Question
Calculate the pH of solutions having these $\mathrm{H}^{+}$ion concentrations:(a) $1 \times 10^{-7} \mathrm{M}$(b) 0.50 M(c) 0.00010 M
Step 1
The pH of a solution is calculated using the formula: \[ \text{pH} = -\log[\mathrm{H}^+] \] where \([\mathrm{H}^+]\) is the concentration of hydrogen ions in moles per liter (M). Show more…
Show all steps
Your feedback will help us improve your experience
David Collins and 86 other educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Calculate the pH of each solution. (a) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.7 \times 10^{-8} \mathrm{M}$ (b) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.0 \times 10^{-7} \mathrm{M}$ (c) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=2.2 \times 10^{-6} \mathrm{M}$ (d) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=7.4 \times 10^{-4} \mathrm{M}$
Calculate the $\left[\mathrm{OH}^{-}\right], \mathrm{pH},$ and $\mathrm{pOH}$ for each of the following solutions in which the $\mathrm{H}^{+}$ concentrations are (a) $3.5 \times 10^{-7} M$ (c) $2.5 \times 10^{-11} M$ (b) $0.0017 M$ (d) $7.9 \times 10^{-2} M$
Calculation of Hydrogen Ion Concentration from $\mathrm{pH}$ What is the $\mathrm{H}^{+}$ concentration of a solution with $\mathrm{pH}$ of (a) $3.82 ;$ (b) $6.52 ;$ (c) $11.11 ?$
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD