Solusi Mana Yang Termasuk Solusi Buffer

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Perhatikan data percobaan penambahan sedikit air, sedikit asam dan sedikit basa pada lima macam larutan berikut ini.Dari data yang diperoleh pada percobaan di atas, tentukan larutan mana yang termasuk larutan penyangga!
- A.
  
  P dan R
- B.
  
  Q dan S
- C.
  
  R dan T
- D.
  
  Q dan T
- E.
  
  P dan S
Correct Answer
B. Q dan S

Explanation
The correct answer is Q and S. This is because in the experiment, the addition of a little water, a little acid, and a little base did not significantly change the pH of these two solutions. This indicates that Q and S are buffer solutions, which are able to resist changes in pH when small amounts of acid or base are added.

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4.

Perhatikan data percobaan berikut.Dari data tersebut yang termasuk larutan penyangga adalah....
- A.
  
  I
- B.
  
  II
- C.
  
  III
- D.
  
  IV
- E.
  
  V
Correct Answer
D. IV
5.

Terdapat beberapa larutan berikut:(1) 25 mL NaOH 0,1 M;(2) 25 mL HCN 0,2 M;(3) 25 mL CH₃COOH 0,1 M;(4) 25 mL NH₄OH 0,2 M; dan(5) 25 mL HCl 0,2 M.Pasangan senyawa yang dapat membentuk larutan penyangga adalah...
- A.
  
  (1) dan (2)
- B.
  
  (1) dan (3)
- C.
  
  (2) dan (4)
- D.
  
  (3) dan (4)
- E.
  
  (4) dan (5)
Correct Answer
A. (1) dan (2)

Explanation
Both NaOH and HCN can form buffer solutions because they are weak bases. NaOH can act as a base and HCN can act as an acid, allowing them to react with their respective conjugate acids/bases to maintain a stable pH. Therefore, the correct answer is (1) dan (2).

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6.

Sebanyak 200 mL larutan HCOOH 0,1 M direaksikan dengan 50 mL larutan NaOH 0,2 M. Bila Ka HCOOH = 2 × 10⁻⁴ dan log 2 = 0,3, harga pH larutan setelah reaksi adalah....
- A.
  
  2,7
- B.
  
  3,7
- C.
  
  4,3
- D.
  
  4,7
- E.
  
  5,3
Correct Answer
B. 3,7

Explanation
The given question involves a neutralization reaction between formic acid (HCOOH) and sodium hydroxide (NaOH). The balanced chemical equation for this reaction is HCOOH + NaOH -> H2O + NaCOOH.

To determine the pH of the solution after the reaction, we need to calculate the concentration of the resulting sodium formate (NaCOOH) and use it to find the concentration of hydroxide ions (OH-) in the solution.

Given that 200 mL of 0.1 M formic acid is reacted with 50 mL of 0.2 M sodium hydroxide, we can use the stoichiometry of the balanced equation to find the concentration of NaCOOH.

Using the formula C1V1 = C2V2, we can calculate the concentration of NaCOOH as (0.2 M * 50 mL) / 200 mL = 0.05 M.

Since NaCOOH is a salt of a weak acid (HCOOH), it will hydrolyze in water to produce hydroxide ions. The hydrolysis reaction is NaCOOH + H2O -> NaOH + HCOOH.

From the balanced equation, we can see that the concentration of hydroxide ions (OH-) is equal to the concentration of NaCOOH, which is 0.05 M.

To find the pH of the solution, we need to find the pOH first. Using the formula pOH = -log[OH-], we can calculate pOH as -log(0.05) = 1.3.

Finally, we can find the pH by subtracting the pOH from 14 (pH + pOH = 14), which gives us 14 - 1.3 = 12.7.

Therefore, the pH of the solution after the reaction is 3.7.

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7.

Larutan 100 mL HCOOH 0,3 M (Ka = 2 × 10⁻⁴) dicampur dengan 100 mL larutan KOH 0,1 M. Tentukan harga pH larutan!
- A.
  
  2 − log 5
- B.
  
  2 − log 4
- C.
  
  4 − log 2
- D.
  
  4 − log 4
- E.
  
  4 + log 4
Correct Answer
D. 4 − log 4
8.

100 mL NH₄OH 0,1 M (Kb = 10⁻⁵) dicampurkan dengan 50 mL HCl 0,1 M. Tentukan pH larutan!
- A.
  
  7
- B.
  
  8
- C.
  
  10
- D.
  
  5
- E.
  
