step 3: create a model solution of ph = 6 with more h⁺ ions than oh⁻ ions\ncalculate the ratio of h⁺ ions to…

step 3: create a model solution of ph = 6 with more h⁺ ions than oh⁻ ions\ncalculate the ratio of h⁺ ions to oh⁻ ions at a ph = 6.\nfind the concentration of h⁺ ions to oh⁻ ions listed in table b of your student guide. then divide the h⁺ concentration by the oh⁻ concentration. record this calculated ratio in table a of your student guide.\ncompare your approximated and calculated ratios of h⁺ ions to oh⁻ ions at a ph = 6. are they the same? why or why not? record your explanation in table a.\nwhat is the concentration of h⁺ ions at a ph = 6?\nmol/l\nwhat is the concentration of oh⁻ ions at a ph = 6?\nmol/l\nwhat is the ratio of h⁺ ions to oh⁻ ions at a ph = 6?\n:1

step 3: create a model solution of ph = 6 with more h⁺ ions than oh⁻ ions\ncalculate the ratio of h⁺ ions to oh⁻ ions at a ph = 6.\nfind the concentration of h⁺ ions to oh⁻ ions listed in table b of your student guide. then divide the h⁺ concentration by the oh⁻ concentration. record this calculated ratio in table a of your student guide.\ncompare your approximated and calculated ratios of h⁺ ions to oh⁻ ions at a ph = 6. are they the same? why or why not? record your explanation in table a.\nwhat is the concentration of h⁺ ions at a ph = 6?\nmol/l\nwhat is the concentration of oh⁻ ions at a ph = 6?\nmol/l\nwhat is the ratio of h⁺ ions to oh⁻ ions at a ph = 6?\n:1

Answer

Explanation:

Step1: Calculate $[H^+]$ concentration

The formula for pH is $pH = -\log[H^+]$. Given $pH = 6$, we can solve for $[H^+]$ as follows: $6=-\log[H^+]$, then $[H^+]=10^{-pH}$. So $[H^+]=10^{- 6}\text{ mol/L}$.

Step2: Calculate $[OH^-]$ concentration

We know that at $25^{\circ}C$, $[H^+][OH^-]=10^{-14}$. Since $[H^+]=10^{-6}\text{ mol/L}$, we can solve for $[OH^-]$: $[OH^-]=\frac{10^{-14}}{[H^+]}=\frac{10^{-14}}{10^{-6}} = 10^{-8}\text{ mol/L}$

Step3: Calculate the ratio of $[H^+]$ to $[OH^-]$

The ratio of $[H^+]$ to $[OH^-]$ is $\frac{[H^+]}{[OH^-]}=\frac{10^{-6}}{10^{-8}}=100:1$

Answer:

What is the concentration of $H^+$ ions at a pH = 6? $10^{-6}$ mol/L What is the concentration of $OH^-$ ions at a pH = 6? $10^{-8}$ mol/L What is the ratio of $H^+$ ions to $OH^-$ ions at a pH = 6? $100:1$