Question

0.2 M urea solution can
be isotonic with
0.1 M KBr solution
0.1 M glucose solution
0.15 m NaCl solution
O 0.2 M KBr solution​

Answer 1

Answer:

• 15 m Nacl solution.
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Answer 2

Answer:

Given 0.2M solution of urea can be isotonic with 0.1M solution of KBr.

Therefore, option (1) is correct.

Explanation:

• Two solutions are isotonic, if they have same osmotic pressure across the semipermeable membrane.
• We know that osmotic pressure, $\pi =iCRT$ , where $i$ = (no. of moles after dissociation)/(no. of moles of before dissociation) and C is the concentration.
• Osmotic pressure of 0.2M urea solution

           $\pi =()\frac{1}{1} (0.2M)RT$

          $\pi _{urea}=0.2RT$

• Osmotic pressure of 0.1M KBr solution:

          $\pi _{KBr}=(\frac{2}{1} )(0.1)RT$

          $\pi _{KBr}=0.2RT$

• Osmotic pressure of 0.1M glucose solution:

         $\pi _{glucose}=(\frac{1}{1} )(0.1)RT$

         $\pi _{glucose}=0.1RT$

• Osmotic pressure of 0.15M NaCl solution

        $\pi _{NaCl}=(\frac{2}{1} )(0.15)RT$

        $\pi _{NaCl}=0.3RT$

• Osmotic pressure of 0.2M KBr solution:

         $\pi _{NaCl}=(\frac{2}{1} )(0.2)RT$

        $\pi _{NaCl}=0.4RT$

Therefore, $\pi _{urea}=\pi _{KBr}$

Therefore, the 0.2M urea solution is isotonic with 0.1M KBr solution.