Question

What is the H3O of a solution with a pH of 1.90

Answer 1

`\text{Answer: 1.26 }\cdot10^(-2)molL^(-1)`

Given that

pH = 1.90

`\begin{gathered} pH=-log(H^+_3O) \\ pH\text{ = 1.90} \\ \text{Take the log of both sides} \\ 1.90=-log(H^+_3O) \\ 10^(-1.9)=H^+_3O \\ H^+_3O\text{ = }1.26\cdot10^(-2)molL^(-1) \end{gathered}`