(a) Calculate the pH of the 0.30 M NH3 / 0.35 M NH4Cl buffer.   What is the pH of the buffer after the addition of 0.030 mol HCl?   note: Ka  (NH4+) = 5.6 x 10 -10   NH3 (aq) + H+ (aq) → NH4+ (aq)   (b) What are the hydronium [H3O+] and hydroxide [OH-] ion concentrations at 25°C in a 4.0 M aqueous Mg(OH)2.

For 480.0 mL of a buffer solution that is 0.120 M in HC2H3O2 and 7.50×10−2 M in NaC2H3O2 , calculate the initial pH and the final pH after adding 1.5×10−2 mol of HCl . ( Ka(HC2H3O2)=1.8×10−5 .)

с $ 4 Micquam Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH₂ (aq) and 0.100 M in NH₂Cl(aq). Consult the table of ionization constants as needed. 11 ApH = Calculate the change in pH when 7.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH = % G Search or type URL 5 A tv 6 9 MacBook Pro & 7 * 00 8 by Machman Learning Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books O ( 9 ) 2 AB O delete

Given 1.00 L of a solution that is 0.100 M in sodium propionate (NaC3H5O2 ) and 0.300 M in propionicacid (HC3H5O2 ), what is the pH after 0.0400 mole of HNO3 is added? Assume that the volume does notchange upon addition of the HNO 3 . Ka for HC3H5O2 = 1.3 × 10−5