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stepladder [879]
2 years ago
12

Find the [H+] in an acetic acid solution that has a pH of 5.12

Chemistry
1 answer:
Eva8 [605]2 years ago
3 0
<span>Data:
pH = 5.2
[H+] = ?

Knowing that: (</span><span>Equation to find the pH of a solution)</span>
pH = -log[H+]
<span>
Solving:
</span>pH = -log[H+]
5.2 = - log [H+]
Knowing that the exponential is the opposite operation of the logarithm, then we have:
[H+] = 10^{-5.2}
\boxed{\boxed{[H+] = 6.30*10^{-6}}}\end{array}}\qquad\quad\checkmark
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galvanic cell is powered by the following redox reaction: (g) (aq) (l)(aq) (s) (aq) Answer the following questions about this ce
kotykmax [81]

Answer:

Explanation:

1. the 1/2 reaction that occurs at the cathode

3Cl2(g) +6e^- -------------> 6Cl^- (aq)

2 the 1/2 reaction that occurs at the anode

2MnO2(s) + 8OH^-(aq) ----------> 2MnO4^- (aq) + 4H2O(l) +6e^-      

2MnO2(s) + 8OH^-(aq) ----------> 2MnO4^- (aq) + 4H2O(l) +6e^-

E0 = -0.59v

3Cl2(g) +6e^- -------------> 6Cl^- (aq)                                                  

E0 = 1.39v

3Cl2 (g) + 2MnO2 (s) + 8OH^(−) (aq)---------> 6Cl^(−) (aq) + 2MnO4^(−) (aq) + 4H2O (l)  

E0cell = 0.80v

5 0
3 years ago
How many moles of glucose (C6H12O6) are in 1.5 liters of a 4.5 M C6H12O6 solution?
lisov135 [29]
Moles of glucose = Molarity x volume solution 
                              = 4.5 x 1.5
                              = 6.75 moles.

Hope this helps, have a great day ahead!
3 0
3 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
The pOH of a solution of KOH is 11.30. What is the [H*] for this solution?​
Sloan [31]

Answer: The concentration of hydrogen ions for this solution is 1.99 \times 10^{-3}.

Explanation:

Given: pOH = 11.30

The relation between pH and pOH is as follows.

pH + pOH = 14

pH + 11.30 = 14

pH = 14 - 11.30

= 2.7

Also, pH is the negative logarithm of concentration of hydrogen ions.

pH = - log [H^{+}]

Substitute the values into above formula as follows.

pH = -log [H^{+}]\\2.7 = -log [H^{+}]\\conc. of H^{+} = 1.99 \times 10^{-3}

Thus, we can conclude that the concentration of hydrogen ions for this solution is 1.99 \times 10^{-3}.

4 0
3 years ago
Pt.3 of my questions because a bot answer it and no one could answer it
Andrei [34K]

Answer:

I cant see the whole question but to my knowledge it is the 3rd law

Explanation:

because the third law states what the applied force is when two objects interact

4 0
2 years ago
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