Answered: Determine the pH change when 0.075 mol…

Determine the pH change when 0.075 mol HClo, is added to 1.00 L of a buffer solution that is 0.327 M in HF and 0.368 M in F. pH after addition - pH before addition = pH change =

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 15QAP: A solution with a pH of 9.22 is prepared by adding water to 0.413 mol of KX to make 2.00 L of...

See similar textbooks

Related questions

Q: A buffer solution contains 0.373 M NaH2PO4 and 0.228 M K2HPO4. Determine the pH change when 0.048…

A: To determine the pH change when 0.048 mol HBr is added to 1.00L of a buffer solution containing…

Q: A buffer solution contains 0.329 M NaH2PO4 and 0.324 M Na2HPO4. Determine the pH change when 0.080…

A: The chemical reactions involved are:1. H2PO4^- <-> H^+ + HPO4^2-2. HCl -> H^+ + Cl^-When…

Q: A 94.0 mL sample of 0.0300 M HIO, is titrated with 0.0600 M NaOH solution. Calculate the pH after…

Q: What is the number of moles of 10.0 g NH₄Cl? What is the molar concentration of NH₄Cl? What is…

Q: Calculate the pH of the solution after the addition of each of the given amounts of 0.0530 M HNO, to…

A: We have to calculate the pH of solution

Q: A buffer solution contains 0.371 Mhydrocyanic acid and 0.449 M potassium cyanide. If 0.0218 moles of…

A: pH = pKa + log[salt]/[acid]

Q: If your lab partner misread the concentration of the sodium hydroxide solution and recorded a number…

A: Given: Lab partner misread the concentration of NaOH solution and recorded a number that was too…

Q: Consider a buffer solution that consists of two separate components: the weak acid ch3coo aq), and…

A: In the given question, buffer of weak acid and its conjugate base is given i.e., CH3COOH and…

Q: A 94.0 mL sample of 0.0300 M HIO, is titrated with 0.0600 M NaOH solution. Calculate the pH after…

Q: A 36.0 ml. sample of a 0.446 M aqueous hypochlorous acid solution is titrated with a 0.205 M aqueous…

Q: A 27.69 mL aliquot of weak acid that has a concentration of 0.648 M will be titrated with 0.33 M…

A: Since, you have posted multiple questions, we will answer the first the first one. If you want any…

Q: Example Calculate the molarity of an HCI solution if 26.4 mL of the solution neutralizes 30.0 mL of…

Q: If a buffer solution is made from 300.0 mL of 2.2 M pyridine salt mixed with 350.0 mL of 2.0 M…

A: Buffer solution pH is determined using Henderson–Hasselbalch equation. Which relates salt…

Q: Use the References to access important values if needed for this question. A buffer solution…

Q: A buffer solution contains 0.414 M NaH2PO4 and 0.226 M Na2HPO4. Determine the pH change when 0.059…

Q: Determine the pH change when 0.112 mol HCl is added to 1.00 L of a buffer solution that is 0.443 M…

Q: Determine the pH change when 0.122 mol KOH is added to 1.00 L of a buffer solution that is 0.431 M…

A: The given information is: Moles of KOH added = 0.122 mol Volume of buffer = 1.0 L Conc. of HClO =…

Q: A buffer solution contains 0.295 M acetic acid and 0.345 M sodium acetate. If 0.0443 moles of…

Q: A buffer solution contains 0.387 M NaH,PO4 and 0.212 M K,HPO4. Determine the pH change when 0.061…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: les of present in the buffer system. the solution will get slightly | The pH does not change

A: Buffer solution is the mixture of weak Acid /base with its conjugate base/acid. Buffer solution is…

Q: Determine the pH change when 0.072 mol HBr is added to 1.00 L of a buffer solution that is 0.309 M…

Q: A buffer solution contains 0.222 M hypochlorous acid and 0.318 M sodium hypochlorite. If 0.0380…

A: Given buffer solution contains: 0.222 M hypochlorous acid(HClO) and 0.318 M sodium…

Q: Which of the following combinations of chemicals makes a buffer? Mark all that apply. (Identifying…

Q: Determine the pH change when 0.063 mol KOH is adde to 1.00 L of a buffer solution that is 0.310 M in…

A: We have to calculate the change in pH

Q: Which of the following aqueous solutions are good buffer systems? O 0.27 M ammonium bromide + 0.37 M…

A: A buffer solution is a solution that changes pH only slightly when small amounts of a strong acid or…

Q: A 32.19 mL aliquot of weak base that has a concentration of 0.557 M will be titrated with 0.493 M…

A: Since you have posted multiple questions we will solve only first question for you, to get other…

Q: A buffer solution contains 0.350 M NaH₂PO4 and 0.391 M Na₂HPO4. Determine the pH change when 0.088…

A: Given,i. Molarity of NaH2PO4 =0.350 MMolarity of Na2HPO4 =0.391 MKa2 of…

Q: Comment on the shape of your graph. Thoroughly explain the chemical cause of each flat or steep…

A: The titration curve is a graph of the volume of titrant, plotted against the pH.

Q: Determine the pH change when 0.095 mol HBr is added to 1.00 L of a buffer solution that is 0.316 M…

A: 1. pH= pKa +log [ CH3C00-]/[CH3COOH] =4.75 ( Pka of acetic acid ) + log (0.319 /0.316)=4.7538

Q: The Solubility Product Constant for iron(II) sulfide is 4.9 x 10-18. The molar solubility of…

A: Since you have posted multiple questions, we will provide the solution only to the first question as…

Q: Determine the pH change when 0.070 mol HCl is added to 1.00 L of a buffer solution that is 0.345 M…

Q: Determine the pH change when 0.072 mol HNO3 is added to 1.00 L of a buffer solution that is 0.377 M…

A: we have to determine the pH change for the solution

Q: Determine the pH change when 0.077 mol HClO4 is added to 1.00 L of a buffer solution that is 0.331 M…

Q: Determine the pH change when 0.095 mol HBr is added to 1.00 L of a buffer solution that is 0.316 M…

A: Here weak acid is CH3COOH and conjugate base is CH3COO- [CH3COOH]=0.316 M , [CH3COO-]=0.319 M Moles…

Q: Determine the pH change when 0.069 mol HCIO4 is added to 1.00 L of a buffer solution that is 0.349 M…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.It is…

Q: Consider a solution that is 0.046 M HF and 0.022 M NaF. 1) What is the pH of this solution? 2) What…

A: Given: Concentration of HF = 0.046 M And concentration of NaF = 0.022 M

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

Determine the pH change when 0.075 mol HClo, is added to 1.00 L of a buffer solution that is 0.327 M in HF and 0.368 M in F.
pH after addition - pH before addition = pH change =

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

A solution with a pH of 9.22 is prepared by adding water to 0.413 mol of KX to make 2.00 L of solution. What is the pH of the solution after 0.368 mol of HX 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?
Calculate the pH of these buffers.
Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
Sulfanilic acid (NH2C6H4SO3H) is used in manufacturing dyes. It ionizes in water according to the equilibrium equation NH2C6H4SO3H(aq)+H2O(l)NH2C6H4SO3(aq)+H3O+(aq)Ka=5.9104 A buffer is prepared by dissolving 0.20 mol of sulfanilicacid and 0.13 mol of sodium sulfanilate (NaNH2C6H4SO3) in water and diluting to 1.00 L. Compute the pH of the solution. Suppose 0.040 mol of HCl is added to the buffer.Calculate the pH of the solution that results.
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.
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.
7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?
A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
Which of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00? Explain your reasons: formic acid, lactic acid, nitrous acid.