### Problem 6: Titration of HCl with NaOH**Task:** Calculate the pH of a solution during a titration of 2.5M HCl with 35mL of 1.25M NaOH.#### Part A: 12mL of HCl#### Part B: 30mL of HCl#### Part C: Equivalence PointHow many mL of HCl are needed to reach the equivalence point?---To solve these problems, one needs to understand the principles of acid-base titration and the concept of equivalence point—where moles of acid equal moles of base. The pH at different stages of titration can be determined using stoichiometry and the properties of the substances involved.#### Steps to Solve:1. **Determine the moles of NaOH and HCl used**: - Moles of NaOH = Volume (L) × Molarity (M) - Moles of HCl = Volume (L) × Molarity (M)2. **Calculate the point at which equivalence is reached** (Acid moles = Base moles).3. **For Part A & B**: - Determine the remaining moles of acid/base after neutralization. - Calculate the concentration of H+ or OH- ions. - Use the concentration to find the pH or pOH (and convert as necessary to find pH if needed).4. **For Part C**: - Set the moles of NaOH equal to the moles of HCl and solve for the volume of HCl.---This method will ensure a comprehensive understanding of titration calculations and the specific points along the titration curve.

Given: The molarity of HCl = 2.5 M The molarity of NaOH = 1.25 M The volume of NaOH = 35 mL

Answered: 6. Calculate the pH of a solution…

6. Calculate the pH of a solution during a titration of 2.5M HCI with 35mL of 1.25M NaOH A. 12mL of HCI? B. 30mL of HCI? C. How many mL of HCl are needed to reach the equivalence point?

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: Consider the titration of 50.0 mL of 0.250 M HF (Ka = 6.6 x 10^-4) with 0.250 M NaOH. Calculate the…

A: Answer:- This question is answered by using the simple concept of calculation of pH of weak acid…

Q: The pH at the equivalence point of a solution differs for each type of titration. The highest pH at…

A: pH of base is above 7 while pH of acid is below 7.

Q: 15. Which of the following statements is TRUE of the titration of a weak monoprotic acid by a strong…

A: answer- the true statement is option c . the moles of base is greater than the moles of acid at the…

Q: Consider the titration of a 25.0-mL sample of 0.175 M CH;NH2 with 0.150 M HBr. Determine each…

A: Since you have posted multiple sub-parts, the answer for first three sub-parts are given below.…

Q: A student titrates 50.0 mL of an unknown concentration of HI with 85 mL of a 1.0 M solution of NaOH…

A: Given -> Volume of HI = 50.0 ml = V1 Volume of NaOH = 85 ml = V2 Molarity of NaOH = 1.0 M = M2…

Q: 9. What can be Statement can be TRUE about acidic buffer? a. It is made ofa mixture odf strong acid…

A: According to the our policy we should solve one question if any subparts present then first three…

Q: titrated with 0.220 M KOH. 1. titular agent: 2. reaction between acid and base: 3. what is the pH…

A: The titular agent is KOH. Titrant is a solution of known concentration that is added to analyte to…

Q: 75.0 mL of a 0.15 M solution of N2OH is titrated with 0.25 M HC1. After 45.0 mL of the HC1 has been…

A: Provided volume of NaOH 75ml Or, Volume (V1) of NaOH= 0.075litre Molarity (M1) of NaOH=0.15M…

Q: 31.1 mL sample of a 0.190 M solution of NaCN is titrated by 0.230 M HCl. Kb for is CN- is…

A: The question is based on the concept of titrations. we are titrating a weak base with a strong…

Q: Which of the following mixtures would result in a buffered solution when 1.0 L of each of the two…

A: (A) HNO3 is a strong base, whereas HF is also an acid. Hence, it will not form a buffer solution.

Q: A chemist titrates 20.0 mL of 0.20 M HBRO (see Appendix) with 0.10 M NaOH. What is the pH: a) before…

Q: 20. A solution containing which one of the following pairs of substances will be a buffer solution?…

A: A mixture of weak acid and its conjugate ion with strong base forms an acidic buffer solution. A…

Q: . calculate the pH of the solution when an additional 5.0 mL of potassium hydroxide has been added;…

A: The question is based on the concept of titrations. we are titrating a weak acid with a strong base.…

Q: What is the unknown concentration of a 25 ml HCl sample that requires 40 ml of 0.45M NaOH to reach…

