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InterviewSolution
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What is the pH of the resulting solution whenequal volumes of 0.1 M NaOH and 0.01 M HCl aremixed?[Re-AlPMT-2015] |
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Answer» It is given that equal volumes of HCl and NaOH are present, so let us assume that each has a volume = 1litre. Volume of NaOH= 1litreMolarity of NaOH = 0.1Moles of NaOH = 0.1x 1 =0.1 [ As the formula says Mole = [Concentration in M x volume in L)] Volume of HCl present = 1 litreMolarity ofHClpresent = 0.01Moles of HCl = 0.01 x1= 0.01 Equal volume of HCl balance equal volumes of HCl according to the reactionHCl + + NaOH>>NaCl+ H2OThereforeNaOH is present in excess = 0.1-0.01= 0.09molesTotal volume of the solution = 2LConcentration of OH-ions =pOH = -log[OH-] = - log[0.045] = 1.347We know that pH = 14- pOHHence pH of the resultant solution = 14- 1.347 = 12.65 |
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