A 0.025M solution of hydrochloric acid is titrated with 0.020M of sodium hydroxide. If 250mL of the acid requires 30.0mL of the base for neutralization,calculate the initial concentration of hydrochloric acid.

A 0.025M solution of hydrochloric acid is titrated with 0.020M of sodium hydroxide. If 250mL of the acid requires 30.0mL of the base for neutralization,calculate the initial concentration of hydrochloric acid.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Sketch an accurate titration curve by plotting pH as a function of mL of HCl added when a 40 mL solution of 0.100 M ammonia is titrated with 0.100 M HCl include pH values when:0mL of HCl is added, 10 mL, 20 mL, 30mL and 40 mL
A 19.8 mL sample of a 0.412 M aqueous hydrocyanic acid solution is titrated with a 0.327 M aqueous sodium hydroxide solution. What is the pH at the start of the titration, before any sodium hydroxide has been added? pH = Submit Answer Retry Entire Group 2 more group attempts remaining
A weak diprotic acid is titrated past the end points with a strong base. Identify which of the following statements is true. O pH at end point 1 and pH at end point 2 are numerically smaller than 7. O the volume of titrant added to reach end point 1 will be the same additional volume of titrant as between end point 1 and end point 2. O the volume of titrant added to reach end point 1 will be twice the additional volume of titrant as between end point 1 and end point 2. O the volume of titrant added to reach end point 1 will be half the additional volume of titrant as between end point 1 and end point 2. O pH at end point 1 and pH at end point 2 ak numerically larger than 7.
A student is titrating a 100 mL of 0.50 M solution of hydrofluoric acid (HF) with 1.0 M strong base (NaOH). a) at the equivalence point, what ions/compounds will be present in the solution? A complete answer will also be specific as to what ions/compounds are not present in solution. b) calculate the pH at the equivalence point.
2. In the second titration, the molar mass of an unknown monoprotic acid is calculated. If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question Which is 0.1186
In a particular titration experiment a 30.0 mL sample of an unknown monoprotic acid required 25.0 mL of 0.200 M NaOH for the end point to be reached. What is the concentration of the acid?
Consider a solution of a weak acid being titrated with a solution of a strong base to beyond the equivalence point. Which of the following statements is incorrect? a. The pH will increase intially and then change very little until the equivalence point is reached b. Only a small percentage of the weak acid will react with the added base c. The volume of the base solution required to reach the equivalence point can be less than, equal to, or more than the volume of the acid solution. d. At the equivalence point, the solution will be basic e. Beyond the equivalence point, the solution will be basic f. None of the above g. The pH of the solution in the tiration flask is affected by the total volume at any given point
Determine the pH during the titration of 21.9 mL of 0.277 M perchloric acid by 0.206 M sodium hydroxide at the following points: (1) Before the addition of any sodium hydroxide (2) After the addition of 14.8 mL of sodium hydroxide (3) At the equivalence point (4) After adding 35.4 mL of sodium hydroxide
Determine the pH during the titration of 15.4 mL of 0.276 M hydrobromic acid by 0.210 M sodium hydroxide at the following points: (1) Before the addition of any sodium hydroxide (2) After the addition of 10.1 mL of sodium hydroxide (3) At the equivalence point (4) After adding 26.1 mL of sodium hydroxide
Use the References to access important values if needed for this question. A buffer solution contains 0.445 M nitrous acid and 0.206 M sodium nitrite. If 0.0225 moles of sodium hydroxide are added to 150 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding sodium hydroxide.) pH
(Answer highlighted questions please) A 50.050.0 mL solution of 0.1390.139 M KOHKOH is titrated with 0.2780.278 M HClHCl. Calculate the pH of the solution after the addition of each of the given amounts of HClHCl. 20.0 mLpH=20.0 mLpH= 24.0 mLpH=24.0 mLpH= 25.0 mLpH=25.0 mLpH=
Select ALL of the following that can be determined from the titration of a strong, monoprotic acid with a standardized solution of sodium hydroxide? moles of acid in the titration moles of hydroxide ions used in the titration mass of acid titrated | volume of sodium hydroxide used in the titration Select ALL of the following quantities that must be used in a titration calculation to find the identity of an unknown strong acid: concentration of the standardized base solution stoichiometric ratio of acid to base volume of the acid solution used in the titration volume of the base used in the titration at the equivalence point Need Help?