A 1.00 L phosphate buffer solution that contains 0.1270 moles of dihydrogen phosphate (H2PO4) and 0.0800 moles of hydrogen phosphate (HPO,2-) was prepared. The pKa of dihydrogen phosphate is 7.20 at 25 °C. Calculate the pH of the buffer at this temperature.

A 1.00 L phosphate buffer solution that contains 0.1270 moles of dihydrogen phosphate (H2PO4) and 0.0800 moles of hydrogen phosphate (HPO,2-) was prepared. The pKa of dihydrogen phosphate is 7.20 at 25 °C. Calculate the pH of the buffer at this temperature.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 106GQ: The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106....

See similar textbooks

Related questions

Q: What is the pH when 25% of the acid H3AsO4 (pKa = 2.22) has reacted with NaOH in a titration?

A: The reaction of H3AsO4 with NaOH results in the conversion of 25% of the acid into its conjugate…

Q: A buffer solution is made using a weak acid, HA, that has a pK, of 5. If the pH of the buffer is 6,…

A: Given :- pH of the buffer solution = 6 pKa of acid = 5 To calculate :- [A-]/[HA]

Q: A buffer solution is 0.100 M in both HC¬H5O2 and LICH5O2 and has a pH of 4.19. Which of the…

A: Buffer solution is the solution which resist change in pH on addition of small amount of acid and…

Q: A buffer is created by adding 0.321 moles of bromoacetic acid (pKa = 2.902) and 0.555 moles of…

A: Given that : Moles of acid (bromoacetic acid) = 0.321 moles Moles of salt (sodium bromoacetate) =…

Q: A buffer solution is prepared by dissolving 1.0 mole of the weak acid CH3COOH (pKa = 4.74) and 1.0…

A: The initial pH of the buffer can be calculated as follows-

Q: buffer of pH = 7.5 is desired. Which two of the following compounds should be dissolved in water in…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: The concentration of fluoride ions in a saturated solution of barium fluoride is M. The solubility…

Q: What is the pH of a buffer that is 0.140 M in formic acid (HCHO2) and 0.010 M in potassium formate…

A: Given: [Acid] = 0.140 M [Salt] = 0.010 M Ka = 1.8 * 10-4 We have to calculate pH of buffer…

Q: The molar solubility of sulfathiazole (pKa 7.2) is 0.001 M. What is precipitation pH or least…

A: Given :- pKa of sulfathiazole = 7.2 Molar solubility of sulfathiazole = 0.001 M We have calculate…

Q: Determine the molar solubility of phosphate in Zn(OH)2 (Ksp = 1.8 x 10-14) in a solution of 0.025 M…

Q: A buffer solution is made using a weak acid, HA, that has a pK, of 4. If the pH of the buffer is 1,…

Q: A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in…

Q: pka = 1.95 (HClO2) If you have 500 mL of a 0.10 M solution of the acid, what mass of the…

A: pH of buffer solution is calculated by using Henderson Hassel balch equation

Q: Calculate the buffer capacity of a buffer solution prepared by mixing 0.215M sodium acetate and…

A: Given = Concentration of sodium acetate = 0.215M Conc of acetic acid = 0.125M pKa = 4.76

Q: 134 grams of potassium sorbate KCH3 (CH)4CO2 is fully dissolved in 100.00 mL of water, which is…

Q: 9. If 6.2 mL of 0.0160 M KOH solution must be added to 5.0 mL of 0.240 M CaCl₂ solution to just form…

A: Solubility product is the multiplication of molar solubility of the constituent ions of the…

Q: Suppose you have a buffer, comprised of 0.350 mol of weak base and 0.250 mol of weak acid. Ifthe pH…

A: The of a buffer solution can be calculated using Henderson Hasselbalch Equation written as follows:…

Q: If a 50.00 mL sample of 0.127 M nitrous acid is titrated with 17.55 mL of 0.102 M NaOH, what is the…

Q: What is the concentration of a lactic acid buffer (pK = 3.9) that contains 0.25M CH3CH(OH)COOH and…

A: pH = pKa + log salt / acid

Q: Determine the pH at the equivalence (stoichiometric) point in the titration of 44.27 mL of 0.138 M…

