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**Problem**: What is the mass percent of chlorine in hydrochloric acid?

###### FREE Expert Solution

###### FREE Expert Solution

We are asked to calculate for the **mass percent (mass %) of Cl **in **HCl. **

**T**o do that we’re going to use the **mass percent formula **shown below:

$\overline{){\mathbf{mass}}{\mathbf{\%}}{\mathbf{}}{\mathbf{Cl}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{mass}\mathbf{}\mathbf{of}\mathbf{}\mathbf{Cl}}{\mathbf{mass}\mathbf{}\mathbf{of}\mathbf{}\mathbf{HCl}}{\mathbf{}}{\mathbf{x}}{\mathbf{}}{\mathbf{100}}{\mathbf{\%}}}$

First, we need to get the molar mass of **HCl.**

**Molar mass of HCl:**

**HCl**** 1 **

**H x**

**1**

**g/mol H =**

**1.00 g/mol H**

** 1 **

**Cl x****35****g/mol Cl**

__=____35.45 g/mol Cl__

**Sum =**

**36.45 g/mol HCl**

###### Problem Details

What is the mass percent of chlorine in hydrochloric acid?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Mass Percent concept. You can view video lessons to learn Mass Percent Or if you need more Mass Percent practice, you can also practice Mass Percent practice problems .

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Based on our data, we think this problem is relevant for Professor Cavanaugh's class at San Diego Mesa College.