Final answer:
The statement that a larger Ka value signifies a stronger acid is true, as a higher Ka indicates more complete ionization in solution. Conversely, a smaller Ka value denotes a weaker acid with lesser ionization. This concept is fundamental in acid-base chemistry and helps differentiate between weak and strong acids.
Step-by-step explanation:
The statement is True. The acid dissociation constant (Ka) indicates the strength of an acid. A larger Ka value implies that the acid more fully dissociates into its ions in solution, meaning that it is a stronger acid as it releases more hydronium ions (H3O+). Conversely, a smaller Ka value indicates a weaker acid because it dissociates to a lesser extent, producing fewer hydronium ions.
The relationship between Ka and acid strength is integral to understanding acid-base chemistry. The term pKa is also used and is the negative logarithm of the Ka value (pKa = -log10(Ka)). Hence, a smaller pKa value reflects a larger Ka and a stronger acid. This is important for weak acids, which are not 100% ionized in solution unlike strong acids, where the concentration of the non-ionized form becomes negligible and the Ka is very high, often considered to be close to infinity.