A: Given Volume of HCl (V1) = 25 mL Volume of NaOH (V2) = 40 mL Molarity of NaOH (M2)…

Q: 20.0mL sample of 0.030M formic acid is titrated with 0.015M KOH solution. What is the pH at the…

Q: • 0.200 M of 1.0L methyl amine (CH3NH2), a weak base was titrated with 0.1 M HCl. pK of methyl amine…

A: To address this problem, we need to analyze each statement based on the titration setup:1. **0.200 M…

Q: 25.0 mL of 0.10 M CH3NH2 solution is titrated with 0.10 HCl solution. Find pH of the solution: a)…

A: We will calculate pH for each of the scenarios. We will use Henderson Hesselbalch equation in the…

Q: Determine whether the mixing of each pair of solutions results in a buffer. a) 50.0 mL of 0.10 M…

A: Only ones solution results in buffer

Q: Which of the following would be best for a buffer with a pH of 7.5? a. HF/F- b. H3PO4/H2PO4- c.…

A: The pH of the buffer given is 7.5.

Q: Calculate the pH at the following points in the titration of 20.00 ml of 0.350 M HBr with 0.350 M…

A: The solution is as follows:

Q: NaHSO3 has a pKa of 7.21. 35.00 mL of 0.100M NaHSO3 are titrated with 0.150 M NaOH. How many mL of…

A: NaHSO3 is an amphoteric salt made from weak dibasic acid and strong base. NaHSO3→H2SO3 +NaOHNaHSO3…

Q: 2. Calculate the pH at each stage in the titration for the addition of 0.110 M HCL to 35.0 mL of…

Q: 6. Calculate the pH of a solution during a titration of 2.5M HCI with 35mL of 1.25M NaOH A. 12mL of…

Q: Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid, Ka = 4.9 x 10-5, with…

A: The relation for ionic product of water is as follows, Kw = Ka × Kb The…

Q: You are titrating 50 mL of 0.100 M HF with 0.050 M NaOH. What is the pH after: a. 50 mL of NaOH…

A: Since we know that pH = - log [H+] From given solution first of all we find the concentration of…

Q: 9. Which point in titration is it where the added titrant is chemically equivalent to the amount of…

A: Titration is a method of quantitatively chemical analysis in which a solution of known concentration…

Q: At the equivalence point of a strong acid-strong base titration, the resulting solution will be a.…

Q: 10. A 30 ml sample of 0.200 M HCN(aq) (Ka= 6.2 x 10-1º) is being titrated with 0.100 KOH(aq).…

A: In multiple subparts, we solve only first three subparts according to the Bartleby guidelines. Find…

Q: A 500 mL buffer solution is 0.1 M in HNO2 and 0.150 M in KNO2. Determine if each addition would…

A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…

Q: Consider the titration of a 23.0 – mL sample of 0.110 M HC2H3O2 with 0.13o M NaOH. Determine each of…

Q: A 50 mL solution of 0.08 M KCN (aq) is titrated with 0.125 M HCl (aq). Calculate the pH at the…

Q: QUESTION 4 a conjugate acid-base pair. Select the pair of substances which is not OA HF/F O B.…

Q: Answer questions a through c: a. Explain the difference between the end point and the equivalence…

A: Titration is a process that is majorly used in the laboratory to identify the unknown concentration…

Q: exactly 25ml of 0.01 hcl was taken diluted with sufficient quantity of water to measure 250 ml and…

A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Q: Consider the titration of 100.0 mL of 0.200 M CH3NH2 by 0.100 M HCl. Calculate the pH for through…

Q: 40.00 mL of 0.09M NaOH is diluted to 100 mL and titrated with 0.1M HCl. Calculate the pH after the…

Q: A strong acid is titrated with a strong base. Which of the following pH values can be determined…

A: In an acid-base titration, an acid reacts with a base to form a salt and water. The main purpose of…

Q: What weight of sodium formate must be added to 400.0 mL of 1.00 M formic acid to produce a buffer…

A: Formic acid and sodium formate form buffer solution

Q: A 1.0-L buffer solution is 0.125 M in HNO2 and 0.195 M in NaNO2 . A: Determine the concentrations…

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

### Problem 6: Titration of HCl with NaOH

**Task:** Calculate the pH of a solution during a titration of 2.5M HCl with 35mL of 1.25M NaOH.

#### Part A: 12mL of HCl

#### Part B: 30mL of HCl

#### Part C: Equivalence Point
How many mL of HCl are needed to reach the equivalence point?

---

To solve these problems, one needs to understand the principles of acid-base titration and the concept of equivalence point—where moles of acid equal moles of base. The pH at different stages of titration can be determined using stoichiometry and the properties of the substances involved.

