Answer:
pH of Buffer Solution 5.69
Explanation:
Mole of anhydrous sodium acetate = 
= 
= 0.18 mole
100 ml of 0.2 molar acetic acid means
= M x V
= 0.2 x 100
= 20 mmol
= 0.02 mole
Using Henderson equation to find pH of Buffer solution
pH = pKa + log![\frac{[Salt]}{[Acid]}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BSalt%5D%7D%7B%5BAcid%5D%7D)
= 4.74 + log
= 4.74 + log 9
= 5.69
So pH of the Buffer solution = 5.69
2C₃H₇OH + 9O₂ = 6CO₂ + 8H₂O
a₀=2
a₁=9
a₂=6
a₃=8
Answer:
It has an electrolyte that acts as a salt bridge.
Explanation:
Answer:
92.9 °C
Explanation:
Step 1: Given data
- Initial volume (V₁): 450. mL
- Initial temperature (T₁): 55.0 °C
- Final volume (V₂): 502 mL
Step 2: Convert 55.0 °C to Kelvin
We will use the following expression.
K = °C + 273.15 = 55.0 + 273.15 = 328.2 K
Step 3: Calculate the final temperature of the gas
If we assume constant pressure and ideal behavior, we can calculate the final temperature of the gas using Charles' law.
T₁/V₁ = T₂/V₂
T₂ = T₁ × V₂/V₁
T₂ = 328.2 K × 502 mL/450. mL = 366 K = 92.9 °C
