Discussion:- 1- Write the chemical structure of (M-O )Indicator ? qverag = 2-Write the properties of the standard substances ? 3- Solution containing (3.3gm) of (Nazco3.10H20)in (15ml) find the Normality and Molarity solution?
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- The following statements are true, EXCEPT: (a) The purpose of a titration is to determine the concentration of the analyte solution. (b) The role of an indicator is to help the titrant and analyte react successfully. (c) The buret is used for delivering increments of the titrant solution. (d) The purpose of washing the buret with water is to help see the color of indicator better. Choices: I and III II and IV I and II III and IV200 ml of a water sample required 20 ml 0.025M Hydrochloric acid using methyl orange as indicator but did not give any coloration with phenolphthalein. What type of alkalinity is present? Express in mg/L5. How would you prepare a liter of “carbonate buffer” at a pH of 10.10? H2CO3 ↔ H+ + HCO3- Ka = 4.2 x 10-7 HCO3-↔ H+ + CO3-2 Ka = 4.8 x 10-11 a 1stbuffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution b 2ndbuffer is preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution c 1stbuffer preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution d 2nd buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution
- A 25.00-mL sample of vinegar is diluted with deionized to 100.0 mL. Then a 10.00-mL aliquot (portion) of the dilute vinegar solutionis titrated with 0.1055MNaOHsolution using phenolphthalein as theindicator. (a) If 19.60mL of the base solution is required to reach the end-point, calculate the molar concentration of acetic in dilute vinegar solution. (b) What is the molar concentration of acetic acid in the original (undiluted) vinegar? At the end-point, the volume of NaOH consumed was found to be 32.00 mL. The acid-base reaction occurs as follows: HC2H3O2(aq) + NaOH(aq) --> H2O(l) + NaC2H3O2(aq)A 250.0-mg sample of an organic weak acid is dissolved in an appropriate solvent and titrated with 0.0556 M NaOH, requiring 32.58 mL to reach the end point. Determine the compound’s equivalent weight.Two aliquot of a water sample is titrated against a strong acid using phenolphthalein and bromocresol green indicator. The volume for the phenolphthalein endpoint and for the bromocresol green endpoint are equal, what is/are the probable source of alkalinity? a) Hydroxide b) Bicarbonate c) Carbonate d) Both Hydroxide and Carbonate In addition, what would be the probable source of alkalinity if the volume for bromocresol green endpoint is 13.5mL and there was no phenolphthalein endpoint?
- Please answer the following questions: 1. The phenolphthalein HIn indicator forms this equilibrium in an aqueous solution: HIn + H2O ↔ H3O+ + In-. During the course of titrating the acid content of samples, the concentration of H3O+ _________ , shifting the equilibrium towards _________ , until end-point is reached. a.decreases, In- b.increases, HIn c.decreases, HIn d.increases, In- 2. In the distillation of 70% isopropyl alcohol, which of the following is TRUE? a.The temperature was maintained at the boiling point of water. b.The 20 mL sample was distilled to dryness. c.The thermometer was allowed to touch the solution in the distilling flask. d.None of the above 3. Some Chem 16.1 students performed the ideal gas experiment on a hot summer day. Upon doing their experiment, the recorded temperature was 302 K.The pressure of the trapped air was found to be 763.0 torr. Given the following vapor pressures of water at certain temperatures, calculate the pressure of…An acid-base indicator is usually a weak acid with a characteristic color in the protonated and deprotonated forms. Because bromocresol green is an acid, it is convenient to represent its rather complex formula as HBCG. HBCG ionizes in water according to the following equation: HBCG + H2O ⇌ BCG- + H3O+ (yellow) (blue) a. Write the Ka expression for bromocresol green based on the equation above. b. When [BCG-] = [HBCG], then show that the expression simplifies to Ka = [H3O+]. If you know the pH of the solution, then the [H3O+] and Ka can be determined. c. What would be the color of the solution if there were equal concentrations of HBCG and BCG-?A sufficient quantity of each of the following aqueous solutions has been made available to you: (i) 0.2M NaH2PO4; (ii) 0.1M Na2HPO4 (a) How many ml of each of these two solutions would you require to mix together in order to prepare one litre of a 0.01M phosphate buffer pH 7.2? [For H3PO4: pKa1 = 2.15; pKa2 = 6.82; pKa3 = 12.38]. (Ans. = 14.7 ml 0.2M NaH2PO4; and 70.6 ml Na2HPO4). (b) Having calculated these volumes (of 0.2 M NaH2PO4 and 0.1M Na2HPO4) required, what further steps would you take to prepare the 0.01M phosphate buffer solution of pH 7.2?
- The acid-base indicator ethyl orange turns from red to yel-low over the pH range 3.4 to 4.8. Estimate Kₐ for ethyl orange.Calculate the volume in liters of 0.545 M KOH necessary to titrate 0.0113 moles of hydrochloric acid, HCl, to a phenolphthalein end-point. Report the answer with three significant figures.A 3.00 mL aliquot of 0.001 M NaSCN is diluted to 25.0 mL with 0.1 M HNO3. How many moles of SCN- are present?