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JIPMER 2017
Exam
JIPMER
Year
2017
Subject
Chemistry
Chapter
Ionic Equilibrium

JIPMER 2017 · Chemistry · Ionic Equilibrium

When 750 mL of 0.5 M HCl is mixed with 250 mL of 2 M NaOH solution,...

When 750 mL of 0.5 M HCl is mixed with 250 mL of 2 M NaOH solution, the value of pH will be

Options

  1. ApH=7\mathrm{pH}=7
  2. BpH>7\mathrm{pH}\gt7
  3. CpH<7\mathrm{pH} \lt 7
  4. DpH=0\mathrm{pH}=0

Correct answer

B. pH>7\mathrm{pH}\gt7

Step-by-step solution

nHCl=MHCl×VHCl and nNaOH=MNaOH×VNaOH\begin{aligned}n_{\mathrm{HCl}} & =M_{\mathrm{HCl}} \times V_{\mathrm{HCl}} \text{ and } \\ n_{\mathrm{NaOH}} & =M_{\mathrm{NaOH}} \times V_{\mathrm{NaOH}} \end{aligned} where, n=n= number of moles M= molarity, V= volume ∴nHCl=0.5×750=375 milimoles. nNaOH=2.0×250=500 milimoles. ∵nNaOH>nHCl\begin{aligned}& M=\text{ molarity, } V=\text{ volume } \\ & \therefore n_{\mathrm{HCl}}=0.5 \times 750=375 \text{ milimoles. } \\ & n_{\mathrm{NaOH}}=2.0 \times 250=500 \text{ milimoles. } \\ & \because n_{\mathrm{NaOH}} > n_{\mathrm{HCl}} \end{aligned} The solution is basic and has pH>7\mathrm{pH} > 7.
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