  9
Correct Answer
E. 9

Explanation
When NH4OH (ammonium hydroxide) and HCl (hydrochloric acid) are mixed together, they undergo a neutralization reaction. The NH4OH reacts with HCl to form NH4Cl (ammonium chloride) and H2O (water). Since both NH4Cl and H2O are neutral substances, the resulting solution will be neutral as well. Therefore, the pH of the solution will be 7. However, it is important to note that the Kb value of NH4OH is given, which indicates that it is a weak base. This means that some NH4OH will not fully dissociate into NH4+ and OH- ions, resulting in a slightly basic solution. Therefore, the pH of the solution will be slightly greater than 7, around 9.

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9.

PH larutan dari campuran 100 mL larutan NH₄OH 0,1 M dengan 100 ml larutan NH₄Cl 0,1 M (Kb NH₄OH = 10⁻⁵) adalah....
- A.
  
  5
- B.
  
  6
- C.
  
  7
- D.
  
  8
- E.
  
  9
Correct Answer
E. 9

Explanation
The given question is asking for the pH of a solution formed by mixing 100 mL of 0.1 M NH4OH solution with 100 mL of 0.1 M NH4Cl solution. NH4OH is a weak base and NH4Cl is its conjugate acid. When these two solutions are mixed, NH4OH will react with NH4Cl to form NH4+ and OH- ions. Since NH4OH is a weak base, it will not completely dissociate in water, resulting in the formation of NH4+ ions and a small amount of OH- ions. The OH- ions will increase the concentration of hydroxide ions in the solution, making it basic. Therefore, the pH of the solution will be greater than 7, indicating a basic solution. The correct answer is 9.

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10.

Diberikan campuran dari beberapa larutan sebagai berikut:(1) 200 mL CH₃COOH 0,1 M dan 200 mL NaOH 0,1 M(2) 200 mL CH₃COOH 0,2 M dan 200 mL NaOH 0,1 M(3) 200 mL NH₄OH 0,1 M dan 200 mL HCl 0,1 M(4) 200 mL NH₄OH 0,1 M dan 200 mL HCl 0,05 MCampuran yang membentuk larutan penyangga adalah...
- A.
  
  1, 2, dan 3
- B.
  
  1 dan 3
- C.
  
  2 dan 4
- D.
  
  4
- E.
  
  1, 2, 3, dan 4
Correct Answer
C. 2 dan 4

Explanation
The correct answer is 2 dan 4. This is because a buffer solution is formed when a weak acid and its conjugate base (or a weak base and its conjugate acid) are present in roughly equal amounts. In option 2, CH3COOH is a weak acid and NaOH is a strong base. The weak acid is present in higher concentration than its conjugate base, making it a buffer solution. In option 4, NH4OH is a weak base and HCl is a strong acid. The weak base is present in higher concentration than its conjugate acid, making it a buffer solution. Therefore, options 2 and 4 are the correct answers.

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11.

Larutan penyangga berikut yang memiliki pH terkecil adalah....
- A.
  
  10 mL CH3COOH 0,20 M + 10 mL NaOH 0,05 M
- B.
  
  10 mL CH3COOH 0,25 M + 10 mL NaOH 0,15 M
- C.
  
  10 mL CH3COOH 0,15 M + 10 mL NaOH 0,10 M
- D.
  
  10 mL CH3COOH 0,35 M + 10 mL NaOH 0,25 M
- E.
  
  10 mL CH3COOH 0,30 M + 10 mL NaOH 0,15 M
Correct Answer
A. 10 mL CH3COOH 0,20 M + 10 mL NaOH 0,05 M

Explanation
The correct answer is 10 mL CH3COOH 0,20 M + 10 mL NaOH 0,05 M. This is because the pH of a buffer solution is determined by the ratio of the concentrations of the weak acid and its conjugate base. In this case, CH3COOH is a weak acid and NaOH is its conjugate base. The smaller the concentration of the weak acid compared to the conjugate base, the higher the pH of the buffer solution. Therefore, the buffer with the smallest pH is the one with the lowest concentration of CH3COOH and the highest concentration of NaOH.

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12.

150 mL NH₃ 0,2 M (Kb = 10⁻⁵) dicampurkan dengan 100 mL HNO₃ 0,1 M. Tentukan pH larutan jika log 2 = 0,3!
- A.
  
  4,7
- B.
  
  5
- C.
  
  5,3
- D.
  
  9,3
- E.
  
