A solution is made by dissolving 35.5 g of Ba(NO$_2$)$_2$ in 500.0 mL of water. What is the value of K$_b$ for NO$_2^-$? The K$_a$ of HNO$_2$ is 4.5 x 10$^{-4}$.
Added by Deborah B.
Close
Step 1
5 \times 10^{-4}$. We need to find the $K_b$ of NO$_2^-$. We can use the relationship between $K_a$ and $K_b$: $K_a \times K_b = K_w$ where $K_w$ is the ion product constant for water, which is $1.0 \times 10^{-14}$ at 25°C. Show more…
Show all steps
Your feedback will help us improve your experience
Sima Sarker and 73 other Chemistry 101 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
A solution is made by dissolving 44.9 g of Ba(NO2)2 in 500.0 mL of water. What is the value of Kb for NO2-? The Ka of HNO2 is 4.5 * 10-4.
Sima S.
Determine $K_{\mathrm{b}}$ for the nitrite ion, $\mathrm{NO}_{2}^{-} .$ In a 0.10 -M solution this base is 0.0015$\%$ ionized.
A solution is made by dissolving 26.5 g of Ba(NO₂)₂ in 500.0 mL of water. Using Kb(NO₂⁻) = 2.2 × 10⁻¹¹, determine the pH of the solution.
Adi S.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD