Answer:
527.68 mL
Explanation:
We will assume that nitrogen is behaving as ideal gas here.
For ideal gas the gas law is:
Where
P1= initial pressure = 740 torr
V1= initial volume = 500mL
T1= initial temperature = 25⁰C = 298 K
P2= final pressure = 760 torr
V2= final volume = ?
T2= final temperature = 50⁰C = 323 K
Putting values in the gas law
Final volume = 
Answer:
Isotopes are variations of chemical elements that have the same number of protons but different number of neutrons.
Explanation:
First we dissociate the salt
NaOCl ⇒ Na⁺ + OCl⁻
note that [NaOCl] = [OCl⁻]
note that Na⁺ does not undergo hydrolysis so it is a spectator.
OCl⁻ can reform HOCl in an equilibrium, with OCl⁻ acting as the base.
OCl⁻ + H₂O ⇄ OH⁻ + HOCL
<span>Ka for HOCl = 3.0x10^-8, therefore
Kb for OCL</span>⁻ = Kw / (Ka for HOCl)
= 1.0 × 10⁻¹⁴ / 3.0 <span>× 10⁻⁸
= 3.3 × 10⁻⁷
</span>since Kb for OCl⁻ is given, and the pH is given, then [OCl⁻] must be found, and [OCl⁻] = [NaOCl]
convert the pH into [OH⁻]:
pOH = 14 - pH = 14 - 10.3 = 3.7
[OH⁻] = 10^(-3.7) = 1.995 × 10⁻⁴
set up equib table
OCl⁻ + H₂O ⇄ OH⁻ + HOCl
ST x 0 0
+Δ -1.995 × 10⁻⁴ +1.995 × 10⁻⁴ +1.995 × 10⁻⁴
---------------------------------------------------------------------------------
EQ: x -1.995 × 10⁻⁴ 1.995 × 10⁻⁴ 1.995 × 10⁻⁴
Kb = [OH⁻][HOCl] / [OCl⁻]
3.3 × 10⁻⁷ = (1.995 × 10⁻⁴)² / (x -1.995 × 10⁻⁴ )
x = 1.1963 × 10⁻¹ M = [OCl⁻] = [NaOCl]
The concentration of the salt formed, <span>NaOCl,</span> is 1.2 × 10⁻¹ M
The Law of Conservation of Mass says that there can be no more or no less mass after a chemical reaction, so 24.4g+ 12.3 g has to equal the mass of Ca(OH)2
