(B) Given: $[H^+] = 6 \times 10^{-4} \ M$. The formula for $pH$ is $pH = -\log[H^+]$. $pH = -\log(6 \times 10^{-4})$. $pH = -(\log 6 + \log 10^{-4})$.

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(B) Given: $[H^+] = 6 \times 10^{-4} \ M$. The formula for $pH$ is $pH = -\log[H^+]$. $pH = -\log(6 \times 10^{-4})$. $pH = -(\log 6 + \log 10^{-4})$. $pH = -(\log 6 - 4)$. $pH = 4 - \log 6$. Since $\log 6 \approx 0.778$,$pH = 4 - 0.778 = 3.222 \approx 3.22$.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Water hydrolysis and pH scale

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The concentration of hydrogen ions in a given solution is $6 \times 10^{-4} \ M$. The $pH$ of the solution is:

A
$6$
B
$3.22$
C
$4$
D
$2$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Water hydrolysis and pH scale

At $100\, ^oC$,the $K_w$ of water is $55$ times its value at $25\, ^oC$. What will be the $pH$ of a neutral solution at this temperature? $(\log 55 = 1.74)$

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The concentration of hydrogen ions in a given solution is $6 \times 10^{-4} \ M$. The $pH$ of the solution is:

Similar Questions

At $100\, ^oC$,the $K_w$ of water is $55$ times its value at $25\, ^oC$. What will be the $pH$ of a neutral solution at this temperature? $(\log 55 = 1.74)$

At $25\,^oC$,the $pH$ of a solution is $2$. If the $pH$ is doubled,the concentration of hydronium ions in the solution will ............

At $25^{\circ}C$,if $[OH^{-}] = 10^{-9} \ M$,find the $pH$ value of the solution.

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