An aqueous solution of 1 M NaCl and lM HCl is: (a) Not a buffer but pH<7 (b) Not a buffer but pH

step 1 An aqua solution of 1M NACL and 1MHCL is not a buffer but the value of pH is less than 7. So opt

An aqueous solution of 1 M NaCl and lM HCl is: (a) Not a...

An aqueous solution of $1 \mathrm{M} \mathrm{NaCl}$ and $\mathrm{lM} \mathrm{HCl}$ is:
(a) Not a buffer but $\mathrm{pH}<7$
(b) Not a buffer but $\mathrm{pH}>7$
(c) A buffer with $\mathrm{pH}<7$
(d) A buffer with $\mathrm{pH}>7$

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Key Concepts

pH and Acid-Base Behavior

pH is a measure of the hydrogen ion concentration in a solution, determining its acidity or basicity. In the context of acid-base behavior, a low pH indicates a high concentration of hydrogen ions, which is characteristic of strong acid solutions. Understanding how different substances influence pH is crucial in fields like analytical chemistry and biochemistry.

Salts in Aqueous Solutions

Salts like sodium chloride (NaCl) are generally formed from a strong acid and a strong base and typically do not affect the pH of the solution significantly, as their ions do not hydrolyze in water. Their role in the solution is mainly to contribute ionic strength without altering the acid-base balance critically.

Buffer Solutions

Buffer solutions are mixtures that resist changes in pH when small amounts of acid or base are added. They typically consist of a weak acid and its conjugate base or a weak base and its conjugate acid. The absence of such a pair in a solution means that the solution lacks the capacity to maintain a stable pH, especially when strong acids or bases are present.

Strong Acids

Strong acids, such as hydrochloric acid (HCl), completely dissociate in water, releasing a significant concentration of hydrogen ions (H+). This complete ionization drastically lowers the pH of the solution, making it more acidic.

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