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makvit [3.9K]
3 years ago
11

Determine the pH at the point in the titration of 40.0 mL of 0.200 M H₂NNH₂ with 0.100 M HNO₃ after 100.0 mL of the strong acid

has been added. The value of Kb for H₂NNH₂ is 3.0 × 10⁻⁶.
Chemistry
1 answer:
Irina-Kira [14]3 years ago
6 0

Answer:

pH = 1.85

Explanation:

The reaction of H₂NNH₂ with HNO₃ is::

H₂NNH₂ + HNO₃ → H₂NNH₃⁺ + NO₃⁻

Moles of H₂NNH₂ and HNO₃ are:

H₂NNH₂: 0.0400L ₓ (0.200mol / L) = 8.00x10⁻³ moles of H₂NNH₂

HNO₃: 0.1000L ₓ (0.100mol / L) = 0.01 moles of HNO₃

As moles of HNO₃ > moles of H₂NNH₂, all H₂NNH₂ will react producing H₂NNH₃⁺, but you will have an excess of HNO₃ (Strong acid).

Moles of HNO₃ in excess are:

0.01 mol - 8.00x10⁻³ moles = 2.00x10⁻³ moles of HNO₃ = moles of H⁺

Total volume is 100.0mL + 40.0mL = 140.0mL = 0.1400L.

Thus, [H⁺] is:

[H⁺] = 2.00x10⁻³ moles / 0.1400L = 0.0143M

As pH = - log [H⁺]

<h3>pH = 1.85 </h3>
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expeople1 [14]

Aluminum hydroxide \text{Al}(\text{OH})_3 can behave as a base and neutralize sulfuric acid \text{H}_2\text{SO}_4 as in the following equation:

2\;\text{Al}(\text{OH})_3 \; (s) + 3\; \text{H}_2\text{SO}_4 \; (aq) \to \text{Al}_2(\text{SO}_4)_3 \; (aq) + 6 \; \text{H}_2\text{O} \; (l) (Balanced)


(a)

n = m/M. Thus the ratio between the number of moles of the two reactants available:

n(\text{Al}(\text{OH})_3, \text{supplied}) / n(\text{H}_2\text{SO}_4, \text{supplied})\\= [m(\text{Al}(\text{OH})_3)/ M(\text{Al}(\text{OH})_3)] / [n(\text{H}_2\text{SO}_4) / M(\text{H}_2\text{SO}_4)]\\= [23.7 / (26.98 + 3 \times(16.00 + 1.008))]/[29.5 / (2 \times 1.008 + 32.07 + 4 \times 16.00)]\\\approx 1.01

The value of this ratio required to lead to a complete reaction is derived from coefficients found in the balanced equation:

n(\text{Al}(\text{OH})_3, \text{theoretical}) / n(\text{H}_2\text{SO}_4, \text{theoretical}) = 2/3 \approx 0.667

The ratio for the complete reaction is smaller than that of the reactants available, indicating that the species represented on the numerator, \text{Al}(\text{OH})_3, is in excess while the one on the denominator, \text{H}_2\text{SO}_4, serves as the limiting reagent.


(b)

The quantity of water produced is dependent on the amount of limiting reactants available. 29.5 / (2 \times 1.008 + 32.07 + 4 \times 16.00) = 0.301 \; \text{mol} of sulfuric acid is supplied in this reaction as the limiting reagent. 6 moles of water molecules are produced for every 3 moles of sulfuric acid consumed. The reaction would thus give rise to 0.301 \; \text{mol} \times 6/3 = 0.602 \; \text{mol} of water molecules, which have a mass of 0.602 \times (2 \times 1.008 + 16.00) = 10.8 \; \text{g}.


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\text{Percentage Yield}\\= \text{Actual Yield} / \text{Theoretical Yield} \times 100 \; \%\\= 2.21 / 10.8 \times 100 \; \%\\= 20.4 \; \%


(d)

The quantity of \text{Al}(\text{OH})_3, the reactant in excess, is dependent on the number of moles of this species consumed in the reaction and thus the quantity of the limiting reagent available. The consumption of every 3 moles of sulfuric acid, the limiting reagent, removes 2 moles of aluminum hydroxide \text{Al}(\text{OH})_3 from the solution. 0.301 \; \text{mol} of sulfuric acid is initially available as previously stated such that 0.301 \; \text{mol} \times 2/3 = 0.201 \; \text{mol}, or 0.201 \times (26.98 + 3 \time (16.00 + 1.008)) = 15.7 \; \text{g}, of \text{Al}(\text{OH})_3 would be eventually consumed.

23.7 - 15.7 = 8.0 \; \text{g} of \text{Al}(\text{OH})_3 would thus be in excess by the end of the reaction process.

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Answer:

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Explanation:

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a sample of hydrogen gas (h2) is mixed with water vapor (h2o (g)). the make sure has a total pressure of 811 torr, and the water
Alborosie

Answer:

n=0.430molH_2

Explanation:

Hello!

In this case, considering the partial Dalton's law of partial pressures, we can notice that the total pressure equals the pressure of steam and the pressure of hydrogen, which can be determined as shown below:

p_T=p_H+p_w\\\\p_H=811torr-12torr=799torr*\frac{1atm}{760torr}\\\\p_H=1.05atm

Thus, by using the ideal gas law, we can compute the moles of hydrogen as shown below:

PV=nRT\\\\n= \frac{PV}{RT}=\frac{1.05atm*10.0L}{0.082\frac{atm*L}{mol*K}*298K}\\\\n=0.430molH_2

Best regards!

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