a solution is made by taking 100.0 mL of 2.0x10^ - 2 molar NaOH (aq) and mixing in 50 mL of 3.0x10^-2 molar HCI (aq) The acidity of a small portion was tested using Tyrolian blue indicator, for which the pKind 12.5, and the colors are blue for Hind, and yellow for ind. What color would be observed as a result of the testing? A) blue B) green C) yellow D) orange E) red

a solution is made by taking 100.0 mL of 2.0x10^ - 2 molar NaOH (aq) and mixing in 50 mL of 3.0x10^-2 molar HCI (aq) The acidity of a small portion was tested using Tyrolian blue indicator, for which the pKind 12.5, and the colors are blue for Hind, and yellow for ind. What color would be observed as a result of the testing? A) blue B) green C) yellow D) orange E) red

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 65QAP: Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105)....

See similar textbooks

Similar questions

A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
For the determination of basic species in 0.1878 g Talcid sample; 20 ml of 0.1009 M HCl solution was added to the sample and the necessary procedures were carried out and titrated with O.1097 M NaOH solution. Since 10.2 mL of base solution is consumed at the end of the titration, which of the following is the% base amount in CaCO3 in the sample? (CACO3: 100,087 g/mol) A. 23.96 B. 55.1 C. 45.1 D.42.1
A 75.0 mL sample of 0.0200 M HBrO4 is titrated with 0.0400 M RbOH solution. Calculate the pH after the following volumes of base have been added. (a) 16.9 mLpH = (b) 36.0 mLpH = (c) 37.5 mLpH = (d) 38.3 mLpH = (e) 61.1 mLpH =
For the determination of basic species in 0.1878 g Talcid sample; 20 mL of 0.1009 M HCl solution was added to the sample and the necessary procedures were carried out and titrated with 0.1097 M NaOH solution. Since 10.2 mL of base solution is consumed at the end of the titration, which of the following is the% base amount in CaCO3? (CaCO3: 100,087 g / mol)
What is an acid–base indicator? Define the equivalence(stoichiometric) point and the end point of a titration.Why should you choose an indicator so that the twopoints coincide? Do the pH values of the two pointshave to be within 60.01 pH unit of each other?Explain.
7. You are given a 500 ml solution of 0.1 M HNO3 and an indicator Hin (Ka = 3.2x10) which changes from yellow (Hin) to green (In'). If you add two drops of indicator to the solution: (a) What colour is the solution initially? (b) What pH would the colour change become visible if you were adding 0.10M NaOH?