# Can you answer the following question from my practice titration lab: Using the data from questions 3 and 4, calculate the

Excerpt
x 0.1mol/L) / (0.25L) = 0.042mol/L :. initial acid concentration is 0.042mol/L Given: Initial pH = 3.30 pH = -log(H30″] can be used [H30*] = 10PH M [H30*] = 103.30M [H30°] = 5.0119 x 10“ M .. Initial [H30*] is 5.01 x 104 mol/L ल

Can you answer the following question from my practice titration lab: Using the data from questions 3 and 4, calculate the experimental value of K a for ts unknown acid using an ICE table . HA(aq) + NaOH(aq) → H2O(l) + NaA(aq) Transcribed Image Text: 3|
Given:
V of unknown acid = 0.25L
V of 0.1M NaOH = 0.105L
HA (ag) + NaOH (aq) -> NaA (aq) + H20)
meaning its a 1:1 reaction
Vi*Sı = V2*S2 can be used
C unknown acid = (0.105L x 0.1mol/L) / (0.25L)
= 0.042mol/L
:. initial acid concentration is 0.042mol/L
Given:
Initial pH = 3.30
pH = -log(H30″] can be used
[H30*] = 10PH M
[H30*] = 103.30M
[H30°] = 5.0119 x 10“ M
.. Initial [H30*] is 5.01 x 104 mol/L