Prepare a theoretical titration curve for titration of 25.0 mL of 0.1037M formic acid (HCOOH; pKa=3.75) solution (diluted to 100 mL volume with deionized water) by 0.0964M solution of KOH determine the volume of KOH solution needed to reach the equivalence point. calculate pH of the starting solution (remember, it was diluted to 100 mL) calculate pH at the equivalence point (the total volume is now more than 100 mL!) calculate pH at points between the start of titration and equivalence point; choose points so that they will be more dense where change in pH is faster. calculate pH at points from equivalence point up until 150% of volume at equivalence point.

answer

watching

197

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Elin HesselLv2

28 Sep 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

Part A: Watch the animation and observe the titration process of a standard 0.100 M sodium hydroxide solution with 50.0 \rm ml of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding acid-base titration are correct. Check all that apply. a - The titration process is based on a chemical reaction. b - The \rm pH of the solution at the equivalence point is 7. c - At the endpoint, the \rm pH of solution is 10 and the color of solution is pink. d - At the beginning of the titration process, the \rm pH of the solution increases rapidly. e - The chemical reaction involved in an acid-base titration is a neutralization reaction. f - Before any base is added to the solution, the \rm pH of the solution is high. g - In a titration process, the endpoint is reached before the equivalence point. h - The \rm pH of the solution changes very slowly at the equivalence point. Part B: 100 \rm mL of 1.00 M HCl solution is titrated with 1.00 M~ \rm NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point/endpoint. Drag the appropriate items to their respective bins 10.0mL of 1.00 M NaOH 150 mL of 1.00 M NaOH 5.00 mL of 1.00 M NaOH 50.0 mL of 1.00 M NaOH 200 mL of 1.00 M NaOH BINS: Before equivalent point At equivalent point After equivalent point Part C: A volume of 90.0 mL of a 0.400 M HNO3 solution is titrated with 0.470 M KOH. Calculate the volume of KOH required to reach the equivalence point.

Part A: Watch the animation and observe the titration process of a standard 0.100 M sodium hydroxide solution with 50.0 \rm ml of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding acid-base titration are correct.Check all that apply.a - The titration process is based on a chemical reaction.b - The \rm pH of the solution at the equivalence point is 7.c - At the endpoint, the \rm pH of solution is 10 and the color of solution is pink.d - At the beginning of the titration process, the \rm pH of the solution increases rapidly.e - The chemical reaction involved in an acid-base titration is a neutralization reaction.f - Before any base is added to the solution, the \rm pH of the solution is high.g - In a titration process, the endpoint is reached before the equivalence point.h - The \rm pH of the solution changes very slowly at the equivalence point.Part B: 100 \rm mL of 1.00 M HCl solution is titrated with 1.00 M~ \rm NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point/endpoint.Drag the appropriate items to their respective bins10.0mL of 1.00 M NaOH150 mL of 1.00 M NaOH5.00 mL of 1.00 M NaOH50.0 mL of 1.00 M NaOH200 mL of 1.00 M NaOHBINS:Before equivalent pointAt equivalent pointAfter equivalent pointPart C:A volume of 90.0 mL of a 0.400 M HNO3 solution is titrated with 0.470 M KOH. Calculate the volume of KOH required to reach the equivalence point.

a. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution?

b. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with 0.1 M NaOH (aq), at what volume of NaOH (aq) is the equivalence point reached? Is the pH at the equivalence point greater than, less than or the same as in problem #a above? Explain.

c. What is the initial pH expected for a 0.1 M solution of phosphoric acid (H3PO4)? For 25.0 mL of 0.1M H3PO4 (aq), what volume of 0.1 M NaOH (aq) is required to fully titrate all three protons to their end points?

d. In the titration of a weak acid with a strong base, how is the half equivalence point determined and what is its significance? How are the pKa and Ka of the weak acid determined from the half equivalence point?

Weekly leaderboard

Home

Homework Help 3,900,000

Chemistry 830,000

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard