What is an appropriate acid/conjugate base pair for preparing a buffer at pH 10.0?

The pH of a buffer is higher than the pH at which it would have the greatest buffering capacity in both directions. In which direction would the buffer have a larger buffering capacity? O Against the addition of an base O Against the addition of an acid

4. Consider a buffer made by adding 0.050 mol NaC2H302 and 0.040 mol HC2H3O2 to a liter of water. a) What is the pH of this buffer? b) What is the pH after addition of 0.010 mol NaOH? c) What is the pH after addition of 0.010 mol HCI to the original buffer solution?

Phosphoric acid is a triprotic acid (?a1=6.9×10^3Ka1=6.9×10^3, ?a2=6.2×10^8 Ka2=6.2×10−8, and ?a3=4.8×10^13Ka3=4.8×10^13). Calculate the pH of a buffer solution obtained by dissolving 19.0 g of KH2PO4(s) and 30.0 g of Na2HPO4(s) in water and then diluting to 1.00 L. pH=

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

6. After adding NH3 (g) to a buffer solution consisting of the conjugate acid/base pair: NH4*/NH3 (without changing the solution volume), which of the following statements is true? K, (NH¼*) = 5.6 x 10 1º. a) The pH of the solution will decrease. b) The concentration of H3O* will increase. c) The concentration of NH4 will increase. d) none of the above

What information can be obtained by examining the titration curve of a weak acid the concentration of the base solution O the initial pH of the acid O the identity of the salt formed by the neutralization reaciton O the heat of formation of the acid

A solution of weak base is titrated to the equivalence point with a strong acid. a Which one of the following statements is most likely to be correct? The pH of the solution is greater than 13.0. The pH of the solution at the equivalence point is 7.0. The pH of the solution is between 2.0 and 7.0. The pH of the solution is between 7.0 and 13.0. The pH of the solution is less than 2.0. D The reason that best supports the answer above is OBecause the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. Whenever a solution is titrated with a strong acid, the solution will be very acidic. Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidie

Which pair could be a buffer? NaCl and KCl Weak base and its conjugate acid Strong base and a strong acid Strong base and its conjugate acid

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? The acid's ionization constant is 5.7×10-4