6-Calculate the pH of a H2PO4-/ HPO42- buffer in which the concentration of the weak acid component is 0.130M and the concentration of the conjugate base is 0.026M НЗРО4 Ka 7.1 x 103 6.3 x 108 4.5 x 1013 1st 2nd 3rd

6-Calculate the pH of a H2PO4-/ HPO42- buffer in which the concentration of the weak acid component is 0.130M and the concentration of the conjugate base is 0.026M НЗРО4 Ka 7.1 x 103 6.3 x 108 4.5 x 1013 1st 2nd 3rd

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.126EP: What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base?...

See similar textbooks

Related questions

Q: Calculate the pH of the above buffer after 10.00 mL of 1.000 M NaOH (0.01000 mol OH-1) was added to…

A: Here we are required to find the pH of the buffer solution after addition of 10 ml of 1M NaOH.

Q: 40. If you add 8.0 mL of 0.10 M HCl to 25 mL lactic acid/lactate buffer that is 0.10 M lactic acid…

Q: 12. Assuming equal concentrations of conjugate base and acid, which of the following mixtures is…

Q: Calculate the pH of an acetic acid/acetate ion buffer with the following concentrations: acetic acid…

A: Note - Since you have asked multiple question, we will solve the first question for you. If you…

Q: What is the pH of a buffer solution in which the molar concentration of acetic acid is 0.15M and the…

Q: What is the pH of a buffer made with NH3 ( 0.200M) and NH4Cl (0.300M). Ka NH4+ = 5.68 x 10 -10 (…

Q: Consider a buffer solution contains 0.50 M NaF and 0.60 M HF: (Ka (HF) = 5.0 x 10-4 What is the pH…

Q: Calculate the pH of a solution that is 0.200 M in NH3 and 0.300 M in NH4Cl. Calculate the pH change…

A: Answer: Henderson-hasslebalch equation will be used to calculate the pH of basic buffer solution and…

Q: What is the PH of a buffer system that is 0.200 M hydrocyanic acid (HCN) and 0.120 M sodium cyanide…

A: Given: The concentration of acid, [HCN]= 0.200 M The concentration of salt, [NaCN]=0.120 M…

Q: What is the pH of a buffer that is 0.153 M in a weak acid and 0.227 M in the acid's conjugate base?…

A: Weak Acid concentration = 0.153 M. Conjugate base Concentration = 0.227 M. Ka = 5.7 × 10-4 pKa = -…

Q: A student must make a buffer solution with a pH of 4.50. Determine which weak acid is the best…

A: Concept: Buffer solution: A buffer solution (more precisely, pH buffer or hydrogen ion buffer) is…

Q: Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium…

A: Henderson - Hasselbach equation enables the calculation of pH of a buffer solution made by mixing…

Q: 2. Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is…

Q: 3. What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acid's conjugate…

A: Given that: Concentration of weak acid [HA] = 0.175M [A-] = 0.200M Ka = 5.7×10-4

Q: A student must make a buffer solution with a pH of 2.00. Determine which weak acid is the best…

A: A buffer works best at a pH closer to the pKa value of the acid. Closer the pKa value of the acid to…

Q: Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH…

Q: 5. Which of the following buffer solutions prepared by mixing HCOOH (formic acid) and HCOONA (sodium…

A: Ka = 1.8 × 10-4

Q: Calculate the pH of a base buffer solution composed of 0.20 M NH3 and 0.15 M NH4Cl after the…

A: The formula to calculate the pH of the solution is, pOH+pH=14pH=14-pOH Given, The concentration of…

Q: 5. What is the pH at the equivalence point if it requires 32.50 mL of 0.1500 M KOH to completely…

A: According to Le Chatelier’s principle, “When a system experiences any disturbance in the equilibrium…

Q: Calculate the pH of a buffer that is 0.040 M HA and 0.020 M NaA. HA is a weak acid and its K a is…

Q: A buffer is prepared by adding 150mL of KOH 1.00M to 250mL of H2PO4 1.00M. Calculate the moles of…

A: In the given question we have to calculate the mole of HCl that will be addade to this system to…

Q: A student must make a buffer solution with a pH of 3.00. Determine which weak acid is the best…

Q: The hydronium ion concentration in a buffer solution consists of 0.400 M formic acid and 1.00 sodium…

Q: Which of the following acids is the best choice to prepare a buffer at pH 9.4 when paired with their…

A: The value of pH for titration of weak acid with strong base is calculated by Henderson-Hasselbalch…

Q: If the Ka of a weak acid is 4.89 x 10-4, then what would the pH of a buffer system be if equal…

A: Please find the attachment.

