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Olenka [21]
3 years ago
8

When Phosphoric Acid behaves according to arrhenius theory in water, what are the two products formed by the first proton

Chemistry
1 answer:
bagirrra123 [75]3 years ago
5 0

Answer:

Phosphoric acid is a triprotic acid. This means that it can dissociate in water up to three times, each time releasing a proton into the water as shown in the following reactions:

H3PO4 (s) + H2O (l) is in equilibrium with H3O + (aq) + H2PO4− (aq)

H2PO4− (aq) + H2O (l) is in equilibrium with H3O + (aq) + HPO42− (aq)

HPO42− (aq) + H2O (l) is in equilibrium with H3O + (aq) + PO43− (aq)

Explanation:

Phosphoric acid having contact with water, dissociating from a proton up to three times, that is why the three possible reactions are determined above.

This acid is an acid that belongs to oxo acids and its formula is H3PO4

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If you added 45,000 calories to water that was at 25 degrees C, and the ending temperature was 35 degrees C, how much water did
user100 [1]

<u>Answer:</u>

<em>4.5 L water we have in litres (L).</em>

<em><u></u></em>

<u>Explanation:</u>

Q=m\times c \times \Delta T

where

\Delta T = Final T - Initial T

Q is the heat energy in calories

c is the specific heat capacity (for water 1.0  cal/(g℃))  

m is the mass of water

Plugging in the values  

\\$45000 \mathrm{cal}=m \times 1.0 \frac{\mathrm{cal}}{\mathrm{g}^{\circ} \mathrm{C}} \times\left(35^{\circ} \mathrm{C}-25^{\circ} \mathrm{C}\right)$\\\\$45000 \mathrm{cal}=m \times 1.0 \frac{\mathrm{cal}}{\mathrm{g}^{\circ} \mathrm{C}} \times 10^{\circ} \mathrm{C}$\\\\$m=\frac{45000 \mathrm{cal}}{1.0 \frac{\mathrm{cal}}{\mathrm{g}^{\circ} \mathrm{C}} \times 10^{\circ} \mathrm{C}}$\\\\$m=4500 \mathrm{g}$\\\\Density of water $=\frac{\text { mass }}{\text { volume }}$

So,

Volume of water = mass/density

\\\\=\frac{4500 \mathrm{g}}{\frac{1.09}{\mathrm{mL}}}=4500 \mathrm{mL}$$

=4.5 L (Answer)

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