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Zigmanuir [339]
3 years ago
5

Oxalic acid is a polyprotic acid. Write balanced chemical equations for the sequence of reactions that oxalic acid can undergo w

hen it's dissolved in water

Chemistry
1 answer:
tiny-mole [99]3 years ago
8 0

The chemical formula of oxalic is H_{2}C_{2}O_{4}

When oxalic acid reacts with water, first, oxalic acid removes one proton and results in the formation of mono acids.

After that, in second step, oxalic acid in aqueous solution removes another proton which shows it is a polyprotic acid.

The chemical equations are: (the reactions occurs in two steps due to presence to hydrogen atoms).

When one proton is removed:

H_{2}C_{2}O_{4} (aq)+H_{2}O (l)\rightarrow HC_{2}O_{4}^{-}(aq)+H_{3}O^{+}(aq)

When another proton is removed:

HC_{2}O_{4}^{-} (aq)+H_{2}O (l)\rightarrow C_{2}O_{4}^{2-}(aq)+H_{3}O^{+}(aq)

The dissociation of oxalic acid in water in shown in the image.






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Answer:

MM_{acid}=140.1g/mol

Explanation:

Hello,

In this case, since the acid is monoprotic, we can notice a 1:1 molar ratio between, therefore, for the titration at the equivalence point, we have:

n_{acid}=n_{base} \\\\V_{acid}M_{acid}=V_{base}M_{base}\\\\n_{acid}=V_{base}M_{base}

Thus, solving for the moles of the acid, we obtain:

n_{acid}=0.0215L*0.250\frac{mol}{L}=5.375x10^{-3}mol

Then, by using the mass of the acid, we compute its molar mass:

MM_{acid}=\frac{0.753g}{5.375x10^{-5}mol} \\\\MM_{acid}=140.1g/mol

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The equilibrium constant Kc for the decomposition of phosgene, COCl2, is 4.63x10^-3 at 527 C. Calculate the equilibrium partial
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<u>Answer:</u> The partial pressure of the CO,Cl_2\text{ and }COCl_2 are 0.352 atm, 0.352 atm and 0.408 atm respectively.

<u>Explanation:</u>

We are given:

K_c=4.63\times 10^{-3}

p_{COCl_2}=0.760atm

Relation of K_p with K_c is given by the formula:

K_p=K_c(RT)^{\Delta ng}

Where,

K_p = equilibrium constant in terms of partial pressure = ?

K_c = equilibrium constant in terms of concentration = 4.63\times 10^{-3}

R = Gas constant = 0.0821\text{ L atm }mol^{-1}K^{-1}

T = temperature = 527^oC=527+273=800K

\Delta ng = change in number of moles of gas particles = n_{products}-n_{reactants}=2-1=1

Putting values in above equation, we get:

K_p=4.63\times 10^{-3}\times (0.0821\times 800)^{1}\\\\K_p=0.304

The chemical reaction for the decomposition of phosgene follows the equation:

                   COCl_2(g)\rightleftharpoons CO(g)+Cl_2(g)

At t = 0          0.760            0     0  

At t=t_{eq}      0.760-x          x      x

The expression for K_p for the given reaction follows:

K_p=\frac{p_{CO}\times p_{Cl_2}}{p_{COCl_2}}

We are given:

K_p=0.304\\p_{COCl_2}=0.760-x\\p_{CO}=x\\p_{Cl_2}=x

Putting values in above equation, we get:

0.304=\frac{x\times x}{0.760-x}\\\\x=0.352,-0.656

Negative value of 'x' is neglected because partial pressure cannot be negative.

So, the partial pressure for the components at equilibrium are:

p_{COCl_2}=0.760-0.352=0.408atm\\\\p_{CO}=0.352atm\\\\p_{Cl_2}=0.352atm

Hence, the partial pressure of the CO,Cl_2\text{ and }COCl_2 are 0.352 atm, 0.352 atm and 0.408 atm respectively.

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