#### Steps to Solve:
1. **Determine the moles of NaOH and HCl used**:
- Moles of NaOH = Volume (L) × Molarity (M)
- Moles of HCl = Volume (L) × Molarity (M)

2. **Calculate the point at which equivalence is reached** (Acid moles = Base moles).

3. **For Part A & B**:
- Determine the remaining moles of acid/base after neutralization.
- Calculate the concentration of H+ or OH- ions.
- Use the concentration to find the pH or pOH (and convert as necessary to find pH if needed).

4. **For Part C**:
- Set the moles of NaOH equal to the moles of HCl and solve for the volume of HCl.

---

This method will ensure a comprehensive understanding of titration calculations and the specific points along the titration curve.

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 5

Step 6

Step 7

Step 8

Step 9

Step by step

Solved in 9 steps

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

We used 0.001M of HCl
Determine the pH during the titration of 14.4 mL of 0.130 M perchloric acid by 7.26E-2 M sodium hydroxide at the following points:a. Before the addition of any sodium hydroxide b. After the addition of 12.9 mL of sodium hydroxide c. At the equivalence point d. After adding 33.5 mL of sodium hydroxide
4. A 25ml of 0.01M NAOH was titrated with 0.01M HCI. Calculate the pH at: a) The start before HCl was added b) 15ml of HCl was added c) 25ml of HCl was added d) 30ml of HCl was added
nave *16.46. In an alkalinity titration of a 100.0 mL sample of re from a hot spring, 2.56 mL of a 0.0355 M solution of HCl is needed to reach the first equivalence point (pH = 8.3) and another 10.42 mL is needed to reach the second equivalence point (pH = 4.0). If the alkalinity of the spring water is due only to the presence of carbonate and bicarbonate, what are the concentrations of each? of of O2
What is the unknown concentration of a 25 ml HCI sample that requires 40 ml of 0.45M NaOH to reach the equivalence point in a * ?titration
71. Consider the titration of a 20.0-mL sample of 0.105 M HC,H;O2 with 0.125 M NaOH. Determine each quantity. a. the initial pH b. the volume of added base required to reach the equivalence point c. the pH at 5.0 mL of added base d. the pH at one-half of the equivalence point e. the pH at the equivalence point f. the pH after adding 5.0 mL of base beyond the equivalence point
A 5.36–g sample of NH4Cl was added to 25.0 mL of 1.00 M NaOH and the resulting solution diluted to 0.100 L. a. What is the pH of this buffer solution? b. Is the solution acidic or basic? c. What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to the solution?
Pls help me !! A 150.0 mL sample of 0.21 M HF is titrated with 0.50 M NaOH. Determine the pH at these points: a.At the beginning (before base is added) b.After adding 40.0 mL of NaOH After adding c.63.0 mL of NaOH 9
4. Calculate the pH at each point of a titration where 30.0 ml of 0.25M HNO3 are titrated with the following volumes of 0.15M LiOH. a. 15.0ml b. 25.0ml c. 50.0ml d. 60.0ml
HF is being titrated with NaOH. The equivalence point of this titration would be а. acidic b. basic C. neutral
9. What can be Statement can be TRUE about acidic buffer? a. It is made of a mixture odf strong acid and salt of its conjugate acid b. Concentration of hydrogen ions in acidic buffer is greater than concentration of OH ions which is present in the solution c. Dilution of buffer by adding large amount of water doesnt change the pH of buffer solution d. Acidic buffer usually works effectively at pH range of above 7 10. A buffer solution is made of mixture of aqueous methanoic acid.HCOOH. With aqueous sodium methanoate acid NAHCOO. The equilibrium reaction takes place in buffer solution is: УНСООН HCOO+ H* Small amount of NaOH is then added to that buffer solution. What reaction take places at the buffer solution to resist change of pH caused by addition of base?| а. НСООН +H* НСООН, b. НCОО-+ H* НСООН с. НСООН +ЮН" HCOO+H2O d. HCOOH +ОН" НСООН
What is the pH of a buffer made by combining 45 ml of 0.15M nitrous acid and 20 ml of 0.175 M sodium nitrite a. 3.43 b. 3.64 c. 3.28 d. 3.06