Solve the problem.
-$\mathrm { pH } = - \log _ { 10 } \left[ \mathrm { H } ^ { + } \right]$Find the $\left[ \mathrm { H } ^ { + } \right]$if the $\mathrm { pH } = 1.4$.
A) $2.51 \times 10 ^ { - 1 }$
B) $3.98 \times 10 ^ { - 1 }$
C) $3.98 \times 10 ^ { - 2 }$
D) $2.51 \times 10 ^ { - 2 }$

Question

Quizplus · Accepted Answer

Given $\mathrm { pH } = 1.4$, we can find the concentration of $\mathrm { H } ^ { + }$ ions by rearranging the pH formula: $\left[ \mathrm { H } ^ { + } \right] = 10^{-\mathrm { pH }}$. Substituting $1.4$ for pH, we get $\left[ \mathrm { H } ^ { + } \right] = 10^{-1.4} = 3.98 \times 10^{-2}$.

Solve the Problem pH=−log⁡10[H+]\mathrm { pH } = - \log _ { 10 } \left[ \mathrm { H } ^ { + } \right]pH=−log10​[H+]

Solve the Problem $\mathrm { pH } = - \log _ { 10 } \left[ \mathrm { H } ^ { + } \right]$