Answered: Find the ph at each of the following…

Find the ph at each of the following points in the titration of 25mL of .05 M HClO with .05 M NaOH the Ka is 2.9x10^-8 1. The Intial PH 2. After adding 10ml of .05M NaOH

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.7QAP

See similar textbooks

Related questions

Q: An ammonia buffer contains 0.4 moles of ammonia and 0.6 moles of NH4+ ION. PKa is 9.25. what will be…

A: Given: Moles of NH3 = 0.4 moles Moles of NH4+ = 0.6 moles pKa of NH3 = 9.25 So we have to determine…

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: In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one…

A: Given: Weak base = 0.0200 M Volume of weak base = 50.0 mL Concentration of base = 0.0150 M pKb of…

Q: Consider the following reaction: CH3 COOH + OH- -----> CH3COO- + H2O How much 5.90M NaOH must be…

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 20.0 mL sample of 0.20 M HCl is titrated with 0.10 M KOH. What is the pH at the equivalance point…

A: Given: Titration of HCl using KOH.

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

Q: An unidentified weak acid, HA, has a pK, of 4.75. A 30.0 mL sample of 0.20 M HA is titrated with…

Q: Consider the titration of 40.00 mL 0.200 M NaOH with 0.250 M HF and calculate the pH after each of…

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: Determine the pH during the titration of 26.7 mL of 0.305 M benzoic acid ( Ka = 6.3\times 10 - 5) by…

A: The objective of this question is to calculate the pH at different points during the titration of…

Q: Consider the following reaction: CH3 COOH + OH- -----> CH3COO- + H2O How much 5.90M NaOH must be…

A: CH3 COOH + OH- -----> CH3COO- + H2O

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: Draw the titration curves for the titrations of (a) a strong acid with a strong base, (b) a strong…

A: In the titration curve of acid-base titration, the information about the concentration of acid or…

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…

Q: Calculate the pH of a buffer solution that contains 0.76 M NaH2PO4 and 0.28M Na2HPO4. Calculate…

A: The equilibrium reaction can be represented as,

Q: 20mL of a 0.200M unknown acid is titrated with NaOH. After 15mL of 0.100M NaOH, the pH is 6.1. What…

A: Given,Molarity of unknown acid = 0.200 Mvolume of acid = 20 mLMolarity of NaOH = 0.100 MVolume of…

Q: Consider the titration of 80.0 mL of 0.100 MBa (OH), by 0.400 MHCI, Calculate the pH of the…

Q: Consider the titration of 50.0 mL of 0.134 M HNO3 with 0.0500 M KOH. What is the initial pH of HNO3…

A: pH = -log [H3O+]

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200M H2NNH2 with 0.100 M HNO: after…

A: Given: volume of NH2NH2 = 40.0 mL Molarity of NH2NH2 = 0.200 M volume of HNO3 = 80.0 mL Molarity of…

Q: (b) Shown in the graph below is the titration curve that results when 25.0 mL of 0.200 M HCIO is…

A: pH metric titrations are used to calculate the unknown concentration of solutions of acid or base.…

Q: Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after…

A: a)pH after 4ml addition of HBr:

Q: 50.0 mL of 0.150 M HNO2 is titrated to its equivalence point with 1.00 M NaOH. What is the pH at…

Q: Why is the titration curve steepest at the equivalence point?

A: Equivalence point in the titration curve: It is the point in the titration at which the analyte…

Q: 69 mL of.125 M solution of an acid HA is titrated with .125 m solution of NaOH calculate the PH at…

Q: A titration of 79.0 mL of a tartaric acid (H2C4H4O6) solution of unknown concentration with .805 M…

A: The volume of the tartaric acid solution = 79.0 mLThe volume of the solution = 32.0 mLThe…

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

Find the ph at each of the following points in the titration of 25mL of .05 M HClO with .05 M NaOH the Ka is 2.9x10^-8

1. The Intial PH

2. After adding 10ml of .05M NaOH

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: INTRODUCTION

VIEW

Step 2: pH of weak acid.

VIEW

Step 3: pH of the solution in 2nd case.

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 2 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

When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
The species called glacial acetic acid is 98% acetic acid by mass (d=1.0542g/mL). What volume of glacial acetic acid must be added to 100.0 mL of 1.25 M NaOH to give a buffer with a pH of 4.20?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
The titration of 0.100 M acetic acid with 0.100 M NaOH is described in the text. What is the pH of the solution when 35.0 mL of the base has been added to 100.0 mL of 0.100 M acetic acid?
A 0.400-g sample of propionic acid was dissolved in water to give 50.0 mL of solution. This solution was titrated with 0.150 M NaOH. What was the pH of the solution when the equivalence point was reached?
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
How much solid NaCH3CO23H2O must be added to 0300 L of a 0.50-M acetic acid solution to give a buffer with a pH of 5.00? (Him: Assume a negligible change in volume as the solid is added.)
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.