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Vsevolod [243]
3 years ago
15

A solution is prepared by adding 100 mL of 1.0 M HC₂H₃O₂(aq) to 100 mL of 1.0 M NaC₂H₃O₂(aq). The solution is stirred and its pH

is measured to be 4.73. After 3 drops of 1.0 M HCl are added to the solution, the pH of the solution is measured and is still 4.73. Which of the following equations represents the chemical reaction that accounts for the fact that acid was added but there was no detectable change in pH?
(A) H_3O^+(aq) + OH^-(aq) \rightarrow 2 H_2O(l)
(B) H_3O^+(aq) + Cl^-(aq) \rightarrow HCl(g) + H_2O(l)
(C) H_3O^+(aq) + C_2H_3O_2^-(aq) \rightarrow HC_2H_3O_2(aq) + H_2O(l)
(D) H_3O^+(aq) + HC_2H_3O_2(aq) \rightarrow H_2C_2H_3O^+(aq) + H_2O(l)
Chemistry
1 answer:
anastassius [24]3 years ago
3 0

Answer: Option (c) is the correct answer.

Explanation:

When an acid or base is added to a solution then any resistance by the solution in changing the pH of the solution is known as a buffer.

This is because a buffer has the ability to not get affected by the addition of small amounts of an acid or a base. As a result, it helps in maintaining the pH of the solution.

In the give case, when we add the HCl then more number of protons will dissociate. This causes the acetate to react with the protons and leads to the formation of acetic acid.

We know that acetic acid is a weak acid and it dissociates partially or feebly. Therefore, no change in pH will take place.

Thus, we can conclude that equation H_{3}O^{+}(aq) + C_{2}H_{3}O^{-}_{2}(aq) \rightarrow HC_{2}H_{3}O_{2}(aq) + H_{2}O(l) represents the chemical reaction that accounts for the fact that acid was added but there was no detectable change in pH.

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(30 Points) You need to produce a buffer solution that has a pH of 5.02. You already have a solution that contains 10. mmol (mil
chubhunter [2.5K]
<span>By definition:

pH = pKa + log [acetate]/ [acetic acid]

so

5.02 = 4.74 + log [acetate] / 10 mmole

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8 0
3 years ago
Read 2 more answers
What is the total amount of heat released when 94.0 g water at 80.0 °C cools to form ice at −30.0 °C?
Wewaii [24]

Answer:

The total amount of heat released  is  68.7 kJ

Explanation:

Given that:

mass of water = 94.0 g

moles of water = 94 / 18.02 = 5.216

80⁰C   ------>  0⁰C  -------->    -30⁰C

Q1 = m Cp dT

      = 94 x 4.184 x (0 - 80)

     = -31463.68 J

     = -31.43 kJ

Q2 = 6.01 x 10^3 x 5.216

    = - 31348.16 J

   = -31.35 kJ

Q3 = - 94 x 2.09 x 30

    = - 5893.8 J

   = -5.894 kJ

Total heat = Q1 + Q2 + Q3  = -31.43 kJ  + (-31.35 kJ  ) + (-5.894 kJ )  = -68.7 kJ

Total heat released = -68.7 kJ

Note that the "negative sign" simply indicates heat released, therefore no need to put it in the answer.

6 0
3 years ago
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