In a certain organic compound, one of the carbon atoms is bonded to four atoms. One of these is a carbon atom, and the other thr
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Answer:
The molecular weight is
Explanation:
From the question we are told that
The mass of the sample is
The temperature is
The volume which the gas occupied is
The pressure is
Generally from the ideal gas equation we have that
Here n is the number of moles of the gas while the R is the gas constant with value
=>
=>
Generally the molecular weight is mathematically represented as
=>
=>
Answer:
pH = 9,57
[M²⁻] = 7,948x10⁻²M
[HM⁻] = 4x10⁻⁵M
[H₂M] = 0M
Explanation:
The moles of maleic acid presents in the solution are:
0,923g×=7,952x10⁻³moles of H₂M
60,0mL of 0,265M KOH are:
0,0600L×=0,0159 moles of KOH
The reactions of maleic acid (H₂M) and then with HM⁻ are:
H₂M + KOH → HM⁻ + H₂O + K⁺ (1)
HM⁻ + KOH → M²⁻ + H₂O + K⁺ (2)
For a complete transformation of H₂M in HM⁻ there are necessaries 7,952x10⁻³moles of KOH. As the moles of KOH are 0,0159 moles, the restant moles are:
0,0159 - 7,952x10⁻³ = <em>7,948x10⁻³ moles of KOH</em>
By (2), the moles produced of M²⁻ are the same as moles of KOH, <em>7,948x10⁻³ moles, </em>and moles of HM⁻ are:
7,952x10⁻³ -<em> </em>7,948x10⁻³ <em> = 4x10⁻⁶ moles of HM⁻</em>
Using Henderson-Hasselbalch formula:
pH = pka + log₁₀ [M²⁻] /[HM⁻]
pH = 6,27 + log₁₀ <em>7,948x10⁻³ / 4x10⁻⁶</em>
pH = 9,57
The moles of M²⁻ are 7,948x10⁻³ and volume of the solution is 0,1000L,
[M²⁻] = 7,948x10⁻²M
Moles of HM⁻ are 4x10⁻⁶:
[HM⁻] = 4x10⁻⁵M
And there is not H₂M:
[H₂M] = 0M
I hope it helps!