Answer:
27.98g/mol
Explanation:
Using ideal gas law equation;
PV = nRT
Where;
P = pressure (atm)
V = volume (L)
T = temperature (K)
n = number of moles (mol)
R = gas law constant (0.0821 Latm/molK)
According to the information given:
V = 2.5L
P = 1.4 atm
T = 282K
n = ?
Using PV = nRT
n = PV/RT
n = 1.4 × 2.5/0.0821 × 282
n = 3.5/23.1522
n = 0.151mol
Using the formula to calculate molar mass of the elemental gas:
mole = mass/molar mass
Molar mass = mass/mole
Molar mass = 4.23g ÷ 0.151mol
Molar mass = 27.98g/mol
PH = -log[H₃O⁺]
[H₃O⁺] = 10^-pH
<span>[H₃O⁺] = 10^-2,32
</span>[H₃O⁺] =0,0047863 ≈<u> 4,79×10×10⁻³ mol/dm³</u>
<em>B) -- 4</em><span><em>,79×10⁻³ M</em></span>
Answer:
Around 129 galons
Explanation:
if you divied 3,241 by 4 you get 129 gallons but if you times that by 25 you get 3,225 so a little bit off but close.
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
