4.60 g of formic acid (molar mass 46.0 g/mol) was added to a flask and dissolved in water to make 100.00 mL of solution. It required 40.00 mL of 2.5 M NaOH to reach the equivalence point. What is the pH at the equivalence point of the titration? K₂ = 1.77 x 10-4 a pH = [?] pH Enter

4.60 g of formic acid (molar mass 46.0 g/mol) was added to a flask and dissolved in water to make 100.00 mL of solution. It required 40.00 mL of 2.5 M NaOH to reach the equivalence point. What is the pH at the equivalence point of the titration? K₂ = 1.77 x 10-4 a pH = [?] pH Enter

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 52QAP: A solution is prepared by dissolving 0.350 g of benzoic acid, HC7H5O2, in water to make 100.0 mL of...

See similar textbooks

Related questions

Q: Draw the two major products obtained in the reaction shown. + Br₂ (one equivalent) CH₂Cl₂ . You do…

A: Organic reactions are those in which organic reactant react to form organic products.

Q: HO ∞ H Br KMnO4 NaOH 0 °C 1. KMnO4, NaOH, A 2. dil. H₂SO4, H₂O 1. KMnO4, NaOH, A 2. dil. H₂SO4, H₂O…

A: Here we have to predict the major products formed in the following given reactions.

Q: What explains why many aldehydes and ketones can undergo self- condensation reactions in basic…

Q: Using Zaitsev's rule, choose the most stable alkene among the following. Draw out the structures of…

Q: Draw both resonance structures of the most stable carbocation intermediate in the reaction shown. +…

A: A carbocation is a molecule in which a carbon atom has a positive charge and three bonds. The…

Q: Draw out a multi-step synthesis (show all steps clearly). Synthesize the following product from the…

Q: : 20:28 : 20. Draw the full acetal formation scheme on your paper, and then draw in the curved…

A: Acetals are formed when excess alcohol( 2 equivalent) react with acetaldehyde. The complete…

Q: Draw structures of the following compounds:…

A: Names of two organic compounds are given and their structure have been asked in the question.

Q: A 2.11 gram sample of methane gas has a volume of 805 milliliters at a pressure of 2.97 atm. The…

A: Given Mass of sample = 2.11 g Volume = 805 ml = 805 * 10-3 L Pressure = 2.97 atm

Q: Which compound of each of the following pairs is the STRONGER ACID? (A) (B) O Option A O Option B…

A: Given, Which compound of each of the following pairs is the stronger acid, A) H2SO4 or B) H2SO3…

Q: QUESTION 1 What is the driving force for losing a proton as the last step in an electrophilic…

A: Solution The correct option is D) To restore aromatic system

Q: Marked out of 1.00 Flag question Time left 0:49:41 pka of methanol is higher than pka of water due…

A: We know, pKa is a number that describes the acidity of a particular molecule. Higher the pKa…

Q: 20:24 : E) 03 12. Fill in the box with the major organic product of the first step of the reaction…

Q: Hydrogen peroxide decomposes to water and oxygen according to the reaction below: 2 H2O2(aq) → 2…

A: Solution: In the given question we have to calculate the average rate of disappearance in the first…

Q: For each of the following aqueous reactions BELOW, identify the acid, the base, the conjugate base,…

Q: What is the product of the following reaction sequence? You can ignore and stereochemistry. The…

A: In the first step the reactant is reacted with ethyl magnesium bromide and then with water to obtain…

Q: The following stands for the frequency factor in the Arrhenius equation. Ea R A k

Q: Draw structural formulas for the diene and dienophile that combine in a Diels-Alder reaction to form…

A: The above reaction is proceed by specific mechanism as shown below.

Q: Write TRUE if the underlined word/phrase makes the statement correct. Otherwise, write the correct…

A: According to Q&A guidelines of Bartleby, we are supposed to answer only the first 3 sub-parts of…

Q: Henry titrated 50.00 mL of 0.25 M formic acid with 0.50 M LIOH. Formic acid is monoprotic and has a…

A: we have to calculate the pH of solution after addition of LiOH

Q: The equilibrium concentrations of NH3, N₂ and H₂ are 0.25 M, 0.11M, and 1.91 M respectively. The…

Q: How does the halogenation of an alkene differ from the halogenation of an alkane?

A: substitution reaction, is a chemical reactions in which an atom or groups in a molecule is replaced…

Q: Which compound of each of the following pairs is the stronger acid/base? H3AsO3 or H3AsO4 H2SO4 or…

A: Strong acids or strong base are those acids which are completely or nearly 100% ionized in their…

Q: A 50.00-mL sample of a citrus drink requires 17.62 mL of 0.04166 M NaOH to reach the phenolphthalein…

Q: Electrophilic nitration of benzoic acid gives almost exclusively 3-nitrobenzoic acid. By drawing the…

A: benzoic acid undergoes electrophilic substitution reaction when reacted with Nitration mixture(1:1…

Q: What is the pH of the solution when Maria has added 10.0 mL of 0.25 M NaOH to the 40.00 mL of 0.50 M…

Q: Br К CH3 ICH ALICH °CH, NH₂ NH₂ CH CH₂ 'CH

Q: 2. To prepare a solution of NaCl, you weigh out 2.634 (+0.002) g and dissolve it in a volumetric…

A: Mass of NaCl = 2.634 g (±0.002) Molar mass of NaCl = 58.44 g/mol (±0.0012) Volume of the solution =…

Q: 4. Provide the full mechanism (curved arrows and intermediates) that leads to the product in the…

Q: What are differences between n→π* and π →π* bonding electron transition in Fluorescence? *

A: We know In fluorescence, there are two types of electronic transition occur. • n →π* • π →π*

Q: QUESTION 10 Which of the following is an intermediate in the bromination of toluene? O

A: The aromatic compound reacts with bromine from bromo arenes. The reaction proceeds by the aromatic…

Q: Electrophilic bromination of an equimolar mixture of methylbenzene (toluene) and…

A: Methyl group is Ortho para director due it's inductive and hyperconjugation effects.

Q: A 1.07 mol sample of Ar gas is confined in a 25.2 liter container at 12.3 degrees celcius. If the…

Q: Draw the least stable resonance form for the intermediate in the following electrophilic…

Q: At a certain temperature the rate of this reaction is first order in SO3 with a rate constant of…

A: Given :- The given reaction is 2SO3(g) → 2SO2(g) + O2(g) The reaction follows first order…

Q: Complete the following reaction oto. vo -HCK(+

A: Due to the presence of a lone pair of electrons on the nitrogen atom of amine, the amines are basic…

Q: For which of these equilibria, is Kp / Kc? P (I) 2HgO(s) = 2Hg(l) + O2(g) (II) SO₂Cl₂ (g) = SO2(g) +…

Q: Classify the following substituents according to whether they are electron donors or electron…

Q: Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H₂(9) C4H10(g) AH°…

A: The enthalpy change is a state function and the Hess law states that the change of enthalpy in a…

Q: Write TRUE if the underlined word/phrase makes the statement correct. Otherwise, write the correct…

Q: Draw structures of the following compounds:…

A: In the question, the name of two molecular compounds are given and it is asked in the question to…

Q: Predict the splitting patterns (singlet, doublet, etc.) you would expect for each proton in the…

Q: Provide the correct IUPAC name for the skeletal (line-bond) structure shown here.

Q: For the following pairs of redox processes given, work out the oxidation numbers for the reactions…

A: Balancing of these redox reaction is given by:

Q: soluble + diethyl ether soluble S₁ water-soluble organic compound + H₂O insoluble S₂2 compounds…

Q: Using standard thermodynamic data, calculate Ksp at 298 K for MgCl2.

