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Ymorist [56]
3 years ago
14

How does a buffer work?

Chemistry
1 answer:
Margarita [4]3 years ago
8 0

Answer:

It bonds with the added H+ or OH in solution.

Explanation:

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SOVA2 [1]

Answer:

picture not bright

Explanation:

please a brainliest for tge feedback

7 0
2 years ago
Standard reduction potentials for nickel(II) and copper(II) The standard reduction potential for a substance indicates how readi
AleksandrR [38]

Answer:

The standard potential, E cell, for this galvanic cell is 0.5670V

Explanation:

Ni²⁺(aq)  +  2e⁻   →   Ni(s)           E red =  - 0.23V      ANODE

Cu²⁺(aq) +  2e-    →  Cu(s)          E red = + 0.337V    CATHODE

ΔE° = E cathode - E anode

ΔE° = 0.337V - (0.23V) = 0.5670 V

6 0
2 years ago
A buffer solution contains 0.345 M acetic acid and 0.377 M sodium acetate . If 0.0613 moles of potassium hydroxide are added to
melamori03 [73]

Answer:

pH = 5.54

Explanation:

The pH of a buffer solution is given by the <em>Henderson-Hasselbach (H-H) equation</em>:

  • pH = pKa + log\frac{[CH_3COO^-]}{[CH_3COOH]}

For acetic acid, pKa = 4.75.

We <u>calculate the original number of moles for acetic acid and acetate</u>, using the <em>given concentrations and volume</em>:

  • CH₃COO⁻ ⇒ 0.377 M * 0.250 L = 0.0942 mol CH₃COO⁻
  • CH₃COOH ⇒ 0.345 M * 0.250 L = 0.0862 mol CH₃COOH

The number of CH₃COO⁻ moles will increase with the added moles of KOH while the number of CH₃COOH moles will decrease by the same amount.

Now we use the H-H equation to <u>calculate the new pH</u>, by using the <em>new concentrations</em>:

  • pH = 4.75 + log\frac{(0.0942+0.0613)mol/0.250L}{(0.0862-0.0613)mol/0.250L} = 5.54
6 0
3 years ago
What would cause the equilibrium to shift left in this reaction? CO + 3H2 ? CH4 + H2O A. Adding heat to the product mixture B. A
Irina-Kira [14]

Answer:

Pretty sure the answer is A on Plato

Explanation:

I looked it up, and it said that raising the temperature would cause the equilibrium to shift left.

8 0
3 years ago
Read 2 more answers
The AP Biology teacher is measuring out 638.0 g of dextrose (C6H12O6) for a lab. How many moles of dextrose is this equivalent t
Katena32 [7]

The AP Biology teacher is measuring out 638.0 g of dextrose (C6H12O6) for a lab the moles of dextrose is this equivalent to is 3.6888 moles.

<h3>What are moles?</h3>

A mole is described as 6.02214076 × 1023 of a few chemical unit, be it atoms, molecules, ions, or others. The mole is a handy unit to apply due to the tremendous variety of atoms, molecules, or others in any substance.

To calculate molar equivalents for every reagent, divide the moles of that reagent through the moles of the restricting reagent. The calculation is follows:

  • 655/12 x 6 + 12+ 16 x 6
  • = 655/ 180 = 3.6888 moles.

Read more about moles:

brainly.com/question/24322641

#SPJ1

6 0
1 year ago
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