Answer: The pressure in the can is 4.0 atm
Explanation:
According to ideal gas equation:
P = pressure of gas = ?
V = Volume of gas = 0.410 L
n = number of moles = 
R = gas constant =
T =temperature =
Thus the pressure in the can is 4.0 atm
The Relative Formula Mass of NaH2PO4 is 120 g/mol
Therefore, the number of moles = 6.6/120
= 0.055 moles of NaH2PO4 which is also equal to the number of moles of H2PO4.
[H2PO4-] = Number of moles oof H2PO4-/Volume of the solution in L
= 0.055/ ( 355 ×10^-3)
= 0.155 M
Na2HPO4 undergoes complete dissociation as follows;
Na2HPO4 (aq)= 2Na+ (aq) + HPO4^2- (aq)
1 mole of Na2HPO4 = 142 g/mol
Therefore; number of moles = 8.0/142
= 0.0563 moles
[HPO4 ^-2] is given by no of moles HPO4^2- /volume of the solution in L
= 0.0563/(355×10^-3)
= 0.1586 M
Both H2PO4^2- and HPO4^2- are weak acids the undergoes partial dissociation
Ka of H2PO4- = 6.20 × 10^-8
[H+] =Ka*([H2PO4-]/[HPO4(2-)]
= (6.20 ×10^-8)×(0.155/0.1586)
= 6.059 ×10^-8 M
pH = - log[H+]
= - log (6.059×10^-8)
= 7.218
No more solute will dissolve at that temperature, the temperature would have to be increased in order for more solute to dissolve.
Answer:
Explanation:
Hello,
In this case, by using the general gas law, that allows us to understand the pressure-volume-temperature relationship as shown below:
Thus, solving for the temperature at the end (considering absolute units of Kelvin), we obtain:
Best regards.
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