In a weak acid when [HA]=[A-]the pH = the pKa. What is the pH after adding...
A pH 4 buffer solution is prepared by dissolving one mole of a weak acid HA (pKa=4) and one mole NaA in 1 L of water. When the volume is increased to 10L by adding distilled water, the pH of the resulting solution is closest to. 7.0 6.0 5.0 4.0 3.0
You start with a 150 mL solution of unknown weak monoprotic acid (HA). a) After adding 100 mL of 0.150 M NaOH, you find half the weak acid is now deprotonated. Given that, what was the concentration of the weak acid prior to adding the NaOH? b) After adding the 100 mL of 0.150 M NaOH to consume half the weak acid, the pH of the solution was 4.22. What was the pH of the solution before adding the NaOH?...
PART A. Determine the pH of a 9.553 mM weak acid solution that has a pKa of 8.83 PART B. Calculate the pH of a 319 mM weak base solution with a pKb of 9.04. PART C. Determine the pKa of a weak acid solution that has an initial concentration of 0.334 M and a pH of 4.54. Hint: You know the pH of the solution, so you can easily determine x in your ICE table PART D. Calculate the...
What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.305 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66*10^-7. pH = __________ What is the \rm pH after 0.150 mol of \rm HCl is added to the buffer from Part A? Assume no volumechange on the addition of the acid. pH = _____________ What is the \rm pH after 0.195 mol of \rm NaOH...
1. Calculation of pH. A weak acid HA (pKa = 4.85) reacted with strong base NaOH The reaction is HA + NAOH H20 + NaA. There are 100 mL 0.100 M HA solution, and the concentration of Na OH is 0.100 M. 0 moles a. What is the pH when 0.00 mL of NaOH is added to the 100 mL HA solution? 2 x1 les b. What is the pH when 20.0 mL of NaOH is added to the 100...
A 0.100 molar solution of weak acid HA has pH of 2.45 What is pka? Hint, find [H+] from pH and plug it into into ICE as 'X' HA (+H20) А" <> H30* 0.100 M 0 0 С E 0.100 - X х х solve for Ka, then pka Ka = [H30*1 [A]/[HA] 39 24 6.1 45 5.4 Consider the titration of 25.00 ml of 0.100 MHA with 25.0 0.100 M NaOH. HA +H20 --> A™ + H307 The Ka...
A weak acid (HA) has a pKa of 4.468. If a solution of this acid
has a pH of 4.736, what percentage of the acid is not ionized?
(Assume all H in solution came from the ionization of HA.)
A weak acid (HA) has a pKa of 4.161. If a solution of this acid has a pH of 4.140, what percentage of the acid is not ionized? (Assume all H in solution came from the ionization of HA.)
A weak acid (HA) has a pKa of 4.734. If a solution of this acid has a pH of 4.273, what percentage of the acid is not ionized? (Assume all H in solution came from the ionization of HA.)
A weak acid (HA) has a pKa of 4.679. If a solution of this acid has a pH of 4.876, what percentage of the acid is not ionized? (Assume all H in solution came from the ionization of HA.)