Titus titrates 30 mL of 0.450 M lactic acid (HC₂H₂O3, Ka = 1.5 x 10-4) using 0.500 M NaOH. Calculate the pH of the resulting solution at each of the following points in the titration. After adding 16.5 mL of the NaOH solution: At the equivalence point: After adding 37.7 mL of the NaOH solution:

Titus titrates 30 mL of 0.450 M lactic acid (HC₂H₂O3, Ka = 1.5 x 10-4) using 0.500 M NaOH. Calculate the pH of the resulting solution at each of the following points in the titration. After adding 16.5 mL of the NaOH solution: At the equivalence point: After adding 37.7 mL of the NaOH solution:

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

Related questions

Q: Calculate the pH at the equivalence point in titrating 0.045 M solutions of each of the following…

A: Concept based on the finding out the pH at the he equivalence point between the acid- base…

Q: A 45.0 mL sample of 0.30 M HCI is titrated with 0.15 M aniline (C6H5NH2). The pH will be after…

A: Step 1:From the given data, moles of HCl is than moles of aniline, so upon titration HCl completely…

Q: An acid of molar mass 121.1 g/mol is titrated with a 0.700 M NaOH solution. What volume of titrant…

Q: A 30.00 mL of 0.125 M NaOH solution is titrated with a standard 0.250 M HCl solution. Calculate the…

A: The reaction involved in the titration of sodium hydroxide (NaOH) with hydrochloric acid (HCl) can…

Q: During a titration, 0.5 M NaOH is added to 25.0 mL of 0.7 mol/L HF until the equivalence point is…

A: The objective of this question is to calculate the pH of the mixture at the equivalence point during…

Q: calculate the buffer capacity of a buffer consisiting 0.05 moles each of acetic acid and sodium…

Q: In the titration of a solution of weak monoprotic acid with a 0.1475 M solution of NaOH, the pH half…

A: Answer: Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Calculate the pH at the equivalence point in titrating 0.023 M solutions of each of the following…

A: The initial concentration of each of the acids = 0.023M and the concentration of NaOH every time is…

Q: Sketch the titration curve when 10.0 mL of a 0.20 M solution of the polyprotic weak acid H2CO3 is…

A: H2CO3 is a weak diprotic acid. When it is titrated with NaOH, we see two inflection points.

Q: Calculate the pH at the equivalence point for the titration of 0.160 M methylamine (CH3NH₂) with…

Q: A buffer is prepared by adding 150mL of KOH 1.00M to 250mL of KH2PO4 1.00M. Calculate the moles of…

A: A buffer is prepared by adding 150mL of KOH 1.00M to 250mL of KH2PO4 1.00M. after adding HCl the pH…

Q: A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after…

A: A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after…

Q: calculate the pH at the equivalence point for the following titration: 0.01M HCl versus 0.01 M…

A: Given,Molarity of HCl = 0.01 MMolarity of CH3NH2 = 0.01 MKa of CH3NH3+ = 2.3 x 10-11

Q: Calculate and sketch a correct titration curve for the titration of 25.0 mL of 0.10 M of…

A: N1V1=N2V2 25X0.1 = 0.05XV2 V2 = 25X0.1/0.05 = 50mL of NaOH is required to neutralize HCl.

Q: Calculate the pH in the titration of 15.0 mL of 0.250 M CH3CO2H (acetic acid) solution by 0.250 M…

Q: A 100ml sample of 0.20M HF is titrated with 0.10M NaOH. Determine the pH of the solution after the…

Q: A titration is carried out for 25.00 mL of 0.100 M HCI (strong acid) with 0.100 M of a strong base…

A: Answer: This is the question based on acid-base titration in which base is being added into acid and…

Q: Calculate the pH in the titration of 25.0 mL of 0.100 M acetic acid by sodium hydroxide after the…

A: Given volume of acetic acid is 25.0mL and strength is 0.100 M. Given volume of NaOH is 30.0 mL and…

Q: A 1.48 L buffer solution consists of 0.100 M butanoic acid and 0.294 M sodium butanoate. Calculate…

A: Given that : The volume of buffer solution = 1.48 L The molarity of butanoic acid = 0.100 M The…

Q: A 45.60-mL sample of a 0.476 M solution of acetic acid (HC2H3O2) which is a weak acid with an acid…

