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Ann [662]
3 years ago
9

Someone please help me with this????

Chemistry
1 answer:
tensa zangetsu [6.8K]3 years ago
6 0

Answer:

D po ayan po ang sagot ko salamat po

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In the reaction MgCl2 + 2KOH Mg(OH)2 + 2KCl, if 3 moles MgCl2 are added to 4 moles KOH, what determines how much Mg(OH)2 is made
LenKa [72]
The correct option is C. The amount of MgCl2. we know this because <span>no matter how much you increase KOH, if you dont increase Mgcl2, the amount of Mg(OH)2 remains the same. Hope this works for you</span>
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3 years ago
In aqueous solution amino acids are rarely found in the neutral, unionized form.
True [87]

a. True.

There is always an equilibrium of the type

NH₃⁺CHRCOOH ⇌ NH₃⁺CHRCOO⁻ ⇌ NH₂CHRCOO⁻

The compound is <em>always in an ionized form</em>.

There are no unionized NH₂CHRCOOH molecules in the solution.

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3 years ago
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2 years ago
a student performed an analysis of a sample for it's calcium content and got the following results: 14.92%, 14.91%, 14.88%, 14.9
kramer
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5 0
3 years ago
A 1.00 L buffer solution is 0.112 M in acetic acid and 0.112 M in sodium acetate. Acetic acid has a pKa of 4.74. What is the pH
topjm [15]

Answer:

ΔpH = 1.25

Explanation:

Using Henderson-Hasselbalch formula:

pH = pka + log [CH₃COONa] / [CH₃COOH]

pH = 4.74 + log [0.112] / [0.112]

<em>pH = 4.74</em>

The reaction of sodium acetate (CH₃COONa) with HCl is:

CH₃COONa + HCl → CH₃COOH + NaCl

<em>Producing acetic acid, </em>CH₃COOH.

If 0.1mol of HCl reacts the final moles of CH₃COONa are:

0.112mol - 0,1 mol = 0.012mol

Moles of acetic acid are:

0.112mol + 0,1 mol = 0.212mol

Using Henderson-Hasselbalch formula:

pH = pka + log [CH₃COONa] / [CH₃COOH]

pH = 4.74 + log [0.012] / [0.212]

<em>pH = 3.49</em>

<em></em>

Change in pH, ΔpH = 4.74 - 3.49 =<em> 1.25</em>

I hope it helps!

6 0
2 years ago
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