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2 years ago

Which one of the following combinations cannot function as a buffer solution?

Chemistry

1 answer:

ANEK [815]2 years ago

3 0

Answer:

c.) HNO₃ & NaNO₃

Explanation:

A buffer system has 2 components:

A weak acid and its conjugate base or
A weak base and its conjugate acid

Which one of the following combinations cannot function as a buffer solution?

a.) HCN & KCN. YES. HCN is a weak acid and CN⁻ (coming from KCN) its conjugate base.

b.) NH₃ & (NH₄)₂SO₄. YES. NH₃ is a weak base and NH₄⁺ (coming from (NH₄)₂SO₄) its conjugate acid.

c.) HNO₃ & NaNO₃. NO. HNO₃ is a strong acid.

d.) HF & NaF. YES. HF is a weak acid and F⁻ (coming from NaF) its conjugate base.

e.) HNO₂ & NaNO₂. YES. HNO₂ is a weak acid and NO₂⁻ (coming from NaNO₂) its conjugate base.

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Answer:

T2 = 94.6 C

Explanation:

Use Clausius-Clayperyon equation.

ln P1/P2 = ∆Hvap/R (1/T2 - 1/T1) where R = 8.314 J/mol-K and T is in degrees K

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R = 0.008314 kJ/mole-K (NOTE: change R to units of kJ)

Plug in and solve for T2

ln 760 mmHg/630 mmHg = 40.7 kJ/mole (1/T2 - 1/373K)

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2 years ago

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3 years ago

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A sample of an ideal gas has a volume of 2.31 l at 287 k and 1.10 atm. calculate the pressure when the volume is 1.45 l and the

balu736 [363]

Hello!

The pressure of the Ideal Gas when the volume is 1,45 L and the temperature is 298 K is 1,82 atm.

To solve this problem we need to apply the Ideal Gas Law for the initial conditions and the final ones, clearing the equation for the number of moles (n) and the ideal gas constant (R) which remain constant:

$P_n*V_n=n*R*T_n \\ \\ n*R= \frac{P_n*V_n}{T_n}$

Now we match n*R for the initial conditions (1) and the final ones (2), clearing the equation for P₂

$\frac{P_1*V_1}{T_1}= \frac{P_2*V_2}{T_2} \\ \\ P_2= \frac{P_1*V_1*T_2}{T_1*V_2}= \frac{1,10 atm*2,31 L *298 K}{287K*1,45 L}=1,82 atm$

Have a nice day!

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