A: volume of acetic acid (H C₂ H 30₂) = 45.60 ml molarity of acetic acid = 0.476M Ка (H C₂ H…

Q: Consider the titration of a 20.0-mL sample of 0.100 M HC2H3O3 (Ka=1.8×10−5) with 0.125 M NaOH.…

A: Given question is related to calculating the pH at equivalent point in acid-base titration reaction.…

Q: 10.00mL of O.10M HCI were collected in an Erlenmeyer flask, and 100mL with distilled water. After…

A: HCl is an acid and NaOH is a base and both react to form salt and water. The H+ ions dissociated…

Q: A 29.9 mL sample of 0.252 M dimethylamine, (CH3)₂NH, is titrated with 0.355 M hydrochloric acid. The…

A: Concentration of (CH3)2NH = 0.252 M Kb for (CH3)2NH = 5.9 × 10-4

Q: A 25.0-mL sample of 0.30 M HCl is titrated with 0.30 M KOH. What is the pH of the solution after…

Q: Sketch a titration curve and give the suitable indicato for the following condition of titration: a)…

A: (a) Solution -

Q: Calculate the pH for each of the cases in the titration of 25.0 mL of 0.110 M pyridine, CH-N(aq)…

Q: 15.0 mL of a buffer is made by mixing 10.0 mL of 0.10 M HF and 5.0 mL of 0.10 M NaOH solution. What…

A: Molarity of NaOH=0.10 M The volume of NaOH=5 mL Molarity of HF=0.10 M The volume of HF=10 mL The…

Q: Calculate the pH at the equivalence point in titrating 0.072 M solutions of each of the following…

A: (a) Hydrobromic acid (HBr): Reaction at equivalence point: HBr+NaOH→NaBr+H2O pH=7.0 (neutral) (b)…

Q: The pH values from the CH3COOH-NaOH titration solution and the HCl-NaOH titration solution are…

A: The titration of strong acid Vs strong base, The initial pH is usually low and may be calculated…

Q: Consider the titration of a 21.0 mL sample of 0.100 M HC2H3O2 with 0.130 M NaOH. Determine the…

A: Given- Concentration of weak acid HC2H3O2 = 0.100 M Concentration of strong base NaOH = 0.130 M…

Q: 20.0 mL of 0.075 M aqueous solution of lactic acid CH3CH(OH)COOH, a monoprotic acid, is titrated…

A: volume of NaOH at equivalence point pH at equivalence point pH after adding 5.0 mL of NaOH

Q: The K of a certain indicator is 8 × 10. The color of HIn is green and that of In is red. A few drops…

A: The question is based on the concept of titrations. we need to calculate the pH range in which the…

Q: c) A student titrated 50.0 mL of a 0.10 M solution of a certain weak acid with NaOH. The results are…

A: Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated…

Q: 50.0 mL of a solution which is 0.125 M in HCl and 0.075 M in formic acid (Ka = 1.8 x 10-4 and can be…

A: Since you have asked a question with multiple subparts, we will answer first three subparts for you.…

Q: Calculate the pH at the equivalence point in titrating 0.077 M solutions of each of the following…

A: HCl is a strong acid and NaOH is a strong base. This is the titration of strong acid vs strong base.…

Q: A 100mL sample of 0.20M HF is titrated with 0.10M KOH. What is the pH of the solution after the…

A: HF is a weak monoprotic acid with Ka = 3.5*10-4 KOH is a strong monoacidic base.

Q: An analytical chemist is titrating 72.2 mL of a 0.8900M solution of propionic acid (HC,H,CO,) with a…

A: Given that, An analytical chemist is titrating 72.2 mL of 0.89 (M) solution of propanoic acid with…

Q: A sample of 50.0 mL of 2.0 M HNO, (pKa=3.398) is titrated with 1.0 M KOH. Determine the pH after the…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: 25 mL of a 0.0268 M solution of an unknown monoprotic acid was titrated with 0.0633 M NaOH solution.…

A: Given: Volume of monoprotic acid (assuming HA) = 25 mL = 0.025 L (since 1…

Q: What is the pH at the equivalence point of a weak acid titrated with a strong base? (Hint: what are…

A: The acidity or basicity of a solution is measured by the pH of the solution. If the pH is 7, the…

