You prepared 500 mL buffer solution that contains 0.50 moles monoprotic weak acid (HA) and 0.30 moles conjugate base (NaA). The solution has a pH of 4.20. (a) What is the Kp of the conjugate base, NaA? (b) What is the pH of the buffer solution after adding 400 mL of 0.30 M H,SO4? pH = pKa – log(THA), [A*]

A buffer solution contains 0.77 mol of hydrosulfuric acid (H2S) and 0.43 mol of sodium hydrogen sulfide (NaHS) in 5.70 L.The Ka of hydrosulfuric acid (H2S) is Ka = 9.5e-08.(a) What is the pH of this buffer?(b) What is the pH of the buffer after the addition of 0.44 mol of NaOH? (assume no volume change)(c) What is the pH of the original buffer after the addition of 0.08 mol of HI? (assume no volume change)

Calculate the pH of a 1.00 L solution of 0.100 M NH 3(aq) after the addition of 0.010 mol NH 4Cl(s). For NH 3, pK b = 4.74.

A buffer solution was prepared that contained 0.60 M hydrogen fluoride, HF (Ka = 7.2 x 104) and 1.00M potassium fluoride, KF. The total volume was 250 mL. (a) What ions and molecules are present in the solution? List them in order of decreasing concentration: Decreasing order of Concentration (b) What is the pH of the buffer solution described above? (c) What is the pH of 100. mL of the buffer solution if you add 100. x 10-3 g of NaOH? Assume negligible change in volume. (USEFUL INFORMATION: MM NaOH = 39.997 g mol-1)

You have 25.00 mL of a 0.100 M aqueous solution of the weak base (CH3)2NH (Kb = 7.40 x 10-4). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? ( c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 30.00 mL of acid has been added?

Annette and Marilyn are given four reactions involving acids and bases. A dark arrow facing left (B -->) means the reaction favours the reactants. A dark arrow facing right ( Products L(aq) + HM(aq) HM(aq) +R (aq) HN(aq) + M¯(aq) HL(aq) + N(aq) Based on this information, the girls determine the correct list of BASES from strongest to weakest as: a. R¯(aq) L-(aq) N-(aq) M-(aq) b. N-(aq) M-(aq) R-(aq) L¯(aq) c. L'(aq) R-(aq) M-(aq) N-(aq) d. M (aq) N-(aq) R (aq) L (aq)

Calculate the pH of a 18 M NaCH3COO(aq) (sodium acetate salt of acetic acid)  at 25oC. The acid ionization constant for acetic acid is Ka= 1.8×10–5. Enter your answer with correct units and significant figures.

You prepare a MOPS buffer by adding 0.10 mol MOPS to water then adding 0.040 molNaOH and diluting to a final volume of 500. mL.Calculate the pH of this buffer   C7H14NO3SOH (aq) + NaOH (aq) → C7H14NO3SO− (aq) + Na+ (aq) + H2O (l)

A volume of 500.0 mL of 0.110 M NaOH is added to 585 mL of 0.200 M weak acid (Ką = 2.92 × 10-5). What is the pH of the resulting buffer? HA(aq) + OH¯(aq) – H,O(1) + A¯(aq) pH =

The dissociation expression of a dilute aqueous solution of hydrochloric acid is shown as: HCl(aq)      +     H2O(l) -> Cl-(aq)        +     H3O+(aq) True                                                                  False