How do you make a 0.5 M solution of HCl?

Table of Contents Show

Methanolic Hydrochloric Acid Solution Preparation
Methanolic Hydrochloric Acid Solution Standardization
Chemistry Quick Review of Solution Preparation
Example of How to Prepare a Solution
Important Points to Remember
How would you prepare 0.5 M HCl solution in 100 ml?
How do you make a 1 molar solution of HCl?
What concentration is 0.5 N HCl?
What is the pH of a .5 M solution of HCl?

I assume you want to prepare HCl 0.5 M from HCl 37% (that is, concentrated hydrochloric acid). This is a dilution problem: HCl 37% can be assumed to be about 12 M, so it has to be diluted down to 0.5 M. Use this equation:

M1·V1 = M2·V2

M1 = initial concentration (here, 12 M)

V1 = amount of HCl 12 M you need to pick up and, subsequently, dilute

M2 = final concentration (here, 0.5 M)

V2 = amount of HCl 0.5 M you want to make

Solve for V1, you will have the amount (either in mL or L) of HCl 12 M you must use to make up the final solution till the desired volume.

M1·V1 = M2·V2

M1 = initial concentration (here, 12 M)

V1 = amount of HCl 12 M you need to pick up and, subsequently, dilute

M2 = final concentration (here, 0.5 M)

V2 = amount of HCl 0.5 M you want to make

Solve for V1, you will have the amount (either in mL or L) of HCl 12 M you must use to make up the final solution till the desired volume.

Preparation and standardisation of 0.5 M Methanolic Hydrochloric Acid using anhydrous Sodium Carbonate and Methyl Red solution as indicator used in analysis of pharmaceutical ingredients.

Methanolic Hydrochloric Acid Solution Preparation

Take 40 ml of water in a 1000 ml volumetric flask.
Slowly add 43 ml of hydrochloric acid.
Cool and add methanol to volume.
Standardize the solution in the following manner.

Methanolic Hydrochloric Acid Solution Standardization

Weigh accurately about 800 mg of anhydrous sodium carbonate, previously heated at about 270°C for 1 hour.
Dissolve it in 100 ml of water and add 0.1 ml of methyl red solution.
Add the acid slowly from a burette, with constant stirring, until the solution becomes faintly pink.
Heat the solution to boiling, cool and continue the titration.
Heat again to boiling and titrate further as necessary until the faint pink color is no longer affected by continued boiling.
1 ml of 0.5 M hydrochloric acid is equivalent to 0.02650 g of Na2CO3.
Calculate the molarity of solution by the following formula:

Na2CO3 in mg
M = --------------------------

Chemistry Quick Review of Solution Preparation

COLIN CUTHBERT/SCIENCE PHOTO LIBRARY / Getty Images

Here's a quick overview of how to prepare a solution when the final concentration is expressed as M or molarity.

You prepare a solution by dissolving a known mass of solute (often a solid) into a specific amount of a solvent. One of the most common ways to express the concentration of the solution is M or molarity, which is moles of solute per liter of solution.

Example of How to Prepare a Solution

Prepare 1 liter of 1.00 M NaCl solution.

First, calculate the molar mass of NaCl which is the mass of a mole of Na plus the mass of a mole of Cl or 22.99 + 35.45 = 58.44 g/mol

Weigh out 58.44 g NaCl.
Place the NaCl in a 1-liter volumetric flask.
Add a small volume of distilled, deionized water to dissolve the salt.
Fill the flask to the 1 L line.

If a different molarity is required, then multiply that number times the molar mass of NaCl. For example, if you wanted a 0.5 M solution, you would use 0.5 x 58.44 g/mol of NaCl in 1 L of solution or 29.22 g of NaCl.

Important Points to Remember

Molarity is expressed in terms of liter of solution, not liters of solvent. To prepare a solution, the flask is filled to the mark. In other words, it is incorrect to a 1 liter of water to a mass of sample to prepare a molar solution.
Sometimes it's necessary to adjust the pH of a solution. To do this, add enough water to dissolve the solute. Then add an acid or base solution dropwise (usually a hydrochloric acid or HCl solution for acid or sodium hydroxide or NaOH solution for a base) to reach the desired pH. Then add more water to reach the mark on the glassware. Adding more water won't change the pH value.

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What volume of $0.5\ \mathrm M$ HCl solution is needed to prepare a $500\ \mathrm{ml}$ $10\ \%$ concentration solution, whose density is $1.05\ \mathrm{g/cm^3}$.

I've started off with finding the mass of the final solution, which would be $500\ \mathrm{cm^3} \times 1.05\ \mathrm{g/cm^3} = 525\ \mathrm g$. Next I find the mass of the HCl in it, $52.5\ \mathrm g$. After that, the moles of HCl, approx. $1.4384\ \mathrm{mol}$.

But after that I'm not sure how to proceed. I've tried dividing the molarity by the moles to get the volume, but that didn't work. I think I might have to make a system of equations but I'm bad at math so if that's how it's supposed to be done, I'd like for someone to show me how.

asked May 1, 2019 at 7:50

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As you have calculated, 500 ml of a 10 % HCl solution contain about 1.44 mol HCl. Thus the concentration is about 2.9 mol/l. Therefore, you cannot prepare this solution by diluting a solution with c = 0.5 mol/l HCl.

answered May 1, 2019 at 8:01

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How would you prepare 0.5 M HCl solution in 100 ml?

Dissolve it in 100 ml of water and add 0.1 ml of methyl red solution. Add the acid slowly from a burette, with constant stirring, until the solution becomes faintly pink. Heat the solution to boiling, cool and continue the titration.

How do you make a 1 molar solution of HCl?

1M HCl: add 1mol/12M = 83 ml conc. HCl to 1L of water or 8.3ml to 100ml..

2M HCl: add 2mol/12M = 167 ml conc. HCl to 1L of water or 16.7ml to 100ml..

What concentration is 0.5 N HCl?

Hydrochloric Acid, 0.50N, Standardized …0.5N Composition: Water 98.14%, Hydrochloric Acid 1.86% Boiling Point: 100°C Density: 1.01 Melting Point: 0.0°C Color: Colorless liquid Physical State: Liquid pH Range: 0.3 Solubility Information: Miscible Shelf Life: 24 Months Storage: Ambient DOT: UN1789, HYDROCHLORIC ACID…