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3 years ago

What mass of HCl is needed to prepare 1.00 mole of Cl₂? 2 KMnO₄ + 16 HCl → 2MnCl₂ + 5 Cl₂ + 8 H₂O + 2 KCl

Chemistry

1 answer:

dsp733 years ago

8 0

Answer:

117 g HCl

Explanation:

use a molar ratio to cancel out the moles of Cl2

1.00 mol Cl2 x 16 mol HCl / 5 mol Cl2

multiply by the molar mass of HCl to get the mass of the HCl

3.2 mol HCl x 36.46 g HCl

then you should get around

116.672 g HCl

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2 years ago

Write balanced net ionic equations and the corresponding equilibrium equations for the stepwise dissociation of the triprotic ac

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Answer:

$H_3PO_4(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+H_2PO_4^{-}(aq); \ Ka_1$

$H_2PO_4^{-}(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+HPO_4^{-2}(aq); \ Ka_2$

$HPO_4^{-2}(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+PO_4^{-3}(aq); \ Ka_3$

Explanation:

Hello!

In this case, since the phosphoric acid is a triprotic acid, we infer it has three stepwise ionization reactions in which one hydrogen ion is released at each step, considering they are undergone due to the presence of water, thus, we proceed as follows:

$H_3PO_4(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+H_2PO_4^{-}(aq); \ Ka_1$

$H_2PO_4^{-}(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+HPO_4^{-2}(aq); \ Ka_2$

$HPO_4^{-2}(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+PO_4^{-3}(aq); \ Ka_3$

Moreover, notice each step has a different acid dissociation constant, which are quantified in the following order:

Ka1 > Ka2 > Ka3

Best regards!

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