Q: 4. You need to make a buffer with pH as close to 10.00 as possible. Two sets of weak acids and…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: What is the pH of a buffer that is 0.185 M in a weak acid and 0.227 M in the acid's conjugate base?…

A: Henderson-Hasselbach equation shows the relationship between pH of a solution, the acid dissociation…

Q: 11) Choose the acid below that would make the most effective buffer for a solution to maintain a pH…

A: The solution is given below -

Q: Which of the following acids (listed with Ka values) and their conjugate base would form a buffer…

A: We have to identify which of the below given acids and their conjugate base would form a buffer with…

Q: you add 1.00 mL of 1.00 M HCl to 100.0 mL of buffer solution that is 0.100 M acetic acid and 0.100 M…

A: Given-> Volume of HCl = 1.00 ml Molarity of HCl = 1.00 M Volume of buffer = 100.0 ml Molarity of…

Q: Formic acid, HFor, has a Ka value of 1.8 x 10^-4. You need to prepare a buffer having a pH of 3.25…

Q: You have 500.0 mL of a buffer solution containing 0.250 M acetic acid (CH₃COOH) and 0.240 M sodium…

Q: Lactic acid is mainly produced in muscle cells as an alternative source of energy. Determine the pH…

Q: From the following choose the most appropriate weak base (when added to its conjugate acid) for…

A: Solution

Q: Consider a titration of formic acid (HCOOH, Ka = 1.8 x 10-4) with KOH in water. If 40.00 mL of the…

A: Given that the volume of KOH require at equivalence point is 40.00 mL. Therefore, 20.00 mL of KOH is…

Q: Which weak acid would be best to use when preparing a buffer solution with a pH of 9.1? An acid with…

A: Given: The pH value is 9.1

Q: 1- Calculate the pH of 0.1 M KHCO3.

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: 5- A mixture of 0.123 M NH4CI and 0.246 M NH4OH has volume of 20 mL, calculate its pH value. 1 mL of…

A: The pH value indicates the solution's acidity and basicity. It distinguishes between strong acid and…

Q: If the dissociation constant of a weak acid is 8.1 x 100, at what ratio should you adjust the…

Q: Describe how you will prepare a phosphate buffer (250 mL, 0.0125 M) with a pH of 6.5 from a 0.500 M…

A: Topic- Preparation of Phosphate buffer solution

Q: The hydronium ion concentration in a buffer solution consists of 0.200 M formic acid and 1.00 sodium…

A: We are given a buffer solution of formic acid and Sodium formate. We have to find the concentration…

Q: A chemistry student is asked to maked a buffer of pH = 4.0. Which of the following acids would be…

Q: 1. Calculate the pH of buffers that contain the acid and conjugate base in following concentrations:…

A: Buffer are solution which will resist the change in any pH when bases and /or acid are added…

Q: Determine the pH of a buffer solution made up of 0.500 M of NH3 and 0.456 M of NH4. The Kb is 1.82 x…

Q: 9 If the dissociation constant of a weak acid is 1.4 x 10-5, at what ratio should you adjust the…

A: Dissociation constant of a weak acid is 1.4 ×10–5. Given some ratios of concentration of weak acid…

Q: Which is true about buffer solutions? -they hold the pH close to the pKa -they contain comparable…

A: Buffer solution- It is a chemical added during chemical reaction for control of pH of reaction. For…

Q: Which of the following conjugate acid-base pair would you choose to prepare a buffer solution that…

A: Buffer is a solution that resists the change in pH when small amount of acid or base is added to it.…

Q: What is the pH of a buffer that is 0.174 M in a weak acid and 0.207 M in the acid's conjugate base?…

A: Henderson Hasselbalch equation would be used to calculate the pH of buffer solution

Q: What is the pH of a buffer that is 0.160 M in a weak acid and 0.217 M in the acid's conjugate base?…

A: Given data Concentration of weak acid = 0.160 M Concentration of conjugate base = 0.217 M Ionization…

Q: pH

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

6-Calculate the pH of a H2PO4-/ HPO42- buffer in which the concentration of
the weak acid component is 0.130M and the concentration of the conjugate base
is 0.026M
НЗРО4
Ka
1st
2nd
7.1 x 103
6.3 x 108
4.5 x 10-13
3rd
7.20
6.50
O 7.90
O 7

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 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

A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.
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.
Determine the dominant acid-base equilibrium that results when each of the following pairs of solutions is mixed. Indicate the equilibrium by writing 1 for a strong acid, 3 for a weak acid, 4 for an acidic buffer, 7 for a neutral solution, 10 for a basic buffer, 11 for a weak base, and 13 for a strong base. (a) 10.0 mL of 0.15 M NaOH + 15.0 mL of 0.10 M HNO3 (b) 25.0 mL of 0.10 M HCl + 10.0 mL of 0.25 M NH3 (c) 50.0 mL of 0.050 M NaOH + 50.0 mL of 0.10 M NH3 (d) 50.0 mL of 0.10 M NH3 + 50.0 mL of 0.05 M HCl
Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
2. If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? 100. mL 50. mL 36 mL 18 mL
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
Calculate the pH change when 10.0 mL of 0.100-M NaOH is added to 90.0 mL pure water, and compare the pH change with that when the same amount of NaOH solution is added to 90.0 mL of a buffer consisting of 1.00-M NH3 and 1.00-M NH4Cl. Assume that the volumes are additive. Kb of NH3 = 1.8 × 10-5.
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.