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Katarina [22]
3 years ago
12

Hydroxylamine is a weak molecular base with kb = 6.6 x 10-9. what is the ph of a 0.0500 m solution of hydroxylamine?

Chemistry
1 answer:
7nadin3 [17]3 years ago
4 0
Answer is: pH of hydroxylamine solution is 9,23.

Kb(NH₂OH) = 1,8·10⁻⁵<span>.
c</span>₀(NH₂OH)<span> = 0,0500 M = 0,05 mol/L.
c(NH</span>₂⁺) = c(OH⁻) = x.

c(NH₂OH<span>) = 0,05 mol/L - x.
Kb = c(NH</span>₂⁺) · c(OH⁻) / c(NH₂OH).

0,0000000066 = x² /  (0,05 mol/L - x). 

solve quadratic equation: x = c(OH⁻) = 0,000018 mol/L.<span>
pOH = -log(</span>0,000018 mol/L) = 4,74.<span>
pH = 14 - 4,74 = 9,23.</span>


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Answer : The correct option is, (B) 0.11 M

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First we have to calculate the concentration PCl_3 and Cl_2.

\text{Concentration of }PCl_3=\frac{\text{Moles of }PCl_3}{\text{Volume of solution}}

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\text{Concentration of }Cl_2=\frac{\text{Moles of }Cl_2}{\text{Volume of solution}}

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The given equilibrium reaction is,

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Initially                 0.70        0.70              0

At equilibrium    (0.70-x)   (0.70-x)           x

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K_c=\frac{(x)}{(0.70-x)\times (0.70-x)}

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x=0.59\text{ and }0.83

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The concentration of PCl_5 at equilibrium = x = 0.59 M

Therefore, the concentration of PCl_3 at equilibrium is 0.11 M

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