(i) The volume of NaOH solution = 0 mL
The concentration of HClO = [HClO] = 0.1 M
The Ka of HClO = 3*10-8
i.e. pKa = -LogKa = -Log(3*10-8) = 7.523
Now, pH = 1/2 (pKa - Log[HClO])
= 1/2 (7.523 - Log 0.1)
= 4.26
(ii) The volume of NaOH solution = 1 mL
i.e. The no. of mmol of NaOH (nNaOH) = 1 mL * 0.1 mmol/mL = 0.1 mmol
The no. of mmol of HClO (nHClO) = 40 mL * 0.1 mmol/mL = 4 mmol
Here, 0.1 mmol of NaOH reacts with 0.1 mmol of HClO to form 0.1 mmol of NaClO, the remaining nHClO = 4-0.1 = 3.9
According to Henderson-Hasselbulch equaiton: pH = pKa + Log(nNaOH/nHClO)
i.e. pH = 7.523 + Log(0.1/3.9)
i.e. pH = 5.93
(iii) The volume of NaOH solution = 2 mL
nNaOH = 0.2 mmol and nHClO = 3.8 mmol
Now, pH = 7.523 + Log(0.2/3.8)
i.e. pH = 6.24
(iv) The volume of NaOH solution = 3 mL
nNaOH = 0.3 mmol and nHClO = 3.7 mmol
Now, pH = 7.523 + Log(0.3/3.7)
i.e. pH = 6.43
(v) The volume of NaOH solution = 20 mL
nNaOH = 2 mmol and nHClO = 2 mmol
Now, pH = 7.523 + Log(2/2)
i.e. pH = 7.52 which is the pH at half equivalence point
(vi) The volume of NaOH solution = 40 mL
nNaOH = nNaClO = 4 mmol and nHClO = 0 mmol
Here, [NaClO] = 4 mmol/(40+40) mL = 0.05 M
Formula: pH = 7 + 1/2(pKa + Log[NaClO])
i.e. pH = 7 + 1/2 (7.523 + Log 0.05)
i.e. pH = 10.11 which is the pH at equivalence point
(vii) The volume of NaOH solution = 50 mL
nNaOH = 5 mmol and nNaClO = 4 mmol, i.e. the remaining nNaOH = 5 - 4 = 1 mmol
Here, [NaOH] = [OH-] = 1 mmol/(40+50) mL = 0.011 M
pOH = -Log[OH-] = -Log(0.011)
i.e. pOH = 1.95
pH + pOH = 14
i.e. pH + 1.95 = 14
i.e. pH = 14 - 1.95 = 12.05
The plot of pH versus volume of 0.1 M NaOH solution can be drawn as follows.
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