Solve the following problem: A dilute solution of an unknown weak acid required a titration with 28.62 mL of 0.1084 M NaOH to reach the phenolphthalein end point. The titled solution was then evaporated until it was completely dry. Find the equivalent mass of the acid if the mass of the sodium salt was 0.2110g.

Solve the following problem: A dilute solution of an unknown weak acid required a titration with 28.62 mL of 0.1084 M NaOH to reach the phenolphthalein end point. The titled solution was then evaporated until it was completely dry. Find the equivalent mass of the acid if the mass of the sodium salt was 0.2110g.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter6: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 142IP: Tris(pentatluorophenyl)borane, commonly known by its aeronym BARF, is frequently used to initiate...

See similar textbooks

Similar questions

Tris(pentatluorophenyl)borane, commonly known by its aeronym BARF, is frequently used to initiate polymerization of ethylene or propylene in the presence of a catalytic transition metal compound. It is composed solely of C, F, and B; it is 42.23% C and 55.66% F by mass. a. What is the empirical formula of BARF? b. A 2.251-g sample of BARF dissolved in 347.0 mL of solution produces a 0.01267-M solution. What is the molecular formula of BARF?
A 1.458 g primary-standard grade Na2CO3 (MW = 105.99 g/mol) was used to standardize an HCl solution. Solve for the molarity of HCl if 24.81 mL of HCl was used to reach the endpoint.
To determine the concentration of a solution of nitric acid,a 100.0-mL sample is placed in a flask and titrated with a 0.1279 M solution of potassium hydroxide. A volume of 37.85 mL is required to reach the phenolphthalein endpoint. Calculate the concentration of nitric acid in theoriginal sample.
Calculate the volume in milliliters of 0.362 M KOH necessary to titrate 28.38 mL of 0.279 M diprotic sulfuric acid, H2SO4, to a phenolphthalein end-point. Report the answer to a precision of 2 decimal places.
In standardizing a solution of NaOH against 1.431g of KHC8H4O4, the analyst uses 35.50 mL of the alkali and has to run back with 5.12 mL of acid (1mL = 0.0031g Na20) What is the normality of NaOH? Additional instructions: Make it handwritten Include up to 4 decimal places Please include explanations of the process Thank you so much!
If a buret of 15mL of standardized 0.0024 M K2CrO4 was added to a clean 100mL volumetric flask and diluted to the 100mL mark with NaNO3. What will be the concentration of CrO42- in the solution. Please show all the steps when solving. Thanks
In standardizing a solution of NaOH against 1.431g of KHC8H4O4, the analyst uses 35.50 mL of the alkali and has to run back with 5.12 mL of acid ( 1mL ≎0.0031g Na2O) What is the normality of NaOH?
A sample consisting of an aqueous solution of the monoprotic acetic acid (CH3COOH, 60.05g/mol) is titrated with .2024 M NaOH. A 2.50g sample of the solution requires 22.67 mL of the NaOH solution to reach the endpoint. Calculate the percent by mass of acetic acid in the sample.
Mass of H2C2O4•2H2O = 1.3245 grams Molar Mass of H2C2O4•2H2O = 126.07 Volume of H2C2O4•2H2O solution = 250.0 mL Moles of NaOH at the equivalence point?
A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember, KHP ia potassium hydrogen phthalate, KHC8H4O4, not potassium hydrogen phosphorus).
Assume that the molarity of the standardized KMnO4 solution is 0.025 M and it takes 23.00 mL to reach the endpoint when titrating a dilute sample of H2O2. How many moles of H2O2 are in the diluted sample initially? Group of answer choices
A titrant solution of KMnO was standardized with 0.2000 grams of Na2C2O4 and consumed 27.75 mL to reach end point. Calculate the standardized NORMAL concentration of the titrant.