what is the hydronium ion concentration in a solution of hcl that has a ph of 4.65? round to the nearest…

Explanation:

Step1: Recall pH formula

The formula for pH is $pH = -\log[H_3O^+]$. We can re - arrange it to find $[H_3O^+]=10^{-pH}$.

Step2: Calculate hydronium ion concentration

Given $pH = 4.65$, then $[H_3O^+]=10^{- 4.65}$. Using a calculator, $10^{-4.65}\approx2.24\times10^{-5}\text{ M}$. So for the HCl part, the coefficient is $2.24$ and $n=-5$.

Step3: Recall pOH formula

The formula for pOH is $pOH=-\log[OH^-]$. We can re - arrange it to find $[OH^-]=10^{-pOH}$.

Step4: Calculate hydroxide ion concentration

Given $pOH = 4.65$, then $[OH^-]=10^{-4.65}$. Using a calculator, $10^{-4.65}\approx2.24\times10^{-5}\text{ M}$. So for the $NH_3$ part, the coefficient is $2.24$ and $n = - 5$.

Answer:

For HCl: $2.24\times10^{-5}\text{ M}$, $n=-5$ For $NH_3$: $2.24\times10^{-5}\text{ M}$, $n=-5$