Q: What is the major product of the following reaction? 0000 A B с D A + B =CHCH3 с =CHCH3 D OH

Q: Using curved arrows, show the deprotonation mechanism of phenol with hydroxide (-OH). Also, provide…

Q: What is the pH of the solution at the equivalence point, when Caitlin has added 40.00 mL of the 0.25…

Q: f. 17? If so, plain your answemaximum oxidation number for elements 11 through

A: Oxidation number for an atom indicate the number of electron it should lose or gain to obtain a…

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

4.60 g of formic acid (molar mass
46.0 g/mol) was added to a flask and
dissolved in water to make 100.00 mL
of solution. It required 40.00 mL of 2.5 M
NaOH to reach the equivalence
point. What is the pH at the equivalence
point of the titration?
K₂ = 1.77 x 10-4
a
pH = [?]
pH
Enter

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

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 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

Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
Potassium hydrogen phthalate, known as KHP (molar mass = 204.22 g/mol), can be obtained in high purity and is used to determine the concentration of solutions of strong bases by the reaction HP(aq)+OH(aq)H2O(l)+P2(aq) If a typical titration experiment begins with approximately 0.5 g KHP and has a final volume of about 100 mL, what is an appropriate indicator to use? The pKa for HP is 5.51.
Two acids, each approximately 0.01 M in concentration, are titrated separately with a strong base. The adds show the following pH values at the equivalence point: HA, pH = 9.5, and HB, pH = 8.5. (a) Which is the stronger acid, HA or HB? (b) Which of the conjugate bases, A or B, is the stronger base?
When a diprotic acid, H2A, is titrated with NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at 100.0 mL NaOH added, what volume of NaOH added corresponds to the second equivalence point? b. For the following volumes of NaOH added, list the major species present after the OH reacts completely. i. 0 mL NaOH added ii. between 0 and 100.0 mL NaOH added iii. 100.0 mL NaOH added iv. between 100.0 and 200.0 mL NaOH added v. 200.0 mL NaOH added vi. after 200.0 mL NaOH added c. If the pH at 50.0 mL NaOH added is 4.0, and the pH at 150.0 mL NaOH added is 8.0, determine the values Ka1, and Ka2 for the diprotic acid.
You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?
A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume that volumes are additive.) (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of nitric acid is required to reach the equivalence point? (d) What is the pH of the solution before any HNO3 is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?
The weak base ethanolamine. HOCH2CH2NH2, can be titrated with HCl. HOCH2CH2NH2(aq)+H3O+(aq)HOCH2CH2NH3+(aq)+H2O(l) Assume you have 25.0 mL of a 0.010 M solution of ethanolamine and titrate it with 0.0095 M HCl. (Kb for ethanolamine is 3.2 107.) (a) What is the pH of the ethanolamine solution before the titration begins? (b) What is the pH at the equivalence point? (c) What is the pH at the halfway point of the titration? (d) Which indicator in Figure 17.11 would be the best choice to detect the equivalence point? (e) Calculate the pH of the solution after adding 5.00, 10.0, 20.0, and 30.0 mL of the acid. (f) Combine the information in parts (a), (b), (c), and (e), and plot an approximate titration curve.
When 25.00 mL of HNO3 are titrated with Sr(OH)2, 58.4 mL of a 0.218 M solution are required. (a) What is the pH of HNO3 before titration? (b) What is the pH at the equivalence point? (c) Calculate [NO3-] and [Sr2+] at the equivalence point. (Assume that volumes are additive.)
A buffer is prepared by mixing 525 mL of 0.50 M formic acid, HCHO2, and 475 mL of 0.50 M sodium formate, NaCHO2. Calculate the pH. What would be the pH of 85 mL of the buffer to which 8.6 mL of 0.15 M hydrochloric acid had been added?
A solution is prepared by dissolving 0.350 g of benzoic acid, HC7H5O2, in water to make 100.0 mL of solution. A 30.00-mL sample of the solution is titrated with 0.272 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.
Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong acid HA with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: (a) After a very small volume of titrant has been added to the initial HA solution? (b) Halfway to the equivalence point? (c) When enough titrant has been added to take the solution just past the equivalence point? (d) At the equivalence point? Nanoscale representations for Question 111.
A buffer solution with it pH of 12.00 consists of Na3PO4 and Na2HPO4. The volume of solution is 200.0 mL. (a) Which component of the buffer is present in a larger amount? (b) If the concentration of Na3PO4 is 0.400 M, what mass of Na2HPO4 is present? (c) Which component of the buffer must be added to change the pH to 12.25? What mass of that component is required?