Q: A titration of 3.36 g of an acid requires 43.72mL of 0.100M NaOH to reach the equivalence point.…

Q: How many g of sodium nitrate (NaNO2, 100% ionized in water) do you need to add to 4.00L of 0.500M…

Q: A 29.9 mL sample of 0.253 M dimethylamine, (CH3)2NH, is titrated with 0.292 M hydroiodic acid. (1)…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: Consider the titration of 100.0 mL of 0.100 M acetic acid (Ka = 1.8 x 105). When 50.00 mL of 0.100 M…

A: Given data,Molarity of acetic acid=0.1MVolume of acetic acid=100mLMolarity of NaOH=0.1MVolume of…

Q: A 50.0 ml aliquot of a 0.0010OM solution of acetic acid (K = 1.8 x 10-5) is titrated with 0.00993M…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step by step

Solved in 4 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Calculate the pH for a buffer with 0.20 M NH3 and 0.20 M NH4Cl, then calculate the pH after 10.0 mL of 0.10 M HCl is added to 75.0 mL of the buffer.
When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an indicator initially. You've added 10 mL of KOH to the flask of acid. Ka of CH3COOH = 1.8 x 10^-5 1) Calculate the pH at this point 2) What color would your solution be if you add 40 mL KOH more. And a few drops of clorophenol blue indicator at this point. Why?
Please don't provide handwritten solution
Regarding titrations, which of the following is TRUE? A plot of pH vs. the [base]/[acid] ratio is known as a titration curve. The equivalence point is when the moles of base equals the moles of acid during any acid–base titration. Indicators do not respond to changes in pH. The pH is always 7 once the equivalence volume has been delivered. None of the answers are true.
Predict the equivalence point that occurs for the following titrations: The when C5HSN (aq) is titrated with HBr (aq). The when H2CO3 (aq) is titrated with NaOH (aq). Th V when Ca(OH)2 (aq) is titrated with HNO; (aq). equivalence point >7 equivalence point less than 7 equivalence point = 7
Titus titrates 45 mL of 0.750 M lactic acid (HC₂H₂O², Ka NaOH. = 1.5 × 104) using 0.250 M Calculate the pH of the resulting solution at each of the following points in the titration. After adding 24.750000000000004 mL of the NaOH solution: At the equivalence point: After adding 191 mL of the NaOH solution:
When titrating a weak acid with a strong base, what is the approx. pH expected for the equivalence point (at 25oC.)? Why is this expected to be a different pH than the equivalence point pH for a strong acid with a strong base titration?
15.0 mL of a buffer is made by mixing 10.0 mL of 0.10 M HF and 5.0 mL of 0.10 M NaOH solution. What is the pH of this buffer after 0.24 mL of 1.0 M sodium hydroxide are added to it? The Ka for HF is 6.8 x 10-4.
25.00 mL of 0.100 M HCl solution is titrated with a 0.100 M NaOH solution. What is the pH of the solution after the addition of the following strong base? (pH= - log[H3O+] = - log[H+]) a) initially (Before adding NaOH) b) Before the equivalence point (with the addition of 24.00 mL of 0.100 M NaOH) c) At the equivalence point (with the addition of 25.00 mL of 0.100 M NaOH) d) After the equivalence point (with the addition of 26.00 mL of 0.100 M NaOH)
A 26.7 mL sample of 0.292 M ethylamine, C₂H5NH2, is titrated with 0.322 M perchloric acid. (1) Before the addition of any perchloric acid, the pH is (2) After adding 9.37 mL of perchloric acid, the pH is (3) At the titration midpoint, the pH is (4) At the equivalence point, the pH is (5) After adding 35.8 mL of perchloric acid, the pH is Use the Tables link on the toolbar for any equilibrium constants that are required.
In the titration of a solution of weak monoprotic acid with a O.1450 M solution of NaOH, the pH half way to the equivalence point was 4.38. In the titration of a second solution of the same acid, exactly twice as much of a 0.1450 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?
2) For the titration 100 mL of 0.1 M NH3 with 0.2 M HCI, what will be the pH of the solution after the addition of a) 0.0 mL 0.2 M HCI, b) 25 mL 0.2 M HCI, c) 50.0 mL 0.2 M HCI KB(NH3) = 1.75x10-5