Rashid has performed titrimetric analysis of antacid tablets which solely contain aluminum hydroxide [Al(OH)3, 78.0 g/mol]. For the samplepreparation, he powdered an antacid tablet, dissolved it in 100 mL pre-boiled distilled water, and equally divided the mixture into two Erlenmeyerflasks. Then, he titrated each flask up to the faint pink end point with HCl titrant. Initially, he determined the concentration of the HCl titrant bytitrating 10.0 mL of HCl solution with 0.0998M NaOH in duplicate. Consider the data presented in the table below and answer the succeedingquestions.Volume of titrant, mLStandardization (0.0998M NAOH)25.025.1Titration of sample (x M HCI)38.538.4Can a tablet be sufficient in neutralizing a 100. mL of stomach acid with a pH of 1.50? Hint: H* concentration is antilog(-pH).Answer:

The number of moles is given as the mass of a substance upon its molar mass. The molarity of a…

Answered: Rashid has performed titrimetric…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.102QE

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A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 51 mg of oxalic acid (H2C2O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250 mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 19.2 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution.
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 10.mg of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 12.2mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.
Limestone consists mainly of the mineral calcite, CaCO 3. The carbonate content of 0.5413 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel CO 2: CaCO 3(s) + 2 HCl → CaCl 2 + CO 2(g) + H 2O The excess acid required 39.96 mL of 0.1004 M NaOH for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone.
Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balance chemical equation is given below. If the student used 21.21 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)
Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balanced chemical equation is given below. If the student used 25.71 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 303 mg of oxalic acid, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 104.5 mL of sodium hydroxidesolution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits.
You have been provided with a 35.0 mL sample of hydrochloric acid (HCl) of unknown concentration. You perform a titration with 1.48 M sodium hydroxide (NaOH), and find that 3.81 x 10-2 L are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the hydrochloric acid?
Potassium hydrogen phthalate (KHPKHP) is often used as a primary standard in acid–base titrations. If 20.05 mL NaOH20.05 mL NaOH is required to neutralize 0.397 g KHP,0.397 g KHP, what is the concentration of the NaOH?
A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH)2 as it could hold. A 84.3-mL sample of this solution was withdrawn and titrated with 0.0948 M HBr. It required 64.6 mL of the acid solution for neutralization.(a) What was the molarity of the Ca(OH)2 solution? M(b) What is the solubility of Ca(OH)2 in water, at the experimental temperature, in grams of Ca(OH)2 per 100 mL of solution? g/100mL
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 13.mg of oxalic acid H2C2O4, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 11.9mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits.
A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 22.3 mL of HNO₃ was required. a. Write the balanced chemical equation for the reaction b. What quantity in moles of HNO₃ are used in the titration? c. What quantity in moles of Ca(OH)₂ had to be present in the initial reaction? d. What was the concentration of the initial Ca(OH)₂ solution?
An unknown hydroxide of the formula X(OH)2 is only slightly soluble in water. A scientist is curious as to what hydroxide this is. So, she takes this hydroxide and dissolves enough of it in pure water to make a saturated solution. She then takes 25.00 mL of the saturated solution and titrates it with 0.000100 M HCl. She notes that it takes 2.58 mL of HCl to fully neutralize the saturated solution. 1. Determine the Ksp of the hydroxide. (concentration of X(OH)2 is 1.032 x 10-5 M, pH = 9.31, molar solubility should be 1.032 x 10-5 M)

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