Calculate the ph of a 1.00 liter buffer solution that contains 0.300 m hc2h3o2 and 0.300 m nac2h3o2. (b) calculate the ph of thi
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Hello!
Data:
P (pressure) = 1 atm
V (volume) = 18.5 L
T (temperature) = 300 K
n (number of mols) = ? (in mol)
R (Gas constant) = 0.082 (atm*L/mol*K)
Apply the data to the Clapeyron equation (ideal gas equation), see:
Note: If the feedback is to be considered, the closest response is 0.751 mol Nacl
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I hope this helps. =)
Data:
P (pressure) = 1 atm
V (volume) = 18.5 L
T (temperature) = 300 K
n (number of mols) = ? (in mol)
R (Gas constant) = 0.082 (atm*L/mol*K)
Apply the data to the Clapeyron equation (ideal gas equation), see:
Note: If the feedback is to be considered, the closest response is 0.751 mol Nacl
_________________
_________________
I hope this helps. =)
Answer: The concentration of the diluted solution is 1.566M.
Explanation:
The dilution equation is presented as this: .
·M= molarity (labeled as M)
·V= volume (labeled as L)
·s= stock solution (what you started with)
·d= diluted solution (what you have after)
Now that we know what each part of the formula symbolizes, we can plug in our data.
We cannot leave it like this because the volumes must be in Liters, not milliliters. To convert this, we divide the milliliters by 1000.
Now that we have the conversions, let's plug them into the equation.
The only thing that we need to do now is actually solving the answer.
From the work shown above, the answer is 1.566M.
I hope this helps!! Pls mark brainliest :)
Answer:
The question is incomplete. the compound wasn't attached to the question. Find attached of the compound and the answer too.
1. No
2. No
3. Yes
4. Yes
Explanation:
See the attached file for the answer.
