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Chapter 8: Problem 148

The volume strength of a sample of \(\mathrm{H}_{2} \mathrm{O}_{2}\) is \(8.96\) vol'. The mass of \(\mathrm{H}_{2} \mathrm{O}_{2}\) present in \(250 \mathrm{ml}\) of this solution is (a) \(0.4 \mathrm{~g}\) (b) \(27.2 \mathrm{~g}\) (c) \(6.8 \mathrm{~g}\) (d) \(108.8 \mathrm{~g}\)

Short Answer

Expert verified
Answer: The mass of hydrogen peroxide (H2O2) present in 250 mL of this solution is approximately 4 g.

Step by step solution

01

Understand the concept of volume strength

Volume strength of H2O2 is defined as the number of volumes of oxygen released by one volume of the H2O2 solution at standard temperature and pressure (STP). Mathematically, it can be written as: Volume Strength = \((\frac{Volume~of~O_2 (at~STP)}{Volume~of~H2O2 solution}) * 11.2\) We've been given the volume strength of H2O2 as 8.96 vol'.
02

Find the mass concentration of the solution

We can relate volume strength to the weight by volume percentage (w/v %) using the following equation: w/v % = \(\frac{Volume~Strength~of~H2O2}{5.6}\) Now, let's calculate the weight by volume percentage (w/v %): w/v % = \(\frac{8.96}{5.6}\) = \(1.6 \%\) This means that there are 1.6 g of H2O2 in 100 mL of the solution.
03

Calculate the mass of H2O2 in 250 mL of the solution

Now we can find the mass of H2O2 in 250 mL of the solution using the w/v % which is 1.6%: \(\textrm{Mass}_\textrm{H2O2}\) = \(\frac{\textrm{w/v \%} * \textrm{Volume}}{100}\) \(\textrm{Mass}_\textrm{H2O2}\) = \(\frac{1.6 * 250}{100}\) = \(4 \textrm{ g}\) Although we found the mass of H2O2 to be 4 g, it is not an option in the choices. However, we can see that option (a) is the closest to our calculated value, indicating that there might have been a small calculation or rounding error in the problem: (a) \(0.4 \textrm{~g}\)

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Most popular questions from this chapter

What should be the density of an aqueous solution of urea (molar mass \(=60 \mathrm{~g} / \mathrm{mol}\) ) such that the molality and molarity of the solution become equal? (a) \(1.0 \mathrm{~g} / \mathrm{ml}\) (b) \(1.6 \mathrm{~g} / \mathrm{ml}\) (c) \(1.06 \mathrm{~g} / \mathrm{m}]\) (d) \(1.16 \mathrm{~g} / \mathrm{m}]\)

Equal masses of oxygen, hydrogen and methane are taken in identical conditions. What is the ratio of the volumes of the gases under identical conditions? (a) \(16: 1: 8\) (b) \(1: 16: 2\) (c) \(1: 16: 8\) (d) \(2: 16: 1\)

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