The correct answer is letter <span>C. mixture in which its components retain their identity. A heterogeneous mixture is a mixtures in which the component of the mixed are not uniform. You can see that there are localized regions that have different properties. The components have the capacity to retain their identity.</span>
The molarity of solution made by dissolving 15.20g of i2 in 1.33 mol of diethyl ether (CH3CH2)2O is =0.6M
calculation
molarity =moles of solute/ Kg of the solvent
mole of the solute (i2) = mass /molar mass
the molar mass of i2 = 126.9 x2 = 253.8 g/mol
moles is therefore= 15.2 g/253.8 g/mol = 0.06 moles
calculate the Kg of solvent (CH3CH2)2O
mass = moles x molar mass
molar mass of (CH3CH2)2O= 74 g/mol
mass is therefore = 1.33 moles x 74 g/mol = 98.42 grams
in Kg = 98.42 /1000 =0.09842 Kg
molarity is therefore = 0.06/0.09842 = 0.6 M
11. ionic charge +1, helium.
12. ionic charge 2-, neon.
13. ionic charge 3+, neon.
Answer:
B
Explanation:
A is wrong because heat is what makes the process faster.
B is right because the finer grains are able to dissolve at a higher rate since the amount of one grain reduces it's time to dissolve.
C is wrong because simply adding more water will not increase or decrease the dissolving rate.
Hello!
We have the following data:
ps: we apply Ka in benzoic acid to the solution.
[acid] = 0.235 M (mol/L)
[salt] = 0.130 M (mol/L)
pKa (acetic acid buffer) =?
pH of a buffer =?
Let us first find pKa of benzoic acid, knowing that Ka (benzoic acid) = 
So:
Now, using the abovementioned data for the pH formula of a buffer solution or (Henderson-Hasselbalch equation), we have:
![pH = pKa + log\:\dfrac{[salt]}{[acid]}](https://tex.z-dn.net/?f=%20%20pH%20%3D%20pKa%20%2B%20log%5C%3A%5Cdfrac%7B%5Bsalt%5D%7D%7B%5Bacid%5D%7D%20%20%20)
Note:. The pH <7, then we have an acidic solution.
I Hope this helps, greetings ... DexteR! =)