A: Given data : Concentration of morphine = 0.138 M Volume of morphine = 44.27 mL Concentration of HCl…

Q: A buffer solution with a pH of 4,9, consists of 0,25 mol∙dm–3 acetic acid (HC2H3O2; Ka= 1,8 x 10–5)…

Q: What is the pH of a buffer solution containing 1.0 M hypochlorous acid (HClO, KA = 3.0 × 10^-8) and…

A: We can use Henderson-Hasselbalch equation which for a buffer solution that consists of weak acid and…

Q: Calculate the solubility of aluminum hydroxide, Al(OH)3, in a solution buffered at pH 11.00.

A: Solubility product, Ksp of Al(OH)3 is 1.9×10-33. pH of the solution = 11.00 pOH of the solution = 14…

Q: You have a solution that contains acetic acid, (CH3COOH or HAc). The concentration of acetic acid in…

Q: Calculate the molar solubility of aluminum hydroxide, Al(OH),, in a solution buffered at pH 12.00 Kp…

Q: What is the pH of a buffer solution that contains 0.25 M HClO and 0.35 M NaClO? (pKa HClO = 7.46)…

Q: Calculate the molar solubility of cobalt (III) hydroxide in a solution buffered at pH = 3.00…

A: Given, pH = 3.00 and , Ksp = 1.6×10–44 We know that, for a buffered solution , it resist any…

Q: A buffer solution containing 0.19 M methylammonium and 0.22 M of the conjugate base, methylamine,…

A: Answer: option c. 10.70 is the pH of the buffer solution

Q: Write the relevant chemical reaction and mass-balance expression for 0.1 M NaCl and 0.1 M NaH2PO4.

A: Sodium Dihydrogen Phosphate + Sodium Chloride = Nahpoite + Hydrogen Chloride 0.1 M of aqueous Sodium…

Q: What is the pH of the solution when 20.0 mL of 0.155 M of NH3(ag) is titrated with 15.0 mL of 0.225…

Q: The alkalinity of verde river is 250mg CaCo3/L. Calculate the molar concentration of the following…

A: Alkalinity refers to the ability of a solution to react and neutralize the acids in the water.…

Q: Calculate the pH of a solution of magnesium hydroxide, Mg(OH)2 (Ksp = 5.6 × 10−12), made by…

A: Solubility Product : For a sparingly soluble salt , the product of Solubility (mol/lit) of all the…

Q: Calculate the molar solubility of manganese hydroxide in a solution buffered at pH = 11.50. Mn(OH)2…

Q: A buffer solution was made by dissolving 10 g of sodium acetate (CH3COONa) in 100 ml of 1.0 M Acetic…

Q: A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in…

A: Buffer solution - A solution whose pH is not altered to any great extent by the addition of small…

Q: What is the solubility of magnesium hydroxide in a solution buffered at pH 8.95? K„ (Mg(OH)2) = 1.8…

A: Concentration of OH- can be calculated as follows:

Q: At 25C, 7.8 x 10^-5 mol of silver chromate dissolves in one liter of water. Write a balanced…

A: Given :- Moles of Silver chromate, Ag2CrO4 = 7.8×10-5 mol Volume of water (solution) = 1 L…

Q: Lakes have a natural buffering capacity, especially in regions where limestone gives rise to…

A: Sulphuric acid in the lake contains H3O+ ions. when acid rain falls in the lake that contains…

Q: A buffer solution is 0.100 M in both HC7H5O2 and LIC7H5O2 and has a pH of 4.19. Which of the…

A: The buffer solution is that can resist the small change in PH by the addition of acid or base.

