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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

A hydrogen bond is formed when a weakly positive hydrogen atom already bonded to one electronegative atom (for example, the oxygen in the water molecule) is attracted to another electronegative atom from another polar molecule, such as water (H2O), hydrogen fluoride (HF), or ammonia (NH3). The huge electronegativity difference between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for an N atom), combined with the very small size of an H atom...
Hydrogen Bonds00:26

Hydrogen Bonds

Hydrogen BondsHydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, and has a partial negative charge. The other is a hydrogen atom that has bonded with another electronegative atom and has a partial positive charge.Hydrogen Bonds Control the World!Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are...
Acid Strength and Molecular Structure03:05

Acid Strength and Molecular Structure

Binary Acids and Bases
In the absence of any leveling effect, the acid strength of binary compounds of hydrogen with nonmetals (A) increases as the H-A bond strength decreases down a group in the periodic table. For group 17, the order of increasing acidity is HF < HCl < HBr < HI. Likewise, for group 16, the order of increasing acid strength is H2O < H2S < H2Se < H2Te. Across a row in the periodic table, the acid strength of binary hydrogen compounds increases with increasing...
Strong Acid and Base Solutions03:22

Strong Acid and Base Solutions

A strong acid is a compound that dissociates completely in an aqueous solution and produces a concentration of hydronium ions equal to the initial concentration of acid. For example, 0.20 M hydrobromic acid will dissociate completely in water and produces 0.20 M of hydronium ions and 0.20 M of bromide ions.
Mixtures of Acids01:19

Mixtures of Acids

The pH of a solution containing an acid can be determined using its acid dissociation constant and initial concentration. If a solution contains two different acids, then its pH can be determined using one of several methods depending on the relative strength of the acids and their dissociation constants.
In a strong and weak acid mixture, the strong acid dissociates completely and becomes a source of almost all the hydronium ions present in the solution. In contrast, the weak acid shows...
Mixtures of Acids03:27

Mixtures of Acids

The pH of a solution containing an acid can be determined using its acid dissociation constant and its initial concentration. If a solution contains two different acids, then its pH can be determined using one of several methods depending upon the relative strength of the acids and their dissociation constants.
A Mixture of a Strong Acid and a Weak Acid
In a mixture of a strong acid and a weak acid, the strong acid dissociates completely and becomes a source of almost all the hydronium ions...

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Related Experiment Video

Updated: Jul 12, 2026

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
06:44

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Published on: March 24, 2018

Hydrogen bonding in hydrochloric Acid solutions.

S C Lee, R Kaplow

    Science (New York, N.Y.)
    |July 31, 1970
    PubMed
    Summary

    X-ray diffraction reveals that ions in hydrochloric acid solutions significantly alter water structure. Excess protons create shorter oxygen-to-oxygen distances in water as acid concentration rises.

    Area of Science:

    • Physical Chemistry
    • Solution Chemistry
    • Materials Science

    Background:

    • Understanding the structure of aqueous solutions is crucial for many chemical and biological processes.
    • The influence of ions on the hydrogen bond network of water is a key area of research.
    • Hydrochloric acid solutions are fundamental in various industrial and laboratory applications.

    Purpose of the Study:

    • To investigate the impact of hydrochloric acid on the radial distribution of atom pairs in water.
    • To quantify the changes in water-acid interactions, particularly concerning proton solvation.
    • To determine how varying acid concentrations affect the local structure of water molecules.

    Main Methods:

    • X-ray diffraction was employed to measure the radial distribution functions of atom pairs.

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    A Simple, Low-cost, and Robust System to Measure the Volume of Hydrogen Evolved by Chemical Reactions with Aqueous Solutions
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  • Analysis focused on the pair distribution of oxygen-oxygen atoms in aqueous solutions.
  • Experimental data were correlated with changes in proton concentration.

    • Main Results:

    • Significant alterations in near-neighbor water correlations were observed due to the presence of ions.
    • New oxygen-to-oxygen distances were identified, directly linked to excess protons.
    • These specific oxygen-to-oxygen distances were found to decrease with increasing hydrochloric acid concentration.

    Conclusions:

    • Ions, particularly excess protons in hydrochloric acid, profoundly disrupt the native structure of water.
    • The observed shortening of oxygen-to-oxygen distances indicates a more compact local water environment around protons.
    • These findings provide detailed structural insights into acidic aqueous solutions.