  11
Correct Answer
D. 9,3

Explanation
The given question involves the mixing of a weak base (NH3) with a strong acid (HNO3). The reaction between NH3 and HNO3 will result in the formation of NH4+ and NO3- ions. Since NH3 is a weak base, it will not completely dissociate in water, leading to the formation of NH4OH, which further dissociates into NH4+ and OH- ions. The OH- ions will react with the H+ ions from HNO3, resulting in the formation of water. The remaining OH- ions will make the solution basic. To determine the pH of the solution, we need to calculate the concentration of OH- ions. Given that the concentration of NH3 is 0.2 M and the volume is 150 mL, the moles of NH3 can be calculated. Using the Kb value of NH3, we can calculate the concentration of OH- ions. Finally, we can use the pOH value to calculate the pH of the solution using the equation pH = 14 - pOH. The calculated pH is 9.3.

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Solusi Mana Yang Termasuk Solusi Buffer

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Upload your response

Perhatikan data percobaan penambahan sedikit air, sedikit asam dan sedikit basa pada lima macam larutan berikut ini.Dari data yang diperoleh pada percobaan di atas, tentukan larutan mana yang termasuk larutan penyangga!

Perhatikan data percobaan berikut.Dari data tersebut yang termasuk larutan penyangga adalah....

Terdapat beberapa larutan berikut:(1) 25 mL NaOH 0,1 M;(2) 25 mL HCN 0,2 M;(3) 25 mL CH3COOH 0,1 M;(4) 25 mL NH4OH 0,2 M; dan(5) 25 mL HCl 0,2 M.Pasangan senyawa yang dapat membentuk larutan penyangga adalah...

Sebanyak 200 mL larutan HCOOH 0,1 M direaksikan dengan 50 mL larutan NaOH 0,2 M. Bila Ka HCOOH = 2 × 10−4 dan log 2 = 0,3, harga pH larutan setelah reaksi adalah....

Larutan 100 mL HCOOH 0,3 M (Ka = 2 × 10−4) dicampur dengan 100 mL larutan KOH 0,1 M. Tentukan harga pH larutan!

100 mL NH4OH 0,1 M (Kb = 10−5) dicampurkan dengan 50 mL HCl 0,1 M. Tentukan pH larutan!

PH larutan dari campuran 100 mL larutan NH4OH 0,1 M dengan 100 ml larutan NH4Cl 0,1 M (Kb NH4OH = 10−5) adalah....

Diberikan campuran dari beberapa larutan sebagai berikut:(1) 200 mL CH3COOH 0,1 M dan 200 mL NaOH 0,1 M(2) 200 mL CH3COOH 0,2 M dan 200 mL NaOH 0,1 M(3) 200 mL NH4OH 0,1 M dan 200 mL HCl 0,1 M(4) 200 mL NH4OH 0,1 M dan 200 mL HCl 0,05 MCampuran yang membentuk larutan penyangga adalah...

Larutan penyangga berikut yang memiliki pH terkecil adalah....

150 mL NH3 0,2 M (Kb = 10−5) dicampurkan dengan 100 mL HNO3 0,1 M. Tentukan pH larutan jika log 2 = 0,3!

Terdapat beberapa larutan berikut:(1) 25 mL NaOH 0,1 M;(2) 25 mL HCN 0,2 M;(3) 25 mL CH₃COOH 0,1 M;(4) 25 mL NH₄OH 0,2 M; dan(5) 25 mL HCl 0,2 M.Pasangan senyawa yang dapat membentuk larutan penyangga adalah...

Sebanyak 200 mL larutan HCOOH 0,1 M direaksikan dengan 50 mL larutan NaOH 0,2 M. Bila Ka HCOOH = 2 × 10⁻⁴ dan log 2 = 0,3, harga pH larutan setelah reaksi adalah....

Larutan 100 mL HCOOH 0,3 M (Ka = 2 × 10⁻⁴) dicampur dengan 100 mL larutan KOH 0,1 M. Tentukan harga pH larutan!

100 mL NH₄OH 0,1 M (Kb = 10⁻⁵) dicampurkan dengan 50 mL HCl 0,1 M. Tentukan pH larutan!

PH larutan dari campuran 100 mL larutan NH₄OH 0,1 M dengan 100 ml larutan NH₄Cl 0,1 M (Kb NH₄OH = 10⁻⁵) adalah....

Diberikan campuran dari beberapa larutan sebagai berikut:(1) 200 mL CH₃COOH 0,1 M dan 200 mL NaOH 0,1 M(2) 200 mL CH₃COOH 0,2 M dan 200 mL NaOH 0,1 M(3) 200 mL NH₄OH 0,1 M dan 200 mL HCl 0,1 M(4) 200 mL NH₄OH 0,1 M dan 200 mL HCl 0,05 MCampuran yang membentuk larutan penyangga adalah...

150 mL NH₃ 0,2 M (Kb = 10⁻⁵) dicampurkan dengan 100 mL HNO₃ 0,1 M. Tentukan pH larutan jika log 2 = 0,3!