Suppose you are given solutions of 1.00 M acetic acid and 1.00 M sodium acetate and are asked to make 100.00 mL of buffer at pH 5.00 using only these two solutions. What volume, in milliliters, of acid would you need? The pKa of acetic acid is 4.75.

You need to produce a buffer solution that has a pH of 5.27. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74. Express your answer numerically in millimoles.

An analytical chemist is titrating 74.2 mL of a 0.3000 M solution of methylamine (CH3NH2) with a 0.2500M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 10.4 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. PH = ☐

28. 25.00 mL of a solution of a weak monoprotic acid, HX, was titrated with a 0.0640M solution of NaOH, requiring 18.22 mL to neutralize the acid. If the Ka for the acid is 3.60*106, calculate the number of moles of a salt, NaX, that must be added to produce a pH of 6.00 in 150.00 mL of the original solution. You may assume that the temperature is 25 °C. It is impossible for a solution with this composition to have a pH of 6.00 0.00117 mol 0.0252 mol 0.0466 mol 1.17 mol

Which of the following is true of a buffer solution that contains equivalent amounts of acid and conjugate base?     The pH will always be greater than 7, regardless of the acid and conjugate base.     The pH of the solution will be equal to the pKa of the acid.     The pH of the solution will be equal to Kw.     The pH will be equal to the concentration of the conjugate base.     The pH will be equal to the concentration of the acid.

Enter your answer in the provided box. Calculate the pH of a bicarbonate/carbonate buffer in which the concentration of sodium bicarbonate (NaHCO3) is always 0.31 M, but the concentration of sodium carbonate (Na₂CO3) corresponds to the following value: 0.31 M. (K for HCO3 is 5.6 × 10-11.) Report your answer to four significant figures.

You wish to make a buffer of 500 mL at 0.1 M sodium phosphate at pH 6.5. If the molecular weight of NaH,PO4 and NazHPO4 are 121 g/mol and 143 g/mol, respectively, and the three pk, values for phosphoric acid are 2.14, 6.86, and 12.4, respectively, how many grams each of the two sodium phosphate salts must be dissolved to make 500 mL of a 0.1 M solution that buffers at pH 6.5?

An analytical chemist is titrating 64.8mL of a 0.3000M solution of ammonia NH3 with a 0.7300M solution of HNO3 . The pKb of ammonia is 4.74 . Calculate the pH of the base solution after the chemist has added 31.6mL of the HNO3 solution to it.   Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added.   Round your answer to 2 decimal places.

In a titration of 60.0 mL of a 0.500 M solution of a diprotic acid H₂C₃H₂O₄ (malonic acid) with 0.255 M NaOH, how many mL of base are required to reach the first equivalence point?

You need to produce a buffer solution that has a pH of 5.03. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74. Express your answer numerically in millimoles.