Question
The $\mathrm{pH}$ of an aqueous solution of sodium chloride at $60^{\circ} \mathrm{C}$ is(a) $7.0$(b) $>7.0$(c) $<7.0$(d) 0
Step 1
This means that the product of the concentrations of hydrogen ions ($H^+$) and hydroxide ions ($OH^-$) in pure water is $10^{-14}$ at 25°C. This is represented by the equation: \[ [H^+][OH^-] = 10^{-14} \] Show more…
Show all steps
Your feedback will help us improve your experience
Raj Aggarwal and 71 other Chemistry 102 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
$\mathrm{pH}$ of an aqueous $\mathrm{NaCl}$ solution at $50^{\circ} \mathrm{C}$ should be : (a) 7 (b) $>7$ (c) $<7$ (d) 0
Which salt will produce a solution that is neutral (pH=7.00) when dissolved in water? a. MgF2 b. NH4Cl c. CoCl3 d. NaNO3
What is the $\mathrm{pH}$ of $10^{-7} \mathrm{M}-\mathrm{HCl}$ solution at $25^{\circ} \mathrm{C}$ ? (a) $7.0$ (b) $6.70$ (c) $6.62$ (d) $6.79$
Ionic Equilibrium
Exercises I
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD