In two SEPARATE flasks containing similar component of carbonate mixtures, the following volumes of titrant were obtained for phenolphthalein and methyl orange endpoin respectively: (1) 21.0mL (2) 24.0mL. What is/are the component/s of the mixture that is/are being reacted at the PHENOLPHTHALEIN endpoint? a. NaOH and NaHCO3 b. Na2CO3 only c. NaOH and Na2CO3 d. NaHCO3 only

In two SEPARATE flasks containing similar component of carbonate mixtures, the following volumes of titrant were obtained for phenolphthalein and methyl orange endpoin respectively: (1) 21.0mL (2) 24.0mL. What is/are the component/s of the mixture that is/are being reacted at the PHENOLPHTHALEIN endpoint? a. NaOH and NaHCO3 b. Na2CO3 only c. NaOH and Na2CO3 d. NaHCO3 only

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.20QAP

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A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in a volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M sodium hydroxide to reach the phenolphthalein endpoint From this experiment which is the standard solution used in titration? CH3COOH NaOH NaCH3COO C20H14O4
A 567.9 mg sample containing Na2CO3, NaHCO3 , NaOH and inert material was dissolved and titrated with 0.1002 M HCl. The titration required 24.30 mL to reach the phenolphthalein endpoint and an additional 38.67 mL to reach the methyl red endpoint. Determine the composition of the sample and the % of each titrated component.
15. A 300.00 mL solution of 0.00165 M A2B5 is added to a 230.00 mL solution of 0.00380 M C2D3. What is pQsp for A2D5?
200 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/L
true or false 1.,Carbonic acid, as a contaminant in the assay of sodium bicarbonate, may render the end point to be yellow. 2,.To have a balanced equation in the assay of sodium bicarbonate, the titrant should have a coefficient of one and the sulfate salt of sodium produced should have a coefficient of three. 3.When a weak alkali is titrated with strong acid, the indicator used is methyl red.4 4.Sodium bicarbonate is considered as the primary standard in its own assay. 5.When a strong alkali is titrated with a strong acid, phenolphthalein may be used.
A mixture of sodium carbonate and sodium bicarbonate is dissolved in water and treated with 0.100 M HCl. At the phenolphthalein endpoint, 12.00 mL was used and 34.00 mL to reach the methyl orange endpoint. How many moles of sodium carbonate and sodium bicarbonate are in the sample?
Titration of 0.1 M HCl against a 25mL liquor mixture of NaOH and Na2CO3 using phenolphthalein indicator requires 17.5mL of the acid for the endpoint. After this, methyl orange was added and 3.5mL of HCl was again required for the next endpoint. A. Write separate equations for reactions for the two endpoints B. Calculate the amount in milligrams of NaOH and Na2CO3 in the mixture
2.0 g of mixture involving Na3PO4, Na2HPO4 or NaH2PO4 or involving three of them. The solution is titrated with 16.5 mL of 0.5 M HCl to reach bromocresol green end point. The same solution is also titrated with 7.6 mL of 0.7 M NaOH to reach phenolphthalein end point. What is the composition of that mixture? What are the amounts of species (%) in the mixture (H:1.0078, O:15.99, Na: 22.98, P:30.974)?
Which of the following correlations in the qualitative analysis experiment is incorrect? a. CO32- : evolution of H2 gas b. SCN- : formation of FeSCN2+ complex c. Zn2+ : precipitate is soluble in NaOH and NH3 d. NH4+ : red litmus paper turned blue
In the procedure below for a weak diprotic acid titation experiment what are the independent, dependent, and controlled variables? Prepare your Buret• Condition a 50 mL buret (2x with DI H2O followed by 2x standardized NaOH)• Fill the buret with the standardized NaOH close to but not exactly 0.00 mL Prepare Your Analyte • Your analyte will need to be placed in a 250 mL beaker and should contain thefollowing:*0.5 – 0.75 g KHP** About 100 mL DI water* Magnetic stir bar• Once all contents are in the 250 mL beaker, stir for at least 5 minutes to dissolve. Ifneeded, add a bit more water.* For unknown diprotic acids, use the mass provided by the instructorNext Run the Titration (note you will need to run the titration several times for data collection so you are able to use the average molar mass to find the unknown diaprotic acid).
A student used 9.925 x 10-2 mol/L hydrobromic acid to standardize an aqueous solution of potassium hydroxide and obtained the following titration data using phenolphthalein as an indicator: Concentration of HBr used: 9.925 x 10-2 mol/L Volume of HBr used: 25.00 mL Indicator: phenolphthalein Endpoint colour change: colorless to pale pink Table 1: Volume of Potassium Hydroxide Required Burette reading (mL) Trial 1 Trial 2 Trial 3 Final reading 29.28 36.62 43.98 Initial reading 1.78 9.28 16.62 Volume of KOH used (mL) Average of 2 closest values to within 0.10 mL: Questions Complete Inclosed table Write the molecular equation for the reaction that occurs between potassium hydroxide and hydrobromic acid. Calculate the molar concentration, in mol/L, of the aqueous potassium hydroxide.
1. What is the molar solubility of PbCl2 in a solution of 0.23 M CaCl2? Ksp = 1.6 ✕ 10-5 for PbCl2. 2. What is the Qsp when 32.0 mL of 6.50 ✕ 10-7 M Na3PO4 are mixed with 41.4 mL of 5.50 ✕ 10-5 M CaCl2? Assume the volumes are additive. Ksp = 2.0 ✕ 10-29. 3. What is the Qsp when 61.0 mL of 1.50 ✕ 10-4 M AgNO3 are mixed with 80.0 mL of 5.20 ✕ 10-3 M CaCl2? Assume the volumes are additive. Ksp = 1.6 ✕ 10-10. 4. What [I-1] is needed to start the precipitation of AgI from a saturated solution of AgCl? Ksp = 2.9 ✕ 10-16 for AgI and Ksp = 1.2 ✕ 10-10 for AgCl.