IDNLearn.com: Your go-to resource for finding expert answers. Join our interactive Q&A community and get reliable, detailed answers from experienced professionals across a variety of topics.
Sagot :
To determine the pH of a solution with a given hydronium ion concentration, we use the commonly known formula:
[tex]\[ \text{pH} = -\log_{10} [\text{H}_3\text{O}^+] \][/tex]
Here, the hydronium ion concentration ([tex]\[\text{H}_3\text{O}^+\][/tex]) is given as [tex]\(4.7 \times 10^{-11}\)[/tex].
Following the formula step-by-step:
1. Take the logarithm (base 10) of the hydronium ion concentration:
[tex]\[ \log_{10} (4.7 \times 10^{-11}) \][/tex]
2. Then, apply the negative sign as per the pH formula:
[tex]\[ \text{pH} = - \log_{10} (4.7 \times 10^{-11}) \][/tex]
After calculating this, we find that the pH value is approximately 10.33.
Therefore, the pH of the solution is [tex]\( \boxed{10.33} \)[/tex].
[tex]\[ \text{pH} = -\log_{10} [\text{H}_3\text{O}^+] \][/tex]
Here, the hydronium ion concentration ([tex]\[\text{H}_3\text{O}^+\][/tex]) is given as [tex]\(4.7 \times 10^{-11}\)[/tex].
Following the formula step-by-step:
1. Take the logarithm (base 10) of the hydronium ion concentration:
[tex]\[ \log_{10} (4.7 \times 10^{-11}) \][/tex]
2. Then, apply the negative sign as per the pH formula:
[tex]\[ \text{pH} = - \log_{10} (4.7 \times 10^{-11}) \][/tex]
After calculating this, we find that the pH value is approximately 10.33.
Therefore, the pH of the solution is [tex]\( \boxed{10.33} \)[/tex].
We appreciate your participation in this forum. Keep exploring, asking questions, and sharing your insights with the community. Together, we can find the best solutions. Your search for answers ends at IDNLearn.com. Thank you for visiting, and we hope to assist you again soon.