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ira [324]
4 years ago
6

A buffer consists of 0.45 M CH3COOH (acetic acid) and 0.35 M CH3COONa. The Ka of acetic acid is 1.8 x 10-5 . a) Calculate the pH

of the buffer solution. b) Calculate the pH after 5.0 mL of 2.0 M NaOH have been added to 400 mL of the original buffer solution.

Chemistry
1 answer:
Zigmanuir [339]4 years ago
8 0

Answer:

A) pH of Buffer solution = 4.59

B) pH after 5.0 ml of 2.0 M NaOH have been added to 400 ml of the original    buffer solution = 4.65

Explanation:

This  is the Henderson-Hasselbalch Equation:

 pH = pKa + log\frac{[conjugate base]}{[acid]}

to calculate the pH of the following Buffer solutions.

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Answer:

392

Explanation:

According to the law of conservation of energy, energy cannot vanish,so the lost potential energy must be converted into another form of energy (in this case, Kinetic Energy).

(mass*g*height)-(mass*g*halfway height)=(2*9.8*40)-(2*9.8*20)

784-392=392

This makes sense because since the rock has fallen halfway, half of its potential energy has become kinetic energy. Once the rock reaches a height of 0 Meter, all of its potential energy will be kinetic energy.

8 0
3 years ago
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4 0
3 years ago
Can you please help me?
lorasvet [3.4K]

Answer:

60 moles of NaF

Explanation:

The balanced equation for the reaction is given below:

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From the balanced equation above,

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Therefore, Xmol of NaF will react to produce 20 moles of AlF3 i.e

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Xmol of NaF = 60 moles

Therefore, 60 moles of NaF are required to produce 20 moles of AlF3.

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