Hydrogen ion concentration of tear fluid in newborn infants

Insights

Newborn infant tear pH was measured, revealing a median value of 6.8. This easy and reliable method helps understand tear function in infants.

Area of Science:

  • Ophthalmology
  • Neonatology
  • Physiology

Background:

  • Tear pH is a crucial indicator of ocular surface health.
  • Understanding normal tear pH in newborns is essential for diagnosing potential ocular conditions.
  • Previous research on neonatal tear pH is limited.

Purpose of the Study:

  • To determine the normal tear pH range in newborn infants.
  • To establish a reliable method for measuring tear pH in neonates.
  • To investigate factors influencing tear pH in newborns.

Main Methods:

  • Tear pH was measured in 173 newborn infants using a microcombination glass pH probe.
  • The probe was immersed in the tear fluid within the closed lower conjunctival sac.
  • Data was collected and analyzed for median and mean pH values, along with interpercentile ranges.

Main Results:

  • The median tear pH was 6.8, with a 95% interpercentile range of 6.2 to 7.2.
  • The mean tear pH was 6.74 +/- 0.26 (SD).
  • Tear pH was not significantly related to infant age (within 12 days), mode of delivery, or silver nitrate application.

Conclusions:

  • The microcombination glass pH probe offers an easy and reliable method for assessing tear fluid pH in newborns.
  • This study provides valuable reference data for normal tear pH in neonates.
  • The findings may enhance the understanding of tear function in both normal and pathological neonatal ocular conditions.

Related Concept Videos

Water: A Bronsted-Lowry Acid and Base02:30

Water: A Bronsted-Lowry Acid and Base

The reaction between a Brønsted-Lowry acid and water is called acid ionization. For example, when hydrogen fluoride dissolves in water and ionizes, protons are transferred from hydrogen fluoride molecules to water molecules, yielding hydronium ions and fluoride ions:
pH Scale02:41

pH Scale

Hydronium and hydroxide ions are present both in pure water and in all aqueous solutions, and their concentrations are inversely proportional as determined by the ion product of water (Kw). The concentrations of these ions in a solution are often critical determinants of the solution’s properties and the chemical behaviors of its other solutes. Two different solutions can differ in their hydronium or hydroxide ion concentrations by a million, billion, or even trillion times. A common means of...
Weak Acid Solutions04:02

Weak Acid Solutions

Few compounds act as strong acids. A far greater number of compounds behave as weak acids and only partially react with water, leaving a large majority of dissolved molecules in their original form and generating a relatively small amount of hydronium ions. Weak acids are commonly encountered in nature, being the substances partly responsible for the tangy taste of citrus fruits, the stinging sensation of insect bites, and the unpleasant smells associated with body odor. A familiar example of a...
Polyprotic Acids03:38

Polyprotic Acids

Acids are classified by the number of protons per molecule that they can give up in a reaction. Acids such as HCl, HNO3, and HCN that contain one ionizable hydrogen atom in each molecule are called monoprotic acids. Their reactions with water are:
Solubility Equilibria: Ionic Product of Water01:16

Solubility Equilibria: Ionic Product of Water

Pure water is a weak electrolyte; only a small amount ionizes into hydrogen and hydroxide ions. At any given temperature, the concentration of undissociated water is almost constant, so the ionic product of water is the product of the hydrogen and hydroxide ion concentrations, denoted as Kw. The square root of Kw gives the individual ion concentrations.
The ionic product of water varies with temperature, and its value is 1.0 x 10−14 at standard experimental conditions. Per Le Chatelier's...
Composition of Body Fluids01:29

Composition of Body Fluids

Water functions as a solvent accommodating various solutes, which can be categorized under electrolytes and non-electrolytes. Non-electrolytes are usually held together by covalent bonds, restricting them from dissociating in solution, thereby leading to a lack of electrically charged components upon dissolving in water. They are predominantly organic molecules, such as glucose, creatinine, and urea. Electrolytes, on the other hand, are compounds that can break down into ions in water.