Given the following:
Concentration of residual (NH4)+ = 0.12 - 0.03 = 0.09 mol / L
Concentration of created NH3 = 0.03 mol / L
The (NH4) + reacts with all (OH)- to form NH3 and H2O ( Water )
The resultant solution is NH4+ / NH3 buffer system in which (NH4)+ is acid and the NH3 is base or as called the salt.
For a buffer system :
pH = pKa + Log (acid) / (salt)
= 9.25 + Log [ (NH4)+ ] / [ NH3 ]
= 9.25 + Log [ 0.09 ] / [ 0.03 ]
= 9.25 + Log 3
= 9.25 + 0.4771
pH = 9.7271 or 9.73 which is rounded up to 2 decimal places
Answer:
0.00725 M
Explanation:
Considering for
Mass = 5.66 g
Molar mass of = 80.043 g/mol
Moles = Mass taken / Molar mass
So,
<u>Moles = 5.66 / 80.043 moles = 0.0707 moles</u>
will dissociate as:
Thus 1 mole of yields 1 mole of ammonium ions. So,
<u>Ammonium ions furnished by = 1 × 0.0707 moles = 0.0707 moles</u>
Considering for
Mass = 4.42 g
Molar mass of = 149.09 g/mol
Moles = Mass taken / Molar mass
So,
Moles = 4.42 / 149.09 moles = 0.0296 moles
will dissociate as:
Thus 1 mole of yields 3 moles of ammonium ions. So,
<u>Ammonium ions furnished by = 3 × 0.0296 moles = 0.0888 moles</u>
<u>Total moles of the ammonium ions = 0.0707 + 0.0888 moles = 0.1595 moles</u>
Given that:
Volume = 22.0 L
So, Molarity of the is:
<u>Molarity = Moles / Volume = 0.1595 / 22 M = 0.00725 M</u>
Answer:it a solution that can be easily saturated.
Explanation:
Answer:
3.4 × 10^23 molecules
Explanation:
To find the number of molecules present in C6H14, we multiply the number of moles in the compound by Avagadro's number (6.02 × 10^23 atoms).
number of molecules = number of moles (mol) × 6.02 × 10^23?
Number of molecules = 0.565 × 6.02 × 10^23
3.4 × 10^23 molecules