Formic acid (HCOOH) is a weak acid and hydroc | vedclass

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(D) $1$. $HCl$ is a strong acid,so it dissociates completely,while $HCOOH$ is a weak acid and dissociates partially. Thus,$[H^{+}]_{HCl} > [H^{+}]_{HC

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$pH$ of a solution formed by mixing equimolar quantities of $HCOOH$ and $HCl$ will be less than that of a similar solution formed from $HCOOH$ and $HCOONa$

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(D) $1$. $HCl$ is a strong acid,so it dissociates completely,while $HCOOH$ is a weak acid and dissociates partially. Thus,$[H^{+}]_{HCl} > [H^{+}]_{HCOOH}$. Since $[H^{+}][OH^{-}] = K_w$,it follows that $[OH^{-}]_{HCl} $2$. $A$ buffer solution consists of a weak acid and its conjugate base or a weak base and its conjugate acid. $NaOH$ is a strong base,so $NaOH + HCOONa$ is not a buffer. Option $B$ is incorrect.$3$. For $10^{-9} \ M \ HCl$,the contribution of $H^{+}$ from water cannot be ignored. The $pH$ will be slightly less than $7$,not $9$. Option $C$ is incorrect.$4$. Mixing $HCOOH$ and $HCl$ results in a solution where $HCl$ suppresses the dissociation of $HCOOH$ due to the common ion effect,leading to a very low $pH$. Mixing $HCOOH$ and $HCOONa$ forms an acidic buffer solution with $pH = pK_a + \log([salt]/[acid])$. Since the buffer solution has a higher $pH$ than the strong acid mixture,option $D$ is correct.

Formic acid $(HCOOH)$ is a weak acid and hydrochloric acid $(HCl)$ is a strong acid. It follows that the:

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