/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 72 Automobile batteries contain sul... [FREE SOLUTION] | 91影视

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Chapter 1: Problem 72

Automobile batteries contain sulfuric acid, which is commonly referred to as "battery acid." Calculate the number of grams of sulfuric acid in \(0.500 \mathrm{~L}\) of battery acid if the solution has a density of \(1.28 \mathrm{~g} / \mathrm{mL}\) and is \(38.1 \%\) sulfuric acid by mass.

Short Answer

Expert verified
There are \(243.84 \: \mathrm{g}\) of sulfuric acid in the given volume of battery acid.

Step by step solution

01

Calculate the mass of the battery acid solution

To find the mass of the battery acid solution, we will use the formula: mass = density 脳 volume. We are given the density of the solution (1.28 g/mL) and the volume (0.500 L). First, we need to convert the volume from liters to milliliters: 0.500 L 脳 1000 mL/L = 500 mL. Now we can calculate the mass of the battery acid solution: mass = (1.28 g/mL) 脳 (500 mL) = 640 g
02

Calculate the mass of sulfuric acid in the solution

We are given that the solution is 38.1% sulfuric acid by mass. To find the mass of sulfuric acid in the solution, we will simply multiply the percentage of sulfuric acid by the total mass of the solution: mass of sulfuric acid = (38.1 / 100) 脳 640 g = 243.84 g Thus, there are \(243.84 \: \mathrm{g}\) of sulfuric acid in the given volume of battery acid.

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