a. Use the Ka values provided to chose a weak acid that can effectively buffer a solution at a pH of 6.5 when combined with it's conjugate base. Possible Buffer Reagents Concentration* Ка 2.4 x 10 7.1 x 103 HNO3 0.100 M H3PO4 0.100 M solid 6.3 x 108 NaH2PO4 NHẠCI 5.8 x 1010 -13 4.2 x 101 solid solid Na2HPO4 NH3 Na3PO4 NANO3 *Liquid reagents stored as aqueous solutions, salts stored as solids, any concentration can be made. 0.100 M NA solid NA solid NA b. Report the conjugate base concentration necessary to form the buffer solution when combined with a 0.100 M solution of the weak acid identified in part a.

Calculate the pH of the following buffer solutions:1-    1.7 g/L of NH, and 5.35 g/L of NH,CI.2-    50 mL of I M CH COONa and I L 0.1 M CH COOH3-  50 mL of 1 M NaOH and I L 0.1 M CH.COOH.4-  10 mL 0.1 H,PO + 25 mL 0.1 NaOH5-   10 mL 0.1 HPO + 25 mL 0.1 Na PO6-   A buffer solution pH=5.00 contains 0.01 M CH COOH.Calculate the concentration of sodium acetate it contains.7-   What weight of NH,CI should be added to I L of 0.1 MNH, solution to get pH=9.00?

Which of the following, if dissolved in 1.0 L of pure water, will produce a buffer solution? 0.1 mole HCL + 0.1 mole KCl 0.1 mole NaH2PO4 + 0.1 mole Na2HPO4 0.1 mole NaCl + 0.1 mole KCl 0.1 mole of H3O+ + 0.1 mole OH- I am guessing option 2, but need clarification please!

10) An aqueous solution has [HC/HsO₂) = 0.100 M and (Ca(C7H5O2)2] = 0.200 M. K. = 6.3 × 105 for HC-H₂O₂. The solution volume is 5.00 L. What is the pH of the solution after 10.00 mL of 5.00 M NaOH is added?

1. calculate the pH of a solution obtained by mixing 30.4 mL of 0.03 M HCL with 31.4 mL of o.1 M HNO3 solution 2.A given weak acid  has a pKa of 8.27.  Calculate the percent ionized in 0.34 M of the weak acid. 3. Calculate the pH of 0.021 M Sr(OH )2 PLEASE DO ALL THREE

Calculate the pH of each of the following solutions   a. 0.10 M propanoic acid, CH3CH2COOH, Ka = 1.3 x 10-5   b. 0.10 M sodium propanoate, NaCH3CH2COO.   c. A mixture containing 0.10 M propanoic acid and 0.10 M sodium propanoate   d. Calculate the pH after 0.020 mole of HCl is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate   e. Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate

5. A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant is 1.815×10-5. A student is preparing a pH buffer solution with 2.561 M NH3 solution and (NH4)2SO4 solid. Please answer the following questions. A. B. What is the best pH buffer range of the buffer solution that can be prepared by NH3 solution and (NH4)2SO4 solid? Please put down "1" if the answer is pH = 4.741 ± 1, please put down "2" if the answer is pH = 4.741 ± 10, please put down "3" if the answer is pH = 9.26 ± 1, please put down "4" if the answer is pH = 9.26 ± 10. Your answer follows. Assume that the addition of the solid will NOT change the volume, how many grams of is needed to prepare a pH = 8.66 buffer solution? The volume of the buffer solution is 250.0 mL. grams

Data:     Mass of Sodium Acetate :4.0 g    Volume of Sodium Acetate Solution: 100.00mL   Acetic Acid Concentration (mass percent from label) :4.5%   pH of Prepared Buffer Solutions   Buffer Solution Acetic Acid; 4.5% Sodium Acetate Solution Recorded pH A 5.0 mL 5.0 mL 4.3 B 5.0 mL 1.0 mL 4.2 C 10.0 mL 1.0 mL 3.4 D 1.0 mL 10.0 mL 5.0 E 1.0 mL 5.0 mL 4.5      The answers must have the correct units and the correct number of significant figures 1. Sodium acetate moles __________________________ (molar mass = 82.0 g/mol)   Molarity of sodium acetate = _______________________   Concentration of acetic acid (from bottle) = ____________        Molarity of acetic acid = ___________________________                        (molar mass = 60.0 g/mol; density of the solution is 1.0 g/mL)

8. Which of the following conjugate acid-base pair would you choose to prepare a buffer solution that has a pH of 4.20? A. HSO4-/SO42- (Ka = 1.2x10-²) B. C6H5COOH and C6H5COO-(Ka = 6.3 x 10-5) C. HCIO and CIO- (Ka = 3.5 x 10-8) D. HPO4-2 and P04-3 (Ka = 3.6 x 10-¹³) E. None of the choices

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