The larger the value of Ka

Question

BlackTom AI · Accepted Answer

When evaluating the relationship between acid strength and the acid dissociation constant Ka, it helps to recall the definition of Ka and what it implies about dissociation in solution.
Option 1: 'the more highly dissociated the acid and the stronger the acid.' This is correct because Ka measures the extent to which an acid donates protons in water. A larger Ka indicates a greater degree of dissociation, which corresponds to a stronger acid.
Option 2: 'the less highly dissociated the acid and the stronger the acid.' This contradicts the fundamental idea that stronger acids dissociate more in solution. Less dissociation would imply a weaker acid, not stronger.
Option 3: 'the less highly dissociated the acid and the weaker the acid.' While this statement correctly links less dissociation with weaker acids, it misstates the primary relationship being asked about: a weaker acid does not have a larger Ka. Thus this option is incorrect.
Option 4: 'the more highly dissociated the acid and the weaker the acid.' This mixes up the correlation: high dissociation should align with strong acids, not weaker ones, so this is inconsistent with Ka concepts.
In summary, the core idea is that Ka increasing reflects greater dissociation and greater acid strength, so the option that aligns both ideas is the one stating that more dissociation corresponds to a stronger acid. The other choices invert or misapply this relationship, leading to false conclusions.

The larger the value of KaSingle choice

Similar Questions

Write an expression for the acid ionization constant (Ka) for the dissociation of the following weak acid H2CO3.

A 0.10 M solution of a weak acid, HX, is 0.059% ionized. Evaluate Ka for the acid.

The pH of a solution of a 0.15 M solution of HOCl is 4.14. What is the Ka for HOCl?

For the dissociation of a very weak acid, HA, in water

The pH of a 0.800 M aqueous solution of a weak acid is 1.99. What is the value of Ka for this acid?

A 0.025 M solution of a weak acid has a percent ionization of 3.2%. What is the Ka of the weak acid?

Based on the following titration curve, what is the Ka for this weak acid?

More Practical Tools for Students Powered by AI Study Helper

Homework AI Solver

Stylized AI Paper Writer

Plagiarism Checker Assistant

Citation AI Academic Writing Tool

In-Class Translation Assistant

AI Note Generator

AI Quiz Answers

Past Exam Questions from University Test Bank

Smart Practice Assistant

Adaptive Practice

Making Your Study Simpler