Q: You have prepared an acetic acid buffer solution (pKa = 4.76) containing 0.1 mole each of acetic…

A: A buffer solution is prepared by mixing 0.1 mole each of the acetic acid and sodium acetate. Now…

Q: Calculate the molar solubility of Fe(OH); (K-p = 2.79 x 10 3) in a %3D solution that is buffered at…

A: The molar solubility of a compound is defined as the number of moles of solute dissolved in per…

Q: You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization…

A: Applying similar concept of kw and pH as like water because it also involves in auto ionisation like…

Q: From titrating a sample of saturated Ca(OH)2 solution at 25 °C, it is found to have a OH–…

A: The dissociation reaction of calcium hydroxide is written below. Ca(OH)2 → Ca2+ + 2OH- The…

Q: Aniline, C6H7N (molar mass = 93.13 g/mol), is a weak base that is used as a precursor in the…

A: 924 mg of aniline is dissolved in enough water to make a total volume of 1.00 L. pKb of aniline…

Q: pH of the buffer after the addition of the NaOH

A: pKa(CH3COOH) = 4.74 Moles = M × V (L) Moles of Acetic acid = M × V(L) = 0.281 × 0.300 =…

Q: Write a balanced net ionic equation to show why the solubility of Zn(CN)2(s) increases in the…

Q: A buffer is made by adding 0.18 mol/L of sodium propanoate (NaPr) to 0.12 mol/L solution of…

A: All solutions hold specific characteristics in pH value terms. This value describes how acidic or…

Q: molar solubility

Q: Aniline, C6H7N (molar mass = 93.13 g/mol), is a weak base that is used as a precursor in the…

A: The solution is given below -

Question

A 1.00 L phosphate buffer solution that contains 0.1270 moles of dihydrogen phosphate (H2PO4) and 0.0800 moles of
hydrogen phosphate (HPO,2-) was prepared. The pKa of dihydrogen phosphate is 7.20 at 25 °C.
Calculate the pH of the buffer at this temperature.

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 3 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Apatite, Ca5(PO4)3OH, is the mineral in teeth. On a chemical basis explain why drinking milk strengthens young children’s teeth. Sour milk contains lactic acid. Not removing sour milk from the teeth of young children can lead to tooth decay. Use chemical principles to explain why.
Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ion
What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 105)? What is the pH of the solution?
During the fermentation of wine, a buffer system consisting of tartaric acid and potassium hydrogen tartrate is produced by a biochemical reaction. Assuming that at some time the concentration of potassium hydrogen tartrate is twice that of tartaric acid, calculate the pH of the wine. The pKa of tartaric acid is 2.96.
The primary buffer in the blood is carbonate-bicarbonate buffer. If the pKa is 6.1 and the pH is set at 7.4, what is the ratio of the concentrations of carbonate to bicarbonate. Describe the buffering capacity of this buffer.
What is the pH of a buffer solution that contains 0.245 M weak acid and 0.450 M of the conjugate base? The pKa for the acid is 5.53.
We dissolve 2.77 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution of HA(aq) is 1.33. We titrate this solution with a 0.250 M solution of NaOH. It takes 41.8 mL of the NaOH solution to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the pKa value of HA(aq)? (c) What is the pH at the equivalence point? (d) What is the pH one third along the titration when you still have twice as much HA(aq) as A-(aq)?
d. During the fermentation of wine, a buffer system consisting of tartaric acid and potassium hydrogen tartrate is created as the result of a biochemical reaction. Assuming that at some point in the process, the concentrations of the two components are approximately equal, determine the pH of the wine. The pKa of tartaric acid is 2.96.
Given the pKa of hypochlorous acid, HOCl, is 7.54. What is the pH of a solution which consists of 0.20 M HOCl and 0.70 M OCl-?
Phenylacetic acid (C6H5CH2COOH, simplified here to HPAc is a monoprotic acid. It builds up in the blood of persons with phenylketonuria, that if untreated, causes mental retardation and death. A study of the acid shows that the pH of 0.120 M HPAc is 2.62. What are (a) the Ka and (b) pKa of phenylacetic acid?
One of the buffer systems the human body has to regulate pH is based on the phosphate anion. If blood has a pH of 7.40, and the three Ka values for phosphoric acid are 7.52 × 10−3, 6.23 × 10−8, and 4.8 × 10−13, write the chemical equilibrium equation showing the phosphate species that are involved in this buffer.
Consider a biochemical reaction that is taking place in a 0.1 M buffer. The initial pH is 7.4, and the pKa of the buffer is 7.2. If, in a final reaction volume of 1.0 mL, 10 micromol of protons are generated, what would be the final pH of the solution?