 pH=4.00

Q: Calculate the volume in liters of 0.545 M KOH necessary to titrate 0.0113 moles of hydrochloric…

A:

Q: Change of indicators colour is related to the change of the .A Structure .B Intramolecular…

A:

Q: The indicator phenolphthalein may be regarded as a weak monobasic acid. Explain briefly why the…

A: Monobasic acid: The acid which gives one H+ ion in the solution. While the indicator is a substance…

Q: 1,2 g of marble (calcium carbonate) containing sand as the only impurity is dissolved in 50,0 cm of…

A: Mass of marble = 1.2 g  Molarity of HCl = 1.0 mol dm-3  Volume of HCl = 50.0 cm3 = 50.0 * 10-3 dm3…

Q: Finely ground mineral (0.9315 g) was dissolved in 25 mL of boiling 4 M HCl and diluted with 175 mL…

A: To provide an explanation for the following: a)The unknown solution heated to boiling and the…

Q: A weak acid (HA) with a pKa of 4.0 has a distribution constant of 5.2 between an organic and aqueous…

A: The fraction of HA acid in the organic phase at pH 2 and 6 is calculated:

Q: Sn(OH), 48 = 5.45 x 10-27 CUCN K,= S =3.47 x 10- MgF; = 45- 5.16 x 10-1 NICO, K„ = s² = 1.42 × 10-7…

A: Given Substance        KspSn(OH)2         Ksp = 4S3 = 5.45×10-27CuCN             Ksp  = S2 = 3.47…

Q: The acid-base indicator "Thymol Blue" has two transition ranges as listed below (with the…

A: The pKa values of the forms of thymol blue can be calculated as:   pKa=-log Ka

UV Visible Spectroscopy

Spectroscopy refers to the absorption or emission of light or other radiations by matter. When a substance or chemical absorbs light or radiation, they reach an excited state followed by de-excitation or emission of the light or radiation forming distinct spectra. UV-visible spectroscopy or  ultraviolet-visible refers to the absorption and emission in the ultraviolet and visible regions of the electromagnetic spectrum.