me of 500.0 mL of 0.170 M NaOH is added to 535 mL of 0.200 M weak acid (K₁ = 3.14 x 10-5). What is the pH of the ng buffer? HA(aq) + OH(aq) → H₂O(1) + A (aq) X10 TOOLS
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- 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*]1. Consider the titration of 25.0 mL of a weak acid, 0.100 M HCOOH (Ka = 1.8 x 10- 4) with 0.100 M NaOH. NaOH (aq) + HCOOH(aq) →H2O(1) + NaCHO2(aq) (i) What is the pH of the solution after adding 5.00 mL of NAOH? (ii) After adding 12.5 mL 2 Veq= midpoint pH = pKa = 3.74In a titration of acetic acid by sodium hydroxide, what is the pH of a 100.0 mL of a 0.1000 M CH3CHO2H(aq) solution after 25.00 mL of 0.2000 M NaOH(aq) has been added? The Ka of acetic acid is 1.75 x 10-5,
- 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 =A volume of 500.0 mL of 0.160 M NaOH is added to 525 mL of 0.250 M weak acid (K₁ = 3.24 × 10-5). What is the pH of the resulting buffer? pH = HA(aq) + OH¯(aq) H,O(l) + A(aq)A volume of 500.0 mL of 0.100 M NaOH is added to 525 mL of 0.200 M weak acid (K, = 6.27 x 10), What is the pH of the resulting buffer? HA(aq) + OH (aq) H,O() + A (aq) pH = If a buffer solution is 0.190 M in a weak acid (K, = 5.7 x 10-) and 0.550 M in its conjugate base, what is the pH? pH =
- Consider the titration of 25.0 mL of 0.125 M acetic acid (CH, COOH, pKa = 4.75) with 0.102 M NaOH. CH, COОН(aq)+NaOH(aq) — СH, СОО" (аq) + H,О1) + Na*(aq) Determine the initial pH of the 0.125 M acetic acid solution before NaOH is added. pH = Determine the pH of the solution after 10.0 mL of 0.102 M NaOH is added. pH = Determine the volume of 0.102 M NaOH required to reach halfway to the stoichiometric point of the titration.A volume of 500.0 mL of 0.180 M NaOH is added to 545 mL of 0.250 M weak acid (Ka = 6.39 × 10). What is the pH of the resulting buffer? НА(аq) + ОН (aq) - → H, O(1) + A (aq) pH =Which statement describes the action of a buffer composed of acetic acid (CH3COOH) and sodium acetate (NaCH3COO)? How does a buffer resist change in pH upon addition of a strong acid? By titration, it is found that 73.3 mL of 0.189 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
- (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.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)Consider the titration of 25.0 mL of 0.124 M acetic acid (CH₂COOH, pK, = 4.75) with 0.125 M NaOH. CH3COOH(aq)+NaOH(aq) CH₂COO (aq) + H₂O(l) + Na+ (aq) Determine the initial pH of the 0.124 M acetic acid solution before NaOH is added. pH = Determine the pH of the solution after 10.0 mL of 0.125 M NaOH is added. pH = Determine the volume of 0.125 M NaOH required to reach halfway to the stoichiometric point of the titration. volume NaOH: - Determine the pH of the solution when enough NaOH has been added to reach halfway to the stoichiometric point. pH = Determine the volume of 0.125 M NaOH that is required to reach the stoichiometric point of the reaction. volume NaOH: Calculate the pH of the solution when the stoichiometric point of the titration has been reached. pH = mL mL