Which of the following is TRUE? An effective buffer has a [base]/[acid] ratio in the range of 10 - 100. A buffer is most resistant to pH change when [acid] = [conjugate base] An effective buffer has very small absolute concentrations of acid and conjugate base. A buffer can not be destroyed by adding too much strong base. It can only be destroyed by adding too much strong acid. None of the above are true.

Which of the following is TRUE? An effective buffer has a [base]/[acid] ratio in the range of 10 - 100. A buffer is most resistant to pH change when [acid] = [conjugate base] An effective buffer has very small absolute concentrations of acid and conjugate base. A buffer can not be destroyed by adding too much strong base. It can only be destroyed by adding too much strong acid. None of the above are true.

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

Similar questions

Which of the following aqueous solutions are good buffer systems?. 0.12 M potassium acetate + 0.20 M acetic acid 0.18 M nitrous acid + 0.18 M potassium nitrite 0.31 M ammonium bromide + 0.35 M ammonia 0.38 M hydrocyanic acid + 0.21 M potassium cyanide 0.24 M hydroiodic acid + 0.23 M sodium iodide
2) calculate the pH of 15 mL of water after 0.15 mL of 1 M HCl is added? 3) calculate the pH of the buffer after the addition of 0.15 mL of 6 M HCl based on the known value of Ka for acetic acid? *buffer solution by mixing 20.00 mL of 0.100 M sodium hydroxide and 40.00 mL of 0.100 M acetic acid
You are in charge of making a Tris buffer at pH 7.5. You could start with solid Tris base as you did in lab, but you found stock solutions of 1.0M Tris base and 1.0M Tris Hydrochloride (the conjugate acid form) in the lab and decided to make the buffer with those. How much of each of the stock solutions would you mix together to make 200.0 mL of 1.0M Tris buffer at pH 7.5?
A buffer pair consists of a conjugate weak acid0weak base pair that will resist a change in pH from the addition of a strong acid or base. Decide whether each pair below is a good example of a buffer.a. HCN and NaCN Good Buffer or Not a Bufferb. H2CO3 and Na2CO3 Good Buffer or Not a Bufferc. H2SO4 and NaHSO4 Good Buffer or Not a Buffer
Which combination would be preferable to form a buffer? OWeak acid and its conjugate base Weak acid and its conjugate acid Strong acid and a strong base Weak acid and a weak base Strong acid and its conjugate base
Which of the following is not a characteristic of buffer solutions? O They cannot be tailored to maintain a specified pH. O They contain a conjugate base of a weak acid. O They contain a weak acid. O They have a finite capacity for accommodating added acid or base. O They can maintaln their pH, even when small amounts of acid or base are added. QUESTION 10 The capacity of a buffer solution is greater when there are large amounts of a weak acid and its conjugate base in solution. O True O False
A student wants to make a 0.75 mol/L buffer solution using potassium hydrogen sulfate, KHSO4, and a conjugate base. Which of the following options could be used as a conjugate base to make this buffer solution? Answer choices a 0.80 mol/L solution of H2SO4 a 0.50 mol/L solution of K2SO4 a 0.002 mol/L solution of K2SO4 a 9.0 mol/L solution of KHSO4
A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kp (C2H5NH2) = 4.3 x 104 Express value to three decimal places. Determine the number of moles of base that can be added before the buffer capacity is exceeded. moles base F TOOLS x10
9 If the dissociation constant of a weak acid is 1.4 x 10-5, at what ratio should you adjust the concentration of the weak acid and its conjugate base in order to prepare a buffer that has a pH of 4.85? a) 0.100 M weak acid with 0.0100 M conjugate base b) 0.0100 M weak acid with 0.100 M conjugate base c) 0.100 M weak acid with 0.200 M conjugate base d) 0.300 M weak acid with 0.300 M conjugate base e) 0.500 M weak acid with 0.250 M conjugate base
You are interested in making a buffer with a pH of 7.30. Which of the following weak acid/conjugate base pairs would be most suitable to use? acid H3PO4 HCO₂H CH3CO₂H H₂PO4 NH4 HCO3 HPO4²- conjugate base H₂PO4 HCO₂ CH3CO₂ HPO4²- NH3 2- CO3²- PO4³- OHCO₂H/HCO₂ OCH3CO₂H/CH3CO₂ H₂PO4/HPO42- NH4 /NH3 2- HCO3 / CO3²- pka 2.16 3.75 4.75 7.21 9.25 10.33 12.32
Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is the best choice for making a buffer solution with an optimum pH in the range of 3.1-3.5? O O O NaNO2/HNO2 (K₂ = 4.6 x 10-4) KCH3COO/CH3COOH (K₂ = 1.75 x 10-5) CH3NH2/CH3NH3CI (K₂ = 2.3 x 10-11) NaOCN/HOCN (K₂ = 2.0 x 10-4) NaNO3/HNO3 20