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nekit [7.7K]
3 years ago
12

Why will the conjugate base of a weak acid affect pH? Select the correct answer below: it will react with hydroxide

Chemistry
1 answer:
GREYUIT [131]3 years ago
4 0

The question is incomplete; the complete question is;

Why will the conjugate base of a weak acid affect pH? Select the correct answer below: O it will react with hydroxide

O it will react with water

O it will react with hydronium

O none of the above Content attribution

Answer:

O it will react with hydronium

Explanation:

If we have a weak acid HA, the weak acid ionizes as follows;

HA(aq) ----> H^+(aq) + A^-(aq)

A^- is the conjugate base of the weak acid.

H^+ interacts with water to form the hydronium ion as follows;

H^+(aq) + H2O(l) ----> H3O^+(aq)

The pH=[H3O^+]

But the conjugate base of the weak acid reacts with this hydronium ion thereby affecting its concentration and the pH of the system as follows;

A^-(aq) + H3O^+(aq) ------> HA(aq) + H2O(l)

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1.33 dm3 of water at 70°C are saturated by 2.25
astraxan [27]

Given that 4.50 dm³ of Pb(NO₃)₂ is cooled from 70 °C to 18 °C, the

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<h3>How can the amount of solute deposited be found?</h3>

The volume of water 1.33 dm³ of water 70 °C.

The number of moles of Pb(NO₃)₂ that saturates 1.33 dm³ of water at 70 °C  = 2.25 moles

At 18 °C, the number of moles of Pb(NO₃)₂ that saturates 1.33 dm³ of water = 0.53 moles

Therefore;

Number of moles of Pb(NO₃)₂ in 4.50 dm³ at 70 °C is therefore;

1.33 dm³ contains 2.25 moles.

Number \ of \ moles \ in \ 4.50 \ dm^3 = \dfrac{2.25}{1.33} \times 4.50 \approx \mathbf{7.613 \, moles}

Number of moles of Pb(NO₃)₂ in 4.50 dm³ at 70 °C ≈ 7.613 moles

Number of moles of Pb(NO₃)₂ in 4.50 dm³ at 18 °C is therefore;

1.33 dm³ contains 0.53 moles

Number \ of \ moles \ in \ 4.50 \ dm^3 = \dfrac{0.53}{1.33} \times 4.50 \approx \mathbf{1.79 \, moles}

Number of moles of Pb(NO₃)₂ in 4.50 dm³ at 18 °C ≈ 1.79 moles

The number of moles that precipitate out = The amount of solute deposited

Which gives;

Amount of solute deposited = 7.613 moles - 1.79 moles = 5.823 moles

The molar mass of Pb(NO₃)₂ = 207 g + 2 × (14 g + 3 × 16 g) = 331 g

The molar mass of Pb(NO₃)₂ = 331 g/mol

The amount of solute deposited = Number of moles × Molar mass

Which gives;

The amount of solute deposited = 5.823 moles × 331 g/mol =<u> 1,927.413 g </u>

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The lightest weight that is not a gas
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Explanation:

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