1 , M NaCl and 1 , M HCl are present in an aq | vedclass

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(A) buffer solution is defined as a solution that resists changes in $pH$ upon the addition of small amounts of acid or base. It typically consists of

Vedclass · Accepted Answer

Not a buffer solution with $pH < 7$

Vedclass · Answer

(A) buffer solution is defined as a solution that resists changes in $pH$ upon the addition of small amounts of acid or base. It typically consists of a weak acid and its conjugate base,or a weak base and its conjugate acid.$HCl$ is a strong acid and $NaCl$ is a salt of a strong acid and a strong base.Since $HCl$ is a strong acid,it dissociates completely in water,making the solution highly acidic with a $pH Because there is no weak acid-conjugate base pair present,this mixture does not act as a buffer solution.Therefore,the correct description is that it is not a buffer solution and has a $pH < 7$.

$1 \, M$ $NaCl$ and $1 \, M$ $HCl$ are present in an aqueous solution. The solution is:

Similar Questions

What is the ratio of concentration of salt to concentration of weak acid in a buffer solution to maintain its $pH$ value at $7.2$ $(pK_{a} = 6.2)$?

Assertion : In a titration of weak acid and $NaOH$,the $pH$ at half equivalence point is $pK_a$.
Reason : At half equivalence point,it forms an acidic buffer and the buffer capacity is maximum where $[acid] = [salt]$.

What is the value of $[H^{+}]$ when $0.1 \ mol$ of $CH_3NH_2$ is mixed with $0.08 \ mol$ of $HCl$? Given $K_b = 5 \times 10^{-4}$.

The $pK_a$ of a weak acid is $4.8$. What should be the ratio of $\frac{[\text{acid}]}{[\text{salt}]}$, if a buffer of $pH = 5.8$ is required?

$0.1 \ mol$ of $CH_3NH_2$ $(K_b = 5 \times 10^{-4})$ is mixed with $0.08 \ mol$ of $HCl$ and diluted to $1 \ L$. What will be the $[H^{+}]$ concentration in the solution?

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