Which of the following solutions will have pH | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The $pH$ of a solution is calculated using the formula $pH = -\log[H^+]$.For $pH = 2$,the concentration of hydrogen ions $[H^+]$ must be $10^{-2}

Vedclass · Accepted Answer

$0.01 \, M \, HCl$

Vedclass · Answer

(A) The $pH$ of a solution is calculated using the formula $pH = -\log[H^+]$.For $pH = 2$,the concentration of hydrogen ions $[H^+]$ must be $10^{-2} \, M = 0.01 \, M$.$(A)$ $0.01 \, M \, HCl$: $HCl$ is a strong monoprotic acid,so $[H^+] = 0.01 \, M$. Thus,$pH = -\log(0.01) = 2$.$(B)$ $0.02 \, M \, HCl$: $[H^+] = 0.02 \, M$,so $pH = -\log(0.02) \approx 1.7$.$(C)$ $0.01 \, M \, H_2SO_4$: $H_2SO_4$ is a strong diprotic acid,so $[H^+] = 2 	imes 0.01 = 0.02 \, M$. Thus,$pH = -\log(0.02) \approx 1.7$.$(D)$ $0.02 \, M \, H_2SO_4$: $[H^+] = 2 	imes 0.02 = 0.04 \, M$,so $pH = -\log(0.04) \approx 1.4$.Therefore,the correct option is $A$.

Which of the following solutions will have $pH = 2$?

Similar Questions

Which of the following statements is correct about an aqueous solution of an acid and of a base?
$(i)$ Higher the $pH$,stronger the acid
$(ii)$ Higher the $pH$,weaker the acid
$(iii)$ Lower the $pH$,stronger the base
$(iv)$ Lower the $pH$,weaker the base

In a basic aqueous solution,if the concentration of $[OH^-]$ decreases,what happens to the $pH$?

How is an aqueous solution with $pH = 2$ compared to an aqueous solution with $pH = 4$?

What will be the $OH^{-}$ concentration in an aqueous solution having $pH = 8$?

In a basic aqueous solution,how does the basicity of the solution change as the concentration of $[OH^{-}]$ ions decreases?

Vedclass Test Series

Exam Paper Generator

Online Exam Module