500.0 mL of 0.150 M NaOH is added to 555 mL of 0.200 M weak acid (Ka = 6.24 × 10-5). What is the pH of the resulting buffer?
The Acid -Base equilibria is given by-
From the above amounts of number of moles in the solution,we see that the NaOH is in lesser amount present in the solution.So,NaOH is the Limiting Reagent here i.e. NaOH would be consumed entirely in the reaction.
At Equilibrium,the No. of moles of weak acid and the No of moles of its Conjugate Base will be-
now,using the Henderson equation for Buffers,the pH of the solution is given by-
Hence the pH of the resulting buffer is-4.524.
500.0 mL of 0.130 M NaOH is added to 555 mL of 0.200 M weak acid (Ka = 7.11 × 10-5). What is the pH of the resulting buffer?
500.0 mL of 0.120 M NaOH is added to 605 mL of 0.200 M weak acid (Ka = 7.26 × 10-5). What is the pH of the resulting buffer?
A volume of 500.0 mL of 0.140 M NaOH is added to 555 mL of 0.250 M weak acid (Ka-5.49 x 10-5). what is the pH of the resulting buffer? HA(aq) +OH(aq)H,0) + A (aq) PH-
A volume of 500.0 mL of 0.170 M NaOH is added to 545 mL of 0.200 M weak acid (Ka=6.26×10−5). What is the pH of the resulting buffer? HA(aq)+OH−(aq)⟶H2O(l)+A−(aq) pH??
A volume of 500.0 mL of 0.160 M NaOH is added to 605 mL of 0.200 M weak acid.(Ka=8.12×10−5). What is the pH of the resulting buffer? HA(aq)+OH−(aq)⟶H2O(l)+A−(aq)
500.0 mL of 0.160 M NaOH is added to 565 mL of 0.200 M weak acid (K resulting buffer? 3.77x 105). What is the pH of the HA(aq)+OH-(aq) → H2O()-A-(aq) Number
500.0 mL of 0.170 M NaOH is added to 615 mL of 0.250 M weak acid (Ka = 1.08 × 10-5). What is the pH of the resulting buffer?
500.0 mL of 0.140 M NaOH is added to 535 mL of 0.250 M weak acid (Ka = 4.06 × 10-5). What is the pH of the resulting buffer?
500.0 mL of 0.100 M NaOH is added to 535 mL of 0.250 M weak acid (Ka = 7.69 × 10-5). What is the pH of the resulting buffer?
A volume of 500.0 mL of 0.150 M NaOH is added to 525 mL of 0.250 M weak acid (?a=4.43×10−5). What is the pH of the resulting buffer? HA(aq)+OH−(aq)⟶H2O(l)+A−(aq) pH=