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faust18 [17]
3 years ago
12

2.5 moles of sodium chloride is dissolved to make 0.050 liters of solution

Chemistry
1 answer:
Hitman42 [59]3 years ago
7 0

The answer is:

the molarity = 50 moles/liters

The explanation:

when the molarity is = the number of moles / volume per liters.

and when the number of moles =2.5 moles

and the volume per liters = 0.05 L

so by substitution:

the molarity = 2.5moles/0.05L

                    = 50 moles /L

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Phosphorous acid, H 3 PO 3 ( aq ) , is a diprotic oxyacid that is an important compound in industry and agriculture. p K a1 p K
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Explanation:

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3 years ago
Which subatomic particle is the identity of the atom and why?
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Phosphoric acid is a triprotic acid ( K a1 = 6.9 × 10 − 3 Ka1=6.9×10−3, K a2 = 6.2 × 10 − 8 Ka2=6.2×10−8, and K a3 = 4.8 × 10 −
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<u>Answer:</u> To calculate the pH of the buffer composed of H_2PO_4^-\text{ and }HPO_4^{-2}, we use the K_a2

<u>Explanation:</u>

Phosphoric acid is a triprotic acid and it will undergo three dissociation reaction each having their respective dissociation constants.

The chemical equation for the first dissociation reaction follows:

H_3PO_4\rightleftharpoons H_2PO_4^-+H^+;K_a1=6.9\times 10^{-3}

The chemical equation for the second dissociation reaction follows:

H_2PO_4^-\rightleftharpoons HPO_4^{2-}+H^+;K_a2=6.2\times 10^{-8}

The chemical equation for the third dissociation reaction follows:

HPO_4^{2-}\rightleftharpoons PO_4^{3-}+H^+;K_a3=4.8\times 10^{-13}

To form a buffer composed of H_2PO_4^-\text{ and }HPO_4^{-2}, we use the K_a of second dissociation process

To calculate the pK_a, we use the equation:

pK_a=-\log (K_a)\\\\pK_a=-\log(6.2\times 10^{-8})\\\\pK_a=7.21

To calculate the pH of buffer, we use the equation given by Henderson Hasselbalch:

pH=pK_a2+\log(\frac{[\text{conjugate base}]}{[\text{weak acid}]})

pH=pK_a2+\log(\frac{[HPO_4^{2-}]}{[H_2PO_4^-]})

We are given:

pK_a2 = negative logarithm of second acid dissociation constant of phosphoric acid = 7.21

[HPO_4^{2-}] = concentration of conjugate base

[H_2PO_4^{-}] = concentration of weak acid

Hence, to calculate the pH of the buffer composed of H_2PO_4^-\text{ and }HPO_4^{-2}, we use the K_a2

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